Name: ______Date: ______

1. In an ionic compound of formula MmXn, the metal (M) occupies a face-centered cubic lattice and the anions occupy four positions inside the unit cell. Determine the formula of the compound.

A) MX B) MX2 C) M2X D) MX3 E) M3X

2. Which one of the following is not a property of gases?

A) particles in definite positions B) relatively low densities C) fills any container completely D) expand upon heating E) easily compressed

3. Give the systematic name for the following binary compound: S2F10

A) Disulfur decafluoride B) fluoride C) Sulfur decafluoride D) Disulfur pentafluoride E) Disulfur fluoride

4. Which one of the following is not one of the hypotheses of Dalton's atomic theory?

A) Atoms are composed of protons, neutrons, and electrons. B) All atoms of a given element are identical; the atoms of different elements are different and have different properties. C) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions. D) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. E) Each element is composed of extremely small particles called atoms.

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5. What is the (g/mol) of sodium sulfite?

A) 126.05 B) 142.05 C) 119.05 D) 103.05 E) 149.03

6. reacts with oxygen gas to form nitric (NO) and water vapour as follows: 4NH3 + 5O2 → 4NO + 6H2O What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react?

A) 1.88 mol B) 1.56 mol C) 3.52 mol D) 3.91 mol E) 2.35 mol

7. Ethylene (C2H4), can be prepared by heating hexane (C6H14) at high temperature. C6H14 C2H4 + other products (assume the equation is already balanced). If the percent yield of ethylene is 42.5 %, what mass of hexane must be used to produce 481 g of ethylene?

A) 3.48 x 103 g B) 1.13 x 103 g C) 2.33 x 102 g D) 2.83 x 102 g E) 3.36 x 104 g

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8. A metal, M, was converted to the , M2(SO4)3. Then a solution of the sulfate was treated with barium chloride to give BaSO4 as follows:

M2(SO4)3(aq) + 3BaCl2(aq) → 2MCl3(aq) +3BaSO4(s)

If 1.200 g of the metal gave 6.026 g of BaSO4, what is the identity of the metal?

A) Ga B) Ni C) Fe D) Cr E) In

9. You mix 25.0 mL of 0.234 M FeCl3 with 42.5 mL of 0.453 M NaOH. What is the molar concentration of the excess reactant remaining in solution?

A) 0.025 M NaOH B) 0.0017 M NaOH C) 0.0017 M FeCl3 D) 0.0023 M FeCl3 E) 0.023 M FeCl3

10. Which of the following is/are weak electrolyte(s) in aqueous solution?

I. CH3COOH II. HF III. NH3

A) All of them B) I only C) I and II only D) I and III only E) II only

11. Which of the following has/have resonance structures? - I. SO3 II. C2H4 III. NO2

A) I and III only B) I only C) II and III only D) I and II only E) All of them

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12. Rank the following compounds in order of increasing Lattice Energy. BaSe MgO CaS

A) BaSe < CaS < MgO B) BaSe < MgO < CaS C) CaS < MgO < BaSe D) MgO < CaS < BaSe E) CaS < BaSe < MgO

13. How many protons and electrons are present in the Se2- ion?

A) 34 protons and 36 electrons B) 79 protons and 81 electrons C) 34 protons and 32 electrons D) 79 protons and 77 electrons E) 34 protons and 34 electrons

14. .Which one of the following elements has the largest first ionization energy?

A) Cl B) Ca C) Se D) Te E) Ga

15. The electronic configuration of a ground–state Chromium (Cr) is

A) [Ar]4s13d5 B) [Ar]4s23d4 C) [Ne]4s23d7 D) [Ne]4s13d6 E) [Ar]4s24d7

16. Which statement about electromagnetic radiation is false?

A) As wavelength increases, energy increases. B) As frequency increases, wavelength decreases. C) As wavelength increases, frequency decreases. D) Wavelength and frequency are inversely proportional. E) Wavelength and energy are inversely proportional.

