Give the electronic configurations of the following ions :
`(i) H^- " "(ii) Na^(+)`
`(iii) F^(-) " " (iv) Mg^(2+)` .

Explanation

To find the electronic configurations of the given ions, we need to start with the atomic number of each element and then adjust the number of electrons based on the charge of the ion. Here’s the step-by-step solution:

### Step 1: Determine the electronic configuration of H⁻
1. **Identify the atomic number of Hydrogen (H)**: The atomic number of Hydrogen is 1, which means it has 1 electron.
2. **Write the electronic configuration for neutral Hydrogen**: The configuration is \(1s^1\).
3. **Adjust for the ion (H⁻)**: The negative charge indicates that one electron has been added. Therefore, the configuration becomes \(1s^2\).

### Step 2: Determine the electronic configuration of Na⁺
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