Chemistry Properties and Intermolecular Forces

A comprehensive set of flashcards covering the key concepts, vocabulary, and definitions related to the properties of liquids and solids based on the kinetic molecular model and intermolecular forces.

Kinetic Molecular Model of Solids

Describes solid particles as closely packed with limited vibrational motion.

Definite shape

Solids maintain a fixed shape due to close particle packing.

High density

Solids have tightly clustered particles resulting in minimal space.

Slow diffusion

In solids, particle movement is limited, allowing only slight diffusion.

Kinetic Molecular Model of Liquids

Liquids have close particles that can slide past one another due to translational motion.

Definite volume

Liquids maintain a fixed volume but no fixed shape.

Moderate density

Liquids have greater spacing between particles compared to solids.

Faster diffusion than solids

Liquid particles have more mobility compared to solid particles.

Low compressibility

Liquids resist volume changes under pressure due to minimal empty space.

Intermolecular Forces (IMF)

Attractive forces between molecules; weaker than intramolecular bonds.

London Dispersion Forces (LDFs)

Weakest IMF, occurs due to temporary dipoles in all substances.

Dipole-Dipole Forces

Attractive forces between polar molecules caused by permanent dipoles.

Hydrogen Bonding

Strongest type of dipole-dipole interaction involving H bonded to electronegative atoms.

Ion-Dipole Forces

Attraction between an ion and the oppositely charged end of a polar molecule.

Order of IMF strength

London dispersion forces < dipole-dipole forces < hydrogen bonding < ion-dipole forces.

Boiling point effect of IMFs

Stronger IMFs result in higher boiling points due to energy required to escape.

Solubility rule

'Like dissolves like'; similar IMFs mix well.

Surface tension

The cohesive force that minimizes a liquid’s surface area.

Viscosity

Resistance of a liquid to flow, influenced by molecular interactions.

Vapor pressure

Pressure exerted by vapor in equilibrium with its liquid.

Molar heat of vaporization

Energy required to convert liquid to gas at boiling point.

Water’s unique properties

High boiling point, surface tension, and capacity due to hydrogen bonding.

Crystalline solids

Ordered arrangement of particles in a repeating pattern (crystal lattice).

Amorphous solids

Disordered arrangement of particles without long-range order.

Phase Diagram

Graph showing stable phases of a substance at various temperatures and pressures.

Triple Point

Condition where solid, liquid, and gas phases coexist stably.

Heating Curve

Graph plotting temperature vs. heat added, showing phase changes and temperature increase.

Cooling Curve

Graph plotting temperature vs. heat removed, illustrating reversing phase transitions.

Percent by mass

Mass of solute per 100 parts by mass of solution.

Percent by volume

Volume of solute per 100 parts by volume of solution.

Mole fraction

Ratio of moles of one component to total moles of the solution.

Molarity (M)

Moles of solute per liter of solution.

Molality (m)

Moles of solute per kilogram of solvent.

Parts per million (ppm)

Mass of solute per million parts of solution.

Colligative properties

Properties that depend only on the number of solute particles.

Vapor pressure lowering

Addition of solute decreases the vapor pressure of the solution.

Boiling point elevation

Solutions have a higher boiling point than pure solvents.

Freezing point depression

Solutions freeze at lower temperatures than pure solvents.

Osmotic pressure

Pressure needed to stop solvent from flowing across a semipermeable membrane.