General Chemistry Semester 2 Final Review

What is composition stoichiometry?

Deals with the mass relationships of elements in compounds.

What is reaction stoichiometry?

Involves the mass relationships between reactants and products in a chemical reaction.

What is mole ratio?

Conversion factor that relates amounts in moles of any two substances in a chemical reaction.

What is a limiting reactant?

Reactant that limits the amount of the other reactant that can combine and the amount of product that can form.

What is an excess reactant?

Substance that is not used up completely in a reaction.

What is theoretical yield?

Maximum amount of product that can be produced from a given amount of reactant.

What is actual yield?

Measured amount of product obtained from a reaction.

What is percentage yield?

\frac{\text{actual yield}}{\text{theoretical yield}} \times 100

What is the Kinetic Molecular Theory (KMT)?

Particles of matter are always in motion; explains properties of solids, liquids, and gases.

What is an ideal gas?

Hypothetical gas that perfectly fits all assumptions of KMT.

What is an elastic collision?

No net loss of total kinetic energy (KE).

What is diffusion?

Spontaneous mixing of particles of two substances by their random motion.

What is effusion?

Gas particles pass through a tiny opening.

What is a real gas?

Gas that does not behave completely according to the assumptions of KMT.

What is Surface Tension?

Force that tends to pull adjacent parts of a liquid's surface together, decreasing surface area.

What is Capillary Action?

Attraction of the surface of a liquid to the surface of a solid.

What is Vaporization?

Process by which a liquid or solid changes to a gas.

What is Evaporation?

Particles escape from the surface of a non-boiling liquid and enter the gas state.

What is Boiling?

Change of a liquid to bubbles of vapor that appear throughout the liquid.

What is Melting point?

Temperature at which a solid becomes a liquid.

What is a Crystal?

Substance in which particles are arranged in an orderly, geometric, repeating pattern.

What is an Amorphous solid?

Noncrystalline solid where particles are arranged randomly.

What is Crystal Structure?

Total 3-dimensional arrangement of particles of a crystal.

What is a Unit Cell?

Smallest portion of a crystal lattice that shows the 3D pattern of the entire lattice.

What is a Crystal Lattice?

Coordinate system representing the arrangement of particles in a crystal.

What is a Phase?

Any part of a system with uniform composition and properties.

What is Condensation?

Process by which a gas turns into a liquid.

What is Equilibrium?

Dynamic condition where two opposing changes occur at equal rates in a closed system.

What is Equilibrium Vapor Pressure?

Pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature.

What is Boiling Point?

Temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure.

What is Molar Enthalpy of Vaporization?

Heat needed to vaporize 1 mole of liquid at its boiling point at constant pressure.

What is Freezing Point?

Temperature at which the solid and liquid are in equilibrium at 1 atm pressure.

What is Sublimation?

Change of a solid directly to a gas.

What is Deposition?

Change of a gas directly into a solid.

What is a Phase Diagram?

Graph of pressure vs temperature showing conditions under which phases of substances exist.

What is Pressure (P)?

Force per unit area on a surface: P = \frac{Force}{Area}

What is Standard Temperature and Pressure (STP)?

Standard conditions of 1 atm pressure and 0 degrees Celsius.

What is Dalton’s Law of Partial Pressures?

Total pressure of a gas mixture is the sum of the partial pressures of the component gases.

What is Boyle’s Law?

The volume of a fixed mass of gas varies inversely with the pressure at constant temperature: P1V1 = P2V2

What is Charles’s Law?

Volume of a gas at constant pressure varies directly with the temperature in Kelvins: \frac{V1}{T1} = \frac{V2}{T2}

What is Gay-Lussac’s Law?

Pressure of a gas at constant volume varies directly with the temperature in Kelvins: \frac{P1}{T1} = \frac{P2}{T2}

What is the Combined Gas Law?

Expresses the relationship between pressure, volume, and temperature of a fixed amount of gas: \frac{P1V1}{T1} = \frac{P2V2}{T2}

What is Avogadro’s Law?

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules: V = kn

What is Graham’s Law of Effusion?

Rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses.

What is a Solution?

Homogeneous mixture of two or more substances uniformly dispersed throughout a single phase.

What is a Solvent?

Dissolving medium in a solution.

What is a Solute?

Substance dissolved in a solution.

What is a Suspension?

Mixture where particles are large and settle out unless constantly stirred.

What is a Colloid?

Mixture with particles of intermediate size between solutions and suspensions.

What is a Saturated Solution?

Solution that contains the maximum amount of dissolved solute

What is a Unsaturated Solution?

Solution that contains less solute than a saturated solution

What is Supersaturated Solution?

Solution that contains more solute than a saturated solution under the same conditions

What is "Like Dissolves Like"?

Polar substances dissolve polar substances; nonpolar substances dissolve nonpolar substances

What is Henry's Law?

The solubility of a gas in a liquid is tethered to the partial pressure of the gas on the surface of the liquid

What is Enthalpy of Solution?

The net amount of energy absorbed by a solution when a part of a solute dissolves

What is Molarity (M)?

Moles of solute per liter of solution

What is Molality (m)?

Moles of solute per kilogram of solvent

What is Dissociation?

Separation of ions when an ionic compound dissolves in water.

What is Ionization?

Formation of ions from molecular compounds in solution.

What is Strong Electrolyte?

Compound that fully dissociates into ions when dissolved in water

What is Weak Electrolyte?

Compound that partially dissociates into ions when dissolved in water

What is Net Ionic Equation?

Equation showing only the species that actually participate in a reaction.

What are Spectator Ions?

Ions that do not participate in the chemical reaction.

What is an Arrhenius Acid?

Compound that increases concentration of H^+ in aqueous solution.

What is an Arrhenius Base?

Compound that increases concentration of OH^- in aqueous solution.

What is a Bronsted-Lowry acid?

Molecule or ion that donates a proton (H^+).

What is a Bronsted-Lowry base?

Molecule or ion that accepts a proton (H^+).

What is a Lewis acid?

Atom, ion, or molecule that accepts an electron pair to form a covalent bond.

What is a Lewis Base?

Atom, ion, or molecule that donates an electron pair to form a covalent bond.

What does it mean for something to be Amphoteric?

Species that can react as either an acid or a base.

What is Self-ionization of water?

Two water molecules produce a hydronium ion and a hydroxide ion by a transfer of a proton: H2O(l) + H2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq)

What is pH?

Negative logarithm of the hydronium ion concentration: pH = -log[H_3O^+]

What is pOH?

Negative logarithm of the hydroxide ion concentration: pOH = -log[OH^-]

What are Acid-base indicators?

Compounds whose colors are sensitive to pH.

What is an Equivalence point?

Point at which the two solutions used in a titration are present in chemically equivalent amounts.

What is the End point in titration?

The point in a titration at which an indicator changes color

What is Thermochemistry?

Study of the transfers of energy as heat that accompany chemical reactions and physical changes.

What is a Calorimeter?

Device used to measure the energy absorbed or released as heat in a chemical or physical change.

What is Specific heat (cp)?

Amount of energy required to raise the temperature of one gram of a substance by one Celsius degree.

What is Enthalpy (H)?

Energy absorbed as heat during a chemical reaction at constant pressure. Only changes in enthalpy can be measured

What is an Exothermic process?

A reaction in which energy is released; \Delta H is negative.

What is an Endothermic process?

A reaction in which energy is absorbed; \Delta H is positive.