1. Which of the following is NOT paired with the proper classification?

a) Silicon/metalloid
b) Aluminum oxide/compound
c) Skim milk/homogenous mixture
d) Iodine dissolved in alcohol/heterogenous mixture

2. Will a precipitate form when aqueous solutions of Ca(Cl3)2 and AgNO3 are mixed? If a precipitate does form, identify the precipitate and give the NET ionic equation for the reaction.

a) Ca(NO3)2 precipitates according to Ca2+(aq) + 2 NO3-(aq) ---> Ca(NO3)2(s)
b) Ca3N2 precipitates according to 3 Ca2+(aq) + 2NO3-(aq) ---> Ca3N2(s) + 3 O2(g)
c) AgCl precipitates according to AgNO3(aq) + Cl-(aq) ---> AgCl (s) + NO3-(aq)
d) AgCl precipitates according to Ag+(aq) + Cl-(aq) ---> AgCl (s)
e) No precipitate forms.

3. Which is the oxidation number of arsenic in K3AsO4?

a) +2
b) +3
c) +4
d) +5
e) +6

4. A graduated cylinder is filled to the 12.0 mL line with water. A solid with a mass of 14.52 g is placed in the graduated cylinder and is completely immersed in the water. If the density of the solid is 11.2 g/mL what will be the new volume reading on the graduated cylinder?

a) 1.29 mL
b) 10.71mL
c) 13.29 g/mL
d) 14.52 mL

5. Which one of the following compounds is NOT a salt (ionic solid)?

a) LiI
b) Al(ClO4)3
c) CNBr
d) Fe(ClO3)3
e) NH4Br

6. The reaction of 5.0 g of fluorine with excess chlorine produced 5.6 g of ClF3. What percent yield of ClF3 was obtained? Cl2 + 3 F2 ---> 2 ClF3

a) 58%
b) 69%
c) 76%
d) 86%
e) 92%

7. The percent manganese is potassium manganate, K2MnO4 is:

a) 13.2%
b) 22.6%
c) 29.0%
d) 34.8%
e) 27.8%

8. Determine the simplest formula for a hydrocarbon if the complete combustion of a sample produces 5.28 g of CO2 and 1.62 g H2O.

a) C2H3
b) CH2
c) CH3
d) CH
e) C2H5

9. What mass of ZnCl2 can be prepared from the reaction of 3.27 grams of zinc with 3.30 grams of HCl?

Zn + 2HCl ---> ZnCl2 + H2

a) 6.89 g
b) 6.82 g
c) 6.46 g
d) 6.17 g
e) 6.02 g

10. Which of the following name/formula pairs is INCORRECT?

a) calcium carbonate, CaCO3
b) iron(III) hydroxide, Fe(OH)2
c) ammonium nitrate, NH4NO3
d) aluminum chloride, AlCl3
e) zinc sulfate, ZnSO4

11. The specific gravity of commercial nitric acid solution is 1.42 and it is 70.0% HNO3 by mass. Calculate its molarity.

a) 18.0 M
b) 15.8 M
c) 12.8 M
d) 99.4 M
e) 26.2 M

12. Which of the following properties of I2 is a physical property?

a) One of its isotopes is radioactive.
b) It sublimes at 55°C.
c) It forms I3- in solutions of KI.
d) It combines with H2 to form HI.

13. Which of the following does NOT have the same number of grams of carbon as 45 g of methane, CH4?

a) 2.8 moles of CO2
b) 39.4 g C2H4
c) 1.2 x 1024 molecule CH4
d) 1.69 x 1024 atoms of graphite, C(s)
e) 1.40 mole H2C2O4

14. What volume of 0.130 M HCl solution will just react with 0.424 gram of Ba(OH) 2?

2 HCl + Ba(OH) 2 ---> BaCl2 + 2 H2O

a) 38.1 mL
b) 32.6 mL
c) 24.1 mL
d) 18.6 mL
e) 96.7 mL

15. 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."

RbOH + H3PO4 ---> Rb3PO4 + H2O

a) 8
b) 10
c) 12
d) 4
e) 6

16. Which of the following compounds would have an electronic arrangement most similar to NCl3 in terms of the Lewis picture of bonding?

a) BCl3
b) BrF3
c) Pbr3
d) SO3

17. Which of the following electron configurations is INCORRECT?

a) Na+ = 1s22s22p6
b) S2- = 1s22s22p63s23p6
c) Mn = [Ar] 3d54s2
d) Sb = [Kr] 5s25p3

18. Identify the INCORRECT statement.

a) Non-metals tend to gain electrons and have relatively large negative (much less than zero) electron affinities.
b) Metals tend to lose electrons and have low ionization energies.
c) Non-metals tend to share electrons when forming compounds with other non-metals.
d) Metals form oxides which, when reacted with water, produce acidic solutions.

