Chapter 8, Problem 111A

Interpretation Introduction

Interpretation: The ions having the same no. of electrons as a noble gas is to be selected.

Concept introduction:

The electron configuration of an element defines how its electrons are arranged throughout its atomic orbitals. Standard notation is used to represent atomic electron configurations, placing all electron-containing atomic subshells in sequential order. The number of electrons held by the subshell is indicated by superscript.

Answer to Problem 111A

All options are correct.

Explanation of Solution

Option a. ${\text{Al}}^{3+}$

The atomic no. of Al is 13 and after losing three electrons, the no. of electrons becomes 10. The no. of electrons in neon is 10.

Option b. ${\text{O}}^{2-}$

The atomic no. of O is 8 and after gaining two electrons, the no. of electrons becomes 10. The no. of electrons in neon is 10.

Option c. ${\text{Br}}^{-}$

The atomic no. of Br is 35 and after gaining two electrons, the no. of electrons becomes 36. The no. of electrons in krypton is 36.

Option 4. ${\text{N}}^{3-}$

The atomic no. of N is 7 and after gaining three electrons, the no. of electrons becomes 10. The no. of electrons in neon is 10.

Thus, all have noble gas electrons.