Question

Write the electron configuration for the following at sunsheel level ;
Mg, S²- ,K+

Answer 1

To write the electron configurations at the subshell level for magnesium (Mg), sulfide ion (S²⁻), and potassium ion (K⁺), we first need to know the atomic number of each element or ion:

1. **Magnesium (Mg)**:
- Atomic number: 12
- Electron configuration: \(1s^2 2s^2 2p^6 3s^2\)

2. **Sulfide ion (S²⁻)**:
- Atomic number of sulfur (S): 16
- For S²⁻, we add 2 electrons, giving it a total of 18 electrons.
- Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6\) (This is the same as argon, which has 18 electrons.)

3. **Potassium ion (K⁺)**:
- Atomic number of potassium (K): 19
- For K⁺, we subtract 1 electron, giving it a total of 18 electrons.
- Electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6\) (Again, the same as argon.)

So, the electron configurations are as follows:

- Mg: \(1s^2 2s^2 2p^6 3s^2\)
- S²⁻: \(1s^2 2s^2 2p^6 3s^2 3p^6\)
- K⁺: \(1s^2 2s^2 2p^6 3s^2 3p^6\)

Notice that S²⁻ and K⁺ have the same electron configuration as argon (which has 18 electrons).