Question

Using complete subshell notation (not abbreviations, 1s²2s²2p⁶, and so forth), predict the electron configuration of each of the following atoms:

a. Carbon (C) : 1s²2s²2p²

b. Calcium (Ca) : 1s²2s²2p⁶ 3s²3p⁶ 4s²

c. Fluorine (F) : 1s²2s²2p⁵

d. Phosphorus (P) : 1s²2s²2p⁶ 3s²3p³

Answer 1

Electron configurations for N³⁻ and Ca²⁺ ions are 1s²2s²2p⁶ and 1s²2s²2p⁶ 3s²3p⁶, respectively, resembling the configurations of noble gases Neon and Argon.

Step-by-step explanation:

The student has asked the question: Using complete subshell notation (1s²2s²2p⁶, and so forth), predict the electron configurations of the following ions: N³⁻ (a) and Ca²⁺ (b).

Complete Electron Configurations

• (a) N³⁻ (Nitride ion): Since a “N³⁻” ion gains three electrons compared to a neutral nitrogen atom, the complete electron configuration will be 1s²2s²2p⁶. This configuration corresponds to that of the neon atom, indicating that the nitride ion has a filled second shell.
• (b) Ca²⁺ (Calcium ion): A “Ca²⁺” ion loses two electrons compared to a neutral calcium atom. The electron configuration of the calcium ion will thus be 1s²2s²2p⁶ 3s²3p⁶, which is the electron configuration of an argon atom. The fourth shell (4s) electrons are removed when forming the Ca²⁺ ion.