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,

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 concept behind 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