Download chem final review

Chemistry Final Review
1) The difference between a scientific theory and a
11) Which of the following is a true statement about
scientific law is that _____ .
compounds?
A) a law only summarizes observations; a theory
A) They are pure substances.
attempts to explain observations
B) They can be physically separated into their
B) a theory only summarizes observations; a law
constituent elements.
attempts to explain observations
C) They have properties similar to those of their
C) There is no difference.
constituent elements.
2) An important characteristic of an accepted
D) They have variable compositions.
scientific theory is that _____ .
12) One difference between a mixture and a
A) it is agreed upon by all scientists.
compound is that
B) it can be proven true.
A) a compound is made up of more than one
C) it cannot be modified.
phase.
D) it can be disproved at any time.
B) a mixture must be uniform in composition.
3) Matter is defined as anything that _____ .
C) a mixture can only be separated into its
A) has a fixed volume and weight
components by chemical means.
B) has mass and takes up space
D) a compound can only be separated into its
C) can be weighed on a balance
components by chemical means.
D) has a definite volume
13) The chemical formula of a compound indicates
4) A vapor is which state of matter?
the _____.
A) plasma
B) gas
A) three-dimensional structure of the compound
C) liquid
D) solid
B) relative proportions of the elements in the
5) Which state of matter is characterized by having an
compound
indefinite shape, but a definite volume?
C) type and arrangement of the bonds in the
A) plasma B) gas
C) solid
D) liquid
compound
6) Which of the following materials is a pure
D) identity of the elements in the compound only
substance?
14) Consider the chemical reaction in which carbon
A) diamond
B) air
reacts with oxygen to produce carbon dioxide. What
C) brass
D) tea
mass of carbon dioxide would be produced if 24
E) gasoline
grams of carbon reacted completely with 64 grams of
7) All of the following are physical properties of
oxygen?
matter EXCEPT
A) 64 g
B) 48 g
C) 40 g
A) color
B) explosiveness
D)130 g
E) 88 g
C) hardness
D) mass
15) Which of the following is a chemical property of
E) melting point
an antacid tablet?
8) All of the following are physical properties of a
A) tart taste
B) lack of color
substance in the liquid state EXCEPT _____.
C) ability to neutralize acid
D) white color
A) definite mass
16) The diameter of a carbon atom is 0.000 000 000
B) indefinite shape
154 m. What is this number expressed in scientific
C) virtual incompressibility
notation?
D) indefinite volume
A) 1.54 x 1010 m
B) 1.54 x 10-12 m
9) Which of the following does NOT involve a
C) 1.54 x 1012 m
D) 1.54 x 10-10 m
physical change?
17) What is 5928 km expressed in scientific notation?
A) melting
B) grinding
A) 5.928 x 10-3
B) 5.928 x 102
C) mixing
D) tarnishing
C) 5.928 x 100
D) 5.928 x 103
10) Which of the following is a homogeneous
18) How many significant figures are there in the
mixture?
measurement 40 500 mg?
A) beef stew
B) raisin bread
A) four
B) five
C) three
C) soil
D) sand and water
D) two
E) This cannot be determined.
E) brine
Page 1 of 9
19) What is the quantity 7896 millimeters expressed
in meters?
A) 7.896 m
B) 789 600 m
C) 78.96 m
D) 789.6 m
E) 7 896 000 m
20) Which of the following equalities is NOT correct?
A) 1 cm3 = 1 mL
B) 1000 kg = 1 g
C) 1000 mm = 1 m
D) 100 cg = 1 g
21) What is the density of an object having a mass of
8.0 g and a volume of 25 cm3?
A) 2.0 g/cm3
B) 3.1 g/cm3 C) 200 g/cm3
3
D) 0.32 g/cm
E) none of the above
22) What is the volume of 45.6 g of silver if the
density of silver is 10.5 g/mL?
A) 4.34 mL
B) 0.23 mL C) 479 mL
D) none of the above
23) How are the numerator and denominator in a
conversion factor related?
A) They each have the same units.
B) One is greater than or less than the other.
C) Both equal the value 1.
D) They are equal.
24) Which of the following conversion can be used to
change centimeters to kilometers?
