Chapter 8, Problem 1PS

Give the periodic group number and number of valence electrons for each of the following atoms.

1. (a) O
2. (b) B
3. (c) Na
4. (d) Mg
5. (e) F
6. (f) S

Interpretation Introduction

Interpretation: The periodic group number and number of valence electron for the given atom should be identified.

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,

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

Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.

Answer to Problem 1PS

Oxygen (O) atom belongs to Group 6A and carrying six valence electrons.

Explanation of Solution

Oxygen (O) atom belongs to Group 6A so it must be carrying six valence electrons.

Interpretation Introduction

Interpretation: The periodic group number and number of valence electron for the given atom should be identified.

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,

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

Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.

Answer to Problem 1PS

Boron (B) atom belongs to Group 3A so it must be carrying three valence electrons.

Explanation of Solution

Boron (B) atom belongs to Group 3A so it must be carrying three valence electrons.

Interpretation Introduction

Interpretation: The periodic group number and number of valence electron for the given atom should be identified.

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,

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

Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.

Answer to Problem 1PS

Sodium (Na) atom belongs to Group 1A so it must be carrying one valence electron.

Explanation of Solution

Sodium (Na) atom belongs to Group 1A so it must be carrying one valence electron.

Interpretation Introduction

Interpretation: The periodic group number and number of valence electron for the given atom should be identified.

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,

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

Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.

Answer to Problem 1PS

Magnesium (Mg) atom belongs to Group 2A so it must be carrying two valence electrons.

Explanation of Solution

Magnesium (Mg) atom belongs to Group 2A so it must be carrying two valence electrons.

Interpretation Introduction

Interpretation: The periodic group number and number of valence electron for the given atom should be identified.

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,

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

Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.

Answer to Problem 1PS

Fluorine (F) atom belongs to Group 7A so it must be carrying seven valence electrons

Explanation of Solution

Fluorine (F) atom belongs to Group 7A so it must be carrying seven valence electrons

Interpretation Introduction

Interpretation: The periodic group number and number of valence electron for the given atom should be identified.

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,

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

Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.

Answer to Problem 1PS

Sulphur(S) atom belongs to Group 6A so it must be carrying six valence electrons.

Explanation of Solution

Sulphur (S) atom belongs to Group 6A so it must be carrying six valence electrons.