19+ Covalent Oxide Example:Facts That You Should Know

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Covalent Oxides are binary compounds formed by the reaction of the oxygen with a non-metal which are held together by covalent-bonds. Some metalloids and transition metals also form covalent oxides. Here we will know about covalent oxide example

The examples covalent oxides formed by non-metals, transition metals, metalloids and alkaline earth metals are:

  1. Dinitrogen monoxide (N2O)
  2. Nitrogen monoxide (NO)
  3. Dinitrogen trioxide (N2O3)
  4. Nitrogen dioxide (NO2)
  5. Dinitrogen tetraoxide (N2O4)
  6. Dinitrogen pentoxide (N2O5)
  7. Nitrogen trioxide (NO3)
  8. Phosphorus(III) oxide (P4O6)
  9. Phosphorus(V) oxide (P4O10)
  10. Carbon monoxide (CO)
  11. Carbon dioxide (CO2)
  12. Carbon suboxide (C3O2)
  13. Sulfur dioxide (SO2)
  14. Chromium trioxide (CrO3)
  15. Manganese heptoxide (Mn2O)
  16. Silicon dioxide (SiO2)
  17. Diboron trioxide (B2O3)
  18. Arsenic pentoxide (As2O5)
  19. Antimony pentoxide (Sb2O5)
  20. Beryllium oxide (BeO)

1)Dinitrogen monoxide (N2O)   

It is a covalent oxide example formed by a non-metal. It is a colourless gas and has a pleasant odour. It is called as laughing gas .

2)Nitrogen monoxide (NO)

It is a covalent oxide example formed by a non-metal. It exists as colorless gas, colorless liquid and also as solid when pure. It is produced by oxidizing nitrogen

3)Dinitrogen trioxide (N2O3)

It is a covalent oxide example formed by a non-metal. It is a blue liquid. It exists only in liquid and solid state.

4)Nitrogen dioxide (NO2)          

It is a covalent oxide example formed by a non-metal. It exists as a brown gas. The molecules of nitrogen dioxide are paramagnetic in nature.

5)Dinitrogen tetroxide (N2O4)

It is a covalent oxide example formed by a non-metal. It exists as colorless liquid with an unpleasant odor. It is diamagnetic in nature.

6)Dinitrogen pentoxide (N2O5)    

It is a covalent oxide example formed by a non-metal. It exists as colorless solid.

7)Nitrogen trioxide (NO3)

It is a covalent oxide example formed by a non-metal. It exists as unstable radical. They are used in fertilizers.

8)Phosphorus(III) oxide (P4O6)

It is a covalent hexoxide example formed by a non-metal. It exists as white crystalline solid or liquid and smells like garlic. Though the correct name is tetraphosphorus hexoxide but the name phosphorus trioxide is still used today.

covalent oxide example
Phosphorus(III) oxide ( P4O6 )

9)Phosphorus(V) oxide (P4O10)

It is a covalent oxide example formed by a non-metal. It is a white flocculent powder. It is an acid anhydride of orthophosphoric acid.

image 4
Phosphorus(V) oxide (P4O10 )

10)Carbon monoxide (CO)

It is a covalent oxide example formed by a non-metal. It exists as a colorless, tasteless and odorless. It contains a triple bond between carbon and oxygen.

11)Carbon dioxide (CO2)

It is a covalent oxide example formed by a non-metal. It exists as colorless gas with no odor. It is a greenhouse gas.

12)Carbon suboxide (C3O2)

It is a covalent oxide example formed by a non-metal. It is a colorless and foul smelling gas.This gas is produced by dehydrating malonic acid

13)Sulfur dioxide (SO2)

It is a covalent oxide example formed by a non-metal. It exists as gas at room temperature.It is a colorless gas. It has choking smell.

Read more about H2CO lewis structure

14)Chromium trioxide(CrO3)

It is a covalent oxide example formed by a transition metal. It is a dark purple solid (when anhydrous) while bright orange (when wet).

15)Manganese heptoxide (Mn2O7)

It is a covalent oxide example formed by a transition metal. It is a volatile liquid. It is a basic oxide and is highly reactive.

16)Silicon dioxide (SiO2)

It is a covalent oxide example formed by a metalloid. It is also known as silica. It is a white or a colorless crystalline compound.

17)Diboron trioxide (B2O3)

It is a covalent oxide example formed by a metalloid. It is a colorless and a transparent solid. It is also known by the name Boric oxide.

18)Arsenic pentoxide (As2O5)

It is an example of a covalent oxide formed by a metalloid. It is a glassy, white solid. It is also known as Arsenic (V) oxide.

19)Antimony pentoxide (Sb2O5)

it is an example of a covalent oxide formed by a metalloid. It is a yellow powdered solid. It exists in the hydrated form.

20)Beryllium Oxide (BeO)

It is an example of covalent oxide formed by a alkaline earth metal. It is amphoteric in nature. It is the only element which forms a covalent oxide from group 2.

Conclusion:

Covalent oxides are formed by non-metals. Covalent oxides are acidic in nature. Covalent oxides react with base to form salt.When Covalent oxides react with water, they form acids.When covalent oxides react with bases, they form salts.

11 Facts on Hcl + H2o :With Several Elements Reaction

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In this article, we are going to discuss details on the reaction between HCl + H2O and also how to balance reactions with examples. HCl is one of the components of gastric juice

Hydrogen Chloride (HCl) gas which is highly soluble in water on dissolving in water forms Hydrochloric acid. The formula of hydrochloric acid is also HCl. Hydrochloric acid then dissociates in water and forms ions.

                 

 HCl + H2O Type of reaction  Exothermic reaction(as heat is evolved) 
Reversible chemical reaction(as equilibrium is formed)
Ionization Reaction (as ions are formed in the reaction)
Conjugate AcidHas one hydrogen more than the base
Conjugate BaseHas one hydrogen less than the acid
Conjugate acid-base pairs in  HCl + H2HCl and Cl
H3O+ and H2O
Type of ions formed in  HCl + H2O reactionH+(aq) or H3O+ and Cl(aq)  
In HCl + H2O reaction Acid is  HCl (Proton donor)
In HCl + H2O reaction Base is H2O (Proton acceptor)
Details of Reaction HCl + H2O
hcl + h2o
Dissolution Of HCl in water(HCl+H2O)

What happens when HCl reacts with H2O?

When hydrogen chloride gas (HCl) reacts water, it forms hydrochloric acid.

Hydrochloric acid (also has formula HCl) thus formed, dissociates completely in water to form H+ and Cl ions and large amount of heat is evolved in this reaction. Thus, this is an exothermic and ionization reaction

So, the reaction can be represented as

image 188

What type of reaction is HCl and H2O?

The reaction between HCl and H2O is an exothermic, reversible chemical reaction and an ionization reaction

image 189
  • Exothermic Reactions are those reactions in which heat is evolved and the temperature of the solution rises.
  • Reversible chemical reactions are those reactions in which the reactants react to give products and products can react to give the reactants back. In short reversible reactions are those reactions which can be reversed.
  • Ionization reactions is a chemical reaction in which a neutral atoms or molecules are converted into charged atoms or ions by give or take of electrons.  

What is conjugate acid-base pair? Explain giving example of HCl + H2O reaction.

According to Bronsted and Lowry Theory –

An acid is the species which donates a proton(H+) and base is the species which accepts a proton(H+).

  • The conjugate base is a substance formed when an acid loses a proton(H+) to a base.
  • The conjugate acid is a substance formed when a base gains a proton(H+) from an acid.

Thus in short, an acid-base pair differs from each other either by the presence of a proton or by the absence of a proton.

For Example –

image 211

In the above example –

HCl and Cl are the conjugate acid-base pairs and H2O and H3O+ are the conjugate acid-base pairs.

Is HCl and H2O an Exothermic or Endothermic reaction?

HCl + H2O is an exothermic reaction as large amount of heat is evolved in this reaction and temperature of the solution rises.

Write the net ionic Equation of HCl + H2O reaction.

The reaction HCl + H2O takes place as follows –

image 197

 

Equation 3) is the net ionic Equation of HCl + H2O reaction.

In the reaction HCl + H2O, which one is acting as acid and which is acting as base?

According to Bronsted-Lowry definition of acids and bases

An acid is the species which donates a proton(H+)

A Base is the species which accepts a proton(H+).

Now our reaction is –

image 199

In the above equation, same subscript is used for each acid-base pair.According to Bronsted-Lowry theory, an acid is a species which donates a proton to a base so in the above equation

  • HCl is an acid which donates a proton to the base H2O and in doing so HCl gets converted to Clwhich is the conjugate base of HCl.
  • H2O is a base which accepts a proton from HCl and in doing so H2O get converted into H3O+which is the conjugate acid of H2O

The conjugate base, Cl is one hydrogen less than its acid HCl

The conjugate acid, H3O+ is one hydrogen more than its base H2O

How to balance the following Reaction?

Given reaction is-

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When Hydrogen Chloride gas reacts with water, it forms Hydrochloric acid which being a strong dissociates completely dissociates in water to form hydrogen ion and Chloride ion.

To balance this equation, we will count the atoms on both the reactant and the product sides-

ElementNumber of atoms in the Reactants (LHS)Number of atoms in the Products (RHS)
Hydrogen3 3
Chlorine11
Oxygen11
Balancing the number of the elements on the Reactant and Product side

The number of atoms at both the reactant and product side are the same so the reaction is a balanced one.

so the balanced Equation is –

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How to balance the reaction Al2O3 + HCl?

Al2O3 (Aluminium Oxide) reacts with dilute HCl (Hydrochloric acid) and produce AlCl3 (Aluminium Chloride) and H2O (water)

Given reaction is –

image 202

Balancing the reaction –

image 204
ElementNumber of atoms in the Reactants (LHS)Number of atoms in the Products (RHS)
Aluminium2*2 = 41*4 = 4
Oxygen3*2 = 61*6 = 6
Hydrogen1*12=122*6 = 12
Chlorine1*12=123*4 = 12
Balancing the number of the elements on the Reactant and Product side

As all the atoms have become equal on both sides of the reaction so the reaction is now balanced.

Balanced reaction is –

image 204

How to balance the reaction COCl2 + HCl?

Cobalt(ll) Chloride reacts with hydrogen chloride and forms tetrachlorocobaltate(2-) and hydrogen gas.

Given reaction is –

image 187

 Balancing the Reaction –

image 206
ElementNumber of atoms in the Reactants (LHS)Number of atoms in the Products (RHS)
Cobalt11
Chlorine2 + 1*2 = 44
Hydrogen1*2=22
Balancing the number of the elements on the Reactant and Product side

As all the atoms have become equal on both sides of the reaction so the reaction is now balanced.

Balanced reaction is –

image 208

Is HCl(l) + H2O(l) equal to HCl(aq)?

No, this is not the correct Equation. It should be written as

image 209

The term aqueous means a solution in which solvent is water, so when we are writing the phase of the substance as aqueous no need to write plus water (refer equation 2)

As Hydrogen Chloride (HCl) exists as a gas at STP that is at standard temperature and pressure so HCl is commonly stored as a concentrated aqueous solution that is Hydrochloric acid.

