   Chapter 7, Problem 31PS

Chapter
Section
Textbook Problem

Which of the following groups of elements is arranged correctly in order of increasing ionization energy?(a) C < Si < Li < Ne(b) Ne < Si < C < Li(c) Li < Si < C < Ne(d) Ne < C < Si < Li

Interpretation Introduction

Interpretation:

The correct order of ionization energy has to be arranged for given the different periodic elements.

Concept Introduction:

Ionization energy (IE): The ionization energy is the required to remove an electron from an atom in the gas phase.

General formula of ionization energy = Atom in the ground state(g)Atom+(g)+eΔU=Ionizationenergy(IE)

Increase and decrease electro negativity: The less vacancy electrons an atoms has the least it will gain of electrons. Moreover the electron affinity decrease down the groups and from right to left across the periods on the periodic table, the reason is electrons are placed in a higher energy level far from the nucleus thus a decrease from its pull.

Explanation

Reason for correct options:

• Analyzing for Lithium (Li) atom

The ionization energies always have positive values, when electron far from the nucleus generally has smaller ionization energy and electron closer to the nucleus has larger ionization energy. Let us consider the lithium atom (Li), Here Li is s-block elements and its ionization energy is shown below.

First ionization energy (IE1) = 513 kJ/mol.

Li(g)Li+(g)+ eElectronconfiguration:1s22s1 1s22s0

• Analyzing for Silicon (Si) atom

The atomic number of silicon (Z=14) and 3rd period position in periodic table than this ionization energy is discussed below.

First ionization energy (IE1) = 787 kJ/mol.

Si(g) Si+(g) + e[Ne]3s23p2        [Ne]3s23p1

• Analyzing for Chlorine (Cl) atom

The atomic number of chlorine (Z=17) and 3rd period position in periodic table than this ionization energy is discussed below

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