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17. What is the height of a column of methyl alcohol that will be supported by one atmospheric pressure? The density of methyl alcohol is 0.787 g/cm3. [1 Pa = 1 kg/m·s2 and 1 atm = 101325 Pa; gravitational constant = 9.80665 m/s2]

A) 13.1 m B) 10.3 m C) 7.87 m D) 9.80 m E) 12.3 m

18. At 40.0 C a sample of nitrogen gas exerts a pressure of 2.2 atm. What is the pressure when the volume of the gas is reduced to one-fifth of the original value at the same temperature?

A) 11 atm B) 10. atm C) 2.2 atm D) 4.4 atm E) 5.0 atm

19. Analysis of a volatile liquid shows that it contains 62.04% carbon, 10.41% hydrogen, and 27.54% oxygen by mass. At 150.°C and 1.00 atm, 500. mL of the vapor has a mass of 0.8365 g. What is the molecular formula of the compound?

A) C3H6O B) C6H12O2 C) C12H24O4 D) C4H6O E) C2H5OH

20. Consider the following reaction (at STP) and identify the false statement. C2H2(g) + N2(g)→ 2HCN(g)

A) Producing exactly 22.4 L of HCN requires the complete reaction of 28 g of N2. B) This is a combination reaction. C) 26 g of C2H2 react to yield 44.8 L of HCN. D) 22.4 L of C2H2 react to yield 44.8 L HCN. E) 22.4 L of N2 react to yield 44.8 L HCN.

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21. The average kinetic energy of ideal gas molecules is directly proportional to the ____.

A) absolute temperature of the sample B) density of the sample C) mass of the molecule D) pressure of the sample E) volume of the sample

22. What is the molar mass of an unknown gas, which effuses with a rate equal to one third (1/3) the rate of helium gas?

A) 36 g/mol B) 72 g/mol C) 18 g/mol D) 54 g/mol E) 92 g/mol

23. Which of the following is the correct approach to prepare a 100.0 mL of a 1.00 M H2SO4 solution from a 10.0 M H2SO4 stock solution?

A) Add 10.0 mL of the stock solution to 80.0 mL of H2O, stir and dilute to 100.0 mL. B) Add 50.0 mL of the stock solution to 25.0 mL of H2O, stir and dilute to 100.0 mL C) Add 25.0 mL of the stock solution to 50.0 mL of H2O, stir and dilute to 100.0 mL. D) Add 90.0 mL of stock solution to 10.0 mL of H2O and stir the solution. E) Add 1.0 mL of the stock solution to 99.0 mL of H2O and stir the solution.

24. Consider the combustion of hydrogen given below:

H2(g) + ½ O2(g) → H2O(g) ΔH = -241.8 kJ/mol

What is the enthalpy change, in kJ, when the reaction is started with 52.5 g of H2 and 52.5 g of O2 ?

A) -793 kJ B) -537 kJ C) -192 kJ D) -645 kJ E) -564 kJ

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25. If the internal energy of a system decreases by 135 J and at the same time it absorbs 24 J of heat, what is the work?

A) -159 J B) 111 J C) -111 J D) 213 J E) 159 J

26. According to the VSEPR model, the predicted molecular geometries of Ammonia (NH3), (HCN) and Phosphorus pentachloride (PCl5) respectively are

A) trigonal pyramidal, linear and trigonal bipyramidal. B) trigonal planar, linear and trigonal pyramidal. C) trigonal pyramidal, bent and trigonal bipyramidal. D) tetrahedral, linear and octahedral. E) linear, bent and trigonal bipyramidal.

2– 27. According to the VSEPR model, what is the predicted F–Si–F bond angle in SiF6 ?

A) 90° B) 109.5° C) 120° D) 145° E) 130°

28. How many π and σ bonds are there in the molecule shown below?

A) 3 π and 18 σ B) 2 π and 16 σ C) 3 π and 15 σ D) 2 π and 19 σ E) 3 π and 10 σ

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29. What is the total number of electron domains around the central atom in XeF2 ?

