Intermolecular forces hold molecules together to form solids and liquids. Related questions How do intermolecular forces differ from attraction between ions?
What is the strongest intermolecular force of attraction? What type of intermolecular force of attraction is found in ICl? When do intermolecular forces of attraction occur?
What does IMF do? How can I calculate intermolecular forces of attraction? Is SO2 a liquid, a solid, or a gas at room temperature? Why do Van der Waals forces increase down a group? Why do Van der Waals forces increase with the size of molecules? Intermolecular forces are attractive forces, but not chemical bonds. Thus, intermolecular forces are much weaker than intramolecular forces.
These forces determine the physical characteristics of a substance. One of their most important physical characteristics is the ability to determine the state of a substance — whether it is solid, liquid or gas. These forces are responsible for the random motion of gasses and the existence of liquids and solids as they hold liquid and solid molecules together.
Hence, intermolecular forces determine the melting and boiling point of the matter. Melting or boiling point is proportional to the strength of intermolecular forces. At a given temperature, the strengths of intermolecular forces of gas, liquid and solid are as follows.
There are three types of intermolecular forces known as dipole-dipole forces, London dispersion forces and hydrogen bonding forces. All these bonds occur due to electric charges resulting from the arrangement of electrons and nuclei in the molecules. Among the three types, hydrogen bonds are the strongest form of intermolecular bonds. Water molecules are held by hydrogen bonds due to the presence of partial charges at specific locations on the molecules.
Forces that hold atoms in a molecule are called intramolecular forces. These forces are responsible for the formation of chemical bonds. Thus, intramolecular forces are much stronger than intermolecular forces. Chapter 3: Molecules, Compounds, and Chemical Equations. Chapter 4: Chemical Quantities and Aqueous Reactions.
Chapter 5: Gases. Chapter 6: Thermochemistry. Chapter 7: Electronic Structure of Atoms. Chapter 8: Periodic Properties of the Elements.
Chapter 9: Chemical Bonding: Basic Concepts. Chapter Solutions and Colloids. Chapter Chemical Kinetics. Chapter Chemical Equilibrium. Chapter Acids and Bases. Chapter Acid-base and Solubility Equilibria. Chapter Thermodynamics. Chapter Electrochemistry. Chapter Radioactivity and Nuclear Chemistry.
Chapter Transition Metals and Coordination Complexes. Chapter Biochemistry. Full Table of Contents. This is a sample clip. Sign in or start your free trial. JoVE Core Chemistry. Previous Video Next Video. Next Video Embed Share. Chemical substances form when atoms or ions interact electrostatically. A covalent bond is formed when nonmetal atoms share their valence electrons. Please enter your institutional email to check if you have access to this content. Please create an account to get access.
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