Academic Chemistry Spring 2010 Final Exam Review Problems

Chapters 6 & 7

  1. When the equation Fe2O3 Fe + O2 is balanced, the coefficient for O2 is:

A4C2

B3D1

  1. The reaction in question 1 is an example of a(n):

AdecompositionCsingle displacement

BsynthesisDcombustion

  1. In a double displacement reaction:

Aone of the products is always a gas

Bone of the products must be an element

Cpositive ions are exchanged between two compounds

Dall of the above

  1. A double displacement reaction takes place when aqueous K2SO4 reacts with aqueous Pb(NO3)2. You would expect one of the products of this reaction to be:

AK2SCPbSO4

BNaPbDCNO3

  1. Water is often a product in:

Acombustion reactionsCsingle-displacement reactions

Bdecomposition reactionsDdecomposition reactions

  1. The following would be classified as which type of reaction?

CH4 + 2 O2  CO2 + 2 H2O

AsynthesisBcombustion

Csingle displacementDdouble displacement

  1. Which of the following describes the products of a synthesis reaction?

Acarbon dioxide and waterBa single product

Can element and a compoundDtwo ionic compounds

  1. Predict the products from the following reactants:

MgSO4 + Na 

AMg +Na2SO4BMgNa + SO4

CMgSO4 + NaDMg + NaSO4

  1. When the following equation is balanced, what is the coefficient that goes with water?

_____ Mn(OH)3 + _____ H2SO3  _____ Mn2(SO3)3 + _____ H2O

A2B3

C6D12

  1. O2, N2, Cl2, and I2 are examples of—

Adiatomic moleculesBcompounds

Cionic compoundsDatoms

  1. Which compound will be a precipitate (solid) in the following equation?

_____ (NH4)2SO4 + _____ Pb(NO3)2  _____ PbSO4 + _____ NH4NO3

A(NH4)2SO4 BPb(NO3)2

CPbSO4 DNH4NO3

  1. Which of the following compounds will be soluble in water?

AAgClBKOH

CMgCO3DAlPO4

Chapter 9

  1. How many moles of oxygen gas will react with excess sulfur according to produce 1.25 mol of sulfur trioxide according to the following equation?

__1__ S8 + __12__ O2  __8__SO3

A0.833 molB1.25 mol

C1.88 molD10.0 mol

  1. What is the molar mass of iron (III) sulfate, Fe2(SO4)3?

A104.0 g/molB312.0 g/mol

C335.7 g/molD399.9 g/mol

  1. How many moles of H2O will be produced when 3.7 x 1023 molecules of NH3 react with excess O2 according to the following equation?

4 NH3 + 7 O2 4 NO2 + 6 H2O

A0.922 mol H2OB0.410 mol H2O

C16.6 mol H2OD3.68 mol H2O

  1. Given the reaction Zn + 2 HCl  ZnCl2 + H2, if 2.0 mol Zn and 5.0 mol of HCl are allowed to react:

AZn is the limiting reactantBHCl is the limiting reactant

C1.0 mol of ZnCl2 is producedD5.0 mol of H2 is produced

  1. Given the reaction CaCO3 CaO + CO2, if 50.0 g of CaCO3 react to produce 20.0 g of CO2, what is the percent yield of CO2?

A66.7%B40.0%

C90.9%D250%

Chapter 10

  1. How many electrons can be held in the 2nd energy level?

A2B8

C18D32

  1. Which element is represented by the following electron configuration?

1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p4

AThalliumBPolonium

CBismuthDAstatine

  1. Which of the following is the correct short hand electron configuration for Barium?

A[Kr]5s2B[Xe]5s2

C[Xe]6s1D[Xe]6s2

  1. Which element is represented by the following short hand configuration?

[Kr]5s24d105p4

ATelluriumBBromine

CSeleniumDIndium

  1. What part of the following electron configuration is not in the correct order?

1s22s22p63s13p64s24d104p6

A3p6B4d10

C4p6D4s2

  1. How many sublevel does each “d” sublevel contain?

A1B3

C5D7

  1. What is the maximum number of electrons that each “p” orbital can hold?

A2B6

C10D14

  1. Put the following elements in order of increasing atomic radii: Fe, S, F, Ba, Ca

AF, S, Fe, Ba, CaBBa, Ca, Fe, S, F

CF, S, Fe, Ca, BaDCa, F, Fe, Ba, S

  1. Put the following elements in order of increasing electronegativity: Rb, O, F, Sr, Mn

ARb, Sr, F, Mn, OBRb, O, F, Sr, Mn

CO, Mn, F, Sr, RbDRb, Sr, Mn, O, F

  1. Which of the following elements requires the smallest amount of energy to remove an electron (ionization energy): C, Se, K, or Sc?

