Academic Chemistry Spring 2010 Final Exam Review Problems
Chapters 6 & 7
- When the equation Fe2O3 Fe + O2 is balanced, the coefficient for O2 is:
A4C2
B3D1
- The reaction in question 1 is an example of a(n):
AdecompositionCsingle displacement
BsynthesisDcombustion
- 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
- 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
- Water is often a product in:
Acombustion reactionsCsingle-displacement reactions
Bdecomposition reactionsDdecomposition reactions
- The following would be classified as which type of reaction?
CH4 + 2 O2 CO2 + 2 H2O
AsynthesisBcombustion
Csingle displacementDdouble displacement
- Which of the following describes the products of a synthesis reaction?
Acarbon dioxide and waterBa single product
Can element and a compoundDtwo ionic compounds
- Predict the products from the following reactants:
MgSO4 + Na
AMg +Na2SO4BMgNa + SO4
CMgSO4 + NaDMg + NaSO4
- When the following equation is balanced, what is the coefficient that goes with water?
_____ Mn(OH)3 + _____ H2SO3 _____ Mn2(SO3)3 + _____ H2O
A2B3
C6D12
- O2, N2, Cl2, and I2 are examples of—
Adiatomic moleculesBcompounds
Cionic compoundsDatoms
- 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
- Which of the following compounds will be soluble in water?
AAgClBKOH
CMgCO3DAlPO4
Chapter 9
- 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
- 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
- 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
- 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
- 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
- How many electrons can be held in the 2nd energy level?
A2B8
C18D32
- Which element is represented by the following electron configuration?
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p4
AThalliumBPolonium
CBismuthDAstatine
- Which of the following is the correct short hand electron configuration for Barium?
A[Kr]5s2B[Xe]5s2
C[Xe]6s1D[Xe]6s2
- Which element is represented by the following short hand configuration?
[Kr]5s24d105p4
ATelluriumBBromine
CSeleniumDIndium
- What part of the following electron configuration is not in the correct order?
1s22s22p63s13p64s24d104p6
A3p6B4d10
C4p6D4s2
- How many sublevel does each “d” sublevel contain?
A1B3
C5D7
- What is the maximum number of electrons that each “p” orbital can hold?
A2B6
C10D14
- 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
- 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
- Which of the following elements requires the smallest amount of energy to remove an electron (ionization energy): C, Se, K, or Sc?
ACBSe
CKDSc
- What is the electron configuration for Arsenic?
A1s22s22p63s23p64s23d104p3
B1s22s22p63s23p64s23d94p4
C1s22s22p63s23p64s13d104p4
D1s22s22p63s23p64s23d104p6
- 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
- How many unshared electrons will Silicon have in its orbital notation?
A0B1
C2D3
Chapter 11
- How many valence electrons does C2ClO3-3 contain?
A32B36
C33D29
- 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