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Science Chemistry ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM

The reason behind greater value of lattice energy of lithium chloride than that of rubidium chloride has to be explained. Concept Introduction: Three-dimensional array of ions constitute the ionic compound lattice. They are stabilized because of attractive forces between oppositely charged ions that lower the potential energy. Stability of ionic compound depends upon two factors and that is size and charge. Higher the charge and less will be the stability of ionic compound and vice-versa. Smaller the size of anion more will be the stability Lower is the potential energy of interaction and more stable is the ionic solid. Hence the compounds that have high charge density on small space are most stable ionic solids. For example, calcium phosphate is made up of Ca 2 + and PO 4 3 − . The highly charged ions have stronger interionic interactions and this accounts for rigidity of calcium phosphate. The lattice energy of strong ionic solids is often very large because of small and densely charged ions.

The reason behind greater value of lattice energy of lithium chloride than that of rubidium chloride has to be explained. Concept Introduction: Three-dimensional array of ions constitute the ionic compound lattice. They are stabilized because of attractive forces between oppositely charged ions that lower the potential energy. Stability of ionic compound depends upon two factors and that is size and charge. Higher the charge and less will be the stability of ionic compound and vice-versa. Smaller the size of anion more will be the stability Lower is the potential energy of interaction and more stable is the ionic solid. Hence the compounds that have high charge density on small space are most stable ionic solids. For example, calcium phosphate is made up of Ca 2 + and PO 4 3 − . The highly charged ions have stronger interionic interactions and this accounts for rigidity of calcium phosphate. The lattice energy of strong ionic solids is often very large because of small and densely charged ions.

Solution Summary: The author explains the reason behind greater value of lattice energy of lithium chloride than that of rubidium.

ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM

ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM

7th Edition

ISBN: 9781319403959

Author: ATKINS

Publisher: MAC HIGHER

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Question

Chapter 2, Problem 2A.29E

Interpretation Introduction

Interpretation:

The reason behind greater value of lattice energy of lithium chloride than that of rubidium chloride has to be explained.

Concept Introduction:

Three-dimensional array of ions constitute the ionic compound lattice. They are stabilized because of attractive forces between oppositely charged ions that lower the potential energy.

Stability of ionic compound depends upon two factors and that is size and charge. Higher the charge and less will be the stability of ionic compound and vice-versa. Smaller the size of anion more will be the stability

Lower is the potential energy of interaction and more stable is the ionic solid. Hence the compounds that have high charge density on small space are most stable ionic solids. For example, calcium phosphate is made up of Ca2+ and PO43−. The highly charged ions have stronger interionic interactions and this accounts for rigidity of calcium phosphate. The lattice energy of strong ionic solids is often very large because of small and densely charged ions.

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Chapter 2, Problem 2A.28E

Chapter 2, Problem 2A.30E

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Chapter 2 Solutions

ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM

Ch. 2 - Prob. 2A.1AST Ch. 2 - Prob. 2A.1BST Ch. 2 - Prob. 2A.2AST Ch. 2 - Prob. 2A.2BST Ch. 2 - Prob. 2A.3AST Ch. 2 - Prob. 2A.3BST Ch. 2 - Prob. 2A.4AST Ch. 2 - Prob. 2A.4BST Ch. 2 - Prob. 2A.1E Ch. 2 - Prob. 2A.2E

