From the given set of ions the ion that is suitable for the replacement of Ga 3+ should be determined. 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 specific name as follows, Group-1 → Alkali metal Group-2 → Alkaline metals Group-16 → Chalcogens Group-17 → Halogens Group-18 → Noble gases 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. In periodic table the horizontal rows are called periods and the vertical column are called group. Electronic configuration: It is used to denote the distribution of electrons placed over orbitals that present in the atom. The rules followed by the electrons are as follows, The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital( Aufbau principle) , pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled ( Hund’s Rule ) and finally, no two electrons that have same set of quantum numbers ( Pauli’s Exclusion Principle ).

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Chapter 4, Problem 4.95QP

Interpretation Introduction

Interpretation: From the given set of ions the ion that is suitable for the replacement of Ga3+ should be determined.

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 specific name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

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.

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

Electronic configuration: It is used to denote the distribution of electrons placed over orbitals that present in the atom.

The rules followed by the electrons are as follows,

The electrons gets distributed strictly following the order starting from lower energy orbital to higher energy orbital(Aufbau principle), pairing of electrons in subshell starts only when all the orbitals in the subshell are singly filled (Hund’s Rule) and finally, no two electrons that have same set of quantum numbers (Pauli’s Exclusion Principle).

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