Question

Identify the complete electron configuration for an ion of the element potassium (K).

A. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰
B. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹
C. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
D. 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s²

Answer 1

The complete electron configuration of a potassium ion (K+) is 1s2 2s2 2p6 3s2 3p6, which reflects the noble gas configuration of argon (Ar) after losing one electron.

Step-by-step explanation:

The electron configuration for a potassium ion (K+) reflects the loss of one electron from the neutral atom's configuration. Potassium, with an atomic number of 19, has the electron configuration of [Ar]4s1 for the neutral atom. However, when it loses an electron to form a K+ ion, it achieves the noble gas configuration of argon, resulting in the electron configuration [Ar], which is equivalent to 1s2 2s2 2p6 3s2 3p6. Therefore, the complete electron configuration of a potassium ion is 1s2 2s2 2p6 3s2 3p6, which can also be referred to as the noble gas configuration of argon (Ar).