About This Chapter
OAE Chemistry: Intermolecular Forces - Chapter Summary
Get up to speed on the intermolecular forces concepts you learned about in college as you ready yourself for the OAE Chemistry exam. These lessons cover all the essential topics, such as:
- Hydrogen bonding, ion-dipole and dipole-dipole forces
- London dispersion forces
- Metallic bonding
Your study of this topic is guided by subject experts, who present information in an easy-to-use format that utilizes graphics and illustrations to make your learning experience stress-free and fun. You'll find useful tools that help you prepare for the exam, including video tags that let you review just the main points of each lesson.
OAE Chemistry: Intermolecular Forces - Chapter Objectives
The OAE Chemistry exam is used to assess your comprehension of chemistry and ability to teach chemistry topics to students. You'll answer questions that are in multiple-choice format and cover five different domains. Intermolecular forces are part of the energy and chemical bonding domain where you'll find 23% of the exam's 150 questions. Questions might ask you to read a passage and answer questions about what you read or to perform calculations and pick the best answer from the options presented. You can prepare for these questions with our self-assessment quizzes that mimic the format of the questions found on the exam.
1. Hydrogen Bonding, Dipole-Dipole & Ion-Dipole Forces: Strong Intermolecular Forces
Learn about intermolecular vs. intramolecular forces. Learn the different intermolecular bonds (including hydrogen bonding and dipole-dipole and ion-dipole forces), their strengths, and their effects on properties, such as boiling and melting points, solubility, and evaporation.
2. London Dispersion Forces (Van Der Waals Forces): Weak Intermolecular Forces
Learn how London dispersion forces are created and what effect they have on properties such as boiling and melting points. Discover this weak intermolecular force and how it is one of the Van der Waals forces.
3. Metallic Bonding: The Electron-Sea Model & Why Metals Are Good Electrical Conductors
Learn why metallic bonding is called the electron sea model. Discover why metals bond the way they do and why they are shiny, malleable and conduct electricity well.
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Other chapters within the Ohio Assessments for Educators - Chemistry (009): Practice & Study Guide course
- OAE Chemistry: Scientific Principles
- OAE Chemistry: Interdisciplinary Relationships in Science
- OAE Chemistry: Properties of Matter
- OAE Chemistry: Atomic Theory & the Periodic Table
- OAE Chemistry: Chemical Bonds
- OAE Chemistry: Liquids & Solids
- OAE Chemistry: Gases
- OAE Chemistry: Solutions & Solubility
- OAE Chemistry: Chemical Reactions & Kinetics
- OAE Chemistry: Chemical Equilibrium
- OAE Chemistry: Acids & Bases
- OAE Chemistry: Thermodynamics
- OAE Chemistry: Inorganic & Organic Compounds
- OAE Chemistry: Redox Reactions & Electrochemistry
- Ohio Assessments for Educators Chemistry Flashcards