A) ( 1 m/100 cm) x ( 1000 m/1 km)
B) ( 100 cm/1 m) x ( 1 km/1000 m)
C) ( 100 cm/1 m) x ( 1000 m/1 km)
D) ( 1 m/100 cm) x ( 1 km/1000 m)
25) If 20 gits equal 1 erb, and 1 futz equals 2 hews,
and 10 erbs equal 1 futz, how many gits equal 5 hews?
A) 500 gits
B) 50 gits
C) 100 gits
D) 1000 gits
26) What is the smallest particle of an element that
retains the properties of that element?
A) an atom
B) a proton C) an electron
D) a molecule
E) a neutron
27) Dalton's atomic theory included which idea?
A) Atoms of different elements always combine in
one-to-one ratios.
B) When an atom of an element changes into
another element, a chemical reaction takes
place.
C) Individual atoms can be seen with a
microscope.
D) Atoms of the same element are always
identical.
E) All atoms of all elements are the same size.
28) Why did J. J. Thomson reason that electrons must
be a part of the atoms of all elements?
A) Cathode rays were always accompanied by
anode rays.
B) Cathode rays can be deflected by magnets.
C) Cathode rays are always made of electrons,
regardless of the gas used.
D) Cathode rays are negatively-charged particles.
E) An electron is 2000 times lighter than a
hydrogen atom.
29) As a consequence of the discovery of the nucleus
by Rutherford, which model of the atoms is believed to
be true?
A) A model in which the nucleus is made of
protons, electrons, and neutrons
B) A model in which the nucleus is made of
neutrons only
C) A model in which the nucleus is made of
electrons and protons.
D) A model in which the protons, electrons, and
neutrons are evenly distributed throughout the
volume of the atom
E) A model in which the region outside the nucleus
is largely empty space in which the electrons are
situated
30) In which of the following sets are the symbol of
the element, the number of protons, and the number of
electrons given correctly?
A) In, 49 protons, 49 electrons
B) Cs, 55 protons, 132.9 electrons
C) Zn, 30 protons, 60 electrons
D) He, 4 protons, 4 electrons
E) F, 19 protons, 19 electrons
31) Consider an element Z that has two naturally
occurring isotopes with the following percent
abundances: the isotope with a mass number of 20 is
25% abundant; the isotope with a mass number of 22
is 75% abundant. What is the average atomic mass for
element Z?
A) 42.0 g
B) 2.0 g
C) 21.0 g
D) 21.5 g
E) 20.5 g
32) Which subatomic particle plays the greatest part
in determining the physical and chemical properties of
an element?
A) electron
B) neutron C) proton
D) quark
E) muon
33) In which of the following is the symbol for the ion
and the number of electrons it contains correct?
A) Br- has 34 electrons. B) Al3+ has 16 electrons.
C) Ca2+ has 18 electrons. D) S2- has 2 electrons.
+
E) H has 1 electron.
Page 2 of 9
34) Which of the following statements is true
concerning the composition of ionic compounds?
A) They are formed from two or more nonmetallic
elements.
B) They are formed from two or more metallic
elements.
C) They are composed of anions only.
D) They are composed of cations only.
E) They are composed of anions and cations.
35) Which of the following formulas represents an
ionic compound?
A) Kr
B) BaI2
C) PCl3
D) N2O4
E) CS2
36) In which of the following groups of ions are the
charges all shown correctly?
A) Ca2+, Al3+, BrB) Be2+, Cl2-, Sr2+
C) Li-, O2-, S2+
D) Na+, I-, RbE) K2-, F-, Mg2+
37) In which of the following are the symbol and
name for the ion given correctly?
A) PO33- phosphate; PO34-phosphite
B) NH4+ ammonia; H+: hydride
C) C2H3O2- acetate; CO32- carbonite
D) OH- : hydroxide; O2-: oxide
E) HSO4- hydrogen sulfate; HSO32- hydrogen
sulfite
38) What is the ionic charge on the zirconium ion in
the ionic compound zirconium oxide, ZrO2?
A) 2B) 4+ C) 2+ D) 0 E) 439) Which of the following compounds contains the
Mn3+ ion?
A) MnO
B) MnS
C) Mn3O2
D) MnBr2
E) Mn2O3
40) Which set of chemical name and chemical
formula for the same compound is correct?
A) iron(III) phosphate, FePO4
B) potassium chlorine, K2Cl2
C) ammonium sulfite, (NH4)2S
D) magnesium dichromate, MgCrO4
E) lithium carbonate, LiCO3
41) Which of the following shows both the correct
formula and correct name of an acid?
