CHEMISTRY FINAL EXAM REVIEW GUIDE 2012 Scott
DISCLAIMER: THIS IS A SAMPLE OF QUESTIONS/PROBLEMS FROM THIS YEAR. PLEASE BE SURE TO REVIEW YOUR NOTES, LABS, COJ’S, OBJECTIVE SHEETS, ETC. DO NOT RELY ONLY ON THIS REVIEW GUIDE.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____1)Which of the following observations is quantitative?
a. / The liquid turns blue litmus paper red.b. / The liquid boils at 100C.
c. / The liquid tastes bitter.
d. / The liquid is cloudy.
____2)The symbols for units of length in order from largest to smallest are
a. / m, cm, mm, km. / c. / km, mm, cm, m.b. / mm, m, cm, km. / d. / km, m, cm, mm.
____3)A volume of 1 milliliter is equivalent to
a. / 1 cubic centimeter. / c. / 1 liter.b. / 1 gram. / d. / 10–1 cubic decimeters.
____4)Which pair of quantities determines the density of a material?
a. / mass and weight / c. / volume and concentrationb. / volume and weight / d. / volume and mass
____5)A sample of gold has a mass of 96.5 g and a volume of 5.00 cm3. The density of gold is
a. / 0.0518 g/cm3. / c. / 101.5 g/cm3.b. / 19.3 g/cm3. / d. / 483 g/cm3.
____6)The number of grams equal to 0.5 kg is
a. / 0.0005. / c. / 500.b. / 0.005. / d. / 5000.
____7)If 1 inch equals 2.54 cm, how many centimeters equal 1 yard?
a. / 0.0706 cm / c. / 30.5 cmb. / 14.2 cm / d. / 91.4 cm
____8)A chemist obtained the values 5.2246 g, 5.2353 g, and 5.2501 g for the mass of a sample. Without knowing the true mass of the sample, it can be said that these values have
a. / good precision.b. / good accuracy.
c. / poor precision.
d. / poor accuracy.
____9)The measurement 0.035550 g rounded off to two significant figures would be
a. / 0.03 g. / c. / 0.036 g.b. / 0.35 g. / d. / 3.5 102 g.
____10)When 64.4 is divided by 2.00, the correct number of significant figures in the result is
a. / 1. / c. / 4.b. / 3. / d. / 6.
____11)According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is ____ the sum of the masses of the individual elements.
a. / equal to / c. / less thanb. / greater than / d. / either greater than or less than
____12)Which concept in Dalton's atomic theory has been modified?
a. / All matter is composed of atoms.b. / Atoms of different elements have different properties and masses.
c. / Atoms can combine in chemical reactions.
d. / Atoms cannot be divided.
____13)Rutherford's experiments led him to conclude that atoms contain massive central regions that have
a. / a positive charge. / c. / no charge.b. / a negative charge. / d. / both protons and electrons.
____14)Experiments with cathode rays led to the discovery of the
a. / proton. / c. / neutron.b. / nucleus. / d. / electron.
____15)Whose series of experiments identified the nucleus of the atom?
a. / Rutherford / c. / Chadwickb. / Dalton / d. / Bohr
____16)Because most particles fired at gold foil passed straight through, Rutherford concluded that
a. / atoms were mostly empty space. / c. / electrons formed the nucleus.b. / atoms contained no charged particles. / d. / atoms were indivisible.
____17)An atom is electrically neutral because
a. / neutrons balance the protons and electrons.b. / nuclear forces stabilize the charges.
c. / the numbers of protons and electrons are equal.
d. / the numbers of protons and neutrons are equal.
____18)The atomic number of oxygen, 8, indicates that there are eight
a. / protons in the nucleus of an oxygen atom.b. / oxygen nuclides.
c. / neutrons outside the oxygen atom's nucleus.
d. / energy levels in the oxygen atom's nucleus.
____19)Chlorine has atomic number 17 and mass number 35. It has
a. / 17 protons, 17 electrons, and 18 neutrons.b. / 35 protons, 35 electrons, and 17 neutrons.
c. / 17 protons, 17 electrons, and 52 neutrons.
d. / 18 protons, 18 electrons, and 17 neutrons.
____20)Phosphorus-33 contains
a. / 33 protons. / c. / 33 neutrons.b. / 18 neutrons. / d. / 18 protons.
