Strontium is a chemical element with the symbol Sr and atomic number 38. It belongs to the alkaline earth metal group on the periodic table. The electron configuration of an atom describes how its electrons are distributed among the various atomic orbitals. In the case of strontium, the electron configuration can be represented as 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2, with a total of 38 electrons. This configuration indicates that strontium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbital, two in its 3s orbital, six in its 3p orbital, two in its 4s orbital, ten in its 3d orbital, six in its 4p orbital, and two in its 5s orbital. Understanding the electron configuration of an element is crucial in determining its chemical properties and behavior.
Key Takeaways
- The electron configuration of strontium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2.
- Strontium has 38 electrons distributed across its energy levels and orbitals.
- The electron configuration of strontium can be represented using the noble gas notation as [Kr] 5s^2 4d^10 5p^6 6s^2.
Strontium Electron Configuration
The electron configuration of an atom describes how its electrons are distributed among different energy levels and orbitals. In the case of strontium, a chemical element with the atomic number 38, understanding its electron configuration is crucial to comprehend its chemical behavior and reactivity. In this section, we will explore the electron configuration of strontium, including the noble gas notation, the application of Aufbau’s principle, and Hund’s rule. Additionally, we will provide a diagram to visualize strontium’s electronic configuration.
Noble Gas Notation for Strontium’s Electron Configuration
Noble gas notation is a shorthand method used to represent the electron configuration of an atom by referencing the nearest noble gas element. For strontium, the noble gas notation is based on the element that precedes it in the periodic table, which is argon (Ar). Argon has the electron configuration of 1s^2 2s^2 2p^6 3s^2 3p^6, with a total of 18 electrons.
To represent strontium’s electron configuration using noble gas notation, we start with the electron configuration of argon and continue from there. Strontium has 38 electrons, so we add an additional 18 electrons to the noble gas notation of argon. The electron configuration of strontium in noble gas notation is [Ar] 4s^2.
Explanation of Aufbau’s Principle and its Application to Strontium
Aufbau’s principle, also known as the building-up principle, states that electrons fill the available energy levels and orbitals in a specific order. According to this principle, electrons occupy the lowest energy levels first before moving to higher energy levels.
In the case of strontium, the electron configuration follows the Aufbau principle. The first two electrons fill the 1s orbital, followed by the next two electrons filling the 2s orbital. The subsequent six electrons occupy the 2p orbital, and the next two electrons fill the 3s orbital. After that, the 3p orbital is filled with six electrons. Finally, the remaining two electrons occupy the 4s orbital, resulting in the electron configuration of [Ar] 4s^2.
Explanation of Hund’s Rule and its Application to Strontium
Hund’s rule states that when electrons occupy orbitals of the same energy level, they prefer to occupy separate orbitals with parallel spins before pairing up. This rule helps to explain the distribution of electrons within a subshell.
Applying Hund’s rule to strontium, we can observe that the 4s orbital has two electrons with parallel spins, indicating that they occupy separate orbitals before pairing up. This arrangement maximizes the stability of the atom and follows Hund’s rule.
Diagram of Strontium’s Electronic Configuration
To visualize the electron configuration of strontium, we can use a diagram that represents the different energy levels and orbitals. The diagram below illustrates the electron distribution in strontium:
Energy Level | Subshell | Number of Electrons |
---|---|---|
1 | s | 2 |
2 | s | 2 |
2 | p | 6 |
3 | s | 2 |
3 | p | 6 |
4 | s | 2 |
In this diagram, each energy level is represented by a row, and the subshells are listed under the “Subshell” column. The “Number of Electrons” column indicates the number of electrons present in each subshell.
By understanding the electron configuration of strontium, we gain insights into its chemical properties and behavior. The arrangement of electrons in different orbitals and energy levels determines how strontium interacts with other elements and forms compounds.
Strontium Electron Configuration Notation
Explanation of the Electron Configuration Notation for Strontium
When studying the atomic structure of an element like strontium, understanding its electron configuration is crucial. The electron configuration refers to the arrangement of electrons within the atom’s electron orbitals, which are the regions where electrons are most likely to be found.
The electron configuration notation provides a concise way to represent the distribution of electrons in an atom. It follows a specific order based on the filling of electron orbitals, which are grouped into different energy levels known as electron shells.
In the case of strontium, its electron configuration is written as 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2. Let’s break down this notation to understand what each part represents.
- The numbers before the letters (1s, 2s, 2p, etc.) indicate the principal quantum number, which represents the energy level or shell where the electrons are located.