When HCl is dissolved in water, it dissociates completely into H+ and Cl(aq). The H+ formed combines with water to form H3O+that is Hydronium ion.

Conclusion:

HCl + H2O is a reversible reaction. It is an exothermic reaction and large amount of heat is released in this reaction and Haq)and Cl(aq) ions are formed.

7 Steps on N(ch3)3 Lewis Structure, Hybridization( Solved !)

N(ch3)3 Lewis Structure

Trimethylamine (N(CH3)3) has a nitrogen (N) atom with five valence electrons, each bonded to a methyl group (CH3) with one valence electron from carbon (C). The Lewis structure shows three single N-C bonds and a lone pair on nitrogen, totaling 8 electrons around N. The molecular geometry is trigonal pyramidal with bond angles slightly less than 109.5° due to lone pair-bond pair repulsion. The molecule is polar, influenced by the lone pair on nitrogen and the arrangement of methyl groups. The electronegativity of N (3.04) relative to C (2.55) also contributes to its reactivity and interactions.

The present article contains detail information of N(CH3)3 Lewis Structure. N(CH3)3 exists as a gas at room temperature. It is an organic compound which possess a fish-like odor.

The Lewis structure of N(CH3)3 consists of central atom nitrogen and three methyl groups surrounding the central atom. There is a lone pair on central atom nitrogen in the Lewis structure of Trimethylamine.

N(ch3)3 Lewis Structure
N(ch3)3 Lewis Structure

                                   

Molecular formula N(CH3)3 or C3H9N
Chemical Name Trimethylamine
N,N-Dimethylmethanamine
Lone pairs on the central atom 1
Number of valence electrons in N(Ch3)3 26
Molecular Geometry of N(CH3)3 Trigonal pyramidal
Electron Geometry of N(CH3)3 Tetrahedral
Bond Angle C-N-C 108 degrees
Resonance Effect Do not show resonance
Octet Rule Follows the octet Rule
Formal charge 0
Hybridisation of the central atom Sp3
Polar or non-polar Polar
Solubility in water Soluble in water
Acidic or basic Basic
symmetric Or Asymmetric Asymmetric
Characteristics of N(CH3)3
n(ch3)3 lewis structure
Lewis Structure of N(CH3)3

                 

Valence electrons in N(CH3)3 Lewis structure

In the Lewis structure of Trimethylamine the central Nitrogen atom, Carbon and the hydrogen atom has 5,4 and 1 electron respectively.

Types of atoms Valence electrons Number of atoms Valence electrons in N(CH3)3
Nitrogen 5 1 5*1 = 5
Carbon 4 3 4*3 = 12
Hydrogen 9 1 9*1 = 9
                26
Valence Electrons in Lewis structure of N(CH3)3

so, the number of valence electrons in Lewis N(CH3)3 is 26

How to draw N(CH3)3 Lewis structure?

Lewis structures are the drawings which show the patterns of bonding in the compound. These structures show the number of bonding and also the number of non-bonding electrons present in the compound.

Lewis structure of N(CH3)3 can be drawn in the following steps –

Step 1: Calculate the number of valence electrons

Valence electrons in central atom nitrogen, carbon and hydrogen are 5,4 and 1 respectively.

Types of atoms Valence ele ctrons Number of atoms Valence electrons in N(CH3)3
Nitrogen 5 1 5*1 = 5
Carbon 4 3 4*3 = 12
Hydrogen 9 1 9*1 = 9
                26
Valence Electrons in Lewis structure of N(CH3)3

So, the number of valence electrons in Trimethylamine is 26.

Step 2: Find out the central atom

Central atom in the Lewis structure.is usually the atom which has lowest subscript in the compound so Nitrogen is the central atom in N(CH3)3.

The skeletal structure of N(CH3)3 is –

image 113
Skeletal structure of N(CH3)3

                            

Step 3: Place a bond or a electron pair between Nitrogen and Carbon atoms and also Carbon and Hydrogen atoms

Nitrogen forms 3 bonds with 3 carbon atoms in N(CH3)3 Lewis structure.

image 116
Step 3:how to draw lewis structure

               

Step 4: Complete octet of central Nitrogen atom

After completing the octet of the central atom, we see that the central nitrogen atom has a lone pair of electrons.

image 122
Lewis Structure of N(CH3)3

                                 

Step 5: Check for the stability of the Lewis structure by finding out the formal charge on atoms in N(CH3)3

Formula for formal charge:

Formal charge = valence electrons – 0.5*bonding electrons – non-bonding electrons

Formal charge on nitrogen:

Formal charge = 5 – 0.5*6 – 2

= 0

The formal charge on nitrogen is 0

Formal charge on carbon atom:

Formal charge = 4 – 0.5*8 – 0

= 0

Formal charge on carbon is 0

Formal charge on hydrogen atom:

Formal charge = 1 – 0.5*2 – 0

= 0

Formal charge on hydrogen is 0

As the formal charge on all the atoms in N(CH3)3 is 0

So, we have got our perfect Lewis structure.

                                      

How many lone pairs are present in the Lewis structure of N(CH3)3?

Formula to find the lone pairs are –

Lone pairs = 0.5*(Valence Electrons of central atom– Number of atoms attached to the central atom)

= 0.5*(5 – 3)

                   = 1

So, the number of lone pair present on the central Nitrogen atom is 1.

 

Does N(CH3)3 follow the octet rule?

N(CH3)3 contains 26 valence electrons. All the atoms in N(CH3)3 have completed their octet as can be seen from the Lewis structure of N(CH3)3. Thus, N(CH3)3 follows the octet rule.

Formal Charge on each atom in the Lewis structure of N(CH3)3

Formula for formal charge:

Formal charge = valence electrons – 0.5*bonding electrons – non-bonding electrons

Formal charge on nitrogen:

Formal charge = 5 – o.5*6 – 2

= 0

The formal charge on nitrogen is 0

Formal charge on carbon atom:

Formal charge = 4 – 0.5*8 – 0

= 0

Formal charge on carbon is 0

Formal charge on hydrogen atom:

Formal charge = 1 – 0.5*2 – 0

= 0

Why is the C-N-C bond angle in N(CH3)3 is 108 degrees?

Due to the repulsion between the lone pair present on the central nitrogen atom and bonded pairs the tetrahedral angle decreases in trimethylamine from 109.5 degrees to 108 degrees.

image 119
Bond Angle in N(CH3)3

                                          

What is the hybridization of Nitrogen in N(CH3)3?

Hybridization of central atom can be found out by using the formula –

Hybridization number = number of atoms attached to the central atom + number of lone pairs present on the central atom

Hybridization Number for Nitrogen in N(CH3)3 = 3 + 1 = 4

so hybridization of central atom nitrogen in N(CH3)3 is sp3.

What is molecular and electron geometry of N(CH3)3 compound?

We know that hybridization of the central atom in N(CH3)3 is sp3 and 1 lone pair is present on the central atom Nitrogen

So according to AXnEx notation of VSEPR theory,

Where –

A is for the central atom

X is for the surrounding atoms, n is number of surrounding atoms

E is for the lone pairs on the central atom, x is for the number of lone pairs.

AXnEx notation for N(CH3)3 is AX3E1 as nitrogen is bonded to three methyl groups and it has a lone pair on it.

Now, AX3E1 notation corresponds to Molecular geometry as Trigonal Pyramidal and Electron Geometry as Tetrahedral in accordance with the VSEPR Chart.

Total Domains General Formula Bonded atoms Lone Pairs Molecular Shape Electron Geometry
1 AX 1 0 Linear Linear
2 AX2 2 0 Linear Linear
AXE 1 1 Linear Linear
3 AX3 3 0 Trigonal Planar Trigonal Planar
AX2E 2 1 Bent Trigonal Planar
AXE2 1 2 Linear Trigonal Planar
4 AX4 4 0 Tetrahedral Tetrahedral
AX3E 3 1 Trigonal Pyramid Tetrahedral
AX2E2 2 2 Bent Tetrahedral
AXE3 1 3 Linear Tetrahedral
VSEPR chart

so the molecular geometry of N(CH3)3 is Trigonal Pyramidal and the Electron geometry is Tetrahedral.

image 120
Geometry of N(CH3)3

                                                

Why is N(CH3)3 a weak base?

N(CH3)3 is a weak base because of presence of bulky methyl groups around the central nitrogen atoms which makes it difficult for the proton to approach for bonding.  

Why is Trimethylamine a polar compound?

Electronegativity of Nitrogen is 3.0 and carbon is 2.5

A molecule is said to be polar when the difference in the electronegativity of its atoms is greater than 0.4

The difference in electronegativity of Nitrogen and Carbon is 0.5

This means that N(CH3)3 has positive and negative ends. This makes N(CH3)3 molecule polar in nature.

Is N(CH3)3 symmetrical or asymmetrical?

N(CH3)3 (Trimethylamine) is asymmetrical molecule as it is a polar molecule and contains positive and negative ends.

Is N(CH3)3 linear?

No, N(CH3)3 is trigonal pyramidal in shape.

Why does N(CH3)3 compound not show resonance?

  • Resonance is shown by such compounds in which there is a possibility for the delocalization of electrons.

In N(CH3)3, the lone pair is localized on the central atom Nitrogen.

  • For showing resonance, all atoms should lie in one plane. In N(CH3)3, the nitrogen is sp3 hybridized so all atoms do not lie in one plane.

That’s why N(CH3)3 compound does not show resonance.

Is N(CH3)3 tetrahedral?

Yes, the electron geometry of N(CH3)3 is tetrahedral as for electron geometry we consider both the bonded atoms as well as the lone pairs

Conclusion:

In a nutshell, N(CH3)3 is a polar compound. The molecular geometry of N(CH3)3 is Trigonal Pyramidal while the Electron Geometry is Tetrahedral. N(CH3)3 is basic in nature.

Also Read:

Clf5 lewis structure,Characteristics:13 Facts You Should Know

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The present article is about ClF5 (Chlorine Pentafluoride) which is an interhalogen compound. Let’s know some interesting facts about this compound.

In the ClF5 Lewis structure, central Chlorine (Cl) atom is bonded to 5 fluorine(F) atoms by single bonds. The ClF5 molecule contains 16 lone pairs, each Fluorine atom has 3 lone pairs and one lone pair is present on the chlorine atom.

                                                

Molecular Name Chlorine Pentafluoride
Chemical Formula ClF5
Central atom of the lewis structure Chlorine
Number of lone pairs on central atom  1
Molecular Geometry of OF2 Square pyramidal
Electron Geometry of OF2 octahedral
Bond Angle (Cl – F) 90 degree
No. of valence electron for ClF5 42
The formal charge of ClF5 molecule 0
Hybridization of central atom sp3d2
Solubility Reacts with water
Nature Neutral compound
Nature of bonds Covalent bonds
Characteristics Of ClF5
image 78
Lewis structure of ClF5

                                      

How many valence electrons are present in the ClF5 Lewis structure?