____21)The atomic number of neon is 10. The atomic number of calcium is 20. Compared with a mole of neon, a mole of calcium contains
a. / twice as many atoms. / c. / an equal number of atoms.b. / half as many atoms. / d. / 20 times as many atoms.
____22)The mass of a sample containing 3.5 mol of silicon atoms is approximately
a. / 28 g. / c. / 72 g.b. / 35 g. / d. / 98 g.
____23)Refer to the figure below. To which group do fluorine and chlorine belong?
a. / alkaline-earth metals / c. / halogensb. / transition elements / d. / actinides
____24)Across a period in the periodic table, atomic radii
a. / gradually decrease.b. / gradually decrease, then sharply increase.
c. / gradually increase.
d. / gradually increase, then sharply decrease.
____25)Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a. / The nuclear charge increases.b. / The number of neutrons increases.
c. / The number of occupied energy levels increases.
d. / A new octet forms.
____26)The number of valence electrons in Group 17 elements is
a. / 7. / c. / 17.b. / 8. / d. / equal to the period number.
____27)Across a period, ionization energies of d-block elements generally
a. / increase. / c. / remain constant.b. / decrease. / d. / drop to zero.
____28)Among the d-block elements, as atomic radii decrease, electronegativity values
a. / remain constant. / c. / decrease.b. / increase. / d. / drop to zero.
____29)The electrons involved in the formation of a chemical bond are called
a. / dipoles. / c. / Lewis electrons.b. / s electrons. / d. / valence electrons.
____30)If two covalently bonded atoms are identical, the bond is
a. / nonpolar covalent. / c. / dipole covalent.b. / polar covalent. / d. / coordinate covalent.
____31)The B—F bond in BF3 is
a. / polar covalent. / c. / nonpolar covalent.b. / ionic. / d. / metallic.
____32)In a molecule of fluorine, the two shared electrons give each fluorine atom how many electron(s) in the outer energy level?
a. / 1 / c. / 8b. / 2 / d. / 32
____33)The substance whose Lewis structure shows three covalent bonds is
a. / H2O. / c. / NH3.b. / CH2Cl2. / d. / CCl4.
____34)What is the correct Lewis structure for hydrogen chloride, HCl?
a. / A / c. / Cb. / B / d. / D
____35)The Lewis structure for the ammonium ion, NH4, has
a. / nonpolar covalent bond. / c. / polar covalent bond.b. / ionic bond. / d. / metallic bond.
____36)According to VSEPR theory, an AB2 molecule is
a. / trigonal-planar. / c. / linear.b. / tetrahedral. / d. / octahedral.
____37)According to VSEPR theory, the structure of the ammonia molecule, NH3, is
a. / trigonal-planar. / c. / trigonal-pyramidal.b. / bent. / d. / tetrahedral.
____38)Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.
a. / tetrahedral / c. / bentb. / linear / d. / trigonal-planar
____39)Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.
a. / tetrahedral / c. / bentb. / linear / d. / trigonal-planar
____40)The reason the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S) is partially explained by
a. / London forces. / c. / ionic bonding.b. / covalent bonding. / d. / hydrogen bonding.
____41)The following molecules contain polar bonds. The only polar molecule is
a. / CCl4. / c. / NH3.b. / CO2. / d. / CH4.
____42)When Group 2A elements form ions, they ____.
a. / lose two protons / c. / lose two electronsb. / gain two protons / d. / gain two electrons
____43)What is the correct name for the Nion?
a. / nitrate ion / c. / nitride ionb. / nitrogen ion / d. / nitrite ion
____44)Aluminum is a group 3A metal. Which ion does A1 typically form?
a. / Al / c. / Alb. / Al / d. / Al
____45)The nonmetals in Groups 6A and 7A ____.
a. / lose electrons when they form ionsb. / have a numerical charge that is found by subtracting 8 from the group number