- The superscript numbers (2, 6, 10, etc.) represent the number of electrons in each orbital. For example, 2s^2 means there are two electrons in the 2s orbital.
- The letters (s, p, d) represent the different types of orbitals within each energy level. The s orbitals are spherical, the p orbitals are dumbbell-shaped, and the d orbitals have more complex shapes.
By following the electron filling order, we can determine the electron configuration of any element. The filling order is based on the Aufbau principle, which states that electrons fill the lowest energy orbitals first before moving to higher energy levels.
Mention of Krypton (Kr) as the Noble Gas Used in the Notation
To simplify the electron configuration notation, noble gases are often used as a reference point. Noble gases have completely filled electron shells, making them stable and unreactive. In the case of strontium, the noble gas used as a reference is krypton (Kr).
The electron configuration notation for strontium can be further condensed by representing the electron distribution from krypton onwards. In this condensed notation, strontium’s electron configuration is written as [Kr] 5s^2. The [Kr] represents the electron arrangement of krypton, and the 5s^2 indicates the additional electrons in the 5s orbital of strontium.
Using noble gases as reference points allows us to focus on the valence electrons, which are the electrons in the outermost energy level. Valence electrons play a crucial role in determining an element’s chemical properties and its ability to form bonds with other elements.
In summary, the electron configuration notation provides a systematic way to represent the electron arrangement in an atom. Understanding the electron configuration of elements like strontium helps us comprehend their atomic structure and predict their chemical behavior.
Strontium Unabbreviated Electron Configuration
The electron configuration of an atom describes the arrangement of electrons within its electron orbitals. In the case of strontium, a chemical element with the atomic number 38, the unabbreviated electron configuration provides valuable insights into its electron distribution and arrangement.
Description of the Unabbreviated Electron Configuration for Strontium
To understand the unabbreviated electron configuration of strontium, we need to consider its atomic structure. Strontium has 38 electrons, which are distributed across different electron shells and orbitals according to specific rules.
The electron configuration notation represents the distribution of electrons in a simplified manner. However, the unabbreviated electron configuration provides a more detailed account of the electron filling order.
In the case of strontium, the unabbreviated electron configuration can be represented as follows:
Electron Shell | Subshell | Electron Count |
---|---|---|
1s | 2 | 2 |
2s | 2 | 2 |
2p | 6 | 6 |
3s | 2 | 2 |
3p | 6 | 6 |
3d | 10 | 10 |
4s | 2 | 2 |
In the first electron shell, the 1s subshell can accommodate a maximum of 2 electrons. The second electron shell consists of the 2s and 2p subshells, which can hold a total of 8 electrons. The third electron shell contains the 3s, 3p, and 3d subshells, with a combined capacity of 18 electrons. Finally, the fourth electron shell has the 4s subshell, which can hold up to 2 electrons.
By following the electron filling order, we can determine that strontium’s electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s². This notation indicates the number of electrons in each subshell, starting from the lowest energy level and progressing to higher levels.
Understanding the unabbreviated electron configuration of strontium allows us to comprehend its electron arrangement and predict its chemical behavior. The outermost electron shell, known as the valence shell, contains the 4s² subshell, which holds the valence electrons. In the case of strontium, the two valence electrons in the 4s² subshell play a crucial role in determining its chemical properties and reactivity.
In summary, the unabbreviated electron configuration of strontium provides a comprehensive understanding of its electron distribution and arrangement. By examining the electron filling order, we can determine the number of electrons in each subshell and predict the chemical behavior of this fascinating element.
Ground State Strontium Electron Configuration
Explanation of the ground state electron configuration for strontium
The electron configuration of an atom describes how its electrons are distributed among the various energy levels or electron shells. In the case of strontium, a chemical element with the atomic number 38, the ground state electron configuration can be determined by following a specific set of rules.
To understand the electron configuration of strontium, we need to first understand the concept of electron orbitals. Electron orbitals are regions of space around the nucleus where electrons are most likely to be found. Each orbital can hold a maximum of two electrons.
In strontium, the electron configuration can be represented using the electron configuration notation, which is a shorthand way of writing the distribution of electrons in the atom’s orbitals. The electron configuration of strontium is [Kr] 5s^2, where [Kr] represents the electron configuration of the noble gas krypton (with the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6) and 5s^2 represents the two electrons in the 5s orbital of strontium.
Breakdown of the electron distribution in each shell
Let’s break down the electron distribution in each shell of strontium to get a clearer picture of how the electrons are arranged.
