Chemistry 2
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Chemistry 2 - BarCharts, Inc.
Table of Contents
Intermolecular Forces
Changes in Matter
Solutions
Chemical Kinetics
Acids & Bases
Thermodynamics
Electrochemistry
Radioactivity
Intermolecular Forces
Types of Intermolecular Forces
Intermolecular forces: Forces between molecules, atoms, or particles
Can be attractive or repulsive
Are generally weaker than bonding forces
Relates to Coulomb’s law:
E =
=
Dispersion forces (London forces)
Occurs in all molecules and atoms
Created by the variability in the distribution of electrons outside the nucleus
Electrons are randomly arranged at any one point in time
The arrangement creates a temporary/instantaneous dipole
The magnitude is dependent on the ease of polarization of electrons
Polarize: Form a dipole moment
Depends on the molar mass and the molecular Shape
Polarity
Polarity depends on differences in electronegativity (ΔEN)
Electronegativity: Ability of an atom to attract electrons
Nonmetals have higher electronegativity than metals
ΔEN > 2.0: Ionic bond (nonpolar); electrons are transferred
ΔEN 0–0.4: Covalent bond (nonpolar); electrons are shared equally or nearly equally
ΔEN 0.4–2.0: Covalent bond (polar); electrons are shared unequally
Polar molecules have electron-rich and electron-poor areas
Polarity helps determine liquids’ miscibility, the ability to mix
Practical applications
Water is a polar molecule and grease and oil are nonpolar, so they don’t mix
One end of a soap molecule is polar and the other nonpolar, so soap can attract both water and grease
Dipole-dipole force
Occurs in all polar molecules, which have:
A permanent dipole
Dispersion forces
Higher melting and boiling points
Hydrogen bonding
Occurs in polar molecules with hydrogen atoms
Is the strongest of all intermolecular forces
Has a strong dipole-dipole attractive force
Hydrogen atoms bond with fluorine, nitrogen, and oxygen
Water has hydrogen bonds—without it, all Earth’s water