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1.
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A neon sign is being made with 80 grams of neon. How many atoms are
contained the neon sign?
a. | 2.40 x 1024 atoms | c. | 4.80 x 1024
atoms | b. | 6.02 x 1023 atoms | d. | 1.20 x 1024
atoms |
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2.
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Which group contains elements with a total of four electrons in the outermost
energy level (valence shell)?
a. | Group 4A | b. | Group 2A | c. | Group 1A | d. | Group
6A |
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3.
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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 4-chloride | b. | tetracarbon chloride | d. | carbon
tetrachloride |
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4.
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Beryllium is classified as
a. | an alkali metal | c. | an alkaline earth metal | b. | a transition metal
| d. | a noble
gas |
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5.
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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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6.
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How many moles of CH4 are contained in 96.0 grams of
CH4?
a. | 12.0 moles | c. | 6.00 moles | b. | 16.0 moles | d. | 3.00 moles |
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7.
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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. | Gaseous at room temperature and highly reactive | c. | Solid at room
temperature | b. | Solid at room temperature and mostly unreactive with strong acids | d. | Mostly
unreactive |
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8.
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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= 6 to
5 | c. | Energy Level = 5 to 1 | d. | Energy Level = 5 to
2 |
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9.
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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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10.
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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. | 3.00 mol | b. | 1.50 mol | d. | 2.50 mol |
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11.
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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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12.
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Logan is studying a substance. Which property of the substance is
chemical?
a. | its density | c. | its temperature | b. | its melting point | d. | its
flammability |
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13.
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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. | 1.0 M | b. | 0.25 M | c. | 0.50 M | d. | 0.33 M |
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14.
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When the
reaction
is completely balanced using smallest whole numbers, the coefficient of
H2O will
be
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15.
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According to the Arrhenius definition, a substance that is classified as an acid
will always produce _______ in solution
a. | H+(aq) | b. | F-(aq) | c. | K+(aq) | d. | I-(aq) |
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16.
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Which of the following elements has the smallest atomic radius?
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17.
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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. | 2.00 M | b. | 1.00 M | c. | 3.00 M | d. | 4.00 M |
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18.
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Which of the following is a correct Lewis dot structure for potassium
chloride?
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19.
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Which kind of bond is formed when two atoms share electrons to form a
molecule?
a. | electovalent | b. | ionic | c. | metallic | d. | covalent |
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20.
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An atom of lithium-7 has an equal number of
a. | positrons and neutrons | c. | positrons and
protons | b. | electrons and protons | d. | electrons and neutrons |
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21.
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What is the percent mass oxygen in acetone (C3H6O)?
a. | 27.6 % | b. | 10.3 % | c. | 62.0 % | d. | 1.00
% |
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22.
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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. | 6.0 x 10- 7 m | c. | 1.7 x 106
m | b. | 2.0 x 10-15 m | d. | 1.5 x 1023 m |
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23.
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What formula represents lead (II) phosphate?
a. | PbPO4 | c. | Pb3(PO4)2 | b. | Pb4PO4 | d. | Pb2(PO4)3 |
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24.
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Which of the following elements has an electron configuration of
1s22s22p63s23p1?
a. | calcium | c. | phosphorous | b. | lithium | d. | aluminum |
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25.
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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. | 37.0 amu | b. | 35.0 amu | c. | 36.0 amu | d. | 35.5
amu |
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26.
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Which of the following models best represents the shape of a compound
with trigonal planar geometry?
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27.
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A solution containing a large
concentration of dissolved ions can be classified as a(n) ________.
a. | weak
solution | c. | suspension | b. | Solvent | d. | Strong electrolyte |
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28.
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What is the total number of electrons present in an atom of  ?
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29.
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Chemical equations must be balanced to satisfy
a. | Avogadro’s principle. | b. | the law of conservation of
mass. | c. | the law of definite proportions. | d. | the law of multiple
proportions. |
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30.
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The covalent bonds in water are
polar because
a. | O and H are equally
electronegative. | c. | O is more
electronegative than H. | b. | H is more electronegative than O. | d. | water molecules are cohesive. |
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31.
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In a solution, litmus paper
turned blue. The pH of this solution could be
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32.
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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
4 | c. | acidic and has a pH of
10 | b. | basic and has a pH of
10 | d. | basic and has a pH of
4 |
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33.
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The bonds present in nitrogen dioxide (NO2) are
a. | covalent | c. | ionic | b. | metallic | d. | van der Waals |
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34.
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Which temperature is the same
as -13 °C?
a. | 773 K | b. | 260 K | c. | 747 K | d. | 286 K |
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35.
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As wavelength increases, what happens to Frequency and Energy?
a. | Both Decrease | c. | Frequency decreases, Energy increases | b. | Both
Increase | d. | Frequency
increases, Energy decreases |
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36.
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In the
reaction
an acid-base conjugate pair is
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37.
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1s22s22p63s23p64s1
is the electron configuration for which element?
a. | potassium (K) | c. | argon (Ar) | b. | calcium (Ca) | d. | aluminum (Al) |
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38.
