Properties of Substances & Mixtures

These flashcards cover key vocabulary and concepts regarding intermolecular forces, gas laws, solutions, and light interactions relevant for understanding the properties of substances and mixtures.

Intermolecular Forces

Forces that exist between molecules, including dipole-dipole, hydrogen bonding, and London dispersion forces.

Coulomb's Law

A law that states the force between two charged particles is directly proportional to the product of the charges and inversely proportional to the square of the distance between them.

London Dispersion Forces

A type of intermolecular force that occurs due to temporary dipoles induced in atoms or molecules; the weakest form of attraction.

Permanent Dipole

A dipole that occurs in a molecule with polar bonds, leading to a permanently uneven distribution of charges.

Hydrogen Bonding

A strong type of dipole-dipole interaction that occurs between molecules where hydrogen is bonded to electronegative atoms like nitrogen, oxygen, or fluorine.

Ideal Gas Law

The relationship between pressure, volume, temperature, and number of moles of a gas, expressed as PV = nRT.

Kinetic Molecular Theory

A model that explains the behavior of gases in terms of particle motion, describing how gas particles are in constant, random motion.

Solubility

The ability of a substance to dissolve in a solvent, depending on the strength of interactions between solute and solvent.

Spectroscopy

The study of the interaction between matter and electromagnetic radiation to gain information about a substance's properties.

Beer-Lambert Law

A law that relates the absorbance of a solution to its concentration and the path length of light through the solution (A = εbc).

Intermolecular Forces

Forces that exist between molecules, including dipole-dipole, hydrogen bonding, and London dispersion forces.

Coulomb's Law

A law that states the force between two charged particles is directly proportional to the product of the charges and inversely proportional to the square of the distance between them.

London Dispersion Forces

A type of intermolecular force that occurs due to temporary dipoles induced in atoms or molecules; the weakest form of attraction.

Permanent Dipole

A dipole that occurs in a molecule with polar bonds, leading to a permanently uneven distribution of charges.

Hydrogen Bonding

A strong type of dipole-dipole interaction that occurs between molecules where hydrogen is bonded to electronegative atoms like nitrogen, oxygen, or fluorine.

Ideal Gas Law

The relationship between pressure, volume, temperature, and number of moles of a gas, expressed as PV = nRT.

Kinetic Molecular Theory

A model that explains the behavior of gases in terms of particle motion, describing how gas particles are in constant, random motion.

Solubility

The ability of a substance to dissolve in a solvent, depending on the strength of interactions between solute and solvent.

Spectroscopy

The study of the interaction between matter and electromagnetic radiation to gain information about a substance's properties.

Beer-Lambert Law

A law that relates the absorbance of a solution to its concentration and the path length of light through the solution (A =
\epsilonbc).

Dipole-Dipole Forces

Intermolecular forces that occur between two polar molecules due to the attraction between the positive end of one molecule and the negative end of another.

Electronegativity

The measure of an atom's tendency to attract electrons towards itself in a chemical bond.

Polar Molecule

A molecule that has a net dipole moment due to the uneven distribution of electron density, resulting from differences in electronegativity and molecular geometry.

Solute

The substance that is dissolved in a solvent to form a solution, typically present in a smaller amount.

Solvent

The substance that dissolves a solute, typically present in a larger amount, forming a solution.

Absorbance

A measure of the amount of light absorbed by a sample, directly proportional to the concentration of the absorbing species and the path length of the light.

Molar Absorptivity (Extinction Coefficient)

A constant in the Beer-Lambert Law (\epsilon) that represents how strongly a chemical species absorbs light at a particular wavelength per unit concentration and path length.