Unit 3 - Intermolecular Forces and Properties Practice Flashcards

This set of vocabulary flashcards covers key concepts from Unit 3, including intermolecular forces, gas laws, chromatography, and spectrophotometry, as presented in the Advanced Chemistry Exam review material.

Polar covalent bond

The result of unequal sharing of electrons forming the bond, as the more electronegative atom attracts the electrons more strongly.

Electronegativity

A measure of an atom's ability to attract electrons in a bond, which increases from left to right across a period and decreases down a group.

London dispersion forces

Intermolecular forces caused by instantaneous dipole-induced dipole interactions, which become stronger as the number of electrons and the size of the electron cloud increase.

Polarizability

The ease with which an electron cloud can be distorted; larger electron clouds are more easily polarized, leading to stronger London dispersion forces.

Hydrogen bonding

A strong intermolecular force occurring when a hydrogen atom is connected to a highly electronegative atom such as nitrogen, oxygen, or fluorine.

Miscibility

The ability of substances with similar intermolecular interactions to be soluble in one another, often follows the principle of "like dissolves like."

Dipole moment

A measure of the overall polarity of a molecule, which depends on both the bond polarity and the molecular geometry.

Dalton’s law

States that the total pressure in a container is the sum of the partial pressures of all gases present.

Ideal Gas Law

The mathematical relationship expressed as $PV = nRT$ used to calculate the behavior of gases.

Paper chromatography

A separation technique where components of a mixture travel up a stationary phase at different rates based on their affinity for the mobile phase.

Fractional distillation

A process used to separate miscible liquids based on their different boiling points, which are influenced by their intermolecular forces.

Spectrophotometer

An instrument used to measure the wavelengths of light absorbed by a colored solution to determine its concentration.

Beer-Lambert law

The relationship expressed as $A = \text{Î} \times c \times l$, stating that absorbance is proportional to the concentration ($c$) and path length ($l$) of the solution.

Maxwell-Boltzmann distribution

A graph showing the distribution of speeds for gas particles at a given temperature, where lighter gases move at higher speeds.

Gay-Lussac’s law

A principle stating that for a fixed amount of gas at constant volume, the pressure is directly proportional to the absolute temperature: $$rac{P_1}{T_1} = rac{P_2}{T_2}$ houses.

Real gas

A gas that deviates from ideal behavior at high pressure and low temperature because its particles exert intermolecular forces and occupy a finite volume.

Photoelectron spectroscopy (PES)

An experimental technique used to determine the ground-state electron configuration and binding energy of electrons in an element.

Binding energy

The amount of energy required to remove an electron from a specific shell of an atom, calculated in PES as $\text{Radiation Energy} - \text{Kinetic Energy}$.

Bond energy

The amount of energy required to break a chemical bond, typically measured in $kJ\,mol^{-1}$.

Graham's Law

States that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Hybridization

The concept of mixing atomic orbitals to form new hybrid orbitals, such as the $sp^3$ configuration found in the carbon atom of methanol.

Retardation factor ($R_f$)

The ratio of the distance traveled by a specific component in chromatography to the total distance traveled by the solvent front.