c. / all have ions with a –1 charge
d. / end in -ate
____46)Which of the following compounds contains the Mn ion?
a. / MnS / c. / MnOb. / MnBr / d. / MnO
____47)How are chemical formulas of ionic compounds generally written?
a. / cation then anionb. / anion then cation
c. / Roman numeral first, then anion, then cation
d. / subscripts first, then ions
____48)Which of the following formulas represents an ionic compound?
a. / CS / c. / NOb. / BaI / d. / PCl
____49)Which element, when combined with fluorine, would most likely form an ionic compound?
a. / lithium / c. / phosphorusb. / carbon / d. / chlorine
____50)Which of the following shows correctly an ion pair and the ionic compound the two ions form?
a. / Sn, N; SnN / c. / Cr, I; CrIb. / Cu, O; CuO / d. / Fe, O; FeO
____51)Which of the following compounds contains the lead(II) ion?
a. / PbO / c. / Pb2Ob. / PbCl4 / d. / Pb2S
____52)Which of the following shows both the correct formula and correct name of an acid?
a. / HClO, chloric acid / c. / HPO, phosphoric acidb. / HNO, hydronitrous acid / d. / HI, iodic acid
____53)What is the formula for phosphoric acid?
a. / HPO / c. / HPOb. / HPO / d. / HPO
____54)Select the correct formula for sulfur hexafluoride.
a. / SF / c. / FSb. / FSO / d. / SF
____55)What is the correct name for the compound CoCl?
a. / cobalt(I) chlorate / c. / cobalt(II) chlorateb. / cobalt(I) chloride / d. / cobalt(II) chloride
____56)What is the correct formula for barium chlorate?
a. / Ba(ClO) / c. / Ba(ClO)b. / Ba(ClO) / d. / BaCl
____57)Which of the following is the correct name for NO?
a. / nitrous oxide / c. / nitrogen dioxideb. / dinitrogen pentoxide / d. / nitrate oxide
____58)To balance a chemical equation, it may be necessary to adjust the
a. / coefficients. / c. / formulas of the products.b. / subscripts. / d. / number of products.
____59)A chemical equation is balanced when the
a. / coefficients of the reactants equal the coefficients of the products.b. / same number of each kind of atom appears in the reactants and in the products.
c. / products and reactants are the same chemicals.
d. / subscripts of the reactants equal the subscripts of the products.
____60)Which equation is not balanced?
a. / / c. /b. / / d. /
____61)Which coefficients correctly balance the formula ?
a. / 1,2,2 / c. / 2,1,1b. / 1,1,2 / d. / 2,2,2
____62)The units of molar mass are
a. / g/mol. / c. / amu/mol.b. / mol/g. / d. / amu/g.
____63)In the reaction represented by the equation 2Al2O3 4Al + 3O2, what is the mole ratio of aluminum to oxygen?
a. / 10:6 / c. / 2:3b. / 3:4 / d. / 4:3
____64)The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?
a. / 1.0 mol / c. / 3.0 molb. / 2.0 mol / d. / 6.0 mol
____65)For the reaction represented by the equation 2Fe + O2 2FeO, how many grams of iron(II) oxide are produced from 8.00 mol of iron in an excess of oxygen?
a. / 71.8 g / c. / 712 gb. / 575 g / d. / 1310 g
____66)For the reaction represented by the equation 2Na + Cl2 2NaCl, how many grams of sodium chloride can be produced from 500. g each of sodium and chlorine?
a. / 112 g / c. / 409 gb. / 319 g / d. / 824 g
____67)For the reaction represented by the equation CH4 + 2O2 2H2O + CO2, calculate the percentage yield of carbon dioxide if 1000. g of methane react with excess oxygen to produce 2300. g of carbon dioxide.
a. / 83.88% / c. / 92.76%b. / 89.14% / d. / 96.78%
____68)A catalyst is ____.
a. / the product of a combustion reactionb. / not used up in a reaction
c. / one of the reactants in single-replacement reactions
d. / a solid product of a reaction
____69)Chemical equations must be balanced to satisfy ____.
a. / the law of definite proportions / c. / the law of conservation of massb. / the law of multiple proportions / d. / Avogadro’s principle
____70)In every balanced chemical equation, each side of the equation has the same number of ____.
a. / atoms of each element / c. / molesb. / molecules / d. / coefficients
____71)When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____.
a. / KH BaCl KCl BaH / c. / 2KOH BaCl 2KCl Ba(OH)b. / KOH BaCl KCl BaOH / d. / KOH BaCl KCl BaOH
