Chapter 3, Problem 3.48AP

Interpretation Introduction

Interpretation:

The true and false statements about the ions to be predicted

Concept Introduction:

Formation of ions: 

Atom possesses equal number of protons and electrons and remains electrically neutral. By gaining (accepting electrons) or losing (donating electrons) one or more electrons, convert the neutral atom into a charged particle called IONS.

Cation: The loss of one or more electrons by a neutral atom leaves the atom positively charged called cation.

Anion: The gain of one or more electrons by a neutral atom leaves the neutral atom negatively charged called anion.

The symbolic representation of ions:

The electrons are reside in the principal quantum number ‘n’; by losing and gaining electron, reduces and increases in the electron count in the electronic configuration of the atom; for a cation adding positive charge as a superscript to the symbol of the element and for the anion adding negative charge as superscript to the symbol of the element.

Ionic charges of main group elements can be predicted using the group number and the octet rule:

For $\text{1A}$ and $\text{2A}$ metals: cation charge = group number.

For non-metals in groups $\text{5A, 6A, and 7A}$: anion charge = $\text{8 -}\left(\text{group number}\right)$