In the ClF5 molecule, chlorine atom as well as the fluorine atom has 7 electrons in its valence shell.

Calculating valence electrons in ClF5 molecule-

Atoms in ClF5 Valence Electrons Number of atoms in ClF5 Total Electrons
Chlorine         7           1 7*1 =   7
Fluorine         7           5 7*5 = 35
                 42
Calculation of valence electrons of ClF5

Thus,

  in ClF5 molecule there are total 42 valence electrons.

Steps to draw Lewis structure of ClF5

The step-by-step explanation to draw the Lewis diagram of ClF5 –

 Step 1: Calculate total valence electrons present in ClF5 molecule

We will start by finding the number of valence electrons in ClF5 molecule.

(Valence electrons are the number of electrons present in the valence shell of an atom)

Both the elements that is Fluorine and Chlorine belongs to group 17th so number of valence electrons for both Chlorine and Fluorine is 7.

Calculating valence electrons in ClF5 –

Atoms in ClF5 Valence Electrons Number of atoms in ClF5 Total Electrons
Chlorine         7           1 7*1 =   7
Fluorine         7           5 7*5 = 35
                 42
Valience electrons of ClF5

Step 2: Decide the central atom

While drawing the Lewis dot structure always keep the least electronegative atom in the centre.

As we know that electronegativity increases in a period from left to right and decreases from top to bottom in a group so chlorine is less electronegative than fluorine.

Note: Fluorine is the most electronegative element in the periodic table

keep the least electronegative atom Chlorine in the centre and the 5 Fluorine atom surrounding it and draw the skeletal structure for ClF5 molecule.

                          

image 79
Step 2: Skeletal structure of ClF5

Step 3: Either put a bond or electron pair between Cl and F atom

 Put two electrons (electron pair) between Chlorine and Fluorine atoms to denote a chemical bond.

image 80
step 3: Drawing Lewis structure of ClF5

                               

Step 4: Make the outer atoms happy by completing their octet

Main group elements got happy when they have attained octet configuration of their nearest noble gas element (18th group). This is what we call as Octet Rule (Exception: hydrogen completes the duplet configuration like that of the noble gas He).

image 81
Step 4: Drawing Lewis Structure of ClF5

                                

Step 5: Put the remaining electrons on the central atom:

ClF5 has 42 valence electrons, out of which 10 electrons are used in forming bonds between Cl and F while 30 electrons are present as lone pairs on the surrounding 5 fluorine atoms and two electrons are left.

we will now keep these two electrons on the central Chlorine atom.

                                                      

image 82
Step 5: Drawing Lewis structure of ClF5

Step 6: Check formal charge value

Before confirming this as our final Lewis structure diagram, we will check for the formal charge of each atomic element in the ClF5 molecule.

Formal charge = Valence electrons – 0.5 * bonding electrons – non-bonding electrons

For the central atom Chlorine –

Number of non-bonding electrons of chlorine = 2

Number of bonding electrons of chlorine = 10

Formal Charge for Chlorine = 7 – 0.5*10 – 2 = 0

For the outer atoms Fluorine –

Number of non-bonding electrons of fluorine = 6 (3 lone pairs)

Number of bonding electrons of fluorine = 2

Formal charge for fluorine atom =7 – 0.5*2 – 6 = 0

As the F and O elements have least possible formal charges, that means we have obtained our perfect Lewis structure.

image 83
Lewis structure of ClF5

What is the formal charge of atoms present in the Lewis Structure ClF5 molecule?

Formal charge is the electric charge given to an atom in a molecule when all of the electrons in a bond are shared equally or while ignoring the electronegativity difference of atoms.

Formal charge = Valence electrons – 0.5 * bonding electrons – non-bonding electrons

For the central atom Chlorine –

Number of non-bonding electrons of chlorine = 2

Number of bonding electrons of chlorine = 10

Formal Charge for Chlorine = 7 – 0.5*10 – 2 = 0

For the outer atoms Fluorine –

Number of non-bonding electrons of fluorine = 6 (3 lone pairs)

Number of bonding electrons of fluorine = 2

Formal charge for fluorine atom =7 – 0.5*2 – 6 = 0

Does ClF5 is an exception to octet rule?

As per the octet rule, main group elements tries to get an octet configuration of their nearest noble gas element. In ClF5 molecule, all the 5 Fluorine atoms attain their octet. All the 5 Fluorine atoms have three non-bonded pairs and a bonded pair around them.

But the central Chlorine atom has five bonded pairs and one lone pair around it, making total surrounding electrons 12.

Thus, ClF5 molecule is an exception to the octet rule.

Why is the Electron Geometry of ClF5 is octahedral though the molecule has a square pyramidal geometry?

ClF5 molecule has 42 valence electrons.

Out of 42 electrons –

  • 10 electrons are present as bonded pairs between fluorine and chlorine atoms
  • 30 electrons are present as lone pairs on the five Fluorine atoms.
  • Two electrons are present on central atom Chlorine as lone pairs.

As electron geometry is found by considering both the bonded pairs and lone pairs in a molecule so the electron geometry of Clf5 molecule is square pyramidal.

image 84
Octahedral Geometry of ClF5

Why is the bond angles in ClF5 are slightly less than 90 degrees and not exactly 90 degrees?

Due to the presence of lone pair on the central chlorine atom which causes repulsion with the bond pairs, the bond angle of axial and equatorial F gets distorted which results in less than 90 degrees bond angles.

Thus the bond angles in ClF5 are slightly less than 90 degrees.

image 84
Octahedral Geometry of ClF5

                                                       

How to find out molecular/Electron geometry of ClF5 molecule?

To answer this question, we will use VSEPR model –

The long form of VSEPR is Valence Shell Electron Pair Repulsion theory

By using VSEPR theory, we can know the 3-dimensional molecular geometry of any molecule which we can’t do by  using the Lewis Structure which can  only predicts the 2-dimensional geometry.

Geometry of ClF5 can be found out by the following ways –

1)Number of lone pairs present on the Chlorine (Cl) in its Lewis structure is –

           Lone pair = 0.5*(valence electrons On Cl – No. of Atoms attached to Cl)

                             = 0.5*(7-5)

                             = 1     

2) Hybridization of Chlorine atom –

         Hybridization of Chlorine in ClF5 is –

  Hybridization number = No. of atoms attached to Cl + NO. of lone pairs on Cl

                                          = 5 + 1

                                          = 6

As the hybridization number of 6 so the hybridization of ClF5 molecule is sp3d2

3) Using VSEPR notation to get the molecular geometry –

Now the VSEPR notation is AXnEx

AXnEx notation

Where,

 A is the central atom

 (In ClF5, chlorine is the central atom)

 X are the atoms bonded to the central atom,

(In ClF5, F are the atoms bonded to the central atom)

n is the number of atoms

(In ClF5, n=5)

 E is lone pairs of electrons present on the central atom

x is the number of lone pairs

(In ClF5, x=1)

So, for ClF5 molecule AXnEx formula is AX5E1

According to VSEPR chart, the molecule with AX5E1 formula has molecular shape as Square Pyramidal.

Total Domains General Formula Bonded atoms Lone Pairs Molecular Shape Electron Geometry
1 AX 1 0 Linear Linear
2 AX2 2 0 Linear Linear
  AXE 1 1 Linear Linear
3 AX3 3 0 Trigonal Planar Trigonal Planar
  AX2E 2 1 Bent Trigonal Planar
  AXE2 1 2 Linear Trigonal Planar
4 AX4 4 0 Tetrahedral Tetrahedral
  AX3E 3 1 Trigonal Pyramid Tetrahedral
  AX2E2 2 2 Bent Tetrahedral
  AXE3 1 3 Linear Tetrahedral
5 AX5 5 0 Trigonal bipyramid Trigonal bipyramid
  AX4E 4 1            See Saw Trigonal bipyramid
  AX3E2 3 2 T Shape Trigonal bipyramid
  AX2E3 2 3 Linear Trigonal bipyramid
6 AX6 6 0 Octahedral Octahedral
  AX5E 5 1 Square pyramid Octahedral
  AX4E2 4 2 Square planar octahedral
VSEPR Chart

                                                             

As ClF5 has AX5E1 notation so the molecular geometry of ClF5 is Square Pyramidal 

        

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Description automatically generatedSquare pyramidal geometry of ClF5

                                                                                                                                                                                                                                                                       

Why is ClF5 a polar molecule?

A molecule is called polar when –

  • Electronegativity difference between the bonded atoms is more than O.4
  • It contains a polar bond with a positive and a negative end.
  • It has unsymmetrical geometry so the dipoles do not get cancelled.

But sometimes molecule with polar bond can turn out to be non- polar due to the symmetrical distribution of charges so resultant dipole moment is 0.

Chlorine Pentafluoride (ClF5) is a polar molecule because of the following reasons –

  • Electronegativity difference between Chlorine (Electronegativity 3.16) and Fluorine (Electronegativity 3.98) is 0.82
  • ClF5 is an unsymmetrical molecule as central atom Chlorine has lone pair present on it.

Hybridization in ClF5

Hybridization is the fusion of atomic orbitals of the atom in a molecule to form orbitals of equal energy and orientation

In ClF5, the central Chlorine atom forms five single bonds with 5 fluorine atoms and a lone pair is present on it.

To form bonds with fluorine atoms, the orbitals of Chlorine atom undergoes hybridization .

The ground state electronic configuration of chlorine and fluorine are –

Chlorine (ground state): 1s2 2s2 2p6 3s2 3p5

Fluorine (ground state): 1S2 2S2 2P5

Electronic configuration of Chlorine after gaining electrons by forming bonds with fluorine-

Chlorine 1s2 2s2 2p6 3s2 3p5

Steric Number = Number of sigma bonds surrounding the central atom + Number of lone pairs of electrons on the central atom

Steric Number = 5 + 1 = 6

So, hybridization for chlorine in the ClF5 molecule is Sp3d2

Does ClF5 exhibits resonance?

A molecule can exhibit resonance when –

  • There is an interaction between two pi-bond in the molecule

             or

  • There is an interaction between a pi bond and a lone of electrons present on an adjacent atom in a molecule.

ClF5 do not show resonance as there are no pi-bonds present in ClF5 molecule. 

Why is Chlorine Pentafluoride a covalent compound even though it contains electronegative atoms?

As the electronegativity difference between the halogens, Chlorine and Fluorine is low so ClF5 is a covalent compound.

Is ClF5 neutral in nature?

Yes, ClF5 is a neutral in nature containing two different halogen atoms -One Chlorine and five Fluorine atoms.

Conclusion:

Chlorine Pentafluoride is an interhalogen compound. It does not follow the octet rule. It has a square pyramidal geometry. ClF5 is a polar molecule with a dipole moment of 0.82D. It does not show resonance.It is neutral in nature.

