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1.
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Given the unbalanced
equation:
What is the coefficient in front of the CaSO4 when the equation is completely balanced with
the smallest whole-number coefficients?
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2.
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An atom of lithium-7 has an equal number of
a. | positrons and neutrons | c. | electrons and
protons | b. | positrons and protons | d. | electrons and neutrons |
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3.
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Beryllium is classified as
a. | an alkaline earth metal | c. | a noble gas | b. | a transition metal
| d. | an alkali
metal |
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4.
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Which equation represents a
neutralization reaction?
a. | HNO3(aq) + KOH(aq) 
KNO3(aq) + H2O(l) | b. | H2SO4(aq) + CaCO3(aq) 
CaSO4(aq) + H2O(l)
+CO2(g) | c. | 2 HCl(aq) + Zn(s)  ZnCl2(aq) +
H2(g) | d. | CaO(s) + H2O(l) 
Ca(OH)2(aq) |
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5.
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Which orbital notation shows the lowest energy arrangement of valence electrons
for 1s22s22p3?
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6.
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The gram molecular mass of Ca3(PO4)2 is
a. | 342 g | b. | 310 g | c. | 246 g | d. | 279 g
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7.
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Which of the following elements has the smallest atomic radius?
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8.
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The H3O+ ion concentration of a solution
is 1 x 10-4 M. This solution is
a. | acidic and has a pH of
10 | c. | acidic and has a pH of
4 | b. | basic and has a pH of
4 | d. | basic and has a pH of
10 |
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9.
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The reaction for the
decomposition of PCl5 to
chlorine and PCl3 is shown below.
PCl5(g)  PCl3(g) +
Cl2(g)
If the
equilibrium concentrations are [PCl5] = 1.0 M, [PCl3] = 0.10 M,
[Cl2] = 0.10 M, what is the value of the equilibrium constant?
a. | 1.0 x 102 | c. | 2.0 x 10-2 | b. | 1.0 x 10-4 | d. | 1.0 x 10-2 |
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10.
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A solution containing a large
concentration of dissolved ions can be classified as a(n) ________.
a. | Solvent | c. | suspension | b. | weak solution | d. | Strong electrolyte |
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11.
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A monochromatic beam of light has a frequency of 7.69 x 1014 Hz
(hertz). What is the energy of a photon of this light?
a. | 3.90 x 10-7 J | c. | 2.59 x 10-40
J | b. | 5.10 x 10-19 J | d. | 6.92 x 10-31 J |
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12.
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In the
reaction
an acid-base conjugate pair is
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13.
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Which of the following is a correct Lewis dot structure for potassium
chloride?
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14.
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Which element within any given period of the Periodic Table would always have
the lowest first ionization energy?
a. | a halogen | c. | an alkaline earth metal | b. | an alkali metal
| d. | a noble
gas |
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15.
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A person attemps to fill their car tires with 9.03x1023 molecules of
nitrogen gas (N2). How many moles did the person attempt to put in the tires?
a. | 0.667 moles | c. | 1.50 moles | b. | 33.6 moles | d. | 42.0 moles |
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16.
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Which of the following is an example of a physical change?
a. | burning gasoline | c. | rusting of iron | b. | breaking glass | d. | lighting a match
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17.
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Which set of procedures and observations indicates a chemical change
a. | Large crystals are crushed with a mortar and pestle and become
powder. | b. | A solid is gently heated in a crucible and the solid slowly turns to liquid.
| c. | Ethanol is added to an empty beaker and the ethanol eventually
disappears. | d. | A cool, shiny metal is added to water in a beaker and rapid bubbling
occurs. |
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18.
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Which graph shows the
pressure-temperature realationship expected for an ideal gas?
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19.
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Which pair of elements form an ionic bond with each other?
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20.
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Co(H2O)62+(aq) + 4
Cl-(aq)  CoCl42-(aq) + 6
H2O(l)
Write the Keq expression of the reaction
above
a. | Keq =  | c. | Keq
=  | b. | Keq =  | d. | Keq
=  |
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21.
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Metallic bonds occur between atoms of
a. | sulfur | b. | fluorine | c. | neon | d. | copper |
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22.
