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Chemistry

Covalent Bonding and Molecular Compounds

A High School & College Primer

Covalent bonding shows up on nearly every chemistry exam — and it trips students up at every stage, from drawing Lewis structures to figuring out why water boils at a higher temperature than you would expect. If you have a test coming up, a problem set due, or a unit on molecular compounds that just is not clicking, this guide gets you up to speed fast.

**TLDR: Covalent Bonding and Molecular Compounds** covers the full arc of the topic in under 20 pages. You will learn what electron sharing actually means and why nonmetals do it, how to draw Lewis dot structures step by step (including resonance and formal charge), how VSEPR theory lets you predict molecular geometry from a simple set of rules, and how electronegativity and shape combine to make a molecule polar or nonpolar. The final sections walk through naming binary molecular compounds with Greek prefixes and explain how London dispersion forces, dipole-dipole interactions, and hydrogen bonding determine real-world properties like boiling point and solubility.

This is a high school and early-college chemistry study guide written for students who want clarity, not padding. Every term is defined, every concept comes with worked numbers, and common mistakes are called out directly. Parents helping a student through a confusing unit and tutors prepping a session will find it equally useful.

Pick it up, read it in one sitting, and walk into your next chemistry class ready.

What you'll learn
  • Explain why atoms share electrons and predict when a covalent bond will form instead of an ionic bond
  • Draw correct Lewis structures for simple molecules and polyatomic ions, including ones with multiple bonds and resonance
  • Use VSEPR theory to predict molecular geometry and bond angles
  • Determine whether a bond and a whole molecule are polar or nonpolar using electronegativity and shape
  • Name binary molecular compounds and connect intermolecular forces to physical properties like boiling point and solubility
What's inside
  1. 1. What a Covalent Bond Actually Is
    Introduces electron sharing between nonmetals, contrasts covalent with ionic bonding, and explains the octet rule using H2, O2, and HCl.
  2. 2. Drawing Lewis Structures
    Step-by-step procedure for drawing Lewis dot structures, including single, double, and triple bonds, polyatomic ions, formal charge, and resonance.
  3. 3. Molecular Shape: VSEPR Theory
    Uses electron-pair repulsion to predict the geometry and bond angles of common small molecules.
  4. 4. Bond Polarity and Molecular Polarity
    Connects electronegativity differences to polar bonds and shows how shape determines whether the whole molecule is polar.
  5. 5. Naming Molecular Compounds
    Rules for naming and writing formulas for binary molecular compounds using Greek prefixes, with a brief note on common exceptions.
  6. 6. Intermolecular Forces and Why Properties Differ
    Explains how London dispersion, dipole-dipole, and hydrogen bonding arise from molecular structure and predict boiling points, melting points, and solubility.
Published by Solid State Press
Covalent Bonding and Molecular Compounds cover
TLDR STUDY GUIDES

Covalent Bonding and Molecular Compounds

A High School & College Primer
Solid State Press

Covalent Bonding and Molecular Compounds

A High School & College Primer

Copyright © 2026 Solid State Press.

Published by Solid State Press.

All rights reserved. No part of this book may be reproduced or transmitted in any form without prior written permission, except for brief quotations in critical reviews and educational use.

Part of the TLDR Study Guides series.

Who This Book Is For

If you're a high school student who needs a covalent bonding study guide that actually gets to the point, you're in the right place. This book is equally useful for a sophomore taking honors chemistry, a junior prepping for the AP Chemistry exam, or a freshman in college who just left a lecture on molecular compounds feeling lost.

The pages that follow cover everything from how to draw Lewis dot structures to reading a molecular geometry chart, with a full Lewis structures and molecular geometry review built in. You'll work through VSEPR theory and molecular shape explained in plain terms, learn how bond polarity leads to molecular polarity, practice naming binary molecular compounds using Greek prefixes, and see how intermolecular forces drive differences in boiling point — all the chemistry prep you need, in about 15 pages with no filler.

Read straight through in order, work every example as you go, then test yourself on the problem set at the end.

Contents

  1. 1 What a Covalent Bond Actually Is
  2. 2 Drawing Lewis Structures
  3. 3 Molecular Shape: VSEPR Theory
  4. 4 Bond Polarity and Molecular Polarity
  5. 5 Naming Molecular Compounds
  6. 6 Intermolecular Forces and Why Properties Differ
Chapter 1

What a Covalent Bond Actually Is

Atoms bond because doing so makes them more stable — and the way two atoms split the difference between "I want these electrons" and "so do I" is by sharing them.

A covalent bond forms when two atoms share one or more pairs of electrons. Instead of one atom handing electrons to another (as happens in ionic bonding), both atoms hold onto the shared pair simultaneously, each counting those electrons toward its own stable configuration. The shared pair is called a bonding pair. Electrons that belong to one atom and are not involved in bonding are called lone pairs (sometimes called nonbonding pairs).

Why Sharing Happens: The Octet Rule

Most atoms are most stable when their outermost shell holds eight electrons. This observation is called the octet rule. The outermost electrons of an atom — the ones available for bonding — are its valence electrons. For main-group elements, the number of valence electrons equals the element's group number (under the US numbering, groups 1–18, where Group 1 has one valence electron, Group 17 has seven, and so on).

Hydrogen is the key exception: its outer shell can hold only two electrons, so it is stable at two. This smaller target is called the duet rule.

When two hydrogen atoms approach each other, each has one valence electron and wants two. By sharing their electrons with each other, both atoms simultaneously "see" two electrons in their shells — the stable duet. Neither atom fully owns the shared pair; they hold it jointly.

Example. Show why two hydrogen atoms form $\text{H}_2$ rather than staying as separate atoms.

Solution. Each H atom has 1 valence electron and needs 2 to complete its duet. If the two atoms share their electrons as one bonding pair, each atom counts both electrons in its shell: 1 (its own) + 1 (its partner's) = 2. Both atoms satisfy the duet rule simultaneously. The result is a single covalent bond, written H–H.

Keep reading

You've read the first half of Chapter 1. The complete book covers 6 chapters in roughly fifteen pages — readable in one sitting.

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