A) H2CO3, bicarbonic acid
B) HNO2, hydronitrous acid
C) HClO2, chloric acid
D) HI, iodic acid
E) H3PO4, phosphoric acid
42) How many moles of silver atoms are there in 1.8 x
1020 atoms of silver?
A) 1.1 x 1044
B) 3.0 x 10-4
C) 3.0 x 102
D) 3.3 x 10-3
43) How many molecules are there in 2.10 mol CO2?
A) 1.05 x 10-23
B) 3.49 x 10-24
24
C) 1.26 x 10
D) 3.79 x 1024
E) 2.53 x 1024
44) How many hydrogen atoms are in 5 molecules of
isopropyl alcohol, C3H7O?
A) 5 x (6.02 x 1023)
B) 35 x (6.02 x 1023)
C) 5
D) 35
45) What is the mass, in grams, of 0.450 moles of
Sb?
A) 0.450 g
B) 2.71 x 1023
C) 2.02 x 101
D) 3.55 x 101
E) 5.48 x 101
46) A large weather balloon filled with helium has a
volume of 7.00 x 102 L at STP. Which expression
should be used to find the mass of helium in the
balloon?
A) 22.4 L/mol/7.00 x 10-2 L x 4 g He/mol
B) 7.0 x 102/L x 4 g He/mol
C) 22.4 L/mol x 4 g He/mol
D) 7.00 x 102 L/22.4 L/mol x 4 g He/mol
47) What is the volume, in liters, of 6.8 mol of Kr gas
at STP?
A) 25 L
B) 13 000 L C) 0.30 L
D) 3.3 L
E) 150 L
48) If 20.0 grams of Ca combines completely with
16.0 grams of S to form a compound, what is the
percent composition of Ca in the compound?
A) 20.0%
B) 55.6%
C) 44.4%
D) 80.0%
E) 1.25%
49) Which of the following compounds have the same
empirical formula?
A) C4H10 and C10H4 B) CO2 and SO2
C) C7H14 and C10H20 D) NO and NO2
E) C6H12 and C6H14
50) What are the missing coefficients for the skeleton
equation below?
Cr(s) + Fe(NO3)2(aq) → Fe(s) + Cr(NO3)3(aq)
A) 2,3,3,2
B) 4,6,6,2
C) 2,3,1,2
D) 2,3,2,3
E) 1,3,3,1
Page 3 of 9
51) Which of the following is the correct skeleton
equation for the reaction that takes place when solid
phosphorus combines with oxygen gas to form
diphosphorus pentoxide?
A) P(s) + O(g) → P5O2(g)
B) P2O5 → P2(s) + O2(g)
C) P(s) + O2(g) → P2O5
D) P(s) + O2(g) → PO2(g)
E) P2(s) + O5(g) → P2O5(g)
52) Aluminum chloride and bubbles of hydrogen gas
are produced when metallic aluminum is placed in
hydrochloric acid. What is the balanced equation for
this reaction?
A) Al + HCl3 → AlCl3 + H
B) H2 + AlCl3 → Al + 2HCl
C) H + AlCl → Al + HCl
D) Al + 2HCl → AlCl2 + H2
E) 2Al + 6HCl → 2AlCl3 + 3H2
53) The equation H3PO4 + 3KOH → K3PO4 + 3H2O
is an example of which type of reaction?
A) combination
B) decomposition
C) single-replacement
D) double-replacement
54) A double-replacement reaction takes place when
aqueous Na2CO3 reacts with aqueous Sn(NO3)2. You
would expect one of the products of this reaction to be
_____.
A) CNO3 B) Sn(CO3)2 C) NaNO3 D) NaSn
55) What is conserved in the reaction shown below?
N2(g) + 3F2(g) → 2NF3(g)
A) only atoms
B) only mass
C) only moles
D) only mass and atoms
E) only mass, atoms, moles, and molecules
56) Hydrogen gas can be produced by reacting
aluminum with sulfuric acid. How many moles of
sulfuric acid are needed to completely react with 15.0
mol of aluminum?
2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
A) 10.0 mol
B) 22.5 mol C) 2710
mol
D) 0.100 mol
E) 15.0 mol
57) How many grams of chromium are needed to
react with an excess of CuSO4 to produce 27.0 g Cu?
