write out the electron configurations for each of the metallic ions:
1. Ba^2+
2. Cu^2+
3. Li^+
4. K^+
5. Sr^2+
6. Ca^2+
7. Na^+
with those charges, the ions have lost the valence electrons, so the electron configuration is the same as the Noble Gas configuration in the previous period.
then whats the electron configuration in the Noble Gas configuration in the previous period ?
To determine the electron configurations for each of the metallic ions, we need to identify the element associated with each ion and then remove the appropriate number of electrons based on the charge.
1. Ba^2+ (barium ion):
The atomic number of barium is 56.
The electron configuration of a neutral barium atom 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.
Since Ba^2+ has a charge of +2, we remove 2 electrons, starting from the outermost shell.
Therefore, the electron configuration of Ba^2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10.
2. Cu^2+ (copper ion):
The atomic number of copper is 29.
The electron configuration of a neutral copper atom is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^9.
Since Cu^2+ has a charge of +2, we remove 2 electrons, starting from the outermost shell.
Therefore, the electron configuration of Cu^2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^7.
3. Li^+ (lithium ion):
The atomic number of lithium is 3.
The electron configuration of a neutral lithium atom is: 1s^2 2s^1.
Since Li^+ has a charge of +1, we remove 1 electron.
Therefore, the electron configuration of Li^+ is: 1s^2.
4. K^+ (potassium ion):
The atomic number of potassium is 19.
The electron configuration of a neutral potassium atom is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1.
Since K^+ has a charge of +1, we remove 1 electron.
Therefore, the electron configuration of K^+ is: 1s^2 2s^2 2p^6 3s^2 3p^6.
5. Sr^2+ (strontium ion):
The atomic number of strontium is 38.
The electron configuration of a neutral strontium atom is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2.
Since Sr^2+ has a charge of +2, we remove 2 electrons, starting from the outermost shell.
Therefore, the electron configuration of Sr^2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6.
6. Ca^2+ (calcium ion):
The atomic number of calcium is 20.
The electron configuration of a neutral calcium atom is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2.
Since Ca^2+ has a charge of +2, we remove 2 electrons, starting from the outermost shell.
Therefore, the electron configuration of Ca^2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6.
7. Na^+ (sodium ion):
The atomic number of sodium is 11.
The electron configuration of a neutral sodium atom is: 1s^2 2s^2 2p^6 3s^1.
Since Na^+ has a charge of +1, we remove 1 electron.
Therefore, the electron configuration of Na^+ is: 1s^2 2s^2 2p^6.