CP CHEMISTRY FINAL REVIEW

make an 8 ½ “ x 11” sheet of paper for the final
(FRONT side of paper ONLY)
*use the textbook for studying, looking up concepts and equations, and to check your
answers
Chapter 14: GASES
-Questions starting on page 417 #1,2,5,7,9,11,15-17,23,25,34
Chapter 15 and 16: Water and Solutions
-Questions starting on pg. 449 #2, pg. 477 #3,4, pg. 486 #16,19-21,pg. 490 #24,29,pg.
495 #33, pg. 496 #35
Also know:
 the shape of a water molecule is? _________________
 ice is less dense than water because ice has a molecular structure that is an open
framework (HONEYCOMB shape) that is held together by hydrogen bonds that
allows ice to float on the surface of water.
 What is surface tension? _____________________________________________
 Define an electrolyte:________________________________________________
 Give examples of an electrolyte:_______________________________________
 Define solute and solvent:____________________________________________
 What is a concentrated solution versus a dilute
solution?__________________________________________________________
 Know the equations for boiling point elevation and freezing point depression
 Brackets [ ] are used to denote concentration (MOLARITY)
 Review a solubility curve to determine the solubility of certain compounds at
various temperatures.
Chapter 17: Thermochemistry
Questions starting on pg. 510 #10 (check your answer, it should = 2.36 x 10-1 J/gC), pg.
513 #13
Also know:
 Heat flows from warmer to cooler objects
 endothermic: energy is absorbed into a system, feels cold to touch
 exothermic: energy is released from a system, feels warm/hot to touch
 units for specific heat are: J/gC OR cal/gC
 H means ENTHALPY, the heat of reaction for a chemical reaction
 Calorimetry depends on the LAW of CONSERVATION of ENERGY
 Calculate the amount of energy required to produce 8.00 moles of Cl2O7 on the
basis of the following balanced equation:
2 Cl2 (g) + 7 O2 (g) + 130 kcal  2 Cl2O7 (g)
 turn over
Chapter 18: Equilibrium (only section 18.2)
Questions starting on pg. 555 #6, pg. 581 #49, 51 a &b, #52 (REMEMBER: if the value
of a reversible reaction’s Keq is greater than 1, production of products is favored: if
the Keq is less than 1, the formation of reactants is favored)
 at equilibrium, the rate of production of reactants is the same as the rate of the
production of products (RATE of each reaction is EQUAL)
 What is the reverse reaction of sulfur trioxide decomposing into sulfur dioxide
and oxygen?_______________________________________________________
Chapter 19: Acids and Bases, pH
Questions start on pg. 593 #3, 4, 5, 7 a & b, pg. 596 #9, 10, 11, 13, 15, pg. 611 #24, pg.
616 #35
Know:
 Hydronium ion = H3O+
 pH + pOH = 14
 pH = -log [H+], pOH = -log [OH-]
 Kw = [H+] x [OH-] = 1.0 x 10-14
 Strong acids & bases COMPLETELY dissociate into ions in water, weak acids &
bases PARTIALLY dissociate into ions in water
Chapter 25: Nuclear Chemistry
Questions start on pg. 802 #1-6, pg. 808 #10, 12 b-d, 13
Know:
 What happens in a nuclear chain reaction?________________________________
 Nuclear fusion takes place in the sun
 A GEIGER COUNTER is an instrument that uses a gas-filled metal tube to
routinely check a person’s exposure to radiation
 Define: radioisotope, nuclear fission, nuclear fusion