To solve this problem, let's start by examining the given electron configuration: \(1s^2 2s^2 2p^2\).
1. Identify the total number of electrons:
- The notation \(1s^2\) indicates there are 2 electrons in the 1s orbital.
- The notation \(2s^2\) indicates there are 2 electrons in the 2s orbital.
- The notation \(2p^2\) indicates there are 2 electrons in the 2p orbital.
So, we can sum these electron counts:
[tex]\[
\text{Total electrons} = 2 \text{ (1s)} + 2 \text{ (2s)} + 2 \text{ (2p)} = 6 \text{ electrons}
\][/tex]
2. Determine the number of electrons required for an octet:
An octet configuration means having 8 electrons in the outermost shell (valence shell).
3. Calculate the number of electrons needed to complete the octet:
We have established that the atom currently has 6 electrons in its electron configuration. To achieve an octet, which is 8 electrons, we need:
[tex]\[
\text{Electrons needed} = 8 \text{ (octet)} - 6 \text{ (current electrons)} = 2 \text{ electrons}
\][/tex]
Thus, the atom needs to gain 2 electrons to achieve an octet.
[tex]\[\boxed{2} \text{ electrons}\][/tex]