Also Read:

Cfcl3 lewis structure,Characteristics:13 Must To Know Facts

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This article is about CFCl3 which is a greenhouse gas and is responsible for ozone depletion. Let’s have a look at some of its interesting characteristics –

The CFCl3 Lewis structure consists of one central atom carbon, 3 chlorine atoms and a fluorine atom are present around the carbon atom. The Lewis structure of CFCl3 molecule has 12 lone pairs.

                     

Molecular Name Trichlorofluoromethane
Also known as CFC-11                          
  Freon-11                              
R-11Chemical FormulaCFCl3Central atom of the lewis structureCarbonlone pairs present on the central atom 0Molecular Geometry of CFCl3Tetrahedral  Electron Geometry of CFCl3TetrahedralBond angle in CFCl3109.5No. of valence electron for CFCl3
32
The formal charge of CFCl3 molecule 0
Nature of the compound CFCl3 is an inert compound
Characteristics of CFCl3

How should we draw the Lewis dot structure for CFCl3?

The steps to be followed while drawing the Lewis structure of CfCl3 molecule are as follows –

 Step 1: Find the total valence electrons in the CFCl3 molecule

First step is to find the no. of valence electrons present in CFCl3 molecule.

Carbon is a member of group 14th while Fluorine and Chlorine are the members of group 17th of the periodic table.

Carbon has valence electrons = 4

Chlorine has valence electrons = 7

Fluorine has valence electrons = 7

  Valence electrons Atom In CBr4 Total Electrons
C              4         1  4*1= 4
F              7         1  7*1= 7
Cl              7         3  7*3= 21     
                 32
Valence electrons for CFCl3

Step 2: Get the least electronegative element present in CFCl3

In a period, as we move from left to right Electronegativity increases so carbon is least electronegative than chlorine and fluorine. We have to keep the least electronegative atom in the centre.

The skeletal structure of CFCl3 molecule is as follows –

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Description automatically generatedstep2:
Skeletal Structure of CFCL3

Step 3: Keep two electrons or a bond between C, F and Cl atoms

                                    

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Description automatically generatedStep 3: Drawing Lewis structure of CFCl3

Step 4: Now find the number of electrons which can make the outer atoms happy

The outer atoms will be happy when they have achieved the octet configuration of their nearest noble gas element belonging to group 18th.This is what we call the Octet Rule. Except hydrogen which tries to attain the duplet configuration like He.

Complete the octet of the surrounding atoms

                                                    

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Description automatically generatedstep 4: Drawing Lewis structure Of CFCl3

                                    

Step 5: Place the remaining electrons on the central atom. If the octet of the central atom is not achieved, we can move the lone pairs from the outer atoms to make multiple bonds if required

This step is not required for CFCl3 as the central atom’s octet is already

Completed.

                                 

Step 6: We can now check the stability of the Lewis structure by checking the formal charge values

Before accepting the structure as a perfect Lewis structure, we will check the formal charge for the atoms present in CFCl3

Formal charge = Valence electrons – 1/2*bonding electrons – non-          bonding electrons

The formal charge for Carbon is –

The valence electrons of Carbon are 4

The non-bonding electrons of carbon are 0

The bonding electrons of carbon are 8 (4 pairs)

The formal charge for carbon atom = 4 – 1/2*8 – 0 = 0

The formal charge for Fluorine is –

The valence electrons of Fluorine are 7

The non-bonding electrons of Fluorine are 6 (3 lone pairs)

The bonding electrons for Fluorine are 2

The formal charge for Fluorine atom = 7 – 1/2*2 – 6 = 0

The Formal charge for Chlorine is – 

The valence electrons of Chlorine are 7

The non-bonding electrons of Fluorine is 6 (3 lone pairs)

The bonding electrons for Fluorine are 2

The formal charge for Fluorine atom = 7 – 1/2*2 – 6 = 0

As the C, F and Cl elements have least possible formal charge, we have obtained suitable Lewis structure

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Description automatically generatedLewis structure of CFCl3

What is the formal charge of CFCl3 and how to calculate the formal charge values for CFCl3?

 Let’s calculate the formal charge for CFCl3 –

Formal charge = Valence electrons – 1/2*bonding electrons – non-bonding electrons

The formal charge for Carbon is –

The valence electrons of Carbon are 4

The non-bonding electrons of Carbon are 0

The bonding electrons for Carbon are 8 (4 pairs)

The formal charge for Carbon atom = 4 – (1/2) * 8 – 0 = 0

The formal charge for Fluorine –

The valence electrons of Fluorine are 7

The non-bonding electrons of Fluorine are 6 (3 lone pairs)

The bonding electrons for Fluorine are 2

The formal charge for Fluorine atom =7 – (1/2) * 2 – 6 = 0

The formal charge for chlorine is –

The valence electrons of Chlorine are 7

The non-bonding electrons of Chlorine are 6 (3 lone pairs)

The bonding electrons of Chlorine are 2

The formal charge for Chlorine atom = 7 – (1/2) * 2 – 6 = 0

The formal charge on carbon, fluorine and chlorine atom in CFCl3 Lewis dot structure is zero.

How can we know whether CFCl3 molecule follows the octet rule?

CFCl3 contains 32 valence electrons. Each and every atom of CFCl3 complete its octet that can be confirmed from the Lewis structure of CFCl3 molecule. This confirms that CFCl3 molecule follows the octet rule.

How to find the molecular shape and electron geometry of CFCl3 molecule?

We can find the molecular and electron geometry of CFCl3 molecule in  three simple steps  –

1) Calculate the non-bonding electron pairs on the central atom carbon

 Lone Pair = (1/2) * (V.E. –N.A.)

Here –

V.E. stands for the valence electrons on the central atom

N.A stands for the number of atoms which are bonded to the central atom

The central atom carbon in CFCl3 molecule has 4 valence electrons and 4 atoms are attached to it.

Lone Pairs = (1/2) * (4 – 4) = 0

2) Find out the hybridization number of the central atom

We can know the hybridization of central atom with the help of the formula –

Hybridization number = N.A. + L.P

Where-

N.A. stands for the number of atoms attached to the central atom

L.P.  stands for the number of lone pairs on the central atom

The central carbon atom has 4 atoms bonded to it and there are no lone pairs on it.

 The central atom in CFCl3 molecule is Sp3 hybridized.

3) Determine molecular/electron geometry of CFCl3 molecule by using VSEPR Theory

We have already found out the hybridization of CFCl3 as Sp3 and there are no lone pairs present on the central atom.

Now find the VSEPR notation for CFCl3 molecule according to AXnEx notation of VSEPR theory

In AXnEx notation  –

 A stand for the central atom

 X stands for the number of atoms attached to the central atom

  E stands for the number of lone pairs of electrons on the central atom

In accordance with to the Trichlorofluoromethane Lewis structure, carbon is the central atom to which 1 fluorine atom and 3 chlorine atoms are attached.

The central atom carbon has no lone pairs present on it so the formula of CFCl3 comes out to be AX4

Using the VSEPR chart, molecule having AX4 formula has tetrahedral molecular shape and electron geometry also tetrahedral.

Total Domains General Formula Bonded atoms Lone Pairs Molecular Shape Electron Geometry
1 AX 1 0 Linear Linear
2 AX2 2 0 Linear Linear
  AXE 1 1 Linear Linear
3 AX3 3 0 Trigonal Planar Trigonal Planar
  AX2E 2 1 Bent Trigonal Planar
  AXE2 1 2 Linear Trigonal Planar
4 AX4 4 0 Tetrahedral Tetrahedral
  AX3E 3 1 Trigonal Pyramid Tetrahedral
  AX2E2 2 2 Bent Tetrahedral
  AXE3 1 3 Linear Tetrahedral
VSEPR CHART

           Thus, the molecular geometry and also the electron geometry of CFCl3 is Tetrahedral.                                 

Is CFCl3 molecule polar or non-polar?

CFCl3 is a polar molecule is confirmed by three factors –

1)Electronegativity:

Chlorine (electronegativity 3.0) and Fluorine (electronegativity 4.0) are more electronegative than carbon (electronegativity2.5). As chlorine and fluorine are more electronegative than carbon, there is a separation of charges between carbon and chlorine/fluorine.

Fluorine is even more electronegative so there is a charge separation between carbon and fluorine but charge separation of C-F is in the opposite direction

to that of the charge separation by C-Cl.

A molecule is said to be polar when the difference in electronegativity between the atoms in the given molecule is more than 0.4 debye.

2)Geometrical/Molecular Shape: 

Geometrical Structure of CFCl3 molecule is tetrahedral.

The four dipoles of three C-Cl bonds and one C-F bond are in opposite directions.

3)Dipole Moment:

CFCl3 has Dipole moment of 0.45D

All these factors show that CFCl3 is a polar molecule.

What is the hybridization for CFCl3 molecule?

The four valence electrons of the central atom carbon atom are shared with 3 chlorine atoms and 1 Fluorine atom. To share the electrons with fluorine and chlorine, the orbitals of carbon atom undergo sp3 hybridization.

The electronic configuration of Carbon in ground state is 1s2 2s2 2p2

The electronic configuration of Chlorine in ground state is 1s2 2s2 2p6 3s2 3p5

The electronic configuration of Fluorine in ground state 1s2 2s2 2p5

The electronic configuration of Carbon after carbon has gain four electrons from three Chlorine atoms and one Fluorine atom is –  1s2 2s2 2px2 2py2 2pz2

Steric Number = Number of atoms attached to the central atom + Number of lone pairs of electrons on the central atom

Steric Number = 4 + 0 = 4

So in CFCl3, the central atom carbon is  Sp3 hybridised.

Is CFCl3 molecule show resonance?                                             

A molecule can only show resonance either when the molecule has either conjugate bonds or it has lone pair in conjugation with the double bond.

Trichlorofluoromethane does not possess double bond so CFCl3 do not show resonance.

Is CFCl3 a covalent compound?

CFCl3 is a covalent compound as the C-F and all the three C-Cl bonds in CFCl3 are formed by sharing of electrons.

What Is the geometry of CFCl3?

The C-F and C-Cl bond lengths in CFCL3 are different so CFCl3 has slightly distorted tetrahedral geometry.

                                                     Tetrahedral geometry of CFCl3

What is the bond angle in CFCl3 molecule?

In the CFCl3 molecule, C-Cl and C-Cl bond pair repulsions are more than the C-F and C-Cl bond pair repulsions

The Cl-C-Cl angles measure slightly more than F-C-F bond angle.

The bond angle in CFCl3 is around 109.5 degrees.

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Description automatically generatedBond angle in CFCl3

Is CFCl3 an acidic or a basic compound?

CFCl3 is neither acidic nor basic in nature. CFCl3 is an inert compound.

But as it comes in contact with the ozone, it undergoes photolysis and gives out chlorine atoms which causes depletion of the ozone layer.

Is CFCl3 soluble in water?

No, CFCl3 not soluble in water. This can be known by the fact it does not get washed out from the atmosphere by precipitation.