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First shell (K shell): The first shell can hold a maximum of 2 electrons. In strontium, the first shell is not completely filled, as it only contains 2 electrons in the 1s orbital.
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Second shell (L shell): The second shell can hold a maximum of 8 electrons. In strontium, the second shell is also not completely filled, as it only contains 8 electrons in the 2s and 2p orbitals.
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Third shell (M shell): The third shell can hold a maximum of 18 electrons. In strontium, the third shell is not completely filled, as it only contains 8 electrons in the 3s and 3p orbitals.
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Fourth shell (N shell): The fourth shell can hold a maximum of 32 electrons. In strontium, the fourth shell is not completely filled, as it only contains 18 electrons in the 3d and 4s orbitals.
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Fifth shell (O shell): The fifth shell can hold a maximum of 32 electrons. In strontium, the fifth shell is not completely filled, as it only contains 2 electrons in the 5s orbital.
By examining the electron distribution in each shell, we can see that strontium has a total of 38 electrons. The valence electrons, which are the electrons in the outermost shell, are the ones that are involved in chemical reactions. In the case of strontium, the valence electrons are the 2 electrons in the 5s orbital.
Understanding the electron configuration and electron distribution of strontium is crucial in predicting its chemical behavior and its ability to form compounds with other elements. By knowing the arrangement of electrons, scientists can gain insights into the properties and reactivity of strontium, which has various applications in fields such as medicine, electronics, and pyrotechnics.
Excited State of Strontium Electron Configuration
The electron configuration of an atom describes how its electrons are distributed among the various energy levels, or electron shells. In the case of strontium (Sr), a chemical element with atomic number 38, its electron configuration in its ground state is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2. This configuration indicates that strontium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbital, two in its 3s orbital, six in its 3p orbital, two in its 4s orbital, ten in its 3d orbital, and two in its 4p orbital.
Definition of Excited State
When an atom is in its ground state, all of its electrons occupy the lowest available energy levels. However, under certain conditions, such as when the atom absorbs energy, one or more electrons can be excited to higher energy levels. This results in the atom being in an excited state.
In the excited state, the electron configuration of an atom changes as electrons move to higher energy levels. The excited state electron configuration of strontium (Sr) can be represented as 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 5s^2 5p^6. This configuration indicates that strontium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbital, two in its 3s orbital, six in its 3p orbital, ten in its 3d orbital, two in its 4s orbital, ten in its 4p orbital, and two in its 4d orbital.
Mention of the Excited State Electron Configuration for Sr2+
When strontium loses two electrons, it forms a cation with a charge of +2, known as Sr2+. The electron configuration of Sr2+ in its excited state can be represented as [Kr] 5s^2 4d^10. This configuration indicates that strontium cation has a completely filled 4d orbital and two electrons in its 5s orbital.
It is important to note that the electron configuration of strontium in its excited state or as a cation may vary depending on the specific conditions and the energy levels involved. The electron configuration provides valuable insights into the arrangement of electrons within an atom and helps in understanding its chemical behavior and properties.
Ground State Strontium Orbital Diagram
The ground state electron configuration of an atom describes how its electrons are distributed among the available energy levels or orbitals. In the case of strontium (Sr), a chemical element with atomic number 38, the electron configuration can be represented using an orbital diagram.
An orbital diagram is a visual representation that shows the arrangement of electrons in the different orbitals of an atom. Each orbital can hold a maximum of two electrons, with opposite spins. The orbitals are organized into energy levels, also known as electron shells, which are represented by the letters s, p, d, and f.
Description of the Orbital Diagram for Strontium’s Ground State
In the ground state of strontium, the electron configuration can be written as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s². Let’s break down the electron distribution in each energy level:
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1s²: This represents the first energy level, which contains a single s orbital. The superscript ² indicates that the 1s orbital is fully occupied with two electrons.
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2s²: Moving to the second energy level, we have another s orbital, called the 2s orbital. Like the 1s orbital, it can hold a maximum of two electrons, and in the case of strontium, it is fully occupied.
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2p⁶: The second energy level also includes three p orbitals, labeled 2p. Each p orbital can hold up to two electrons, resulting in a total of six electrons in the 2p orbitals.
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3s²: Transitioning to the third energy level, we find the 3s orbital. Similar to the previous energy levels, the 3s orbital can accommodate two electrons, and in strontium’s ground state, it is fully occupied.
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3p⁶: The third energy level also contains three p orbitals, labeled 3p. Just like the 2p orbitals, each 3p orbital can hold a maximum of two electrons, resulting in a total of six electrons in the 3p orbitals.