Ch. 2 - Prob. 2A.3E Ch. 2 - Prob. 2A.4E Ch. 2 - Prob. 2A.5E Ch. 2 - Prob. 2A.6E Ch. 2 - Prob. 2A.7E Ch. 2 - Prob. 2A.8E Ch. 2 - Prob. 2A.9E Ch. 2 - Prob. 2A.10E Ch. 2 - Prob. 2A.11E Ch. 2 - Prob. 2A.12E Ch. 2 - Prob. 2A.13E Ch. 2 - Prob. 2A.14E Ch. 2 - Prob. 2A.15E Ch. 2 - Prob. 2A.16E Ch. 2 - Prob. 2A.17E Ch. 2 - Prob. 2A.18E Ch. 2 - Prob. 2A.19E Ch. 2 - Prob. 2A.20E Ch. 2 - Prob. 2A.21E Ch. 2 - Prob. 2A.22E Ch. 2 - Prob. 2A.23E Ch. 2 - Prob. 2A.24E Ch. 2 - Prob. 2A.25E Ch. 2 - Prob. 2A.26E Ch. 2 - Prob. 2A.27E Ch. 2 - Prob. 2A.28E Ch. 2 - Prob. 2A.29E Ch. 2 - Prob. 2A.30E Ch. 2 - Prob. 2B.1AST Ch. 2 - Prob. 2B.1BST Ch. 2 - Prob. 2B.2AST Ch. 2 - Prob. 2B.2BST Ch. 2 - Prob. 2B.3AST Ch. 2 - Prob. 2B.3BST Ch. 2 - Prob. 2B.4AST Ch. 2 - Prob. 2B.4BST Ch. 2 - Prob. 2B.5AST Ch. 2 - Prob. 2B.5BST Ch. 2 - Prob. 2B.1E Ch. 2 - Prob. 2B.2E Ch. 2 - Prob. 2B.3E Ch. 2 - Prob. 2B.4E Ch. 2 - Prob. 2B.5E Ch. 2 - Prob. 2B.6E Ch. 2 - Prob. 2B.7E Ch. 2 - Prob. 2B.8E Ch. 2 - Prob. 2B.9E Ch. 2 - Prob. 2B.10E Ch. 2 - 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Prob. 2E.25E Ch. 2 - Prob. 2E.26E Ch. 2 - Prob. 2E.27E Ch. 2 - Prob. 2E.28E Ch. 2 - Prob. 2E.29E Ch. 2 - Prob. 2E.30E Ch. 2 - Prob. 2F.1AST Ch. 2 - Prob. 2F.1BST Ch. 2 - Prob. 2F.2AST Ch. 2 - Prob. 2F.2BST Ch. 2 - Prob. 2F.3AST Ch. 2 - Prob. 2F.3BST Ch. 2 - Prob. 2F.4AST Ch. 2 - Prob. 2F.4BST Ch. 2 - Prob. 2F.1E Ch. 2 - Prob. 2F.2E Ch. 2 - Prob. 2F.3E Ch. 2 - Prob. 2F.4E Ch. 2 - Prob. 2F.5E Ch. 2 - Prob. 2F.6E Ch. 2 - Prob. 2F.7E Ch. 2 - Prob. 2F.8E Ch. 2 - Prob. 2F.9E Ch. 2 - Prob. 2F.10E Ch. 2 - Prob. 2F.11E Ch. 2 - Prob. 2F.12E Ch. 2 - Prob. 2F.13E Ch. 2 - Prob. 2F.14E Ch. 2 - Prob. 2F.15E Ch. 2 - Prob. 2F.16E Ch. 2 - Prob. 2F.17E Ch. 2 - Prob. 2F.18E Ch. 2 - Prob. 2F.19E Ch. 2 - Prob. 2F.20E Ch. 2 - Prob. 2F.21E Ch. 2 - Prob. 2G.1AST Ch. 2 - Prob. 2G.1BST Ch. 2 - Prob. 2G.2AST Ch. 2 - Prob. 2G.2BST Ch. 2 - Prob. 2G.1E Ch. 2 - Prob. 2G.2E Ch. 2 - Prob. 2G.3E Ch. 2 - Prob. 2G.4E Ch. 2 - Prob. 2G.5E Ch. 2 - Prob. 2G.6E Ch. 2 - Prob. 2G.7E Ch. 2 - Prob. 2G.8E Ch. 2 - Prob. 2G.9E Ch. 2 - 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