Conclusion:

The CFCl3 also known as Freon-11 or CFC-11 is a green house gas.The molecular geometry and also the electron geometry of CFCl3 is tetrahedral. The CFCl3 is insoluble in water. CFCl3 is an inert compound.

Also Read:

5 Steps to Draw Cbr4 Lewis Structure,Hybridization (Solved!)

CBr4 Lewis Structure

Carbon tetrabromide (CBr4) has a central carbon (C) atom with 4 valence electrons, bonded to four bromine (Br) atoms, each contributing 7 valence electrons. The Lewis structure shows four single C-Br bonds, with 8 bonding electrons and no lone pairs on carbon. The molecule adopts a tetrahedral geometry with bond angles of about 109.5°. Despite the polar C-Br bonds due to electronegativity differences (C: 2.55, Br: 2.96), CBr4 is nonpolar overall due to its symmetrical structure. This symmetry influences its physical properties and chemical behavior.

CBr4 Lewis Structure
CBr4 Lewis Structure

Facts on CBr4                      

Molecular Name Tetrabromomethane
Carbon Tetrabromide Chemical FormulaCBr4Central atom of the lewis structureCarbonlone pairs present on the central atom 0Molecular Geometry of CBr4TetrahedralElectron Geometry of CBr4TetrahedralBond Angle Br – C – Br109.5 degreeNo. of valence electron for CBr4
32
The formal charge of CBr4 molecule 0
Solubility Insoluble in water Soluble in ether,chloroform,C2H5OH
Acidic or basic nature CBr4 is neither acidic nor basic

How to draw Lewis dot structure for CBr4?

Following are the steps to follow to draw the Lewis structure of CBr4 molecule

 Step 1: Count total valence electrons present in CBr4 molecule

First step is to find the no. of valence electrons present in CBr4 molecule.

Carbon belongs to group 14th and Bromine belongs to group 17th of the periodic table.

Valence electron of Carbon = 4

Valence electron of Bromine = 7

Valence electrons Atom In CBr4 Total Electrons
C              4         1  4*1= 4
Br              7         4  7*4=28
          32

Step 2: Find least electronegative element in CBr4

Electronegativity increases in a period from left to right so Carbon is least electronegative than Bromine. Keep the least electronegative atom in the centre.

Now draw the skeletal structure of CBr4 molecule

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Description automatically generatedCBr4 Skeletal structure

Step 3: Put two electrons or a bond between C and Br atom

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Description automatically generatedStep 3:CBr4 Lewis structure

Step 4: Complete octet of the Outer atoms

Main group elements have tendency to attain octet configuration of their nearest noble gas element present in the 18 group. This is known as Octet Rule. Except hydrogen which completes duplet configuration like He

Complete the octet on outside atoms then move on to central atom

Step 5: Complete octet of central atom or make covalent bonds if necessary

There is no need of this step for CBr4 as the octet of central atom is already complete.

                         

                                                 

Step 6: Check formal charge value

Before we confirm that this is a perfect Lewis structure, we need to check the formal charge values

Formal charge = Valence electrons – (1/2) * bonding electrons – non-          bonding electrons

Valence electrons of Carbon = 4

Non-bonding electrons of carbon = 0

Bonding electrons of carbon = 8 (4 pairs)

Formal charge for carbon atom = 4 – 1/2*8 – 0 = 0

Valence electrons of Bromine = 7

Non-bonding electrons of Bromine = 6 (3 lone pairs)

Bonding electrons of Bromine = 2

Formal charge for Bromine atom = 7 – 1/2*2 – 6 = 0

As the C and Br elements have least possible formal charges, we have obtained suitable Lewis structure

                           

What is the formal charge in CBr4 and how it is calculated?

We can calculate formal charge by using the formula –

Formal charge = Valence electrons – (1/2) * bonding electrons – non-          bonding electrons

Valence electrons of Carbon = 4

Non-bonding electrons of Carbon = 0

Bonding electrons of carbon = 8 (4 pairs)

Formal charge for Carbon atom = 4 – 1/2*8 – 0 = 0

Valence electrons of Bromine = 7

Non-bonding electrons of Bromine = 6 (3 lone pairs)

Bonding electrons of fluorine = 2

Formal charge for Bromine atom =7 – 1/2*2 – 6 = 0

Formal charge on carbon and bromine atom in CBr4 Lewis dot structure is zero.

Does CBr4 molecule follow the octet rule?

CBr4 contains 32 valence electrons and all the atoms in CBr4 complete their octet as can be seen from the Lewis structure of CBr4 molecule. This proves that octet rule is followed by the CBr4 molecule.

How to find the molecular shape and electron geometry of CBr4 molecule?

In order to find the geometry (molecular/electron) of OF2 molecule, the three steps have to be followed. They are –

1)Count the lone pairs present on the central atom in the CBr4 Lewis structure

Or

Number of lone pairs can also be found by using the formula

Lone Pair =1/2*(V.E. –N.A.)

V.E.= valence electron on the central atom

N.A.= Number of atoms which are attached to the central atom

In CBr4 molecule, the valence electrons of central Carbon atom are 4 and four outer atoms are attached to it.

Lone Pairs = 1/2* (4 – 4) = 0

2) Find the hybridization number of CBr4 molecule

Hybridization of central atom can be found out by using the formula.

Hybridization number = N.A. + L.P

Where-

N.A.- is the number of atoms attached to the central atom

L.P. – is the number of lone pairs on the central atom

There are 4 atoms attached to the Carbon with no lone pairs present on it.

Hybridization number = 4 + 0 = 4

Hybridization number of CBr4 molecule is 4

So, hybridization of CBr4 molecule is Sp3

3) Use VSEPR Theory to determine CBr4 molecular/electron geometry

We have determined hybridization of CBr4 as SP3 and no lone pairs present on the central atom.

Now according to AXnEx notation of VSEPR theory we are going to find VSEPR notation for CBr4 molecule

AXnEx notation

Where-

A – is the central atom

X – is the number of atoms attached to the central atom

E – is the number of lone pairs of electrons on the central atom

According to the Lewis dot structure of Carbon Tetrabromide, central atom is Carbon which has 4 fluorine atoms are connected to it and no lone pairs present on it.

So CBr4 formula becomes AX4

According to VSEPR chart, the molecule with AX4 formula has molecular shape as tetrahedral and electron geometry tetrahedral.

Total Domains General Formula Bonded atoms Lone Pairs Molecular Shape Electron Geometry
1 AX 1 0 Linear Linear
2 AX2 2 0 Linear Linear
AXE 1 1 Linear Linear
3 AX3 3 0 Trigonal Planar Trigonal Planar
AX2E 2 1 Bent Trigonal Planar
AXE2 1 2 Linear Trigonal Planar
4 AX4 4 0 Tetrahedral Tetrahedral
AX3E 3 1 Trigonal Pyramid Tetrahedral
AX2E2 2 2 Bent Tetrahedral
AXE3 1 3 Linear Tetrahedral

VSEPR CHART

                       

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Description automatically generatedTetrahedral geometry of CBr4

Is CBr4 molecule polar or non-polar?

CBr4 is a non-polar molecule is confirmed by three factors –

1)Electronegativity:

Bromine (electronegativity 2.96) is more electronegative than Carbon (electronegativity 2.55) Being more electronegative than Carbon, Bromine attracts electrons towards it more strongly.

The molecule is polar when the difference in electronegativity between the atoms in the molecule is greater than 0.4

The electronegativity difference between Carbon and Bromine is 0.41

2)Geometrical/Molecular Shape: 

Geometrical Structure of CBr4 molecule is tetrahedral.

The four dipoles of four C-Br bond are in opposite direction. Now, due to the tetrahedral geometry (which is symmetrical) all the dipoles get cancelled by each other.

3)Dipole Moment:

Due to the symmetric geometry of the CBr4 (tetrahedral) all the 4 dipoles get cancelled by each other resulting in overall 0 dipole moment for CBr4.

All these factors show that CBr4 is a non-polar molecule.

What is the Hybridisation for CBr4 molecule?

The central atom carbon atom shares four electrons with four Bromine atoms. Hence in the Lewis structure there is a presence of four bonding pairs of electrons on the carbon atom in Lewis structure of CBr4 molecule

To share the electrons with the Bromine atoms, the orbitals of Carbon atom undergo hybridization to accommodate the electrons.

The electronic configuration of Carbon and Bromine in ground state is –

Carbon in ground state 1s2 2s2 2p2

Bromine in ground state 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

Electronic configuration of Carbon after gaining four electrons to fulfil the octet by forming bonds with Bromine-

Carbon 1S2 2S2 2Px2 2Py2 2Pz2

Steric Number = Number of atoms bonded to central atom + Number of lone pairs of electrons attached to central atom

Steric Number = 4 + 0 = 4

So, hybridization for the central atom oxygen in CBr4 is Sp3

Does CBr4 molecule shows resonance?                                      

A molecule shows resonance when –

  • The molecule has alternate double and single bonds.
  • The molecule has presence of lone pair in conjugation with the double bond.

Carbon Tetrafluoride does not have a double bond so CBr4 does not show resonance.

Is CBr4 ionic or a covalent compound?

CBr4 is a covalent compound as the bond between Carbon and Bromine is formed by sharing of electrons.

Conclusion:

To summarize what we have discussed in this article –

The hybridisation of CBr4 molecule is Sp3. Both the molecular geometry and electron geometry of CBr4 is tetrahedral. The bond angle Br-C- Br is 109.5 degrees. The total valence electrons present in CBr4 molecule is 32.

.

                    

Also Read:

Alh3 Lewis Structure,Geometry:9 Facts You Should Know

image 236

The Lewis structure of AlH3, also known as aluminum hydride, is a diagram that represents the arrangement of atoms and electrons in the molecule. It helps us understand the bonding and geometry of the compound. In the Lewis structure of AlH3, aluminum (Al) is the central atom surrounded by three hydrogen (H) atoms. Each hydrogen atom forms a single bond with the aluminum atom, resulting in a trigonal planar geometry. The Lewis structure of AlH3 is crucial in predicting the chemical behavior and reactivity of the compound.

Key Takeaways

Atom Number of Valence Electrons
Aluminum (Al) 3
Hydrogen (H) 1

Understanding Lewis Structures

What is a Lewis Structure?

A Lewis structure is a diagram that represents the arrangement of atoms and valence electrons in a chemical compound. It was introduced by Gilbert N. Lewis in 1916 and is also known as a Lewis dot diagram. Lewis structures are widely used in chemistry to understand the chemical bonding and molecular geometry of different compounds.

In a Lewis structure, the valence electrons of an atom are represented by dots or lines around the atomic symbol. These dots or lines indicate the number of valence electrons an atom possesses. For example, the Lewis structure of aluminum hydride (AlH3) shows that aluminum has three valence electrons, while each hydrogen atom has one valence electron.

Lewis structures are essential in understanding chemical bonding. They help us determine how atoms form covalent bonds by sharing electrons. By following the rules of Lewis structures, we can predict the electron pair arrangement and molecular geometry of a compound. This information is crucial in understanding the chemical properties and behavior of different substances.