____72)In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that shows the ____.
a. / periodic tableb. / activity series of metals
c. / common polyatomic ions
d. / ionic charges of representative elements
____73)In a double-replacement reaction, the ____.
a. / products are always molecularb. / reactants are two ionic compounds
c. / reactants are two elements
d. / products are a new element and a new compound
____74)Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a. / PbO Pb 2O / c. / PbO 2Pb Ob. / PbO Pb O / d. / PbO Pb O
____75)The equation 2CHOH 9O 6CO 8HO is an example of which type of reaction?
a. / combustion reaction / c. / double-replacement reactionb. / single-replacement reaction / d. / decomposition reaction
____76)A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is ____.
a. / Co(OH) / c. / LiCob. / Co(OH) / d. / LiCl
____77)If a synthesis reaction takes place between rubidium and bromine, the chemical formula for the product is ____.
a. / RuBr / c. / RbBrb. / RbBr / d. / RbBr
____78)What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?
a. / Br NaI NaBr I / c. / Br NaI NaBrIb. / Br 2NaI 2NaBr I / d. / Br NaI NaBr I
____79)Pressure is the force per unit
a. / volume. / c. / length.b. / surface area. / d. / depth.
____80)If force is held constant as surface area decreases, pressure
a. / remains constant.b. / decreases.
c. / increases.
d. / increases or decreases, depending on the volume change.
____81)Why does a can collapse when a vacuum pump removes air from the can?
a. / The inside and outside forces balance out and crush the can.b. / The unbalanced outside force from atmospheric pressure crushes the can.
c. / The atmosphere exerts pressure on the inside of the can and crushes it.
d. / The vacuum pump creates a force that crushes the can.
____82)Convert the pressure 0.840 atm to mm Hg.
a. / 365 mm Hg / c. / 638 mm Hgb. / 437 mm Hg / d. / 780 mm Hg
____83)To correct for the partial pressure of water vapor in a gas collection bottle, the vapor pressure of H2O at the collecting temperature is generally
a. / subtracted from the partial pressure of the collected gas.b. / added to the pressure of the collected gas.
c. / subtracted from the atmospheric pressure.
d. / added to the atmospheric pressure.
____84)A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At constant temperature, what volume does the gas occupy when the pressure decreases to 700.0 mm Hg?
a. / 80.0 mL / c. / 600. mLb. / 490. mL / d. / 640. mL
____85)Chlorine is produced by the reaction 2HCl(g) H2(g) + Cl2(g). How many grams of HCl (36.5 g/mol) must be used to produce 10.0 L of chlorine at STP?
a. / 15.8 g / c. / 32.6 gb. / 30.2 g / d. / 36.5 g
____86)Calculate the approximate volume of a 0.600 mol sample of gas at 15.0°C and a pressure of 1.10 atm.
a. / 12.9 L / c. / 24.6 Lb. / 22.4 L / d. / 139 L
____87)Why is a gas easier to compress than a liquid or a solid?
a. / Its volume increases more under pressure than an equal volume of liquid does.b. / Its volume increases more under pressure than an equal volume of solid does.
c. / The space between gas particles is much less than the space between liquid or solid particles.
d. / The volume of a gas’s particles is small compared to the overall volume of the gas.
____88)Why does the pressure inside a container of gas increase if more gas is added to the container?
a. / There is an increase in the number of collisions between particles and the walls of the container.b. / There is an increase in the temperature of the gas.
c. / There is a decrease in the volume of the gas.
d. / There is an increase in the force of the collisions between the particles and the walls of the container.
____89)If a balloon is heated, what happens to the pressure of the air inside the balloon if the volume remains constant?
a. / It increases. / c. / It decreases.b. / It stays the same. / d. / The change cannot be predicted.
____90)If a sealed syringe is heated, in which direction will the syringe plunger move?
a. / out / c. / The plunger will not move.b. / in / d. / The direction cannot be predicted.
____91)If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, the partial pressure of oxygen on Everest is ____.
a. / one-sixth its pressure at sea level / c. / one-half its pressure at sea levelb. / one-third its pressure at sea level / d. / equal to its pressure at sea level
____92)Which of the following best describes temperature?
a. / energy as heat absorbed or released in a chemical or physical changeb. / a measure of the average kinetic energy of the particles in a sample of matter
c. / energy in the form of heat
d. / energy of change
____93)How is a Celsius temperature reading converted to a Kelvin temperature reading?
a. / by adding 273.15 / c. / by dividing by 273.15b. / by subtracting 273.15 / d. / by multiplying by 273.15
____94)What is the energy required to raise the temperature of 1 g of a substance by 1°C or 1 K?
a. / specific heat / c. / heat capacityb. / heat energy / d. / enthalpy of formation
____95)How much energy does a copper sample absorb as energy in the form of heat if its specific heat is 0.384 J/(g·°C), its mass is 8.00 g, and it is heated from 10.0°C to 40.0°C?
