Chemistry Name :

Final Exam Review Date :

A. You should be familiar with the following terms and the concepts associated with them :

Ch. 13-14

- kinetic theory of matter

- heat

- heat of fusion

- heat of vaporization

- heat of condensation

- heat of solidification

- temperature

- boiling point

- normal boiling point

- freezing point

- melting point(ionic vs. molecular)

- dynamic equilibrium

- gas pressure

- vapor pressure

- vacuum

- absolute zero

- sublimation

- states of matter

- condensed states of matter

-plasma

Ch. 15-16

- solution

- suspension

- colloid

- concentrated

- saturated

- unsaturated

- supersaturated

-dilute

- concentrated

- miscible

- immiscible

- surfactants

- solubility

- molarity

- molality

- electrolytes (strong vs. weak)

-nonelectrolytes

Ch. 18

-collision theory

- reaction rate

- elementary reaction

- complex reaction

- reaction mechanism

- intermediate

- activated complex

- catalyst

- enzyme

- inhibitor

- activation energy

- free energy

- enthalpy

- entropy

- endothermic

- exothermic

- endergonic

- exergonic

- spontaneous reaction

-nonspontaneous reactions

Ch. 19

- pH scale

- acids and bases(weak vs strong)

- neutralization

- salt hydrolysis

- amphoteric substances

- hydronium ion

-hydroxyl ion

-normality

- equivalents

- titration

-buffer

Ch. 20-21

-oxidation/reduction

-oxidizing/reducing agent

-corrosion

-electrochemistry

-electrochemical cell

-voltaic cell

-electrolytic cell

-electrode

-anode/cathode

-dry cell

-battery

-fuel cell

-cell potential/standard cell potential

-electrolysis

-electroplating

-anodizing

Chapter 25

-neutron

- proton

-electron

-quark

-nucleon

-nuclide

-alpha particles

-beta particles

-gamma rays

-positron

-neutron emission or capture

-decay series

-half-life

-mass defect

-transuranium elements

-radiotracers

-binding energy

-chain reaction

-control rods

-neutron moderators

--neutron absorbers

-nuclear fission

-nuclear fusion

-critical mass

-subcritical mass

-supercritical mass

-rem

Objectives :

  1. Be familiar with the following gas laws : Charles', Boyles, Gay-Lussac's, Ideal and combined.
  2. Water and its properties.
  3. The effect of air pressure on the boiling point of a liquid.
  4. Use Le Châtelier's principle to predict equilibrium shifts.
  5. Factors affecting solubility
  6. Factors affecting reaction rates.
  7. Determine the orders of reactants, solve for k and determine rates for new concentrations of reactants.
  8. Identify substances reduced/oxidized and oxidizing/reducing agents in redox reactions.
  9. Calculate cell potential.
  10. Use shorthand notation to represent voltaic cells.
  11. State where oxidation and reduction occur in voltaic cells.
  12. Balance redox reactions.
  13. Predict results of electrolysis from molten salts and from mixtures.
  14. Write and balance nuclear equations.
  15. Calculate mass defect and energy from nuclear changes.
  16. Use half-life data to calculate ages of materials.

ChemistryName :

Help Sheet : Final Exam - Ch. 10-12, 17-23Date :

Chapters 13-14 :Ch. 20-21 :

Heat (during phase change)= mass of substance x heat of ZEºcell = Eºred - Eºox

(Z = solidification, fusion, condensation or vaporization)

q = m x c x ΔT

Dalton's law of Partial Pressures : P total = P1 + P2 + P3...

Boyle's law : P1 x V1 = P2 x V2

Charles' law : V1/T1 = V2/T2

Gay-Lussac's Law : P1/T1 = P2/T2

Ideal gas law : PV = nRT (R=.0821(L x atm)/(K x mol)

Combined gas law :

P1 x V1 P2 x V2

T1 T2

Chapter 15 and 16 :

Henry's Law : S1/P1 = S2/P2

Molarity (M)= moles/Liter of solution

moles = V (in L) x M

Grams solute = V x M x molar mass

Dilution using molarity : M1 x V1 = M2 x V2

Molality (m)= moles/Kg of solvent

moles = Kg of solvent x molality

grams solute =kg of solvent x molality x molar mass

Tb = Kb x molality

Tf = Kf x molality

Chapter 18 :

S = S(products) - S(reactants)

H = H(products) - H(reactants)

G = H - TS (T= 298 K)

Chapters 19:

[H3O+] x [OH-] = 1.0 x 10-14 (mol/L)2

pH + pOH = 14.00

pH = -log[H3O+]

[H3O+] = 10 -pH

Calculation of molarity from balanced equation and known volume and concentration:

step 1. Write the balanced equation :

step 2. Calculate moles of given used.

step 3. Calculate moles of unknown neutralized from ratio of balanced equation.

step 4. Calculate molarity of unknown.

gem = molar mass/moles of H+ or OH- produced per mole

N= Molarity x number of moles of H+ or OH- produced per mole

no. of equivalents = mass of sample x (1 eq./gem)

N= no. of eq./L

no. of equiv = N x V (in L)

Dilution : N1 x V1 = N2 x V2

Titration : NA x VA = NB x VB

Ksp problems :

step 1. Write and balance dissociation equation.

step 2. Write expression for Ksp.

step 3. Solve for unknown.