19. Which of the following compounds does NOT violate the octet rule?

a) BF3
b) SF4
c) BeCl2
d) PCl3

20. In constructing the electron dot formula of HOCl,

a) two single bonds form and 14 valence electrons are present in the formula.
b) a single and double bond are present with 16 valence electrons in the formula.
c) four shared pairs of electrons are present in the formula.
d) an octet of electrons surround all three atoms.

21. The number of completely empty atomic orbitals having a quantum number of n=2 in ground state nitrogen atom is:

a) zero
b) 3
c) 1
d) 2

22. The GENERAL trend as one moves from left to right across a row of the periodic table is that:

a) atomic radii of elements decrease and first ionization energy of elements also decreases.
b) atomic radii of elements increase and electronegativity increases.
c) first ionization energy of elements increase and electronegativity increases.
d) electronegativity decreases and atomic radii of elements decrease.

23. The quantum number which best describes the orientation of an atomic orbital in space is:

a) n
b) l
c) ml
d) ms

24. Which of the following particles would NOT be deflected in an electric or magnetic field?

a) alpha
b) neutron
c) proton
d) electron

25. Consider whether the following statements about molecular electronic structure are true or false:

I. When a central atom of a molecule has lone pairs of electrons on it, the molecule violates the octet rule.
II. When a central atom of a molecule has lone pairs of electrons on it, the molecule exhibits resonance structures.
III. When a central atom of a molecule has NO lone pairs of electrons on it, the molecule's electronic geometry and molecular geometry are the same.

a) all are true
b) all are false
c) only III is true
d) only I and II are true
e) only I and III are true

26. Predict the molecular geometry of SO3.

a) trigonal planar
b) trigonal pyramidal
c) tetrahedral
d) T-shaped

27. Which of the following species is INCORRECTLY named?

a) K2O ; potassium oxide
b) H- ; hydrogen ion
c) O2- ; superoxide ion
d) MgO ; magnesium oxide
e) LiH ; lithium hydride

28. Which of the following elements has the greatest electronegativity?

a) oxygen
b) nitrogen
c) hydrogen
d) carbon

29. What is the energy in kJ of 1.00 mole of photons with a wavelength of blue light, l = 440 nm? (h = 6.6 x 10-34 J-s, c = 3.0 x 108 m/s)

a) 4.5 x 10-19 kJ
b) 4.5 x 10-16 kJ
c) 19.6 kJ
d) 271 kJ

30. Which is an INCORRECT size relationship between two species ("<" means "is smaller than"):

a) Mg < Na
b) Li+ < Li
c) Mg2+ < N3-
d) Cl- < Cl

31. A gas occupies 175 mL at a pressure of 745 torr and a temperature of 288K. What volume will it occupy at STP?

a) 245 mL
b) 163 mL
c) 175 mL
d) 316 mL
e) 480 mL

32. Suppose you have a very tiny hole in your car tire, but don't have the money to fix it. But you do have a choice of what kind of gas to fill the tire with. Which of the following choices would keep the tire inflated for the longest time?

a) He
b) Ne
c) Ar
d) Kr
e) Xe

33. A 0.220 gram sample of an unknown gas occupies 125 mL at 720 torr and at a temperature of 357K. What is the molar mass of this gas?

a) 4.5 g/mol
b) 39.4 g/mol
c) 16.3 g/mol
d) 44.0 g/mol
e) 54.4 g/mol

34. A gas mixture contains 3.0 moles of Ne and 0.50 moles of F2. The total pressure of the gas is 440 torr. What is the partial pressure of F2 in this mixture?

a) 63 torr
b) 73 torr
c) 440 torr
d) 220 torr
e) 18 torr

35. Given the following reaction: 2 HgO(s) ---> 2 Hg(l) + O2(g). Suppose 1.00 mole of HgO(s) is heated and the O2 is collected in a vessel. What volume will be occupied at STP by the O2 produced in this equation?

