Chapter 4, Problem 4.96QP

Interpretation Introduction

Interpretation:

It should be stated that how the given set of properties follows the trend from left to right across the period and top to bottom of the group in the periodic table.

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.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

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

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

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.

Electronegativity: It is the tendency of the element to attract the pair of electrons towards itself.

Interpretation Introduction

Concept Introduction:

Shielding effect: The outermost electrons present in the element gets shielded or screened from the nuclear charge by electron present near to the nucleus that is the electrons that surrounds the nucleus (core electrons).

Effective nuclear charge: It is the total positive charge experienced by the valence electrons from the nucleus.

Atomic radius:

Atomic radius is the distance between the atomic nucleus and outermost electron of an atom.  From the atomic radius, the size of atoms can be visualized.  But there is no specific distance from nucleus to electron due to electron cloud around the atom does not have well-defined boundary.

Electronegativity: It is the tendency of the element to attract the pair of electrons towards itself.

Interpretation Introduction

Concept Introduction:

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

${\text{atom}}_{\left(\text{g}\right)}\to {\text{ion with positive charge}}_{\left(\text{g}\right)}\text{ + electron}$

Electronegativity: It is the tendency of the element to attract the pair of electrons towards itself.

Interpretation Introduction

Concept Introduction:

Acidity of oxides:

The more electronegativity the element has then the respective oxide of the element has more acidity.

Electronegativity: It is the tendency of the element to attract the pair of electrons towards itself.