• 1) A new compound was recently discovered and found to have an atomic weight of 342.38 amu. This element has two isotopes, the lighter of which has a mass of 340.91 amu and an abundance of 68.322%. What is the mass of the heavier isotope?
      • A) 350.21
      • B) 345.55
      • C) 342.38
      • D) 348.67
      • E) 343.29

  • 2) Identify the characteristics of a liquid.
    • A) definite volume and definite shape
    • B) definite volume and no definite shape
    • C) no definite volume and definite shape
    • D) no definite shape and no definite volume

  • 3) What species is represented by the following information?
    • p+ = 12 n° = 14 e- = 10
    • A) Si4+
    • B) Mg
    • C) Ne
    • D) Si
    • E) Mg2+

  • 4) How many moles of Kr are contained in 398 mg of Kr?
    • A) 4.75 × 10-3 moles Kr
    • B) 33.4 moles Kr
    • C) 2.11 × 10-4 moles Kr
    • D) 2.99 × 10-3 moles Kr
    • E) 1.19 × 10-4 moles Kr

  • 5) How many phosphorus atoms are contained in 158 kg of phosphorus?
    • A) 3.07 × 10^27 phosphorus atoms
    • B) 2.95 × 10^27 phosphorus atoms
    • C) 3.25 × 10^28 phosphorus atoms
    • D) 1.18 × 10^24 phosphorus atoms
    • E) 8.47 × 10^24 phosphorus atoms

  • 6) A student performs an experiment to determine the density of a sugar solution. She obtains the following results: 1.11 g/mL, 1.81 g/mL, 1.95 g/mL, 1.75 g/mL. If the actual value for the density of the sugar solution is 1.75 g/mL, which statement below best describes her results?
    • A) Her results are precise, but not accurate.
    • B) Her results are accurate, but not precise.
    • C) Her results are both precise and accurate
    • D) Her results are neither precise nor accurate.
    • E) It isn’t possible to determine with the information given.

  • 7) What answer should be reported, with the correct number of significant figures, for the following calculation? (433.621 - 333.9) × 11.900
    • A) 1.19 × 10^3
    • B) 1.187 × 10^3
    • C) 1.1868 × 10^3
    • D) 1.18680 × 10^3
    • E) 1.186799 × 10^3

  • 8) If an object has a density of 8.65 g/cm3, what is its density in units of kg/m3?
    • A) 8.65 × 10^-3 kg/m3
    • B) 8.65 × 10^-7 kg/m3
    • C) 8.65 × 10^3 kg/m3
    • D) 8.65 × 10^1 kg/m3
    • E) 8.65 × 10^-1 kg/m3

  • 9) Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of
    • 5.49 × 10^14 Hz.
    • A) 2.75 × 10^-19 J
    • B) 3.64 × 10^-19 J
    • C) 5.46 × 10^-19 J
    • D) 1.83 × 10^-19 J
    • E) 4.68 × 10^-19 J

  • 10) Determine the longest wavelength of light required to remove an electron from a sample of potassium metal, if the binding energy for an electron in K is 1.76 × 10^3 kJ/mol.
    • A) 147 nm
    • B) 68.0 nm
    • C) 113 nm
    • D) 885 nm
    • E) 387 nm

  • 11) Determine the mass of a ball with a wavelength of 3.45 × 10^-34 m and a velocity of 6.55 m/s.
    • A) 0.293 g
    • B) 12.6 g
    • C) 293 g
    • D) 346 g
    • E) 3.41 g

  • 12) What are the possible orbitals for n = 3?
    • A) s, p, d
    • B) s, p, d, f
    • C) s
    • D) s, p

  • 13) Determine the energy change associated with the transition from n = 2 to n = 5 in the hydrogen atom. (RH=-2.18 x 10^-18 J)
    • A) -2.18 × 10^-19 J
    • B) +6.54 × 10^-19 J
    • C) +4.58 × 10^-19 J
    • D) -1.53 × 10^-19 J
    • E) +3.76 × 10^-19 J

  • 14) Predict the charge that an ion formed from sulfur would have.
    • A) 1-
    • B) 6+
    • C) 3-
    • D) 4+
    • E) 2-

  • 15) Give the ground state electron configuration for I.
    • A) [Kr]5s2 4d10 5p6
    • B) [Kr]5s2 4d10 5p5
    • C) [Kr]4d10 5p6
    • D) [Kr]5s2 5p6
    • E) [Kr]5s2 5d10 5p6

  • 16) Place the following elements in order of increasing atomic radius.
    • P Ba Cl
    • A) Ba < P < Cl
    • B) P < Cl < Ba
    • C) Cl < P < Ba
    • D) Cl < Ba < P
    • E) Ba < Cl < P

  • 17) Place the following in order of decreasing IE1.
    • Cs Mg Ar
    • A) Cs > Mg > Ar
    • B) Mg > Ar > Cs
    • C) Ar > Mg > Cs
    • D) Cs > Ar > Mg
    • E) Mg > Cs > Ar

