Chapter 9, Problem 9.31QP

Interpretation Introduction

Interpretation:

Electronegativity should be defined using periodic trends and the difference between electronegativity and electron affinity should be explained.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

$\begin{array}{l}\text{Group}\text{-}\text{1}\stackrel{}{\to }\text{Alkali}\text{metal}\\ \text{Group}\text{-}\text{2}\stackrel{}{\to }\text{Alkaline}\text{metals}\\ \text{Group}\text{-}\text{16}\stackrel{}{\to }\text{Chalcogens}\\ \text{Group}\text{-}\text{17}\stackrel{}{\to }\text{Halogens}\\ \text{Group}\text{-}\text{18}\stackrel{}{\to }\text{Noble}\text{gases}\end{array}$

Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.