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Given the
reaction:
How many moles of C6H12O6 (s) are needed to produce 24 moles of carbon
dioxide?
a. | 1.0
mole | b. | 24
moles | c. | 12
moles | d. | 4.0
moles |
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23.
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What is the total number of electrons present in an atom of  ?
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24.
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Which of the following atoms has six valence electrons?
a. | sulfur (S) | c. | magnesium (Mg) | b. | silicon (Si) | d. | argon (Ar) |
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25.
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The bonds present in nitrogen dioxide (NO2) are
a. | metallic | c. | ionic | b. | covalent | d. | van der Waals |
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26.
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Sulfur dioxide is the cause of acid rain and is common pollutant caused by
volcanic eruptions, the burning of fossil fuels, and the exhaust from industrial facilities.
What is the mass in gram of 0.75 mole of SO2? (MM: 64.07 g/mol)
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27.
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A red light is measured to have a wavelength of 6.71 x 10-7 m. Given
the speed of light (3.00 x 108 m/s) and Planck’s constant (6.63 x 10-34
Js), calculate the energy of one photon of this light.
a. | 2.96 x 10-19 J | c. | 1.33 x 10-18
J | b. | 4.42 x 10-3 J | d. | 1.48 x 10-18 J |
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28.
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As wavelength increases, what happens to Frequency and Energy?
a. | Both Decrease | c. | Frequency decreases, Energy increases | b. | Frequency increases,
Energy decreases | d. | Both
Increase |
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29.
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Which group contains elements with a total of four electrons in the outermost
energy level (valence shell)?
a. | Group 2A | b. | Group 6A | c. | Group 4A | d. | Group
1A |
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30.
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Which of the following models best represents the shape of a compound
with trigonal planar geometry?
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31.
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Which of the following atoms have the largest atomic radius?
a. | barium (Ba) | c. | iodine (I) | b. | magnesium (Mg) | d. | chlorine (Cl) |
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32.
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Given the balanced
equation:
AgNO3 + NaCl  NaNO3 +
AgCl
Which compound would
precipitate out of the reaction?
a. | AgNO3 | c. | NaCl | b. | NaNO3 | d. | AgCl |
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33.
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Which temperature is the same
as -13 °C?
a. | 747 K | b. | 286 K | c. | 260 K | d. | 773 K |
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34.
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What is the total number of molecules in 1.0 mole of Cl2 (g)?
a. | 70 | c. | 12 x 1024 | b. | 6.02 x 1023 | d. | 35 |
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35.
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Which sample of matter is a pure substance?
a. | ammonia gas (NH3) | c. | hydrochloric acid solution (HCl +
H2O) | b. | air (O2, N2, CO2) | d. | salt water (NaCl +
H2O) |
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36.
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What is the pH of a 0.01 M
solution of KOH?
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37.
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Carbon reacts with chlorine to form CCl4. What is the name of
this compound?
a. | 1-carbon 4-chloride | c. | carbon tetrachloride | b. | tetracarbon chloride | d. | carbon
4-chloride |
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38.
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What is the Lewis dot structure for nitogen trifluoride (NF3)
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39.
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In theory, how many grams of
H2O can be produced if an
experiment used 12.75 grams of sulfur dioxide and 3.96 grams of hydrosulfuric acid? (MM
H2S = 34.082 g/mol ; MM SO2 = 64.064 g/mol; MM H2O = 18.015 g/mol
)
2
H2S (g) +
SO2 (g)  3 S (g) + 2 H2O
(g)
a. | 1.98
grams | c. | 7.17
grams | b. | 1.50 grams | d. | 3.96 grams |
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40.
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Which of the following factors contributes to the increase in atomic size within
a group in the periodic table as the atomic number increases?
a. | an increase in number of protons | b. | an increase in size of the
nucleus | c. | fewer electrons in the highest occupied energy level | d. | more shielding of
the electrons in the highest occupied energy level |
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41.
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Which type of bond is formed by the transfer of electrons from one atom to
another?
a. | a coordinate covalent bond | c. | an ionic bond | b. | a hydrogen
bond | d. | a covalent
bond |
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42.