Importance of Lewis Structures in Chemistry

Lewis structures play a vital role in the study of chemistry. They provide a visual representation of how atoms are connected and bonded in a molecule. By drawing Lewis structures, we can determine the electron configuration and predict the chemical properties of a compound.

One of the fundamental concepts in Lewis structures is the octet rule. According to this rule, atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons. By applying the octet rule, we can determine the number of bonds an atom can form and the overall stability of a molecule.

Drawing Lewis structures also helps us understand the concept of resonance. Resonance structures occur when there are multiple ways to arrange the electrons in a molecule without violating the octet rule. These resonance structures contribute to the stability and reactivity of the compound.

Lewis structures are also used in molecular structure analysis and predicting bond angles. The VSEPR (Valence Shell Electron Pair Repulsion) theory, combined with Lewis structures, allows us to determine the three-dimensional shape of a molecule and the bond angles between atoms.

How to Draw Lewis Dot Structure for AlH3

image 236

Aluminum hydride (AlH3) is a chemical compound that can be represented using a Lewis dot structure. This structure helps us understand the arrangement of atoms and electrons in the molecule. By following a series of steps, we can draw the Lewis dot structure for AlH3 and gain insights into its chemical bonding and molecular geometry.

Step 1: Count Total Valence Electrons Present in AlH3 Molecule

To begin, we need to determine the total number of valence electrons present in the AlH3 molecule. Valence electrons are the outermost electrons of an atom that participate in chemical bonding. In AlH3, aluminum (Al) belongs to Group 3A of the periodic table and has three valence electrons, while hydrogen (H) has one valence electron. By multiplying the number of valence electrons for each atom by the number of atoms present, we can calculate the total number of valence electrons in AlH3.

Step 2: Identify the Central Atom in AlH3

In AlH3, aluminum (Al) is the central atom as it is less electronegative than hydrogen (H). The central atom is usually the least electronegative element in a molecule and forms bonds with other atoms. By placing the central atom in the center, we can proceed to the next step.

Step 3: Establish a Bond between Al and H Atom

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Next, we need to establish a bond between aluminum (Al) and hydrogen (H) atoms. Aluminum can form three covalent bonds, while hydrogen can form only one. Covalent bonds involve the sharing of electrons between atoms. By connecting the central atom (Al) with the outer atoms (H) using single lines, we represent the covalent bonds in the Lewis dot structure.

Step 4: Complete Octet of the Outer Atoms (or Duplet) for Hydrogen Atom

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Hydrogen (H) atoms in AlH3 only require two electrons to complete their outermost energy level, also known as a duplet. Since hydrogen has only one valence electron, it needs to share one electron with aluminum (Al) to achieve a duplet. By placing two dots around each hydrogen atom, we complete their octet (or duplet) in the Lewis dot structure.

Step 5: Check Formal Charge Value

image 241

Lastly, we need to check the formal charge values of each atom in the Lewis dot structure. Formal charge is a way to determine the distribution of electrons in a molecule. It helps us identify the most stable arrangement of electrons. The formal charge of an atom can be calculated by subtracting the number of lone pair electrons and half the number of shared electrons from the number of valence electrons. By ensuring that the formal charge values are minimized or equal to zero, we can verify the accuracy of our Lewis dot structure.

By following these steps, we can draw the Lewis dot structure for AlH3 and gain a better understanding of its molecular structure and chemical properties. Remember, Lewis structures are a useful tool in chemistry for analyzing and predicting the behavior of chemical compounds.

Understanding Formal Charge in AlH3

What is the Formal Charge in AlH3 and How is it Calculated?

image 242

Formal charge is a concept used in chemistry to determine the distribution of electrons in a molecule or ion. In the case of Aluminum Hydride (AlH3), understanding the formal charge can provide valuable insights into its chemical properties and behavior.

To calculate the formal charge of an atom in a molecule, we need to consider the number of valence electrons it possesses and its bonding arrangement. The formal charge is calculated by subtracting the number of lone pair electrons and half the number of shared electrons from the total number of valence electrons.

In AlH3, aluminum (Al) has three hydrogen (H) atoms bonded to it. Aluminum is a group 3 element and has three valence electrons, while hydrogen has one valence electron. By applying the formal charge calculation, we can determine the formal charge of each atom in AlH3.

Let’s break it down:

  1. Aluminum (Al):
  2. Valence electrons: 3
  3. Lone pair electrons: 0
  4. Shared electrons: 6 (each hydrogen contributes one electron)
  5. Formal charge = 3 – 0 – 6/2 = 0

  6. Hydrogen (H):

  7. Valence electrons: 1
  8. Lone pair electrons: 0
  9. Shared electrons: 2 (shared with aluminum)
  10. Formal charge = 1 – 0 – 2/2 = 0

From the calculations, we can see that both aluminum and hydrogen in AlH3 have a formal charge of 0. This indicates that the distribution of electrons in the molecule is balanced, with no atoms carrying an excess or deficit of electrons.

How to Find Formal Charge from Lewis Structure

A Lewis structure, also known as a Lewis dot diagram, is a visual representation of the arrangement of atoms and valence electrons in a molecule. It can be used to determine the formal charge of each atom in a compound like AlH3.

To find the formal charge from a Lewis structure, follow these steps:

  1. Draw the Lewis structure of AlH3, representing the bonds between aluminum and hydrogen atoms.
  2. Count the number of valence electrons for each atom.
  3. Assign lone pair electrons and shared electrons based on the Lewis structure.
  4. Apply the formal charge calculation for each atom using the formula mentioned earlier.

By following these steps, you can determine the formal charge of each atom in AlH3 and gain a better understanding of its electronic distribution.

It’s important to note that formal charge is a theoretical concept and does not represent the actual charge of the atoms in a molecule. It is a tool used to analyze the electron distribution and predict the reactivity of a compound.

The Octet Rule and AlH3

Does AlH3 Molecule Follow the Octet Rule?

The Octet Rule is a fundamental concept in chemistry that states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons. This rule helps us understand the formation of chemical bonds and the stability of molecules.

Aluminum hydride (AlH3) is a chemical compound that consists of one aluminum atom bonded to three hydrogen atoms. To determine if AlH3 follows the Octet Rule, let’s analyze its Lewis dot diagram and examine its chemical bonding and molecular structure.

In the Lewis dot diagram of AlH3, we represent the valence electrons of each atom as dots or lines around the atomic symbol. Aluminum (Al) has three valence electrons, while hydrogen (H) has one valence electron. Therefore, the total number of valence electrons in AlH3 is [(3 * 1) + 3] = 6.

According to the Octet Rule, atoms tend to gain or lose electrons to achieve a stable electron configuration with eight valence electrons. In the case of AlH3, aluminum has three valence electrons and can form three covalent bonds with hydrogen atoms. Each hydrogen atom contributes one electron, resulting in a total of six valence electrons shared between aluminum and hydrogen.

Although AlH3 does not strictly follow the Octet Rule, it is still a stable molecule due to the presence of covalent bonds. The molecular geometry of AlH3 is trigonal planar, with the aluminum atom at the center and the three hydrogen atoms arranged symmetrically around it.

The electron pair around the aluminum atom in AlH3 is involved in covalent bonding, and the molecule adopts a trigonal planar shape to minimize electron repulsion. This arrangement allows for the most stable molecular structure.

The hybridization of AlH3 involves the mixing of atomic orbitals to form new hybrid orbitals. In this case, aluminum undergoes sp2 hybridization, resulting in three sp2 hybrid orbitals that overlap with the hydrogen 1s orbitals to form the covalent bonds.

The VSEPR theory (Valence Shell Electron Pair Repulsion theory) helps us predict the molecular geometry of AlH3 based on the arrangement of electron pairs. In AlH3, there are three bonding pairs and no lone pairs around the aluminum atom, resulting in a trigonal planar molecular geometry.

While AlH3 does not strictly adhere to the Octet Rule, it is a stable molecule due to the presence of covalent bonds and the adoption of a trigonal planar molecular structure. The chemical properties of AlH3 make it useful in various chemical reactions and as a reducing agent in organic synthesis.

Molecular and Electron Geometry of AlH3

What is the Molecular Geometry and Electron Geometry of AlH3 Molecule?

The molecular geometry and electron geometry of the AlH3 molecule refer to the arrangement of atoms and electron pairs around the aluminum and hydrogen atoms in the compound. To understand the molecular and electron geometry of AlH3, we can utilize the VSEPR (Valence Shell Electron Pair Repulsion) theory.

According to the VSEPR theory, the molecular geometry is determined by the repulsion between electron pairs around the central atom. In the case of AlH3, aluminum (Al) is the central atom, and it is surrounded by three hydrogen (H) atoms. Since AlH3 has no lone pairs of electrons on the central atom, the molecular geometry is trigonal planar. This means that the three hydrogen atoms are arranged in a flat, triangular shape around the aluminum atom.

The electron geometry, on the other hand, takes into account both the bonded electron pairs and the lone pairs of electrons around the central atom. In the case of AlH3, the electron geometry is also trigonal planar, as there are no lone pairs of electrons on the aluminum atom.

Use of VSEPR Theory to Determine Molecular/Electron Geometry of AlH3

The VSEPR theory is a useful tool in determining the molecular and electron geometry of chemical compounds. It is based on the idea that electron pairs, whether they are bonding or non-bonding, repel each other and tend to position themselves as far apart as possible. This repulsion determines the overall shape of the molecule.

To apply the VSEPR theory to AlH3, we consider the Lewis dot diagram of the compound. Aluminum has three valence electrons, while hydrogen has one valence electron each. By following the Lewis structure rules and drawing the Lewis structure of AlH3, we can determine the arrangement of atoms and electron pairs.

In AlH3, the aluminum atom forms covalent bonds with three hydrogen atoms, resulting in a total of three bonding electron pairs. Since there are no lone pairs of electrons on the aluminum atom, the molecular and electron geometry is trigonal planar.

What is the Bond Angle of AlH3 Molecule?

The bond angle of the AlH3 molecule refers to the angle between two hydrogen atoms bonded to the central aluminum atom. In a trigonal planar geometry, the bond angle is 120 degrees. This means that the hydrogen atoms in AlH3 are arranged in a triangular shape around the aluminum atom, with each hydrogen-aluminum-hydrogen bond angle measuring 120 degrees.

Understanding the molecular and electron geometry, as well as the bond angle, of AlH3 is essential in analyzing its chemical properties and reactions. By studying the molecular structure and properties of AlH3, scientists can gain insights into its atomic structure, chemical bonding, and overall behavior in chemical reactions.

Hybridization in AlH3

Find the Hybridization Number of AlH3 Molecule

To determine the hybridization number of the AlH3 molecule, we need to understand the concept of hybridization and its application in chemical bonding. Hybridization is a process in which atomic orbitals mix to form new hybrid orbitals, resulting in the rearrangement of electrons and the formation of covalent bonds.

