Chapter 3, Problem 32P

Interpretation Introduction

(a)

Interpretation:

Two cations and two anions having the same electronic configuration as neon should be stated.

Concept Introduction:

Electron configuration of neon (Ne) is as follows,

  $1s^{2}2s^{2}2p^6$

Noble gases have the most stable electronic configurations; the valence shell is full. When forming ions, loss or gain of electron/s by an atom of a main group element takes place to attain the electronic configuration of the nearest noble gas in the periodic table.

There are two types of ions, cationic and anionic.

Cations are positively charged ions with less electrons than protons.

Anions are negatively charged ions and more electrons than protons.

Interpretation Introduction

(b)

Interpretation:

Two cations and two anions having the same electronic configuration as argon should be stated.

Concept Introduction:

Noble gases have the most stable electronic configurations; the valence shell is full. When forming ions, loss or gain of electron/s by an atom of a main group element takes place to attain the electronic configuration of the nearest noble gas in the periodic table.

When electrons are lost, cations are formed. They are positively charged ions and have fewer electrons than protons.

When electrons are gained, anions are formed. They are negatively charged ions and have more electrons than protons.

Electron configuration of argon (Ar) is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.