To determine what X represents in the partial electron configuration of an atom with 14 electrons (1s² 2s² 2p⁶ 3s² X), we first need to account for the number of electrons represented so far:
- 1s²: 2 electrons
- 2s²: 2 electrons
- 2p⁶: 6 electrons
- 3s²: 2 electrons
Adding these together: \(2 + 2 + 6 + 2 = 12\) electrons accounted for.
Since the atom has 14 electrons, this means there are 2 additional electrons to account for in X.
The available options for X are:
- 2d² (could represent 10 electrons)
- 3s² (already counted)
- 3p² (would add 2 electrons)
- 4s² (would add 2 electrons, but it's in a higher energy level)
Since adding 3p² or 4s² would give us 2 additional electrons, we need to determine what is the most suitable option for the electron configuration proceeding after 3s². According to the typical order of filling orbitals, after 3s², the 3p subshell would be filled before the 4s subshell.
Thus, X represents 3p².
So, the correct answer is 3p².
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