In the case of AlH3, aluminum hydride, we have one aluminum atom (Al) and three hydrogen atoms (H). Aluminum belongs to Group 13 of the periodic table and has three valence electrons. Hydrogen, on the other hand, has one valence electron.

According to the octet rule, atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons. In the case of AlH3, aluminum can achieve this stability by sharing its three valence electrons with three hydrogen atoms.

To determine the hybridization number, we need to consider the number of electron pairs around the central atom, which is aluminum in this case. Each covalent bond consists of one electron pair. Therefore, the total number of electron pairs around aluminum is three.

Based on the VSEPR (Valence Shell Electron Pair Repulsion) theory, the electron pairs around the central atom repel each other and try to maximize their distance. This leads to a trigonal planar molecular geometry for AlH3.

Now, let’s determine the hybridization of aluminum in AlH3. The number of electron pairs (three) corresponds to sp2 hybridization. In sp2 hybridization, one s orbital and two p orbitals combine to form three sp2 hybrid orbitals. These hybrid orbitals are arranged in a trigonal planar geometry around the aluminum atom.

What is the Hybridization for AlH3 Molecule?

The hybridization of the AlH3 molecule is sp2. This means that the aluminum atom in AlH3 undergoes sp2 hybridization, resulting in the formation of three sp2 hybrid orbitals. These hybrid orbitals are involved in bonding with the three hydrogen atoms, forming three sigma bonds.

In the Lewis dot diagram of AlH3, the aluminum atom is represented by the symbol Al, surrounded by three dots representing its valence electrons. The hydrogen atoms are represented by the symbol H, each with a single dot representing its valence electron.

The chemical bonding in AlH3 involves the sharing of electrons between aluminum and hydrogen atoms, resulting in the formation of covalent bonds. The molecular structure analysis of AlH3 reveals a trigonal planar geometry, with the aluminum atom at the center and the three hydrogen atoms arranged symmetrically around it.

Resonance and Solubility of AlH3

Does AlH3 Molecule Show Resonance?

When it comes to the aluminum hydride molecule (AlH3), the question of whether it exhibits resonance arises. Resonance refers to the phenomenon where multiple Lewis structures can be drawn for a molecule, indicating the delocalization of electrons. However, in the case of AlH3, resonance structures are not typically observed.

To understand why AlH3 does not exhibit resonance, let’s take a closer look at its chemical bonding and molecular structure. Aluminum hydride has a Lewis dot diagram where aluminum (Al) is surrounded by three hydrogen (H) atoms. The valence electrons of aluminum and hydrogen participate in covalent bonds, resulting in the formation of the AlH3 molecule.

The molecular geometry of AlH3 is trigonal planar, with the aluminum atom at the center and the three hydrogen atoms arranged symmetrically around it. This arrangement satisfies the octet rule, where each atom in the molecule has a full outer electron shell. The absence of additional resonance structures can be attributed to the stable molecular structure of AlH3, which does not require electron delocalization.

Solubility of Aluminium Hydride

Moving on to the solubility of aluminum hydride (AlH3), it is important to note that AlH3 is not soluble in water. This lack of solubility can be attributed to the nature of the chemical compounds involved.

AlH3 is a covalent compound, and covalent compounds tend to have low solubility in water. This is because water is a polar solvent, meaning it has a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. In order for a compound to dissolve in water, it must have a similar polarity.

However, AlH3 is a nonpolar molecule, as the electronegativity difference between aluminum and hydrogen is relatively small. As a result, the attractive forces between AlH3 molecules are stronger than the interactions between AlH3 and water molecules, leading to insolubility.

Frequently Asked Questions

1. What is the Lewis Structure of AlH3?

The Lewis structure of AlH3 (Aluminum hydride) consists of an Aluminum atom surrounded by three Hydrogen atoms. Each Hydrogen atom shares one electron with Aluminum to form a covalent bond, satisfying the octet rule for Aluminum.

2. How can I identify a Lewis Structure?

A Lewis structure can be identified by its representation of atoms of a molecule, showing how the valence electrons are arranged among the atoms in the molecule. It includes lines to represent covalent bonds and dots to represent non-bonding electrons.

3. What is the Lewis Dot Structure of AlH3?

The Lewis dot structure of AlH3 is similar to its Lewis structure. It shows an Aluminum (Al) atom in the center with three Hydrogen (H) atoms surrounding it. Each Hydrogen atom shares one electron with Aluminum, forming a covalent bond.

4. How can I find the formal charge from a Lewis Structure?

The formal charge of an atom in a Lewis structure can be calculated using the formula: Formal Charge = Valence Electrons – (Non-bonding electrons + 1/2 Bonding electrons).

5. What is the molecular geometry of AlH3 according to its Lewis Structure?

The molecular geometry of AlH3, according to its Lewis structure, is trigonal planar. This is due to the three Hydrogen atoms being evenly distributed around the Aluminum atom, creating a flat, three-sided shape.

6. What is Al3+ in Chemistry?

In chemistry, Al3+ refers to the ion of Aluminum that has lost three electrons, resulting in a positive charge. It is often involved in ionic bonds with negatively charged ions.

7. What are Lewis Structures?

Lewis structures are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. They are used to predict the shape of a molecule and its polarity.

8. Is NH3 a Lewis Structure?

Yes, NH3 (Ammonia) has a Lewis structure. It consists of a Nitrogen atom bonded with three Hydrogen atoms and one lone pair of electrons on the Nitrogen atom.

9. What is the best Lewis Structure for CH2S?

The best Lewis structure for CH2S (Methanethiol) is one where the Carbon atom is in the center, bonded to two Hydrogen atoms and one Sulfur atom. The Sulfur atom also has two lone pairs of electrons.

10. What is the role of the VSEPR theory in determining the molecular geometry of AlH3?

The Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the geometry of molecules based on the number of valence electron pairs. In the case of AlH3, the VSEPR theory predicts a trigonal planar geometry due to the three bonding pairs of electrons around the Aluminum atom.

Also Read:

Are Isotopes Stable?11 Exhaustive Facts You Should Know

image 209

Are isotopes stable? It is very interesting to find out whether all the isotopes are stable or not as Isotopes possess so many applications.

All isotopes are not stable.Atoms present in nature are either stable or unstable isotopes.On the basis of atomic no. (Z) of isotopes and whether the nucleus contains even or odd no. of isotopes we can predict about the stability of isotopes.

Example: Hydrogen has three isotopes Protium, Deuterium and Tritium. Among these three isotopes, Protium and Deuterium are the stable isotopes but tritium is unstable.

image 209
A picture containing drawing

Description automatically generatedProtium
(stable)
image 213
A picture containing drawing

Description automatically generatedDeuterium
(stable)

image 211
A picture containing drawing

Description automatically generatedTritium
(unstable)

Figure: Are Isotopes Stable?

Which isotopes are stable?

The following isotopes are stable –

Isotopes which do not undergo radioactive decay.Isotopes whose atomic no. less than 20 and with n/p ratio close to 1.Isotopes with long half-life or they do not have half-life.Isotopes with atomic number < 82 have one or more than one stable isotope (Except technetium Z= 43 and promethium with Z = 61).

Isotopic nuclei with such number of proton or neutron which make the isotope stable. These magic numbers occur naturally in the isotopes which are stable.

Some isotopes contains of magic nos. for both neutrons and protons. This is called as double magic numbers.

The magic numbers for the number of protons and neutrons are –

proton: 2,8,20,28,50,82,114

neutron: 2,8,20,28,50,82,126,184

Example: Helium having 2 protons and 2 neutrons

                 Lead having 82 protons and 126 neutrons

No. of ProtonNo. of neutronStable isotopes that have these no. either in proton or neutron
    Even     Even        163
    Even    Odd         53
    Odd    Even         50
    Odd    Odd          4
Table: Isotopes that have magic no. of either proton or neutron

 Which isotopes are unstable?

 The following isotopes are unstable –

  • Isotopes with odd number of both protons and neutrons possess higher probability to be unstable (Exception hydrogen-2, lithium-3, boron-10, nitrogen-14).
  • Isotopes with short half-life that can be easily calculated.
  • Isotopes which have atomic number(Z) > 83 are unstable.

Does parent isotope are stable?

No, parent isotopes are never stable isotopes.Radioactive decay starts from the parent isotope itself. Parent isotopes undergo radioactive decay to form daughter isotope. During the decay, parent isotope gives out alpha, beta and gamma particles.

Example- Uranium undergoes alpha decay and form Thorium (daughter isotope).

Are radioactive isotopes stable?

Radioactive isotopes are not stable.The nucleus of radioactive isotope has unstable n/p ratio that is neutron to proton ratio. When the radioactive isotope undergoes radioactive decay, they get converted into different atom. Radioactive isotopes undergo decay spontaneously and release subatomic particles and electromagnetic radiations.

The process of radioactive decay continues till a stable atom is formed and it is no longer radioactive.

Why are some isotopes stable and other unstable?

Stability of nucleus depends on the number of protons and neutrons present in the nucleus.

Some isotopes are stable due to the following reasons-

Strong nuclear forces which hold neutrons and protons together. These forces are stronger than those forces which drive protons and neutrons apart (like the electrostatic repulsion between the positively charged protons).

Their n/p ratio is in the range of 1:1 or 1.5:1

eg: hydrogen has three isotopes

Protium1 protonStable
Deuterium1 proton + 1 neutronStable
Tritium1 proton + 2 neutronsUnstable (Radioactive)
isotopes of Hydrogen

Strong nuclear forces operate over short distances. As the size of nucleus increases, the electrostatic repulsive forces between positively charged protons decreases.

Presence of extra neutrons increases space between the protons and repulsion between protons decreases.

This makes the isotopes stable.

Some isotopes are unstable because of the following reasons-

  • Presence of extra neutrons produces extra energy in the nucleus an excess of energy makes the isotope unstable.

eg: Carbon-14 having 6 protons and 8 neutrons is unstable.

  • The forces between the particles of neutrons and protons are not balanced due to excess presence of either neutrons or protons.
  • Their n/p ratio is either less than 1:1 or greater than 1.5:1
  • Presence of too many or too less neutrons as compared to required optimum ratio.

Stable Isotopes of some elements

stable isotopes of some common elements are as follows –

What are stable isotopes of carbon?

The stable isotopes of carbon are –

Carbon-12
Carbon-13
stable isotopes of carbon

What are the stable isotopes of nitrogen?

The stable isotopes of nitrogen are –

Nitrogen-14
Nitrogen-15
stable isotopes of nitrogen

What are the stable isotopes of Oxygen?

The stable isotopes of Oxygen are –

Oxygen-16
Oxygen-17
Oxygen-18
stable isotopes of oxygen

What are the stable isotopes of hydrogen?

The stable isotopes of hydrogen are –

Hydrogen-1 (protium)
Hydrogen-2(deuterium)
stable isotopes of hydrogen

What are the stable isotopes of Helium?

The stable isotopes of Helium are –

Helium-4
Helium-3
stable isotopes of Helium

What are the stable isotopes of uranium?