  • 18) Why does an electron found in a 2s orbital have a lower energy than an electron found in a 2p orbital in multielectron systems?
    • A) Electrons in the 2s orbital are shielded by electrons in the 2p.
    • B) There are more nodes found in the 2s orbital.
    • C) Electrons in the 2s orbital can penetrate the 1s orbital and be closer to the nucleus .
    • D) The larger number of electrons found in the 2p orbital leads to greater repulsion.
    • E) The shape of the orbital ultimately determines the energy of the electrons

  • 19) Give the structure for sodium perchlorate.
    • A) NaClO
    • B) NaClO2
    • C) NaClO3
    • D) NaClO4

  • 20) Calculate the molar mass for Mg(ClO4)2.
    • A) 223.21 g/mol
    • B) 123.76 g/mol
    • C) 119.52 g/mol
    • D) 247.52 g/mol
    • E) 75.76 g/mol

  • 21) Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen.
    • A) C18H27NO3
    • B) C18H27NO2
    • C) C17H27NO3
    • D) C17H26NO3

  • 22) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?
    • A) C5H2O
    • B) CHO
    • C) C3H6O
    • D) C3H7O
    • E) C6HO3

  • 23) Identify the number of bonding pairs and lone pairs of electrons in water.
    • A) 1 bonding pair and 1 lone pair
    • B) 1 bonding pair and 2 lone pairs
    • C) 2 bonding pairs and 2 lone pairs
    • D) 2 bonding pairs and 1 lone pair
    • E) 3 bonding pairs and 2 lone pairs

  • 24) Choose the best Lewis structure for XeI2
    • A
    • B
    • C
    • D
    • E

  • 25) Which of the following resonance structures for OCN⁻ will contribute most to the correct structure of OCN⁻?
    • A) O(2 lone pairs) double bonded to C double bonded to N (2 lone pairs)
    • B) O(1 lone pair) triple bonded to C single bonded to N(3 lone pairs)
    • C) O(1 lone pair) double bonded to C(2 lone pairs) double bonded to N(1 lone pair)
    • D) O(3 lone pairs) single bonded to C triple bonded to N(with 1 lone pair)
    • E) They all contribute equally to the correct structure of OCN⁻.

  • 26) Draw the best Lewis structure for the free radical, NO2. What is the formal charge on the N?
    • A) 0
    • B) +1
    • C) -1
    • D) +2
    • E) -2

  • 27) Determine the electron geometry (eg) and molecular geometry (mg) of CO2.
    • A) eg = tetrahedral, mg = tetrahedral
    • B) eg = linear, mg = trigonal planar
    • C) eg = trigonal planar, mg = bent
    • D) eg = linear, mg = linear
    • E) eg = trigonal planar, mg = trigonal planar

  • 28) Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms.
    • 1 = trigonal planar, 2 = tetrahedral, 3 = trigonal pyramidal
    • l = tetrahedral, 2 = tetrahedral, 3 =tetrahedral
    • 1 = trigonal planar, 2 = tetrahedral, 3 = tetrahedral
    • 1 = tetrahedral, 2 = tetrahedral, 3 = trigonal planar
    • 1 = trigonal planar, 2 = trigonal pyramidal, 3 = trigonal pyramidal

  • 29) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule.
    • CS2 CF4 SCl2
    • A) CS2 = SCl2 > CF4
    • B) SCl2 > CF4 > CS2
    • C) CF4 > CS2 > SCl2
    • D) CS2 > CF4 > SCl2
    • E) CF4 > CS2 > SCl2

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

  • 31) Use the molecular orbital diagram shown to determine which of the following is most stable.
    • A) C2^2⁺
    • B) N2^2⁺
    • C) B2
    • D) C2^2⁻
    • E) B2^2⁺

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

  • 33) Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2.
  • 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
    • A) 0.640 moles
    • B) 64.0 moles
    • C) 2.56 moles
    • D) 16.0 moles

  • 34) Which should give the least vigorous reaction when dropped in water?
    • A) Li
    • B) Na
    • C) K
    • D) Rb
    • E) Cs

  • 35) Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 15.0 g of Fe2O3.
    • A) 0.0877 g
    • B) 1.26 g
    • C) 3.78 g
    • D) 11.4 g

  • 36) Determine the theoretical yield of H2S (in moles) if 16 mol Al2S3 and 16 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol.
  • Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)
    • A) 48 mol H2S
    • B) 16 mol H2S
    • C) 32 mol H2S
    • D) 24 mol H2S
    • E) 8.0 mol H2S

  • 37) Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.
    • A) 0.0297 M
    • B) 0.0337 M
    • C) 0.0936 M
    • D) 0.0107 M
    • E) 0.0651 M

  • 38) What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution?
  • 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)
    • A) 0.838 g
    • B) 1.72 g
    • C) 0.859 g
    • D) 2.56 g
    • E) 1.70 g

  • 39) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed
    • A
    • B
    • C
    • D
    • E

  • 40) Determine the oxidation state of nitrogen in NO.
    • A) +5
    • B) +3
    • C) 0
    • D) +2
    • E) +4

  • 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) 6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol) is dissolved into water. The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point. What volume of base was used?
    • A) 8.64 mL
    • B) 11.8 mL
    • C) 23.5 mL
    • D) 47.0 mL
    • E) 93.9 mL