• 1) Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O
    • A) eg = tetrahedral, mg = bent, sp3
    • B) eg = trigonal pyramidal, mg = trigonal pyramidal, sp3
    • C) eg = tetrahedral, mg = trigonal pyramidal, sp3
    • D) eg = bent, mg = bent, sp3
    • E) eg = trigonal planar, gm = trigonal planar, sp3

  • 2) place the following in order of decreasing dipole moment
  • I. cis-CHCl=CHCl II. trans-CHCl=CHCl III. cis-CHF=CHF
    • A) III > I > II
    • B) II > I > III
    • C) I > III > II
    • D) II > III > I
    • E) I = III > II

  • 3) Give the hybridization for the O in OF2
    • A) sp
    • B) sp3
    • C) sp2
    • D) sp3d
    • E) sp3d2

  • 4) Give the hybridization for the S in SO3
    • A) sp
    • B) sp3
    • C) sp2
    • D) sp3d
    • E) sp3d2

  • 5) How many of the following molecules have sp2 hybridization on the central atom?
  • HCN SO2 OCl2 XeCl2
    • A) 4
    • B) 3
    • C) 2
    • D) 1
    • E) 0

  • 6) Give the hybridization for the C in C2F2
    • A) sp3d2
    • B) sp3d
    • C) sp3
    • D) sp2
    • E) sp

  • 7) How many p-orbitals participate in the Molecular orbitals in Benzene and how many MOs does this give?
    • A) 0
    • B) 2
    • C) 4
    • D) 6
    • E) 12

  • 8) A chemical change
    • A) occurs when methane gas is burned.
    • B) occurs when paper is shredded.
    • C) occurs when water is vaporized.
    • D) occurs when salt is dissolved in water.
    • E) occurs when powdered lemonade is stirred into water.

  • 9) What is the stoichiometric coefficient for oxygen?
    • B2H6(g) + O2(g) -> B2O3(s) + H2O(g)
  • What is the stoichiometric coefficient for oxygen?
    • A) 1
    • B) 2
    • C) 3
    • D) 4
    • E) 6

  • 10) Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of “one.”
    • Cr2(SO4)3 + RbOH -> Cr(OH)3 + Rb2SO4
    • A) 10
    • B) 12
    • C) 13
    • D) 14
    • E) 15

  • 11) What is the percent yield of C2H2 if 62.80 g of water yields 15.38 g of C2H2 using the following equation.
    • CaC2(s) + 2 H2O(l) → Ca(OH)2(aq) + C2H2(g)
    • A) 13.84%
    • B) 33.90%
    • C) 91.47%
    • D) 48.10%
    • E) 68.52%

  • 12) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al to produce aluminum oxide and Fe. (Al: 26.98, Fe: 55.85)
    • A) 61.03 %
    • B) 28.65 %
    • C) 57.30 %
    • D) 20.02 %
    • E) 81.93 %

  • 13) In the reaction of Zn with hydrochloric acid (HCl) to give zinc(II) chloride and hydrogen, 25.0 grams of Zn have reacted with 17.5 g of HCl. How many grams of H2 will be produced? (Zn: 65.38, Cl: 35.45)
  • A) 0.385 g H2
  • B) 0.484 g H2
  • C) 0.765 g H2
  • D) 25.0 g H2

  • 14) According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H20 = 18.02 g/mol.
    • Al2S3 + 6H2O -> 2Al(OH)3 + 3H2S
    • A) 0 g
    • B) 14.00 g
    • C) 8.33 g
    • D) 19.78 g
    • E) 17.22 g

  • 15) Two samples of calcium and fluoride are decomposed into their constituent elements. The first sample showed that the yield of products was 100% (really!). If the second sample produced 294 mg of fluorine, how many g of calcium were formed? (Ca: 40.08, F: 19.00)
    • A) 0.280 g
    • B) 3.10 * 10^2 g
    • C) 3.13 g
    • D) 0.310 g
    • E) 2.80 * 10^2 g