2Cr(s) + 3CuSO4(aq) → Cr2(SO4)3(aq) + 3Cu(s)
A) 14.7 g
B) 33.2 g
C) 81.5 g
D) 0.005 48 g
E) 18.0 g
58) How many liters of chlorine gas can be produced
when 0.98 L of HCl react with excess O2, at STP?
4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)
A) 0.49 L
B) 0.98 L
C) 2.0 L
D) 3.9 L
E) 0.25 L
59) The reagent present in the smallest amount is
_____ the limiting reagent.
A) never B) always
C) sometimes
60) Methane and hydrogen sulfide form when
hydrogen reacts with carbon disulfide. Identify the
excess reagent and calculate how much remains after
36 L of H2 reacts with 12 L of CS2.
4H2(g) + CS2(g) → CH4(g) + 2H2S(g)
A) 9 L CS2
B) 12 L H2 C) 24 L H2
D) 3 L CS2
E) 6 L CS2
61) What happens to the average kinetic energy of the
particles in a sample of matter as the temperature of
the sample is increased?
A) It decreases. B) It does not change.
C) It increases.
62) What is the volume occupied by 2.20 mol of
hydrogen at STP?
A) 49.3 L
B) 24.6 L
C) 98.6 L D)
2.60 L
E) 2.20 L
63) Equal volumes of nitrogen and oxygen, at the
same temperature and pressure, would _____.
A) have different average kinetic energies
B) contain the same number of particles
C) contain different numbers of particles
D) have the same mass
64) If a liquid is sealed in a container and kept at
constant temperature, how does its vapor pressure
change over time?
A) It rises at first, then falls.
B) It rises continuously.
C) It rises at first, then remains constant.
65) Water could be made to boil at 105°C instead of
100°C by
A) increasing the air pressure on the water
B) applying a great deal of heat
C) decreasing the pressure on the water
D) decreasing the air pressure above the water
66) How many kilocalories of heat are required to
raise the temperature of 225 g of aluminum from 20°C
to 100°C? (specific heat of Al = 0.21 cal/g x °C)
A) 0.59 kcal
B) 85 kcal
C) 3.8 kcal
D) none of the above
Page 4 of 9
67) What is the specific heat of olive oil if it takes
approximately 420 J of heat to raise the temperature of
7 g of olive oil by 30°C?
A) less than the specific heat of water
B) equal to the specific heat of water
C) greater than the specific heat of water
D) Not enough information given.
68) Which of the following equations correctly
represents an endothermic reaction?
A) A + B + heat → C + D
B) A + B → C + D + heat
69) What is the standard heat of reaction for this
reaction:
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
(∆Hf° for Cu2+ = +64.4 kJ/mol; ∆Hf° for Zn2+ = 152.4 kJ/mol)
A) 88.0 kJ created per mole
B) 88.0 kJ absorbed per mole
C) 216.8 kJ absorbed per mole
D) 216.8 kJ created per mole
70) When heat is added to boiling water, its
temperature _____.
A) depends on the amount of water
B) decreases
C) increases
D) stays the same
71) For ammonia, (NH3), ∆Hf° = -46 kJ/mol. This
means that
A) 46 kJ is released when 1 mole of ammonia is
formed from nitrogen and hydrogen
B) it takes 46 kJ to form 1 mole of ammonia from
nitrogen and hydrogen
C) it takes 46 kJ to vaporize 1 mole of liquid
ammonia
D) 46 kJ of heat is released when 1 mole of
ammonia gas condenses
72) Why does the pressure inside a container of gas
increase if more gas is added to the container?
A) because there is a corresponding decrease in
volume
B) because there is a corresponding increase in the
temperature
C) because there is a corresponding increase in the
number of particles striking an area of the wall
of the container per unit time
D) because there is a corresponding increase in the
force of the collisions between the particles and
the walls of the container
73) What happens to the pressure of a gas inside a
container if the temperature of the gas is lowered?
A) The pressure decreases.
B) The pressure does not change.
C) The pressure increases.
74) If the volume of a container holding a gas is
reduced, what will happen to the pressure within the
container?
A) The pressure will decrease.
B) The pressure will not change.
C) The pressure will increase.