a) 11.2 L
b) 22.4 L
c) 16.3L
d) 5.6 L
e) 44.8 L

36. If an ideal gas is initially at 345 torr and a volume of 250 mL, what will the pressure be if the volume in decreased to 200 mL?

a) 280 torr
b) 345 torr
c) 431 torr
d) 172 torr
e) 480 torr

37. What is the mass density of Xe gas at a pressure of 2.40 atm and a temperature of 10°C?

a) 82.3 g/L
b) 384 g/L
c) 13.6 g/L
d) 0.64 g/L
e) 2.40 g/L

38. The kinetic theory of gases does NOT include:

a) The gas particles are very small and very far apart compared to their own sizes.
b) The gas particles repel each other.
c) The gas particles move randomly with a distribution of speeds.
d) The gas particles collide with one another.
e) The collisions between gas particles are elastic (no change in kinetic energy).

39. Which of the following statements is NOT true?

a) If a gas is heated from 50°C to 100°C at constant pressure, the volume will double.
b) If the volume of a gas is doubled at constant temperature, the pressure will be cut in half.
c) If two containers of the same volume contain gases at the same pressure and temperature, the number of moles of gas in the containers are the same, regardless of the types of gases (as long as they behave ideally).
d) An ideal gas has zero volume at a temperature of absolute zero.
e) Real gases attract one another at some distances.

40. Real gases behave most ideally at:

a) low temperature and high pressure.
b) low temperature and low pressure.
c) high temperature and high pressure.
d) high temperature and low pressure.

41. Which of the following intermolecular forces is INCORRECTLY assigned as the principal force in the compound given?

a) CCl4, London
b) NH3, London
c) HF, H-bonding
d) CH3OH, H-bonding
e) H-Br, dipole

42. According to the following phase diagram for a substance X, which of the following statements is FALSE?

a) The normal boiling point of X is 184°C.
b) At 25°C, X will boil if the pressure is lowered enough.
c) X is liquid at 120°C and 1 atm.
d) The melting point of X varies little with pressure.

43. Which of the following is NOT true of covalent (network) solids?

a) The units which occupy the lattice points are atoms.
b) The inter-unit forces are covalent bonds.
c) They typically exhibit low melting points.
d) They are usually very hard.
e) They are usually poor electrical conductors.

44. Chlorine has a critical temperature of 144°C and a critical pressure of 77 atm. Under which of the following conditions would Cl2 most likely be a liquid?

a) 125°C, 70 atm
b) 125°C, 30 atm
c) 150°C, 70 atm
d) 150°C, 30 atm

45. The normal boiling point of ether is 35°C. Comparing ether and water, at the same temperature, which statement below is TRUE?

a) The vapor pressure of both liquids are the same.
b) The vapor pressure of ether is greater than that of water.
c) The vapor pressure of water is greater than that of ether.
d) The vapor pressure of both liquids are equal to the temperature.

46. The term used to describe resistance to flow of a liquid is:

a) surface tension
b) capillary action
c) viscosity
d) vapor pressure
e) vaporization

47. How many atoms are considered to belong to the face-centered cubic unit cell?

a) 1
b) 2
c) 4
d) 6
e) 8

48. Which of the following descriptions of solid type is INCORRECT?

a) Cu ; metallic
b) SiO2(quartz) ; molecular
c) CaCl2 ; ionic
d) H2O ; molecular
e) C(diamond); covalent

49. Which response lists interparticle forces (between molecules of comparable size) in order of increasing strength?

a) London < ionic < H-bonds < dipole
b) dipole < London < H-bond < ionic
c) H-bond < ionic < dipole < London
d) ionic < H-bond < London < dipole
e) London < dipole < H-bond < ionic

50. The molar heat of fusion for nitrogen is 710 J/mole. How many grams of N2, at its melting point, can be melted by 1080 joules of heat?

a) 43 g
b) 1.5 g
c) 21 g
d) .065 g
e) 18 g


1)d 2)d 3)d 4)c 5)c 6)b 7)e 8)a 9)d 10)b 11)b 12)b 13)c 14)a 15)a 16)c 17)d 18)d 19)d 20)a 21)a 22)c 23)c 24)b 25)c 26)a 27)b 28)a 29)d 30)d 31)b 32)e 33)e 34)a 35)a 36)c 37)c 38)b 39)a 40)d 41)b 42)b 43)c 44)a 45)b 46)c 47)c 48)b 49)e 50)a