Book cover for Chemistry

Chemistry

Raymond Chang, Jason Overby

ISBN #9781259911156

13th Edition

3,254 Questions

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26,395 Students Helped

Homework Questions

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Summary
Learning Objectives
Key Concepts
Example Problems
Explanations
Common Mistakes

Summary

This section covers the fundamentals of chemical bonding, beginning with Lewis dot symbols which help in tracking valence electrons. It distinguishes between ionic and covalent bonds, explaining both the transfer of electrons (leading to ionic bonds) and the sharing of electrons (forming covalent bonds). Key concepts such as the octet rule, electronegativity, formal charge, and resonance are discussed to provide a framework for drawing correct Lewis structures. In addition, the concept of bond enthalpy is introduced, enabling the estimation of reaction enthalpies through energy accounting via breaking and forming bonds.

Learning Objectives

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Key Concepts

CONCEPT

DEFINITION

Acids and Bases (Ch 15)

Explains the fundamentals of acid–base chemistry by presenting both the Brønsted and Lewis definitions along with methods to evaluate acid and base strength. •

Example Problems

Example 1

What is a Lewis dot symbol? To what elements does the symbol mainly apply?

Example 2

Use the second member of each group from Group 1A to Group 7 A to show that the number of valence electrons on an atom of the element is the same as its group number.

Example 3

Without referring to Figure $9.1,$ write Lewis dot symbols for atoms of the following elements: (a) $\mathrm{Be},(\mathrm{b}) \mathrm{K},(\mathrm{c}) \mathrm{Ca},(\mathrm{d}) \mathrm{Ga},(\mathrm{e}) \mathrm{O},(\mathrm{f}) \mathrm{Br},(\mathrm{g}) \mathrm{N},(\mathrm{h})$ I, (i) As, (j) F.

Example 4

Write Lewis dot symbols for the following ions: (a) $\mathrm{Li}^{+},(\mathrm{b}) \mathrm{Cl}^{-},(\mathrm{c}) \mathrm{S}^{2-},(\mathrm{d}) \mathrm{Sr}^{2+},(\mathrm{e}) \mathrm{N}^{3-}$

Example 5

Write Lewis dot symbols for the following atoms (g) $\mathrm{Na},$ (h) $\mathrm{Na}^{+}$, (i) $\mathrm{Mg},(\mathrm{j}) \mathrm{Mg}^{2+},(\mathrm{k}) \mathrm{Al},$ (1) $\mathrm{Al}^{3+}$ $(\mathrm{m}) \mathrm{Pb},(\mathrm{n}) \mathrm{Pb}^{2+}$
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Step-by-Step Explanations

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Common Mistakes

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