Answer
See the explanation
Work Step by Step
a. Electron configurations for the cations:
1. Mg2+:
Magnesium (Mg) has an atomic number of 12, with the electron configuration of 1s2 2s2 2p6 3s2.
When Mg forms a cation Mg2+, it loses its two 3s electrons, resulting in the electron configuration of 1s2 2s2 2p6.
2. K+:
Potassium (K) has an atomic number of 19, with the electron configuration of 1s2 2s2 2p6 3s2 3p6 4s1.
When K forms a cation K+, it loses its 4s electron, resulting in the electron configuration of 1s2 2s2 2p6 3s2 3p6.
3. Al3+:
Aluminum (Al) has an atomic number of 13, with the electron configuration of 1s2 2s2 2p6 3s2 3p1.
When Al forms a cation Al3+, it loses its three 3s and 3p electrons, resulting in the electron configuration of 1s2 2s2 2p6.
b. Electron configurations for the anions:
1. N3-:
Nitrogen (N) has an atomic number of 7, with the electron configuration of 1s2 2s2 2p3.
When N forms an anion N3-, it gains three electrons, resulting in the electron configuration of 1s2 2s2 2p6.
2. O2-:
Oxygen (O) has an atomic number of 8, with the electron configuration of 1s2 2s2 2p4.
When O forms an anion O2-, it gains two electrons, resulting in the electron configuration of 1s2 2s2 2p6.
3. F-:
Fluorine (F) has an atomic number of 9, with the electron configuration of 1s2 2s2 2p5.
When F forms an anion F-, it gains one electron, resulting in the electron configuration of 1s2 2s2 2p6.
4. Te2-:
Tellurium (Te) has an atomic number of 52, with the electron configuration of 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4.
When Te forms an anion Te2-, it gains two electrons, resulting in the electron configuration of 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6.