ACBSe

CKDSc

  1. What is the electron configuration for Arsenic?

A1s22s22p63s23p64s23d104p3

B1s22s22p63s23p64s23d94p4

C1s22s22p63s23p64s13d104p4

D1s22s22p63s23p64s23d104p6

  1. Put the following in order of decreasing ionic radii: N - 3, F - 1, Na + 1, Mg + 2, O -2.

AN - 3, F - 1, Na + 1, Mg + 2, O -2

BN - 3, O - 2, F - 1, Na + 1, Mg + 2

CMg +2, Na + 1, F - 1, O - 2, N - 3

DN - 3, O - 2, Mg + 2, F - 1, Na + 1

  1. How many unshared electrons will Silicon have in its orbital notation?

A0B1

C2D3

Chapter 11

  1. How many valence electrons does C2ClO3-3 contain?

A32B36

C33D29

  1. Methane, CH4, contains what type of intermolecular forces?

Ahydrogen bondingBdipole-dipole interactions

Cdispersion forcesDnonpolar covalent bonding

According to the Lewis diagram above, a carbonate ion has a –

Atrigonal planar bent structure and a double bond

Bpolar structure and a single bond

Clinear structure and a triple bond

Dtrigonal planar structure and a single bond

34. Which of the following elements is not an exception to the octet rule?

AHydrogenBBeryllium

CBoronDCarbon

35. Which of the following compounds is considered ionic?

ACOBH2O

CNaClDF2

36. Carbon tetrachloride is a molecule with a tetrahedral shape. This molecule is

ApolarBnonpolar

CionicDmetallic

37. Sulfur dioxide, SO2, contains what type of intermolecular forces?

Ahydrogen bondingBdipole-dipole interactions

Cdispersion forcesDnonpolar covalent bonding

38. The bond that exists between nitrogen and fluorine is

AionicBcovalent

Cpolar covalentDnonpolar ionic

39. When drawing structural formulas, two lines between atoms(as in O = C = O)

represents

A2 electrons in a single bond

B2 electrons in a double bond

C4 electrons in a double bond

D4 electrons in a single bond

40. The bond in the molecule hydrogen bromide, HBr, is considered to be

Anonpolar covalentBpolar covalent

CionicDmetallic

41. How many valence electrons would an atom of aluminum gain or lose when forming

a bond?

Again 3Blose 3

Cgain 5Dlose 5

42. What is the VSEPR shape for SO3-2?

Atrigonal planarB tetrahedral bent

CtetrahedralDtrigonal pyramidal

Chapter 12

43. The average kinetic energy of water molecules is greatest in:

Asteam at 200oCBliquid water at 90oC

Cliquid water at 273 KDice at 0oC

44. An increase in the temperature of a contained liquid:

Acauses the vapor pressure above the liquid to increase.

Bdecreases the vapor pressure above a liquid.

Ccauses fewer particles to escape the surface of the liquid

Dhas no effect on the kinetic energy of the liquid

45. A pressure of 2.5 atm is equivalent to

A41 kPaB1900 mm Hg

C3.0 x 102 torrD2.5 kPa

46. At 80 K, the particles of a gas have:

Atwice the average kinetic energy of the same particles at 40 K

Bhalf the average kinetic energy of the same particles at 40 K

Cone-fourth the average kinetic energy of the same particles at 20 K

Dnone of these

47. A 1.0 mol sample of gas is at a temperature of 20oC and a pressure of 1.2 atm. What

is the volume occupied by the gas? (R = 0.0821 L atm/K mol)?

A20 LB30 L

C40 LD50 L

48. Increasing the volume of a given amount of gas at constant temperature causes the

pressure to decrease because:

Athe molecules are striking a larger area with the same force

Bthere are fewer molecules

Cthe molecules are moving more slowly

Dthere are more molecules

49. A gas occupies a volume of 2.50 L at a pressure of 350.0 kPa. If the temperature

remains constant, what volume would the gas occupy at 1750 kPa?

A5.00 LB0.500 L

C12.5 LD1.40 x 102 L

50. If a sample of oxygen occupies a volume of 2.15 L at a pressure of 58.0 kPa and a

temperature of 25oC, what volume would this sample occupy at 101.3 kPa and

0.0oC?

A1.35 LB1.13 L

C4.10 LD3.44 L