Solutions & IMFs Flashcards

Vocabulary flashcards for Unit 9: Solutions & IMFs, covering key terms, properties of solutions, IMFs, and colligative properties.

Solution

A homogeneous mixture composed of 2 or more substances where the solute is evenly dispersed; can be a solid, liquid, or gas.

Solvent

The component of a solution present in a greater amount; the substance doing the dissolving.

Solute

The component of a solution present in a lesser amount; the substance being dissolved.

Saturated Solution

A solution containing the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.

Unsaturated Solution

A solution containing less than the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.

Homogeneous Mixture

A mixture with uniform composition throughout.

Colloid

A mixture with intermediate particle size between a solution and a suspension.

Molarity (M)

Moles of solute per liter of solution (mol/L).

Molality (m)

Moles of solute per kilogram of solvent (mol/kg).

Miscible

Liquids that are capable of dissolving in each other.

Supersaturated Solution

A solution that contains more dissolved solute than could normally dissolve at a given temperature.

Heterogeneous Mixture

A mixture with non-uniform composition throughout.

Suspension

A heterogeneous mixture containing solid particles that are large enough for sedimentation.

Soluble

Capable of being dissolved.

Dilute Solution

A solution that contains a small amount of solute relative to the amount of solvent.

Crystallization

The process by which solute molecules leave solution and deposit as a solid phase.

Solvation

The process of surrounding solute particles with solvent particles to form a solution.

Colligative Properties

Properties of solutions that depend on the concentration of solute particles but not on the identity of the solute.

Concentrated Solution

A solution containing a large amount of solute relative to the amount of solvent.

Solubility

The amount of solute that can dissolve in a given amount of solvent at a specific temperature.

Intermolecular Force (IMF)

Forces of attraction between molecules.

Lattice Energy

The energy required to separate one mole of a solid ionic compound into gaseous ions.

Intramolecular Force

Forces of attraction within a molecule (ionic, covalent, or metallic bonds).

Hydrogen Bond

A strong intermolecular force between hydrogen atom bonded to a highly electronegative atom (N, O, or F) and another electronegative atom.

Ion-Dipole Force

Intermolecular force between an ion and a polar molecule.

Dispersion Force (London Force)

Weakest intermolecular force, resulting from temporary fluctuations in electron distribution.

Heat of Solution

The amount of heat absorbed or released when a solute is dissolved in a solvent.

Heat of Hydration

The enthalpy change associated with the hydration of one mole of gaseous ions.

Entropy

A measure of the disorder or randomness of a system.

Enthalpy

The heat content of a system at constant pressure.

Exothermic Process

A process that releases heat to the surroundings.

Endothermic Process

A process that absorbs heat from the surroundings.

Solvation

The dissolving of one substance by another

Lattice Energy

The energy released when one mole of ions (in gaseous phase) are brought together from infinity

Hydration Energy

Energy released when one mole of ions are hydrated

Solubility (S)

A quantitative term referring to the amount of solute that can dissolve in a given amount of solvent at a given temperature.

Concentration

A measure of the amount of solute in a given amount of solvent.

6.02 x 10^23 particles

Avogadro’s Number

Serial Dilution

A stepwise dilution of a more concentrated solution

Colligative Property

Properties that depend upon the concentration of solute molecules or ions, but not upon the identity of the solute

Kf

molal freezing point depression constant

van 't Hoff factor (i)

A unitless constant directly associated with the degree of dissociation of the solute in the solvent

Kb

molal boiling point elevation constant