  • 16) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. (Li: 6.941, Br: 79.90)
    • A) 1.50 M
    • B) 1.18 M
    • C) 0.130 M
    • D) 0.768 M
    • E) 2.30 M

  • 17) What is the concentration of HCl in the final solution when 65 mL of a 9.0 M HCl solution is diluted with pure water to a total volume of .15 L?
    • A) 2.1 × 10-2 M
    • B) 3.9 M
    • C) 21 M
    • D) 3.9 × 10^3 M

  • 18) How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution
    • A) 8.29 * 10^22 molecules C12H22O11
    • B) 1.21 * 10^21 molecules C12H22O11
    • C) 6.15 * 10^22 molecules C12H22O11
    • D) 1.63 * 10^23 molecules C12H22O11
    • E) 5.90 * 10^24 molecules C12H22O11

  • 19) What volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M PB(NO3)2 solution?
    • A) 97.4 mL
    • B) 116 mL
    • C) 43.0 mL
    • D) 86.1 mL
    • E) 58.1 mL

  • 20) Which of the following will have the highest electrical conductivity?
    • A) 0.045 M Al2(SO4)3
    • B) 0.050 M (NH4)2CO3
    • C) 0.10 M NaBr
    • D) 0.10 M Kl
    • E) 0.10 M KF

  • 21) K2SO4 is soluble
    • True
    • False

  • 22) Ba2SO4 is soluble
    • True
    • False

  • 23) NH4CO3 is slightly soluble
    • True
    • False

  • 24) Ba(OH)2 is slightly soluble
    • True
    • False

  • 25) Ni(II)I2 is soluble
    • True
    • False

  • 26) Which pair of compounds is soluble in water?
    • A) Hg2Cl2 and HgBr2
    • B) NiS and Li2S
    • C) NH4I and Ni(NO3)2
    • D) LiNO3 and CuCO3

  • 27) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed.
    • A) Li+(aq)+SO4 2-(aq)+Cu+(aq)+NO3 - (aq) → CuS(s)+Li+(aq) + NO3 - (aq)
    • B) Li+(aq) + S- (aq) + Cu+(aq) + NO3 - (aq) → CuS(s) + LiNO3(aq)
    • C) 2Li+(aq)+S2-(aq)+Cu2+(aq) + 2NO3 - (aq)→Cu2+(aq)+S2-(aq) +2LiNO3(s)
    • D) 2 Li+(aq)+S2-(aq)+Cu2+(aq)+2NO3 - (aq)→ CuS(s) + 2Li+ (aq) + 2NO3 - (aq)
    • E) No reaction occurs.

  • 28) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed
    • A) 2H+(aq)+CO3 2-(aq) → H2CO3(s)
    • B) 2Na+(aq)+CO3 2-(aq)+2H+(aq) + 2Cl- (aq) → H2CO3(s)+2NaCl(aq)
    • C) 2H+(aq)+CO3 2-(aq) → H2O(l)+CO2(g)
    • D) 2Na+(aq)+CO3 2-(aq)+2H+(aq)+2Cl- (aq)→H2CO3(s)+2Na+(aq)+2Cl- (aq)
    • E) No reaction occurs.

  • 29) What is the name for an aqueous solution of HIO
    • A) hydroiodic acid
    • B) hypoiodous acid
    • C) iodous acid
    • D) iodic acid
    • E) periodic acid

  • 30) Which of the following is an acid-base reaction?
    • A) C(s) + O2(g) → CO2(g)
    • B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)
    • C) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
    • D) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)
    • E) None of the above are acid base reactions.

