A Chemistry Guide: Properties of Substances and Mixtures

This set of flashcards covers key terms and concepts related to the properties of substances and mixtures in chemistry, including various intermolecular forces, types of solids, gas behavior, and solution chemistry.

London Dispersion Forces (LDF)

The sole force in nonpolar substances, caused by temporary dipoles due to the random motion of electrons.

Dipole-Dipole Forces

Attractive forces between two polar molecules, strengthened by greater polarity and orientation.

Dipole-Induced Dipole

Attraction between a polar molecule and a nonpolar molecule, increasing with more polarity of the polar molecule.

Ion-Dipole Forces

Attraction between an ion and a polar molecule, generally stronger than dipole-dipole interactions.

Hydrogen Bonding

A strong form of dipole-dipole interaction, requiring a partially positive hydrogen attached to N, O, or F, attracted to a partially negative N, O, or F.

Ionic Substances

Compounds with strong interactions between ions, resulting in low vapor pressure and high melting/boiling points.

Covalent Network Solids

Substances with extensive covalent bonds throughout, leading to very high melting/boiling points.

Molecular Solids

Compounds held together by weak intermolecular forces, generally having high vapor pressure and low melting/boiling points.

Metallic Solids

Composed of metal atoms with cations in a sea of electrons, allowing for conductivity.

Kinetic Molecular Theory (KMT)

The theory describing gas behavior, emphasizing constant random motion and elastic collisions of particles.

Ideal Gas Law

Relates pressure, volume, moles, and absolute temperature of a gas: PV=nRT.

Dalton's Law of Partial Pressures

States that the total pressure of a gas mixture equals the sum of the partial pressures of its individual gases.

Molarity (M)

A common unit for concentration, calculated as moles of solute per liter of solution.

Solubility

The property of a solute to mix with a solvent; miscible means they mix, while immiscible means they do not.

Rf Value

A measure used in chromatography that compares the distance traveled by a compound to the distance travelled by the solvent.

Beer-Lambert Law

Describes the relationship between absorbance and concentration of a solution, stating that absorbance increases with concentration.