3.091SC | Fall 2010 | Undergraduate

Introduction to Solid State Chemistry

Bonding and Molecules

9. Drawing Lewis Structures

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Session Overview

Modules Bonding and Molecules
Concepts Lewis structures: octet stability, partial charge, bonding and nonbonding electrons, electronegativity: polar bonds and polar molecules, ionic character of covalent bonds, Coulomb’s law
Keywords cation, anion, Madelung constant, enthalpy, valence electron, Gilbert Lewis, ionization, isoelectronic, metal, nonmetal, ionic bond, electron transfer, electron sharing, covalent bond, percent ionic character, homonuclear bond, heteronuclear bond, triple bond, dative bond, s and p orbitals, Lewis structures, Linus Pauling, hybrid orbital, crystallization energy, bond energy, charge displacement, dipole moment, polar covalency, electronegativity, polar bond, polar molecule
Chemical Substances sodium (Na), chloride (Cl), nitrogen (N), oxygen (O), lithium (Li), beryllium (Be), magnesium (Mg), aluminum (Al), silicon (Si), hydrogen (H), helium (He), sulfuryl chloride (SO2Cl2), methane (CH4), magnesium chloride (MgCl2), hydrogen fluoride (HF), hydrogen chloride (HCl), sodium chloride (NaCl), Freon-12
Applications capacitors, refrigerant, compressor design


Before starting this session, you should be familiar with:

  • Hybridized bonding in molecules, VSEPR, properties of covalent bond, electron domain theory (Session 8)

Looking Ahead

Prof. Sadoway discusses hybridized and molecular orbitals along with paramagnetism (Session 10).

Learning Objectives

After completing this session, you should be able to:

  • Sketch the Lewis structure for a given compound.
  • Explain how octet stability is satisfied by electron sharing and electron transfer.
  • Understand how electron states can be mixed to form hybrid orbitals.
  • Define electronegativity and dipole moment.
  • Calculate the percent ionic character of a heteronuclear bond.
  • Explain how polar bonds may be present in polar and nonpolar molecules.


Archived Lecture Notes #2 (PDF), Section 3

Book Chapters Topics
[Saylor] 7.3, “Energetics of Ion Formation.” Ionization energies; electron affinities; electronegativity
[Saylor] 8.4, “Introduction to Lewis Dot Structures.” Creating a Lewis dot symbol; the octet rule
[Saylor] 8.5, “Lewis Structures and Covalent Bonding.” Using electron structures to describe covalent bonding; using Lewis electron structures to explain stoichiometry; using formal charges to distinguish between Lewis structures; resonance structures
[Saylor] 8.6, “Exceptions to the Octet Rule.” Odd number of electrons; more than an octet of electrons; fewer than an octet of electrons
[Saylor] 8.8, “Properties of Covalent Bonds.” Bond order; the relationship between bond order and bond energy; the relationship between molecular structure and bond energy
[Saylor] 8.9, “Polar Covalent Bonds.” Bond polarity; dipole moments

Lecture Video


Lecture Slides (PDF - 2.9MB)

Lecture Summary

Prof. Sadoway discusses the following concepts:

  • Problems with ionic bonding for diatomic molecules
  • G. N. Lewis – shell filling by electron sharing
    • Lewis dot notation
    • Cooperative use of valence electrons to achieve octet stability = covalent bonds
  • Ionic bond = electron transfer
  • Covalent bond = electron sharing (directional)
  • Carbon
    • s-orbitals “merge” with p-orbitals – sp3 hybridized
    • Results in 4 unpaired electrons, ready to bond
  • Energy of heteronuclear bonds
  • Percent ionic character
  • Polar bonding


Problems (PDF)

Solutions (PDF)

Textbook Problems

[Saylor] Sections Conceptual Numerical
[Saylor] 7.3, “Energetics of Ion Formation.” 1, 10 none
[Saylor] 8.2, “Ionic Bonding.” none 3
[Saylor] 8.6, “Exceptions to the Octet Rule.” none 1, 7
[Saylor] 8.9, “Polar Covalent Bonds.” none 2, 6, 7, 8
[Saylor] 9.1, “Predicting the Geometry of Molecules and Polyatomic Ions.” none 7

For Further Study

Supplemental Readings

Molina, Mario J. and Rowland, F. S. “Stratospheric sink for chlorofluoromethanes: chlorine atomc-atalysed destruction of ozone.Nature 249 (June 28, 1974): 810-812.


Gilbert Lewis

Linus Pauling - 1954 Nobel Prize in Chemistry, 1962 Nobel Prize in Peace

Arnold Sommerfeld

Fritz Haber - 1918 Nobel Prize in Chemistry

Erwin Madelung

Thomas Midgley

Other OCW and OER Content

Content Provider Level Notes
5.111 Principles of Chemical Science MIT OpenCourseWare Undergraduate (first-year)

Lecture 12: Ionic Bonds

Lecture 13: Polar Covalent Bonds and VSEPR Theory

Lecture 14: Molecular Orbit Theory

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Course Info

As Taught In
Fall 2010
Learning Resource Types
Course Introduction
Exams with Solutions
Lecture Notes
Lecture Videos
Problem Sets with Solutions
Recitation Videos
Problem Sets
Exam Materials