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4s²: Moving on to the fourth energy level, we encounter the 4s orbital. As with the previous s orbitals, it can accommodate two electrons, and in the case of strontium, it is fully occupied.
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3d¹⁰: The fourth energy level also includes five d orbitals, labeled 3d. Each d orbital can hold up to two electrons, resulting in a total of ten electrons in the 3d orbitals.
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4p⁶: The fourth energy level also contains three p orbitals, labeled 4p. Each 4p orbital can hold a maximum of two electrons, resulting in a total of six electrons in the 4p orbitals.
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5s²: Finally, we reach the fifth energy level, which includes the 5s orbital. Like the previous s orbitals, it can hold two electrons, and in strontium’s ground state, it is fully occupied.
To summarize, the ground state electron configuration of strontium (Sr) can be represented by the orbital diagram as follows:
Energy Level | Orbital(s) | Electron(s) |
---|---|---|
1s | 1s | 2 |
2s | 2s | 2 |
2p | 2p | 6 |
3s | 3s | 2 |
3p | 3p | 6 |
4s | 4s | 2 |
3d | 3d | 10 |
4p | 4p | 6 |
5s | 5s | 2 |
By understanding the ground state electron configuration and orbital diagram of strontium, we gain insights into its atomic structure and the arrangement of its valence electrons. This knowledge is crucial in understanding the chemical behavior and properties of strontium in various chemical reactions and interactions.
Strontium 2+ Electron Configuration
The electron configuration of an atom describes how its electrons are distributed in different energy levels or orbitals. In the case of strontium (Sr), which has an atomic number of 38, the electron configuration for its 2+ ion (Sr2+) is slightly different from the neutral atom. Let’s explore the explanation behind the electron configuration for Sr2+ and discuss the loss of electrons from the 5s orbital.
Explanation of the Electron Configuration for Sr2+
To understand the electron configuration of Sr2+, we need to first look at the electron arrangement of the neutral strontium atom. The electron configuration of Sr is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2. This configuration follows the Aufbau principle, which states that electrons fill the lowest energy levels first before moving to higher energy levels.
When strontium loses two electrons to form the 2+ ion, the electron configuration changes. The two electrons that are lost come from the highest energy level, which is the 5s orbital. The electron configuration for Sr2+ becomes 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6.
Mention of the Loss of Electrons from the 5s Orbital
The loss of electrons from the 5s orbital in strontium’s electron configuration is a result of ionization. When strontium loses two electrons, it forms a 2+ ion, which means it has two more protons than electrons. This creates an imbalance in charge, resulting in a positively charged ion.
The 5s orbital is the outermost orbital in strontium’s electron arrangement. It is relatively far from the nucleus and has a higher energy level compared to the inner orbitals. When strontium loses two electrons, these electrons are removed from the 5s orbital first because it is the highest energy level that is easily accessible for ionization.
By losing the two electrons from the 5s orbital, strontium achieves a stable electron configuration similar to that of the noble gas krypton (Kr). Krypton has an electron configuration of 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6, which is the same as the electron configuration of Sr2+. This similarity in electron configuration is due to the loss of the two valence electrons from the 5s orbital.
In summary, the electron configuration of strontium’s 2+ ion (Sr2+) involves the loss of two electrons from the 5s orbital. This loss results in a stable electron configuration similar to that of the noble gas krypton. Understanding the electron configuration of ions helps us comprehend the chemical behavior and properties of different elements.
Strontium Chloride Electron Configuration
Explanation of the Electron Configuration for Strontium Chloride
In order to understand the electron configuration of strontium chloride (SrCl2), we first need to examine the electron configurations of the individual elements involved: strontium (Sr) and chlorine (Cl).
Strontium, with an atomic number of 38, has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2. This means that strontium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbital, two in its 3s orbital, six in its 3p orbital, two in its 4s orbital, ten in its 3d orbital, and two in its 4p orbital.
Chlorine, on the other hand, has an atomic number of 17 and an electron configuration of 1s2 2s2 2p6 3s2 3p5. This means that chlorine has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbital, two in its 3s orbital, and five in its 3p orbital.
When strontium and chlorine combine to form strontium chloride, the strontium atom loses two electrons from its outermost 5s orbital, resulting in a stable electron configuration of 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6. This configuration is the same as that of the noble gas krypton (Kr).
Description of the Electron Configuration for Chlorine
Chlorine, as mentioned earlier, has an electron configuration of 1s2 2s2 2p6 3s2 3p5. This means that chlorine has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbital, two in its 3s orbital, and five in its 3p orbital.