75) When the pressure and number of particles are
kept constant for a sample of gas, which of the
following is also constant for the sample?
A) the difference of the volume and temperature
(in kelvins)
B) the product of the volume and temperature (in
kelvins)
C) the sum of the volume and temperature (in
kelvins)
D) the quotient of the volume and temperature (in
kelvins)
76) Which of the following gases will effuse the most
rapidly?
A) hydrogen
B) chlorine C) argon
D) bromine
E) ammonia
77) What is the maximum number of electrons in the
second principal energy level?
A) 32
B) 8 C)18 D) 2
78) In Bohr's model of the atom, where are the
electrons and protons located?
A) The electrons orbit the protons, which are at the
center of the atom.
B) The electrons and protons are located
throughout the atom, but they are not free to
move.
C) The electrons occupy fixed positions around the
protons, which are at the center of the atom.
D) The electrons and protons move throughout the
atom.
79) What did Rutherford's experiment demonstrate?
A) that most of an atom's mass is concentrated in a
relatively small portion of the atom's entire
volume
B) that all neutrons are located in the nucleus
C) that electrons orbit the nucleus
D) that atoms are made of positively and
negatively charged particles
Page 5 of 9
80) What is the electron configuration of potassium?
A) 1s22s23s23p63d1
B) 1s22s22p23s23p24s1
C) 1s22s22p103s23p3
D) 1s22s22p63s23p64s1
81) The atomic emission spectra of a sodium atom on
earth and of a sodium atom in the sun would be _____.
A) different from each other
B) the same as each other only in the ultraviolet
range
C) the same as those of several other elements
D) the same
82) What is the approximate frequency of a photon
having an energy 5 x 10-24 J? (h = 6.6 x 10-34 J s)
A) 1 x 10-11 Hz
B) 1 x 10-10 Hz
C) 7 x 109 Hz
D) 3 x 10-58 Hz
-57
E) 3 x 10
Hz
83) Emission of light from an atom occurs when the
electron
A) jumps from a lower to a higher energy level
B) moves within its atomic orbital
C) falls into the nucleus
D) drops from a higher to a lower energy level
84) What element has the electron configuration
1s22s22p63s23p2?
A) silver
B) selenium
C) silicon
D) nitrogen
85) Which of the following groupings contains only
representative elements?
A) Hg, Cr, Ag
B) Ni, Fe, Zn
C) Cu, Co, Cd D) Al, Mg, Li
86) Which group of the periodic table has the highest
electronegativity?
A) 3A
B) 6A C) 1A
D) 2A
E) 7A
87) Atomic size generally _____.
A) increases as you move from left to right across
a period
B) remains constant within a period
C) decreases as you move down a group
D) decreases as you move from left to right across
a period
88) As you move from left to right across the second
period of the periodic table _____.
A) the atomic mass decreases
B) the atomic radii increase
C) the ionization energy increases
D) the electron affinity decreases
89) Which of the following increases with increasing
atomic number in Group 2A?
A) electron affinity
B) first ionization energy
C) atomic radius
D) number of outermost electrons
90) How many valence electrons are there in an atom
of magnesium?
A) 4
B) 6 C) 5 D) 3 E) 2
91) What is the electron configuration of the gallium
ion?
A) 1s22s22p63s23p54s1 B) 1s22s22p63s23p3
C) 1s22s22p63s23p6
D) 1s22s22p63s23p63d10
E) 1s22s22p63s23p64s24p6
92) What is the formula of the ion formed when
phosphorus achieves a noble-gas electron
configuration?
A) PB) P3+ C) P3- D) P2+
E) P293) How does oxygen obey the octet rule when
reacting to form compounds?
A) It gives up electrons.
B) It does not change its number of electrons.
C) It gains electrons.
94) What is the name of the ionic compound formed
from strontium and phosphorus?
A) strontium phosphorus B) strontium phosphate
C) strontide phosphate
D) strontium
phosphoride
E) strontium phosphide
95) Under what conditions can potassium bromide
conduct electricity?
A) only when melted, or dissolved in water
B) only when melted
C) only when dissolved
D) only when it is in crystal form
E) all of the above
96) Which of the following particles are free to drift
in metals?
A) protons
B) neutrons C) electrons
D) cations
E) pions
97) How many unshared pairs of electrons does the
nitrogen atom in ammonia possess?
