Multiple Choice
Which of the following is the correct electron configuration for boron (atomic number 5)?
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10. Periodic Properties of the Elements
The Electron Configuration
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Which atom in the ground state has a stable (completely filled) electron configuration?
A
Ne (neon)
B
O (oxygen)
C
Na (sodium)
D
Cl (chlorine)
Verified step by step guidance1
Recall that a stable, completely filled electron configuration corresponds to a noble gas or an atom with a full valence shell, typically following the octet rule for main group elements.
Write the electron configurations for each atom in the ground state: \\
$$\text{Neon (Ne)}: 1s^2 2s^2 2p^6$$
$$\text{Oxygen (O)}: 1s^2 2s^2 2p^4$$
$$\text{Sodium (Na)}: 1s^2 2s^2 2p^6 3s^1$$
$$\text{Chlorine (Cl)}: 1s^2 2s^2 2p^6 3s^2 3p^5$$
Identify which configuration has completely filled orbitals in its outermost shell. Neon has a full 2p subshell (2p^6), completing its octet, while the others have partially filled outer shells.
Conclude that the atom with the stable, completely filled electron configuration is Neon (Ne).
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