The electron configuration of chlorine indicates that it has seven valence electrons, which are the electrons in the outermost energy level. Valence electrons play a crucial role in determining the chemical properties of an element. In the case of chlorine, its seven valence electrons make it highly reactive, as it tends to gain one electron to achieve a stable electron configuration, similar to that of the noble gas argon (Ar).
Explanation of the Formation of an Ionic Compound
Ionic compounds are formed when atoms gain or lose electrons to achieve a stable electron configuration. In the case of strontium chloride, strontium loses two electrons from its outermost 5s orbital, while chlorine gains one electron to fill its 3p orbital. This results in the formation of an ionic bond between the positively charged strontium ion (Sr2+) and the negatively charged chloride ion (Cl-).
The electron transfer between strontium and chlorine occurs due to the difference in electronegativity. Electronegativity is a measure of an atom’s ability to attract electrons towards itself in a chemical bond. Chlorine, being more electronegative than strontium, attracts the electrons from strontium, resulting in the formation of an ionic compound.
In summary, the electron configuration of strontium chloride is determined by the electron configurations of strontium and chlorine. Strontium loses two electrons to achieve a stable electron configuration, while chlorine gains one electron. This electron transfer leads to the formation of an ionic bond between the two elements, resulting in the formation of strontium chloride.
Conclusion
In conclusion, the electron configuration of strontium, an alkaline earth metal, is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2. This configuration indicates that strontium has a total of 38 electrons distributed across its energy levels. The electron configuration is a crucial aspect of understanding an element’s chemical behavior and its position in the periodic table. By knowing the electron configuration of strontium, scientists can predict its reactivity, bonding patterns, and other chemical properties. Strontium’s electron configuration places it in the same group as other alkaline earth metals, sharing similar characteristics such as high reactivity with water and the ability to form ionic compounds. Overall, the electron configuration of strontium provides valuable insights into its behavior and helps us comprehend the fascinating world of chemistry.
Frequently Asked Questions
1. What is the electron configuration of a strontium atom in its ground state?
The electron configuration of a strontium atom in its ground state is [Kr] 5s^2.
2. How does a strontium atom lose two electrons to form an Sr2+ ion?
When a strontium atom loses two electrons to form an Sr2+ ion, the electrons are lost from the 5s orbital.
3. What is the full electron configuration of strontium?
The full electron configuration of strontium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2.
4. How can the electron configuration of strontium be represented using an orbital diagram?
The electron configuration of strontium can be represented using an orbital diagram as follows:
1s ↑↓
2s ↑↓
2p ↑↓ ↑↓ ↑↓
3s ↑↓
3p ↑↓ ↑↓ ↑↓
4s ↑↓
3d ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p ↑↓ ↑↓ ↑↓
5s ↑↓
5. What happens when a strontium salt is ignited? How does it burn?
When a strontium salt is ignited, it burns with a characteristic red flame.
6. Can the electron configuration of strontium be in an excited state?
Yes, the electron configuration of strontium can be in an excited state. In an excited state, the electrons occupy higher energy levels or orbitals than the ground state configuration.
7. What is the unabbreviated electron configuration of strontium?
The unabbreviated electron configuration of strontium is 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 5s^2.
8. How does the electron configuration of a strontium ion differ from that of a strontium atom?
The electron configuration of a strontium ion differs from that of a strontium atom by the loss or gain of electrons. An Sr2+ ion, for example, has the electron configuration [Kr].
9. What is the electron configuration of strontium using noble gas notation?
The electron configuration of strontium using noble gas notation is [Kr] 5s^2.
10. Why is strontium important?
Strontium is important for various reasons. It is used in the production of fireworks to create a vibrant red color. It is also used in the manufacture of glass for television screens and in the medical field for certain imaging techniques. Additionally, strontium compounds have applications in the production of ceramics and as additives in metal alloys.
Also Read:
- Bohrium electron configuration
- Seaborgium electron configuration
- Europium electron configuration
- Gallium electron configuration
- Yttrium electron configuration
- Germanium electron configuration
- Ytterbium electron configuration
- Magnesium electron configuration
- Potassium electron configuration
- Bromine electron configuration
Hi….I am Deepali Arora and presently working as a Subject Matter Expert in Chemistry. I have henceforth completed my graduation and post-graduation in life sciences and chemistry respectively. I am highly inquisitive as far as learning and experimental aspects are concerned. I am looking forward to strengthening my career in the same field. I am good at troubleshooting and have a good critical thinking and analytical approach.