A) 4
B) 5 C) 2 D) 1
E) 3
98) How many electrons does carbon need to gain to
obtain a noble-gas electron configuration?
A) 4
B) 8
C) 2
D) 1 E) 3
99) Which of the following diatomic molecules is
joined by a double covalent bond?
A) O2
B) Cl2
C) N2
D) H2
Page 6 of 9
100) According to VSEPR theory, molecules adjust
their shapes
A) an emulsion B) supersaturated
C) unsaturated
D) saturated
114) What is the molarity of a solution containing 9.0
moles of solute in 500.0 mL of solution?
A) 0.18M
B) 4.5M
C) 18M
D) 1.8M
E) 0.45M
115) What is the molarity of a solution that contains 6
moles of solute in 2 liters of solution?
A) 3M
B) 6M
C) 7M
D) 12M
116) Which of the following operations yields the
number of moles of solute?
A) moles of solution ÷ volume of solution
B) molarity x mass of solution
C) molarity x moles of solution
D) molarity x volume of solution
E) mass of solution ÷ volume of solution
117) What is the molality of a solution containing 9.0
moles of solute in 2.4 kg of solvent?
A) 3.8m B) 22m
C) 0.38m
D) 2.4m
118) What is the boiling point of a solution that
contains 3 moles of KBr in 2000 g of water? (Kb =
0.512°C/m; gram formula mass of water = 18 g)
A) 99.7°C
B) 97°C
C) 100°C
D) 101.5°C
E) 103°C
119) Activation energy is _____.
A) the energy given off when reactants collide
B) an energy barrier between reactants and
products
C) generally very high for a reaction that takes
place rapidly
D) the heat released in a reaction
120) Why does a higher concentration make a
reaction faster?
A) There are more collisions per second and the
collisions are of greater energy.
B) Collisions occur with greater energy.
C) There are more collisions per second only.
121) Why does a small particle size generally cause a
reaction to proceed faster?
A) There are more collisions per second and the
collisions are of greater energy.
B) The collisions occur with greater energy.
C) There are more collisions per second only.
122) The rate of a chemical reaction normally _____.
A) increases as reactant concentration increases
B) is slowed down by a catalyst
C) decreases as temperature increases
D) decreases as reactant concentration increases
Page 7 of 9
Problems
158) When a mixture of sulfur and metallic silver is
142) What is the density of an object having a mass of
heated, silver sulfide is produced. What mass of
4.0 g and a volume of 39.0 cubic centimeters?
silver sulfide is produced from a mixture of 3.0 g
143) What is the temperature 198 K expressed in
Ag and 3.0 g S8?
degrees Celsius?
16Ag(s) + S8(s) → 8Ag2S(s)
144) What is the volume of 500.0 g of ice if the
159) How many molecules are present in 33.0 L of
density of ice is 0.92 g/mL?
nitrogen gas at STP?
145) Convert 0.0349 mm to meters.
160) A 55.0 g piece of copper wire is heated, and the
146) List the number of protons, neutrons, and
temperature of the wire changes from 19.0°C to
electrons in each of the following atoms.
86.0°C. The amount of heat absorbed is 343 cal.
What is the specific heat of copper?
161) If 500 g of iron absorbs 22 000 cal of heat, what
will be the change in temperature?
(specific heat of iron = 0.11 cal/(g x °C))
162) A gas has a volume of 590 mL at a temperature
of -55.0°C. What volume will the gas occupy at
30.0°C?
163) A gas has a pressure of 710 mm Hg at 227°C.
What will its pressure be at 27°C, if the volume
147) Name the following compounds: CoCl2, N2O5,
does not change?
and K2Cr2O7.
164) What is the pressure exerted by 32 g of O2 in a
148) Write the formulas for the following compounds:
22.0-L container at 30.0°C?
barium cyanide, sulfur hexafluoride, and
165)
How many electrons are in the highest occupied
mercury(II) chloride.
energy level of a neutral strontium atom?
149) Find the mass in grams of 2.20 x 1023
166) What is the wavelength of light with a frequency
molecules of F2.
of 1.0 x 1020 Hz? (c = 3.0 x 108 m/s)
150) What is the empirical formula of a compound
167) What is the energy of a photon of light with
that is 40.7% carbon, 54.2% oxygen, and 5.1%
frequency
hydrogen?
