Question

(in hindi ti) (subtitle b answers 3)
question 3 what is the electron configuration of a sulfide ion (s²⁻)? how would you describe the configuration?
electron configuration of s²⁻:
table: can that choose the electron configuration:

• 1s²2s²2p⁶3s²3p⁴ = 1s²2s²2p⁶ - 1s²2s²2p⁶3s²3p⁴ - 1s²2s²2p⁶3s² - follow the
• naver one - supersite - wrongsite - naver one - naver one

Explanation:

To determine the electron configuration of a sulfide ion (\(S^{2-}\)), we start by recalling the electron configuration of a neutral sulfur atom (\(S\)). The atomic number of sulfur is 16, so its electron configuration is \(1s^2 2s^2 2p^6 3s^2 3p^4\). When sulfur gains 2 electrons to form the sulfide ion (\(S^{2-}\)), it achieves a stable octet configuration. This means we add 2 electrons to the outermost subshell, which is the \(3p\) subshell.

Step 1: Electron configuration of neutral S

The electron configuration of \(S\) (atomic number 16) is \(1s^2 2s^2 2p^6 3s^2 3p^4\).

Step 2: Electron configuration of \(S^{2-}\)

When \(S\) gains 2 electrons, the \(3p\) subshell, which originally had 4 electrons, now has \(4 + 2 = 6\) electrons. So the electron configuration of \(S^{2-}\) becomes \(1s^2 2s^2 2p^6 3s^2 3p^6\). Looking at the given options, the one that matches this is \(1s^2 2s^2 2p^6 3s^2 3p^6\) (the option labeled as "Neon Core" or the one with this configuration).

Answer:

The correct electron configuration for \(S^{2-}\) is \(1s^2 2s^2 2p^6 3s^2 3p^6\) (the option corresponding to this configuration, likely the one labeled with the correct configuration among the choices, e.g., if the options are as shown, the one with \(1s^2 2s^2 2p^6 3s^2 3p^6\)).