Questions: What is the electron configuration of an F- ion? Multiple Choice (1) 1s^2 2s^2 2ρ^4 (1) 1s^2 2s^2 2p^5 1s^2 2s^2 2p^6 1s^2 2s^2 2p^6 3s^1 1s^2 2s^2 2p^6 3s^2 3p^6

Transcript text: What is the electron configuration of an $F^{-}$ion? Multiple Cholce (1) $1 s^{2} 2 s^{2} 2 \rho^{4}$ (1) $1 s^{2} 2 s^{2} 2 p^{5}$ $1 s^{2} 2 s^{2} 2 p^{6}$ $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}$

Solution

Solution Steps

Step 1: Determine the Atomic Number of Fluorine

Fluorine (F) has an atomic number of 9, which means it has 9 protons and, in its neutral state, 9 electrons.

Step 2: Determine the Electron Configuration of Neutral Fluorine

The electron configuration of a neutral fluorine atom (F) is: \[ 1s^2 \, 2s^2 \, 2p^5 \]

Step 3: Determine the Electron Configuration of the $F^{-}$ Ion

An $F^{-}$ ion has gained one extra electron compared to a neutral fluorine atom. Therefore, it has 10 electrons in total. The electron configuration for 10 electrons is: \[ 1s^2 \, 2s^2 \, 2p^6 \]

Step 4: Identify the Correct Option

Among the given options, the correct electron configuration for the $F^{-}$ ion is: \[ 1s^2 \, 2s^2 \, 2p^6 \]