  • 31) The titration of 25.0 mL of an unknown concentration of H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution?
    • A) 0.20 M
    • B) 0.40 M
    • C) 0.10 M
    • D) 0.36 M
    • E) 0.25 M

  • 32) The titration of 80.0 mL of an unknown concentration of H3PO4 solution requires 126 mL of .218 M KOH solution. What is the concentration of H3PO4 solution (in M)
    • A) 1.03 M
    • B) 0.343 M
    • C) 0.114 M
    • D) 0.138 M
    • E) 0.0461 M

  • 33) Determine the oxidation state of nitrogen in NO2
    • A) +5
    • B) +3
    • C) 0
    • D) +2
    • E) +4

  • 34) What element is undergoing reduction (if any) in the following reaction?
    • Zn(s) + 2AgNO3(aq) -> Zn(NO3)2(aq) + 2 Ag(s)
    • A) Zn
    • B) N
    • C) O
    • D) Ag
    • E) This is not an oxidation-reduction reaction

  • 35) Which choice gives the correct oxidation numbers for all three elements in Rb2SO3 in the order that the elements are shown in the formula?
    • A) -2, +6, -2
    • B) -1, +4, -3
    • C) +2, +4, -2
    • D) +1, +4, -2
    • E) +1, +6, -6

  • 36) Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings?
    • A) q = +, w = -
    • B) q = -, w = +
    • C) q = +, w = +
    • D) q = -, w = -
    • E) None of these represent the system referenced

  • 37) Which of the following signs on q and w represent a system that the surroundings are doing work on, as well as gaining heat from the surroundings?
    • A) q = +, w = -
    • B) q = -, w = +
    • C) q = +, w = +
    • D) q = -, w = -
    • E) None of these represent the system referenced

  • 38) How many of the following molecules are polar?
  • PCl5 COS XeO3 SeBr2
    • A) 2
    • B) 0
    • C) 1
    • D) 3
    • E) 4

  • 39) When an aqueous solution of manganese (II) nitrate is combined with an aqueous solution of ammonium sulfide, what should precipitate out?
    • A) MnS
    • B) Mn(SO3)2
    • C) Mn(SO4)2
    • D) Mn2SO3
    • E) Mn2SO4

  • 40) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed.
    • A) K+(aq) + NO3 - (aq) → KNO3(s)
    • B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3 - (aq) → FeS(s) + 2 K+(aq) + 2 NO3 - (aq)
    • C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3 - (aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s)
    • D) Fe2+(aq) + S2-(aq) → FeS(s)
    • E) No reaction occurs.

  • 41) Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s)
    • A) O
    • B) H
    • C) C
    • D) Fe
    • E) Li

  • 42) Draw the appropriate molecular orbital diagram and determine which of the following are paramagnetic.
    • A) B2^2+
    • B) B2^2-
    • C) N2^2+
    • D) C2^2-
    • E) B2

  • 43) How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol
    • 4KNO3(s) -> 2K2O(s) + 2N2(g) + 5O2(g)
    • A) 0.290 mol N2
    • B) 0.580 mol N2
    • C) 18.5 mol N2
    • D) 0.724 mol N2
    • E) 1.73 mol N2

  • 44) According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? (S: 32.07, H: 1.0079, O: 15.999)
    • 2H2S(g) + SO2(g) -> 3 S(s) + 2H2O
    • A) 99.8 g S
    • B) 66.6 g S
    • C) 56.1 g S
    • D) 44.4 g S
    • E) 14.0 g S

  • 45) Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. (molar mass of BCl3 = 117.16 g/mol, B: 10.81, Cl:35.45, O:15.999, H:1.0079)
    • BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
    • A) 75.9 g HCl
    • B) 132 g HCl
    • C) 187 g HCl
    • D) 56.0 g HCl
    • E) 25.3 g HCl

  • 46) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:
    • CaO(s) + H2O(l) → Ca(OH)2(s)
  • A 5.00-g sample of CaO is reacted with 4.83 g of H2O. How many grams of water remain after the reaction is complete? (Ca:40.08, O:15.999, H:1.0079)
    • A) 0.00
    • B) 0.00991
    • C) 3.22
    • D) 1.04
    • E) 0.179