Chapter 2, Problem 16P

Interpretation Introduction

Interpretation:

Pairs of isoelectronic species from the following list: HF;${\text{CO}}_{\text{2 }}$;${\text{SO}}_{\text{2 }}$;${\text{NH}}_{\text{3}}$;${\text{PF}}_{\text{3}}$;${\text{SF}}_4$;${\text{SiCl}}_4$; ${\left[{\text{H}}_{\text{3}}\text{O}\right]}^{+}$; ${\left[{\text{NO}}_{\text{2}}\right]}^{+}$; ${\left[\text{OH}\right]}^{\text{-}}$; ${\left[{\text{AlCl}}_4\right]}^{\text{-}}$ are to be identified.

Concept Introduction:

Two or more species, if they possess the same number of electrons are called isoelectronic species. For example, ${\text{O}}^{\text{2-}}{\text{,F}}^{\text{-}}\text{,}{\text{Na}}^{\text{+}}\text{and}{\text{Mg}}^{\text{2+}}$ are isoelectronic species of each other

Isoelectronic species that possess the same structure are called isostructural. For example, ${\left[{\text{BH}}_{\text{4}}\right]}^{\text{-}}\text{,}{\text{CH}}_{\text{4}}\text{and}{\left[{\text{NH}}_{\text{4}}\right]}^{\text{+}}$

Atomic number (Z) = number of protons present in the nucleus of an atom of the element = number of electrons present in a neutral atom of the element