A) 5 B) 2 C) 3 D) 4 E) 6

30. What diatomic molecule and/or ion(s) would have the molecular orbital electron configuration given below? 2 * 2 2 * 2 2 1 1s 1s 2s 2s 2py 2pz

+ – A) C2 and B2 – + B) C2 and N2 – + C) C2 and B2 + D) N2 and C2 + E) O2 and N2

- 31. Indicate the type of hybrid orbitals used by the central atom in ClBr2 .

A) sp3d B) sp2 C) sp D) sp3 E) sp3d2

32. What is the molality of 8.6% glucose (C6H12O6) by mass in water?

A) 0.52 m B) 0.32 m C) 0.34 m D) 0.44 m E) 0.67 m

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33. Which observation(s) reflect(s) colligative properties? I. A 0.5 m NaBr solution has a higher vapor pressure than a 0.5 m BaCl2 solution. II. A 0.5 m NaOH solution freezes at lower temperature than pure water III. Pure water freezes at a higher temperature than pure methanol

A) I and II B) I only C) II only D) III only E) I and III

34. A 250 mL solution containing 21.4 g of a non-electrolyte polymer in toluene has an osmotic pressure of 0.055 atm at 27 oC. What is the closest molecular weight of the polymer?

A) 38,000 g/mol B) 44,000 g/mol C) 28,000 g/mol D) 32,000 g/mol E) 15,000 g/mol

35. Which of the following is/are true? I. Hydration is a special case of solvation in which the solvent is water. II. Upon dissoving CaCl2 in water, the oxygen end of water molecules is attracted toward Ca2+ ions. III. Upon dissoving CaCl2 in water, the hydrogen end of water molecules is attracted toward Cl- ions. IV CaCl2 is insoluble in water.

A) I, II and III only B) I and II only C) IV only D) I and IV only E) II and III only

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36. Determine the van't Hoff factor of sodium phosphate in a 0.40 m aqueous solution

whose freezing point is -2.60 C. [The Kf value for water is 1.86 C/m]

A) 3.5 B) 2.7 C) 4.0 D) 3.0 E) 2.9

37. The distance between atomic layers in a crystal is 325 pm. At what angle would you expect X-rays of wavelength 0.154 nm to be diffracted from the crystal in a first order (n = 1) diffraction.

A) 13.7o B) 21.4o C) 18.5o D) 54.2o E) 67.3o

38. Determine the heat required to melt a 0.677 kg piece of lead (Pb) starting with the sample at 25.0 oC. Given the following data: Melting point: 327.4 oC ; Enthalpy of fusion: 4.774 kJ/mol ; Specific heat: 0.134 Jg-1 oC-1

A) 43.0 kJ B) 94.1 kJ C) 75.2 kJ D) 25.8 kJ E) 17.2 kJ

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39. Consider the phase diagram of phosphorus given below.

Which of the following statements is not correct?

A) A sample of solid phosphorus will melt if heated to 590 oC in an open container. B) At 590 oC and 43 atm, the solid, liquid and vapor phases coexist. C) At 595 oC, the vapor will condense if compressed sufficiently. D) Point A represents a solid phase. E) Point B represents a liquid phase.

40. Iron crystallizes in a body-centered cubic lattice with a unit cell length of 287 pm. Calculate the density of iron in g/cm3.

A) 7.85 B) 5.92 C) 9.41 D) 8.53 E) 10.3

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Answer Key

1. A 2. A 3. A 4. A 5. A 6. A 7. A 8. A 9. A 10. A 11. A 12. A 13. A 14. A 15. A 16. A 17. A 18. A 19. A 20. A 21. A 22. A 23. A 24. A 25. A 26. A 27. A 28. A 29. A 30. A 31. A 32. A 33. A 34. A 35. A 36. A 37. A 38. A 39. A 40. A

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