a. / 0.0016 J/(g·°C) / c. / 92.2 Jb. / 0.0016 J / d. / 92.2 J/(g·°C)
____96)Find the specific heat of a material if a 6.0 g sample absorbs 50. J when it is heated from 30°C to 50°C.
a. / 0.60 J / c. / 0.42 Jb. / 0.60 J/(g·°C) / d. / 0.42 J/(g·°C)
____97) is always positive for a
a. / spontaneous reaction. / c. / exothermic reaction.b. / nonspontaneous reaction. / d. / endothermic reaction.
____98)Ice melting is an example of a(n)
a. / exothermic reaction. / c. / endothermic reaction.b. / negative entropic reactions. / d. / catalysed reaction.
____99)A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?
a. / The temperature of the metal will increase.b. / The temperature of the water will increase.
c. / The temperature of the water will decrease.
d. / The temperature of the water will increase and the temperature of the metal will decrease.
Short Answer
100)What is the law of conservation of mass?
101)Describe the nucleus of an atom.
102)What is the atomic number of an atom?
103)What is the mass number of an atom?
104)The element chromium has four naturally occurring isotopes. Use the relative abundance of each to calculate the average atomic mass of chromium.
Cr = 4.34%, Cr = 83.79%, Cr = 9.50%, Cr = 2.37%.
105)In terms of the periodic law, explain which two of these elements are most similar: sodium (element 11), phosphorus (element 15), and sulfur (element 16).
106)What can you predict about the properties of xenon and helium, both in Group 18 in the periodic table? Why?
107)Differentiate/ compare/ contrast an ionic compound and a molecular compound.
108)Why must a chemical equation be balanced to solve stoichiometry problems?
109)Give at least three reasons why the actual yield of a chemical reaction could be less than the theoretical yield.
110)Balance the following equation. Identify the reaction type.
Mg HPO Mg(PO) H
111)Balance the following equation. Identify the reaction type.
CH O CO HO
112)Balance the following equation. Identify the reaction type.
AuO Au O
113)Balance the following equation. Identify the reaction type.
NaPO ZnSO NaSO Zn(PO)
114)Complete and balance the following equation. Identify the reaction type.
Al Cl
115)Complete and balance the following equation. Identify the reaction type.
Fe(SO) Ba(OH)
116)What are standard temperature and pressure? Why is a standard necessary?
117)A gas occupies a volume of 140 mL at 35.0C and 97 kPa. What is the volume of the gas at STP?
118)How many moles of N are in a flask with a volume of 250 mL at a pressure of 300.0 kPa and a temperature of 300.0 K?
119)How can a calorimeter measure energy?
120)Explain the difference between heat and temperature.
121)What mass of KCl (solubility = at 20C) can dissolve in 3.30 10 g of water?
122)What is the molarity of a solution containing 9.0 moles of solute in 2500 mL of solution?
123)If 1.0 mL of 6.0M HCl is added to 499 mL of water to give exactly a 500-mL solution, what is the molarity of the dilute solution?
124)If the volume of solute is 6.0 mL and the volume of solution is 300.0 mL, what is the solute's percent by volume?
125)Calculate the molality of a solution prepared by dissolving 175 g of KNO in 750 g of water.
126)If you supply 36 kJ of heat, how many moles of ice at 0C can be melted, heated to its boiling point, and completely boiled away? (H = 40.5 kJ/mol; H = 6.0 kJ/mol; specific heatwater = 0.0753 )
127)Use the periodic table to determine the number of electrons in a neutral atom of lithium.
128)How many protons are present in an atom of Be-9?
129)Write the charge of a chloride ion.
130)How many atoms are present in 80.0 mol of zirconium?
131)How many moles of iron are equivalent to 1.11 1025 atoms?
132)Determine the mass in grams of 5.00 mol of oxygen.
133)Draw a ball-and-stick model of a water molecule. Include the polarities of the bonds.What type of intermolecular force is present in water?
134)What mass of PCl3 forms in the reaction of 75.0 g P4 with 275 g Cl2?
135)The reaction of 100. g of salicylic acid, C7H6O3, with excess acetic anhydride produces 50.0 g of aspirin, C9H8O4, according to the equation below. What is the percentage yield for this reaction?