Questions: QUESTION 7 Consider the following ground state electron configuration: 1s^2 2s^2 2p^4. Which of the ions has this ground state electron configuration? F^-1 N^+1 c^-2 O^-2

QUESTION 7
Consider the following ground state electron configuration: 1s^2 2s^2 2p^4. Which of the ions has this ground state electron configuration?
F^-1
N^+1
c^-2
O^-2

Transcript text: QUESTION 7 Consider the following ground state electron configuration: $1 s^{2} 2 s^{2} 2 p^{4}$. Which of the ions has this ground state electron configuration? $\mathrm{F}^{-1}$ $\mathrm{N}^{+1}$ $\mathrm{c}^{-2}$ $\mathrm{O}^{-2}$

Solution

Solution Steps

Step 1: Identify the given electron configuration

The given electron configuration is $1s^2 2s^2 2p^4$.

Step 2: Determine the total number of electrons

Count the total number of electrons in the given configuration: \[ 1s^2 \rightarrow 2 \text{ electrons} \] \[ 2s^2 \rightarrow 2 \text{ electrons} \] \[ 2p^4 \rightarrow 4 \text{ electrons} \] Total: $2 + 2 + 4 = 8$ electrons.

Step 3: Identify the neutral atom with 8 electrons

The neutral atom with 8 electrons is oxygen (O), which has an atomic number of 8.

Step 4: Determine the ion with the given electron configuration

The ion must have the same number of electrons as the neutral oxygen atom plus or minus the charge of the ion:

$\mathrm{F}^{-1}$: Fluorine (atomic number 9) with one extra electron, total $9 + 1 = 10$ electrons.
$\mathrm{N}^{+1}$: Nitrogen (atomic number 7) with one less electron, total $7 - 1 = 6$ electrons.
$\mathrm{C}^{-2}$: Carbon (atomic number 6) with two extra electrons, total $6 + 2 = 8$ electrons.
$\mathrm{O}^{-2}$: Oxygen (atomic number 8) with two extra electrons, total $8 + 2 = 10$ electrons.

Step 5: Match the ion to the given electron configuration

The ion with 8 electrons is $\mathrm{C}^{-2}$.