1.0 x 1012 Hz? (h = 6.6 x 10-34 J s)
151) Find the number of moles of argon in 481 g of
168) What is the electron configuration of oxygen?
argon.
169) Which element in the second principal energy
152) Balance the following equation. Complete the
level has the greatest atomic radius?
equation first, if necessary.
170) Give the electron configurations for sulfur and
C3H6 + O2 → CO2 + H2O
its 2- ion.
153) Balance the following equation. Complete the
171) Give the electron configurations for iodine and
equation first, if necessary.
its 1- ion.
Al + Cl2 →
172) How many electrons does a gallium atom give
up when it becomes an ion?
154) Balance the following equation. Complete the
173) Give the electron configuration for the lithium
equation first, if necessary.
ion.
Fe2(SO4)3 + Ba(OH)2→
174) Write the formula for the compound, aluminum
155) How many liters of O2 are needed to react
iodide.
completely with 45.0 L of H2S at STP?
175) How many calories are required to heat 354
2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g)
grams of water from 19°C to 87°C?
156) How many liters of O2 are needed to react
176) How many calories are released when 15 grams
completely with 47.0 L of H2S at STP?
of steam at 100°C condense to 15 grams of water
at 100°C?
2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g)
157) For the reaction 2Na + Cl2 → 2NaCl, how many
grams of NaCl could be produced from 103.0 g
of Na and 13.0 L of Cl2 (at STP)?
Page 8 of 9
Answers
1) A
2) D
3) B
4) B
5) D
6) A
7) B
8) D
9) D
10) E
11) A
12) D
13) B
14) E
15) C
16) D
17) D
18) C
19) A
20) B
21) D
22) A
23) D
24) D
25) A
26) A
27) D
28) C
29) E
30) A
31) D
32) A
33) C
34) E
35) B
36) A
37) D
38) B
39) E
40) A
41) E
42) B
43) C
44) D
45) E
46) D
47) E
48) B
49) C
50) A
51) C
52) E
53) D
54) C
55) D
56) B
57) A
58) A
59) C
60) D
61) C
62) A
63) B
64) C
65) A
66) C
67) A
68) A
69) D
70) D
71) A
72) C
73) A
74) C
75) D
76) A
77) B
78) A
79) A
80) D
81) D
82) C
83) D
84) C
85) D
86) E
87) D
88) C
89) C
90) E
91) D
92) C
93) C
94) E
95) A
96) C
97) D
98) A
99) A
100) A
101) C
102) D
103) B
104) A
105) B
106) A
107) D
108) D
109) A
110) C
111) A
112) B
113) B
114) C
115) A
116) D
117) A
118) D
119) B
120) C
121) C
142) 0.10 g/cm3
143) -75°C
144) 540 mL
145) 0.0000349 m
146) Protons: 6, 7, 10, 5, 4
Neutrons: 7, 8, 10, 6, 5
Electrons: 6, 7, 10, 5, 4
147) cobalt(II) chloride, dinitrogen
pentoxide, potassium dichromate
148) Ba(CN)2 SF6 HgCl2
149) 13.9 g F2
150) Empirical formula = C2H3O2
151) 12.1 mol Ar
152) C3H6 + 3O2 →3CO + 3H2O
153) 2Al + 3Cl2 → 2AlCl3
154) Fe2(SO4)3 + 3Ba(OH)2 →
2Fe(OH)3 + 3BaSO4
155) 67.5 L O2
156) 70.5 L O2
157) Cl2 is limiting reagent: 67.3 g NaCl
158) Answer: Limiting reagent is silver:
3.72 g Ag2S
159) 8.87 x 1023 molecules
Page 9 of 9
160) 9.31 x 10-2 cal/(g x °C)
161) 400°C
162) 820 mL
163) 470 mmHg
164) 1.13 atm or 860 mmHg
165) 2
166) 3.0 x 10-12 m
167) 6.6 x 10-22 J
168) 1s22s22p4
169) lithium
170) S 1s22s22p63s23p4
S2- 1s22s22p63s23p6
171) I
1s22s22p63s23p63d104s24p64d
104f145s25p5
I1s22s22p63s23p63d104s24p64d
104f145s25p6
172) 3
173) 1s2
174) AlI3
175) 2.4 x 104 cal
176) 8.1 x 103cal