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What is the molarity of a KF
(aq) solution containing 116 g of KF in 1.00 L of solution?
a. | 4.00 M | b. | 1.00 M | c. | 2.00 M | d. | 3.00 M |
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43.
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Which atom contains exactly 15 protons?
a. | oxygen-15 | c. | sulfur-32 | b. | nitrogen-15 | d. | phosphorous-32 |
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44.
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What is the maximum number of orbitals in the p sublevel?
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45.
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According to the Arrhenius definition, a substance that is classified as an acid
will always produce _______ in solution
a. | K+(aq) | b. | I-(aq) | c. | H+(aq) | d. | F-(aq) |
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46.
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What is the name for the compound FeS
a. | iron (II) sulfide | c. | iron (II) sulfate | b. | iron (III) sulfate | d. | iron (III)
sulfide |
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47.
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Which subatomic particles are located in the nucleus of a neon atom?
a. | electrons and neutrons | c. | protons and neutrons | b. | protons and
electrons | d. | electrons and
protons |
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48.
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The solid block shown here has a mass of 146 grams. What is the
block’s density? a. | 0.37 g/cm3 | c. | 54 g/cm3 | b. | 8.1 g/cm3 | d. | 2.7
g/cm3 |
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49.
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What trend can be seen as the atomic number increases in period 3?
a. | increasing electronegativity | c. | decreasing atomic
mass | b. | decreasing first ionization energy | d. | increasing atomic radius
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50.
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Which is the correct name of the compound with the formula
NH4NO2?
a. | ammonium nitrite | c. | ammonia nitrate | b. | ammonium nitrate | d. | ammonia nitrite |
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51.
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Chemical equations must be balanced to satisfy
a. | the law of conservation of mass. | b. | the law of multiple
proportions. | c. | the law of definite proportions. | d. | Avogadro’s
principle. |
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52.
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Ethanol (C2H5OH) is used in hand sanatizer. If 115
grams of C2H5OH is used to to make a batch of hand sanatizer, then how many
moles are present in the batch? (MM: 46.08 g/mol)
a. | 1.00 mol | c. | 2.50 mol | b. | 3.00 mol | d. | 1.50 mol |
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53.
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Which kind of bond is formed when two atoms share electrons to form a
molecule?
a. | electovalent | b. | metallic | c. | ionic | d. | covalent |
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54.
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4K(s) + O2(g)  2K2O(s)
Under certain conditions potassium can react with oxygen in air to form
potassium oxide according to the above equation. Which image best represents the amount of
potassium required to completely react with all of the oxygen shown in the flask
below?
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55.
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If 75.0 % of the isotope of an element have a mass of 35.0 amu and 25.0 % of the
isotopes have a mass of 37.0 amu, what is the average atomic mass of the element?
a. | 35.5 amu | b. | 37.0 amu | c. | 35.0 amu | d. | 36.0
amu |
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56.
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Given the
reaction:
How many moles of CO2 are produced when 11.2 liters of C8H16 gas, measured
at STP, reacts completely?
a. | 30.0
mole | b. | 8.00
moles | c. | 10.0
moles | d. | 4.00
mole |
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57.
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What causes NH3 to have it’s shape, according to VSEPR
theory?
a. | repulsive forces between unshared pairs of electrons and bonds | b. | the unusual location
of the free electrons | c. | ionic attraction and
repulsion | d. | interaction between the fixed orbitals of the unshared pairs of
hydrogen |
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58.
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Which of the following atoms has a smallest atomic radius?
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59.
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1s22s22p63s23p64s1
is the electron configuration for which element?
a. | aluminum (Al) | c. | calcium (Ca) | b. | potassium (K) | d. | argon (Ar) |
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60.
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Which statement describes a chemical property of iron?
a. | Iron can be drawn into a wire. | b. | Iron conducts electricity and
heat. | c. | Iron can be flattened into sheets. | d. | Iron combines with oxygen to form
rust. |
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61.
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Orange light has a frequency of 5.0 x 1014 Hz (hertz) in a
vaccuum. What is the wavelength of this light?
a. | 1.5 x 1023 m | c. | 2.0 x 10-15 m
| b. | 1.7 x 106 m | d. | 6.0 x 10- 7 m |
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62.
