Chemistry Final Part II

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  1. Which of the following is a heterogeneous mixture?
    whole wheat bread
  2. All of the following are heterogeneous mixtures except
    tap water
  3. Carbon dioxide dissolved in water is an example of which solute-solvent combination?
  4. Which is not an example of a colloid?
    sugar water
  5. Which mixture is made up of the smallest particles?
    salt water
  6. A metal solution is an
  7. The Tyndall effect is used to distringuish between
    solutions and colloids
  8. Which of the following is an electrolyte?
    sodium chloride
  9. Which of the following is a molecular substance whos aqueous solutions carries an electric current?
    hydrogen chloride
  10. Which of the following does not increase the rate of dissolving a solid in water?
    using larger pieces of solid
  11. Which of the following will dissolve most slowly?
    large salt crystals in unstirred water
  12. Which of the following is at equilibrium when undissolved solute is visible?
    a saturated solution
  13. In a solution at equiilibrium
    the rate of dissolution and the rate of crystallization are equal
  14. Which of the following is likely to produce crystals if disturbed?
    a supersaturated solution
  15. In the expression "like dissolves like" the word like refers to similarity in molecular
  16. Which of the following is an example of a polar solvent
  17. Pressure has the greatest effect on the solubility of
    gases and liquids
  18. The formation of solid-liquid solutions
    always absorbs energy as heat
  19. Effervescevce is the
    escape of gas from a gas-liquid solution
  20. Precipitation is an example of what type of reaction?
  21. The formula for the hydronium ion is
  22. Dissolving HCL in water produces
    H3O+ and Cl-
  23. The law of combining volumes applies only to gas volumes
    measured at constant temperature and pressure
  24. For reactants or products that are gases, the coefficients in the chemical equation indicate
  25. The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to
  26. Equal volumes of diatomic gases under the same conditionsof temperature and pressure contain the same number of
  27. At STP, the standard molar volume can be used to calculate the
    number of moles of gas
  28. Knowing the mass and volume of a gas at STP allows one to calculate the
    molar mass of the gas
  29. The ideal gas combines Boyle's law, Charle's law, Gay-Lssac's Law and
    Avogadro's law
  30. The standard molar volume of a gas is all of the following except
    dependent upon the size of the molecules
  31. What does the constant bombardment of gas molecules against the inside walls of a container produce?
  32. What happens to the volume of a gas during compression
    volume decreases
  33. What instrument meaures atmospheric pressure
  34. Why does a can collapse when a vacuum pump removes air from the can
    Unbalanced outside force from the atmospheric pressure crushes the can
  35. To convert for the partial pressure of water vapor in a gas collection bottle, the vapor pressure of H2O at the collecting temperature is generally
    subtracted from the atmospheric pressure
  36. Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures?
  37. If the temperature of a fixed quantity of a gas decreases and the pressure remains unchanged,
    its volume decreases
  38. What are the values for STP
    1 atm and 0 degress Celsius
  39. Carbon shows a very strong tendency to form
    covalent bonds
  40. How many covalent bonds can a carbon atom usually form?
  41. Carbon atoms readily join with atoms of
    both elements and carbon
  42. Organic compounds are defined as all covalently bonded compounds containin carbon except
    oxides and carbonates
  43. The diversity of organic compounds is so great because
    compounds have many isomers
  44. Which formula shows the numbers and types of atoms in a molecule but not the bonds?
    molecular formula
  45. Isomers are compounds that have the
    same molecular forumla but different structures
  46. Which formula is most useful in distinguishing isomers?
    structural formula
  47. The carbon-hydrogen bonds of alkanes are
  48. Each carbon atom in a molecule forms four single covalrnt bonds with other atoms in a
    saturated hydrocarbon
  49. Hydrocarbons are grouped into series according to the
    bonds between carbon atoms
  50. Which of the following is an alkane
  51. Hydrocarbons in which carbon atoms form only single bonds and are arranged ub a ring are called
  52. What are two allotropic forms of carbon?
    diamond and graphite
  53. Which statement about the hardness of diamond and graphite is correct?
    Diamond is very hard, and graphite is very soft
  54. Which of the following is an atom or a group of atoms responsible for the specific properties of an organic compound?
    functional group
  55. What is the functional group in carboxylic acids
  56. What is the name of the funtional group -OH
    hydroxyl group
  57. The systematic names of ketones end in
  58. What are alkanes called when atoms of flourine, chlorine, bromine, or iodine are substituted for hydrogen atoms?
    alkyl halides
  59. How is the functional group in alkyl halides often written
    - X
  60. What is the general formula for ethers?
  61. A carbonyl group consists of
    one carbon atom and one oxygen atom
  62. Which group of organic compounds can be considered derivatives of ammonia, NH3
  63. What is the general formula of esters?
  64. Carboxylic acids are
    weak acids

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Chemistry Final Part II
2011-12-18 19:41:13

chapter 9-22
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