Electron affinity of the elements or ions is correctly shown in

Options

A. `SgtO^(-)`
B. `OgtS^(-)`
C. `O^(-)gtS^(-)`
D. `N^(-)gtS`

Explanation

To solve the question regarding the electron affinity of elements or ions, we will analyze the concept of electron affinity and compare the electron affinities of specific elements.

### Step-by-Step Solution:

1. **Understand Electron Affinity**:
- Electron affinity is defined as the amount of energy released when an electron is added to a gaseous atom. It is an exothermic process, meaning that energy is released, and thus the change in enthalpy (ΔH) is negative.

**Hint**: Remember that electron affinity is related to how easily an atom can accept an electron.

2. **Analyze the Elements**:
- We will consider the electron affinities of sulfur (S), oxygen (O), and nitrogen (N).
- Sulfur has an electronic configuration of [Ne] 3s² 3p⁴.
- Oxygen has an electronic configuration of [He] 2s² 2p⁴.
- Nitrogen has an electronic configuration of [He] 2s² 2p³.

**Hint**: Write down the electronic configurations to visualize the electron arrangements.

3. **Compare Electron Affinities**:
- **Oxygen**: When an electron is added to oxygen, it goes from 2p⁴ to 2p⁵. There is significant intra-electronic repulsion due to the added electron being placed in the same p orbital, which makes it less favorable for oxygen to gain an electron.
- **Sulfur**: In sulfur, when an electron is added, it goes from 3p⁴ to 3p⁵. The presence of empty d orbitals allows for better accommodation of the added electron, resulting in a higher electron affinity compared to oxygen.
- **Nitrogen**: For nitrogen, adding an electron would lead to an increase in intra-electronic repulsion as well, since it would go from 2p³ to 2p⁴. Thus, nitrogen has a lower electron affinity than sulfur.

**Hint**: Consider the size of the atoms and the presence of empty orbitals when comparing their ability to accept electrons.

4. **Conclusion**:
- Based on the analysis, sulfur has a greater electron affinity than oxygen and nitrogen. Therefore, the correct statement regarding electron affinity is that sulfur has a higher electron affinity than O⁻ (the oxide ion) due to its larger size and the absence of significant intra-electronic repulsion.

**Hint**: Summarize your findings by comparing the electron affinities of the elements directly.

### Final Answer:
The electron affinity of sulfur is greater than that of oxygen and nitrogen, making option A the correct choice.