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A neon sign is being made with 80 grams of neon. How many atoms are
contained the neon sign?
a. | 4.80 x 1024 atoms | c. | 6.02 x 1023
atoms | b. | 1.20 x 1024 atoms | d. | 2.40 x 1024
atoms |
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63.
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Which of the following elements has an electron configuration of
1s22s22p63s23p1?
a. | aluminum | c. | calcium | b. | lithium | d. | phosphorous |
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64.
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Which of the following quantum leaps of an electron would be associated with the
greatest energy of emitted light?
a. | Energy Level = 4 to 5 | b. | Energy Level = 5 to 1 | c. | Energy Level =
5 to 2 | d. | Energy Level= 6 to 5 |
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65.
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The covalent bonds in water are
polar because
a. | O and H are equally
electronegative. | c. | H is more
electronegative than O. | b. | O is more electronegative than H. | d. | water molecules are cohesive. |
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66.
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What is the formula mass of calcium nitrate,
Ca(NO3)2?
a. | 70.0 g | c. | 102 g | b. | 150 g | d. | 164 g |
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67.
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One of the wavelengths emitted by hydrogen atoms is
6.56 x 10-7 m. Calculate
the frequency if the speed of light is 3.00 x 108 m/s..
a. | 1.97 x 1014 Hz | c. | 4.57 x 10-6
Hz | b. | 4.57 x 1014 Hz | d. | 4.57 x 10-7 Hz |
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68.
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According to the
Brønsted-Lowry definition, an acid is any species that can
a. | accept an
electron | c. | donate an
electron | b. | donate a proton | d. | accept a proton |
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69.
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What formula represents lead (II) phosphate?
a. | Pb2(PO4)3 | c. | Pb3(PO4)2 | b. | Pb4PO4 | d. | PbPO4 |
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70.
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When the
reaction
is completely balanced using smallest whole numbers, the coefficient of
H2O will
be
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71.
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What is the name of the compound whose formula is
H2SO4?
a. | sulfuric acid | c. | hydrosulfurous acid | b. | hydrosulfuric acid | d. | sulfurous acid |
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72.
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In a solution, litmus paper
turned blue. The pH of this solution could be
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73.
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What is the mass number of an ion that has 83 protons, 80 electrons, and 126
neutrons?
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74.
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Sodium, mercury, argon and neon are used in the production of lamps. There are
fewer safety guidelines regarding the handling of neon and argon than for mercury and sodium. Which
of the following best describes the properties of elements in the same family as neon and
argon?
a. | Mostly unreactive | c. | Solid at room temperature and mostly unreactive with strong
acids | b. | Solid at room temperature | d. | Gaseous at room temperature and highly reactive |
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75.
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An atom is electrically neutral because the
a. | ratio of the number of neutrons to the number of protons is 2:1. | b. | ratio of the number
of neutrons to the number of electrons is 1:1. | c. | number of protons equals the nubmer of
electrons. | d. | number of protons equals the number of neutrons. |
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76.
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Logan is studying a substance. Which property of the substance is
chemical?
a. | its temperature | c. | its density | b. | its melting point | d. | its
flammability |
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77.
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What is the percent mass oxygen in acetone (C3H6O)?
a. | 1.00 % | b. | 10.3 % | c. | 27.6 % | d. | 62.0
% |
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78.
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The correct formula for sodium oxide is
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79.
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How many moles of CH4 are contained in 96.0 grams of
CH4?
a. | 12.0 moles | c. | 3.00 moles | b. | 16.0 moles | d. | 6.00 moles |
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80.
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When 20 mL of 1.0 M HCl is
diluted to a total volume of 60 mL, the concentration of the resulting solution is
a. | 0.50 M | b. | 1.0 M | c. | 0.33 M | d. | 0.25 M |
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81.
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Given a pH of 3.8, which of the
following is true?
a. | Contains more OH- ions than H+
ions | c. | can be neutralized by a strong
acid | b. | contains more H+ ions than OH- | d. | has a slightly basic pH |
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