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Answer :
- Determine the electron configuration of neutral Mn: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5$.
- Remove two electrons from the 4s orbital to form $Mn^{2+}$: $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5$.
- Identify the preceding noble gas, Argon (Ar).
- Write the abbreviated electron configuration: $\boxed{[Ar] 3d^5}$.
### Explanation
1. Understanding the Problem
We need to determine the abbreviated electron configuration for the $Mn^{2+}$ ion. This means we need to figure out how the electrons are arranged in this ion, using the noble gas that comes before it as a starting point.
2. Electron Configuration of Neutral Mn
First, let's find the electron configuration of a neutral Manganese (Mn) atom. Mn has an atomic number of 25, which means it has 25 electrons. The full electron configuration is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5$.
3. Forming the Mn2+ Ion
Now, let's consider the $Mn^{2+}$ ion. The +2 charge indicates that the Mn atom has lost two electrons. These electrons are removed from the outermost shell, which is the 4s orbital. So, we remove the two 4s electrons, resulting in the electron configuration $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5$.
4. Identifying the Noble Gas Core
To write the abbreviated electron configuration, we need to identify the noble gas that precedes Mn in the periodic table. That's Argon (Ar), which has an atomic number of 18. Argon's electron configuration is $1s^2 2s^2 2p^6 3s^2 3p^6$.
5. Abbreviated Electron Configuration
Finally, we can write the abbreviated electron configuration for $Mn^{2+}$. We replace the part of the electron configuration that matches Argon's with [Ar], and then add the remaining electrons. This gives us $[Ar] 3d^5$.
### Examples
Understanding electron configurations is crucial in chemistry for predicting how elements will interact to form chemical bonds. For example, knowing the electron configuration of manganese ions helps in understanding their role in various chemical reactions, such as in enzymes or in the formation of coordination complexes. This knowledge is also essential in materials science for designing new materials with specific magnetic or electronic properties.
- Remove two electrons from the 4s orbital to form $Mn^{2+}$: $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5$.
- Identify the preceding noble gas, Argon (Ar).
- Write the abbreviated electron configuration: $\boxed{[Ar] 3d^5}$.
### Explanation
1. Understanding the Problem
We need to determine the abbreviated electron configuration for the $Mn^{2+}$ ion. This means we need to figure out how the electrons are arranged in this ion, using the noble gas that comes before it as a starting point.
2. Electron Configuration of Neutral Mn
First, let's find the electron configuration of a neutral Manganese (Mn) atom. Mn has an atomic number of 25, which means it has 25 electrons. The full electron configuration is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5$.
3. Forming the Mn2+ Ion
Now, let's consider the $Mn^{2+}$ ion. The +2 charge indicates that the Mn atom has lost two electrons. These electrons are removed from the outermost shell, which is the 4s orbital. So, we remove the two 4s electrons, resulting in the electron configuration $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5$.
4. Identifying the Noble Gas Core
To write the abbreviated electron configuration, we need to identify the noble gas that precedes Mn in the periodic table. That's Argon (Ar), which has an atomic number of 18. Argon's electron configuration is $1s^2 2s^2 2p^6 3s^2 3p^6$.
5. Abbreviated Electron Configuration
Finally, we can write the abbreviated electron configuration for $Mn^{2+}$. We replace the part of the electron configuration that matches Argon's with [Ar], and then add the remaining electrons. This gives us $[Ar] 3d^5$.
### Examples
Understanding electron configurations is crucial in chemistry for predicting how elements will interact to form chemical bonds. For example, knowing the electron configuration of manganese ions helps in understanding their role in various chemical reactions, such as in enzymes or in the formation of coordination complexes. This knowledge is also essential in materials science for designing new materials with specific magnetic or electronic properties.
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