General Chemistry II Final Exam

All group I cations

NH₄⁺

Nitrates (NO₃⁻)

Acetates (CH₃CO₂⁻)

Perchlorates and Chlorates (ClO₄⁻, ClO₃⁻)

Hydroxides (OH⁻)

Phosphates (PO₄³⁻)

Carbonates (CO₃²⁻)

Sulfides (S²⁻)

OH⁻

O₂²⁻

CN⁻

CO₃²⁻

HCO₃⁻

CH₃CO₂⁻

NO₃⁻

NO₂⁻

NH₄⁺

ClO₄⁻

ClO₃⁻

ClO₂⁻

ClO⁻

SO₄²⁻

SO₃²⁻

HSO₄⁻

HSO₃⁻

MnO₄⁻

Cr₂O₇²⁻

CrO₄²⁻

PO₄³⁻

PO₃³⁻

HPO₄²⁻

HPO₃²⁻

H₂PO₃⁻

Hydrochloric Acid, Hydrobromic Acid, Hydroiodic Acid, Nitric Acid, Perchloric Acid, and Sulfuric Acid

HCl (aq)

HBr (aq)

HI (aq)

HNO₃ (aq)

HClO₄ (aq)

H₂SO₄ (aq)

a state of dynamic equilibrium in which the rate of the forward reaction and the rate of the reverse reaction are equal

describes equilibrium condition

the equilibrium favors the products

the equilibrium favors the reactants

when stress is applied to a system at equilibrium, the system will respond by relieving the stress

heat is a product

heat is a reactant

an equilibrium will shift if a common ion is added to the solution

too many products, favor reverse reaction

too many reactants, favor forward reaction

reaction is at equilibrium

proton donor, proton must be bound to a highly electronegative element

proton acceptor

substance that can react as an acid or a base

100% dissociation of acidic protons

less than 100% acid dissociation

100% base hydrolysis in water

less than 100% base molecules/ions accept protons

limits the acid strength of solutes in a particular solvent

weak acid/weak base conjugate pair that resists pH change

the amount of acid/base that a buffer system can resist before pH starts to change rapidly

point where the reaction ended

point where the indicator changes color

forces holding a molecule together

forces holding molecules or aggregates of ions/atoms together

asymmetrical molecules that have an electronegativity difference greater than or equal to 0.5

these molecules form dilpoles

Ionic Forces > Hydrogen Bonding > Dipoles > London Forces

weak temporarily induced dipoles

the stronger the intermolecular forces, the stronger the surface tension

attraction within the substance/mixture

attraction between different substances

resistance to flow

the stronger the intermolecular forces, the higher the viscosity

Q = mC∆T

Q = m∆H

the majority compound

there can only be one in the any solution

the minority compound

there can be many

compounds which generate ions when dissolved in water

100% of the formula units dissolve into ions

less than 100% of the formula units dissociate into ions

no ions are formed when dissolved in water

the amount of disorder in a system

more than 0.02 moles of compound can dissolve in 1.0 L of water

less than 0.02 moles of compound can dissolve in 1.0 L of water

solution contains maximum amount of solute possible

a solution that is carefully prepared with a concentration that exceeds its solubility

liquid-liquid solubility

liquids mix to form a solution

liquids that do not mix

consists of solute particles distributed throughout a solution

the amount of gas that can be dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid

pressure of evaporated molecules above a liquid

moles of solute per kilogram of solvent

the ratio of a solute’s molar amount to the total number of moles of all solution components

properties that depend on the concentration of the solute and not the identity of the solute

a solution has a lower vapor pressure than that of a pure solvent

the overall pressure of a gas is the sum of the partial pressures of its components

the pressure that must be applied to prevent the net movement of water from the solvent to the solution of higher concentration

external concentration lower than internal concentration

water flows into cell

external concentration higher than internal concentration

water flows out of cell

external and internal concentrations are equal

determines the spontaneity of a chemical reaction

the study of energy, work, and heat

reaction proceeds in direction written

reaction does not proceed in direction written

determines that rate at which the reaction proceeds

energy of collision needed to initiate a reaction