The stable isotopes of Uranium are –

Uranium-234
Uranium-238
Uranium235
Uranium-236
stable isotopes of Uranium

What are the stable isotopes of Beryllium?

The stable isotopes of beryllium are –

Beryllium-9
stable isotope of Beryllium

What are the stable isotopes of calcium?

The stable isotopes of calcium are –

Calcium-40
Calcium-44
Calcium-41
Calcium-43
Stable isotopes of Calcium

What are the stable isotopes of tin?

The stable isotopes of tin are –

Tin-117
Tin-112
Tin-124
Tin-120
stable isotopes of Tin

What are the stable isotopes of lead?

The stable isotopes of lead are-

Lead-204
Lead-206
Lead-207
Lead-208
stable isotopes of Lead

Conclusion:

Isotopes can be stable or unstable. All artificial isotopes are unstable and hence radioactive. Isotopes with n/p ratio 1:1 or 1.5:1 are stable the isotope.

5 Easy Steps for OF2 lewis Structure,Hybridization (Solved)

of2 lewis structure

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The OF2 lewis structure consist of one oxygen atom as the central atom and two fluorine atom are present on the either side of the oxygen atom. The Lewis structure of OF2 molecule contains 16 non-bonding electrons i.e. 8 lone pairs. From the 8 lone pairs, 3 lone pairs are present on the fluorine atom and 2 lone pairs are present on the central atom oxygen.

of2 lewis structure
of2 lewis structure

How to draw Lewis structure for OF2?

Following are the steps to follow to draw the Lewis structure of OF2 molecule

Step 1: Count total valence electrons present in OF2 molecule

First step is to find the no. of valence electrons present in OF2 molecule.

Oxygen belongs to group 16th and fluorine belongs to group 17th of the periodic table.

Valence electron of oxygen = 6

Valence electron of fluorine = 7

  Valence Electrons Atom in OF2 Total Electrons
O 6 1 1*6=6
F 7 2 7*2=14
      20
Table: Total Valence Electrons Of OF2 molecule   

Step 2: Find least electronegative element in OF2 molecule

Electronegativity in a period increases from left to right so oxygen is least electronegative than fluorine. Keep the least electronegative atom in the centre.

Step 3: Put two electrons or a bond between F and O atom

OF2 Lewis Structure step1

Step 4: Complete octet of the Outer atoms

Complete the octet on outside atoms then move on to central atom.

OF2 Lewis Structure Step2

Step 5: Complete octet of central atom or make covalent bonds if necessary

OF2 Lewis Structure Step3

Step 6: Check formal charge value

Before we confirm that this is a perfect Lewis structure, we need to check the formal charge values

Formal charge = Valence electrons – (1/2) * bonding electrons – non-          bonding electrons

Valence electrons of oxygen = 6

Non-bonding electrons of Oxygen = 4 (2 lone pairs)

Bonding electrons of Oxygen= 4 (2 pairs)

Formal charge for Oxygen atom = 6 – 1/2*4 – 4 = 0

Valence electrons of fluorine = 7

Non-bonding electrons of fluorine = 6 (3 lone pairs)

Bonding electrons of fluorine = 2

Formal charge for fluorine atom =7 – 1/2*2 – 6 = 0

As the F and O elements have least possible formal charges, we have obtained suitable Lewis structure

What is the formal charge in OF2 Lewis structure and how it is calculated?

Formal charge is the charge present on an atom in a molecule when all the bonding electrons are shared equally or when the electronegativity difference of atoms is ignored.

Formal charge = Valence electrons – (1/2) * bonding electrons – non-bonding electrons

Valence electrons of oxygen = 6

Non-bonding electrons of Oxygen = 4 (2 lone pairs)

Bonding electrons of Oxygen= 4 (2 pairs)

Formal charge for Oxygen atom = 6 – 1/2*4 – 4 = 0

Valence electrons of fluorine = 7

Non-bonding electrons of fluorine = 6 (3 lone pairs)

Bonding electrons of fluorine = 2

Formal charge for fluorine atom =7 – 1/2*2 – 6 = 0

Thus formal charge on oxygen and fluorine atom in OF2 Lewis dot structure is zero.

OF2 molecule details-

Molecular Name Oxygen difluoride
Chemical Formula OF2
Central atom of the lewis structure Oxygen
Number of lone pairs on central atom 2
Molecular Geometry of OF2 Bent
Electron Geometry of OF2 Tetrahedral
Bon Angle F-O-F 103 degree
No. of valence electron for OF2 molecule 20
The formal charge of oF2 molecule 0

Does OF2 molecule follow the octet rule?

OF2 contains 20 valence electrons and all the atoms in OF2 complete their octet as can be seen from the Lewis structure of OF2 molecule. This proves that octet rule is followed by the OF2 molecule.

Why is the molecular Geometry of OF2 is bent?

 Valence shell electron pair repulsion theory (VSEPR) takes into account the repulsion forces between lone pair – lone pair, lone pair – bond pair and bond pair – bond pair and in this way balancing the stability of molecule.

The bent molecular geometry of OF2 molecule is because of the presence of 2 lone pairs on the central oxygen atom. The presence of lone pairs on oxygen atom produces repulsion with electrons of bonded pairs. Due to repulsive forces, fluorine which are present as outer atoms pushes down so as to minimize the repulsion as per the VSEPR theory.

As molecular geometry considers only the atoms present in the molecule so the Molecular Geometry of OF2 molecule is bent.

What is the Electron Geometry of OF2 molecule?

As the electron geometry considers all the electrons as well as lone pairs to determine shape so Electron Geometry of OF2 molecule is tetrahedral.

How to find the molecular shape and electron geometry of OF2 molecule?

In order to find the geometry (molecular/electron) of OF2 molecule, the three steps have to be followed. They are –

1)Find the number of lone pairs present on the central atom in the Lewis structure of OF2 molecule

Or

Number of lone pairs can also be found by using the formula

Lone Pair =1/2*(V.E. –N.A.)

V.E.= valence electron on the central atom

N.A.= Number of atoms attached to that central atom

In OF2 molecule, the valence electrons of  central oxygen atom is 6 and two outer atoms are attached to it.

Lone Pairs = 1/2* (6 – 2) = 2

2) Find the hybridization number of OF2 molecule

Hybridization of central atom can be found out by using the formula.

Hybridization number = N.A. + L.P

Where N.A.= number of atoms attached to the central atom

L.P. = number of lone pairs on the central atom

There are two atoms attached to the central atom oxygen and  there are two lone pairs present on it.

Hybridization number = 2+2 = 4

Hybridization number of OF2 molecule is 4

So hybridization of OF2 molecule is Sp3

3) Use VSEPR Theory to determine OF2 molecular/electron geometry

We have determined hybridization of OF2 as SP3 and lone pairs 2

Now according to AXnEx notation of VSEPR theory we are going to find VSEPR notation for OF2 molecule

AXnEx notation

Where,

A: central atom

X: number of atoms attached to the central atom

E: number of lone pairs of electrons on the central atom

As per Lewis dot structure of Oxygen difluoride, Oxygen is the central atom which has 2 lone pairs of electrons and 2 fluorine atoms are connected to it.

So OF2 formula becomes AX2N2

According to VSEPR chart, the molecule with AX2N2 formula has molecular shape as bent and electron geometry tetrahedral.

Total Domains General Formula Bonded atoms Lone Pairs Molecular Shape Electron Geometry
1 AX 1 0 Linear Linear
2 AX2 2 0 Linear Linear
  AXE 1 1 Linear Linear
3 AX3 3 0 Trigonal Planar Trigonal Planar
  AX2E 2 1 Bent Trigonal Planar
  AXE2 1 2 Linear Trigonal Planar
4 AX4 4 0 Tetrahedral Tetrahedral
  AX3E 3 1 Trigonal Pyramid Tetrahedral
  AX2E2 2 2 Bent Tetrahedral
  AXE3 1 3 Linear Tetrahedral
VSEPR Chart

Why do Bond Angle of OF2 is less than the normal Value?

The Bond Angle OF2 is 103 degrees as the two lone pairs present on the Oxygen molecule decreases the value of bond angle from the normal value. Due to repulsion between the lone pairs, bond angle is 103 degrees.

The bond length of the O-F bond is 140.5pm

image 201

Is OF2 molecule polar or non-polar?

OF2 is a polar molecule is confirmed by three factors

1)Electronegativity:

Fluorine (electronegativity 4) is more electronegative than oxygen (electronegativity 3.5) Being more electronegative than oxygen, fluorine attracts electrons towards it more strongly.

The molecule is said to be polar If the electronegativity difference between the atoms in the molecule is greater than 0.4

The difference between the electronegativities of Oxygen and fluorine is 0.5.

2)Geometrical/Molecular Shape: 

Shape of OF2 molecule is bent.

The two dipoles – negative charge on fluorine atom and positive charge on the oxygen atom cannot be cancelled because of the bent molecular shape of OF2.

3) Dipole Moment:

The dipole moment exists in OF2 molecule due to polarity of O-F bond. This dipole moment will be towards the more electronegative fluorine atom, as the fluorine atom tries to pull the electron towards it

The bent shape of OF2 molecule is due to the presence of 2 lone pairs of electrons on the central oxygen atom. Due to the bent shape both these dipole moments are not cancelled instead they are sum up, making OF2 a polar molecule.

All these factors show that OF2 is a polar molecule.

The central atom oxygen atom shares two electrons with both fluorine atom. Hence in the Lewis structure there is a presence of two bonding pairs of electrons on the oxygen atom and two non-bonding pairs i.e. two lone pairs on the oxygen atom in the Lewis structure of OF2 molecule

What is the Hybridisation for OF2 molecule?

To share the electrons with the fluorine atoms, the orbitals of oxygen atom undergo hybridization to accommodate the electrons.

The electronic configuration of oxygen and fluorine in ground state is –

Oxygen in ground state 1S2 2S2 2P4

Fluorine in ground state 1S2 2S2 2P5

Electronic configuration of oxygen after gaining two electrons to fulfil the octet by forming bonds with fluorine-

Oxygen 1S2 2S2 2Px2 2Py2 2Pz2

Steric Number = Number of atoms bonded to central atom + Number of lone pairs of electrons attached to central atom

Steric Number = 2+2 = 4

So, hybridization for the central atom oxygen in OF2 is Sp3

Does OF2 molecule shows resonance?

Oxygen difluoride does not have a double bond so it does not show resonance.

A molecule can have resonance if-

  • The molecule has alternate double and single bonds.
  • The molecule has presence of lone pair in conjugation with the double bond.

Conclusion

The OF2 Lewis structure of contains 4 bonding electrons i.e. two bonding pairs and 16 non- bonding electrons i.e. 8 lone pairs.

  • Oxygen Difluoride is made of one oxygen and two fluorine atoms.
  • To summarize what we have discussed in this article, let’s have a look at what we have learned in this article
  • OF2 is a polar molecule with a dipole moment of 0.3D
  • The molecular geometry of OF2 molecule is bent.
  • The OF2 molecule has tetrahedral as the electron geometry.

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