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Which set of procedures and observations indicates a chemical change
a. | A solid is gently heated in a crucible and the solid slowly turns to liquid.
| b. | A cool, shiny metal is added to water in a beaker and rapid bubbling
occurs. | c. | Large crystals are crushed with a mortar and pestle and become
powder. | d. | Ethanol is added to an empty beaker and the ethanol eventually
disappears. |
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39.
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The solid block shown here has a mass of 146 grams. What is the
block’s density? a. | 54 g/cm3 | c. | 0.37 g/cm3 | b. | 2.7
g/cm3 | d. | 8.1
g/cm3 |
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40.
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What is the name for the compound FeS
a. | iron (III) sulfate | c. | iron (II) sulfide | b. | iron (II) sulfate | d. | iron (III)
sulfide |
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41.
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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. | more shielding of the electrons in the highest occupied energy
level | b. | an increase in number of protons | c. | an increase in size of the
nucleus | d. | fewer electrons in the highest occupied energy level |
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42.
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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. | 3.96
grams | c. | 1.50
grams | b. | 7.17 grams | d. | 1.98 grams |
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43.
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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. | 2.0 x 10-2 | c. | 1.0 x 10-2 | b. | 1.0 x 10-4 | d. | 1.0 x 102 |
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44.
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Which graph shows the
pressure-temperature realationship expected for an ideal gas?
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45.
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Given a pH of 3.8, which of the
following is true?
a. | can be neutralized by a strong
acid | c. | contains more H+ ions than
OH- | b. | Contains more OH- ions than H+ ions | d. | has a slightly basic pH |
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46.
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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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47.
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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 1014
Hz | b. | 4.57 x 10-7 Hz | d. | 4.57 x 10-6 Hz |
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48.
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What trend can be seen as the atomic number increases in period 3?
a. | decreasing first ionization energy | c. | decreasing atomic
mass | b. | increasing atomic radius | d. | increasing electronegativity |
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49.
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What is the name of the compound whose formula is
H2SO4?
a. | sulfurous acid | c. | hydrosulfuric acid | b. | sulfuric acid | d. | hydrosulfurous
acid |
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50.
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Which type of bond is formed by the transfer of electrons from one atom to
another?
a. | a covalent bond | c. | a hydrogen bond | b. | an ionic bond | d. | a coordinate covalent
bond |
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51.
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Given the
reaction:
How many moles of C6H12O6 (s) are needed to produce 24 moles of carbon
dioxide?
a. | 12
moles | b. | 24
moles | c. | 1.0
mole | d. | 4.0
moles |
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52.
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Which atom contains exactly 15 protons?
a. | phosphorous-32 | c. | sulfur-32 | b. | nitrogen-15 | d. | oxygen-15 |
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53.
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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. | 10.0
moles | b. | 30.0
mole | c. | 4.00
mole | d. | 8.00
moles |
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54.
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Which pair of elements form an ionic bond with each other?
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55.
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What is the pH of a 0.01 M
solution of KOH?
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56.
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Which of the following atoms has a smallest atomic radius?
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57.
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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. | 42.0 moles | c. | 33.6 moles | b. | 1.50 moles | d. | 0.667 moles |
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58.
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What is the Lewis dot structure for nitogen trifluoride (NF3)
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59.
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Which of the following is an example of a physical change?
a. | rusting of iron | c. | burning gasoline | b. | breaking glass | d. | lighting a match
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60.
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Which equation represents a
neutralization reaction?
a. | H2SO4(aq) + CaCO3(aq)  CaSO4(aq) + H2O(l)
+CO2(g) | b. | 2 HCl(aq) + Zn(s)  ZnCl2(aq) +
H2(g) | c. | CaO(s) + H2O(l) 
Ca(OH)2(aq) | d. | HNO3(aq) + KOH(aq) 
KNO3(aq) + H2O(l) |
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61.
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Metallic bonds occur between atoms of
a. | neon | b. | copper | c. | sulfur | d. | fluorine |
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62.
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Which sample of matter is a pure substance?
a. | air (O2, N2, CO2) | c. | hydrochloric acid solution (HCl +
H2O) | b. | salt water (NaCl + H2O) | d. | ammonia gas
(NH3) |
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63.
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What is the total number of molecules in 1.0 mole of Cl2 (g)?
a. | 35 | c. | 12 x 1024 | b. | 70 | d. | 6.02 x
1023 |
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64.
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What is the maximum number of orbitals in the p sublevel?
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65.
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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. | 5.10 x 10-19 J | c. | 6.92 x 10-31
J | b. | 2.59 x 10-40 J | d. | 3.90 x 10-7 J |
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66.
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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. | 1.48 x 10-18 J | c. | 1.33 x 10-18
J | b. | 4.42 x 10-3 J | d. | 2.96 x 10-19 J |
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67.
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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. | interaction between
the fixed orbitals of the unshared pairs of hydrogen | c. | the unusual location of the free
electrons | d. | ionic attraction and repulsion |
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68.
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Which of the following atoms have the largest atomic radius?
a. | magnesium (Mg) | c. | barium (Ba) | b. | iodine (I) | d. | chlorine (Cl) |
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69.
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What is the formula mass of calcium nitrate,
Ca(NO3)2?
a. | 150 g | c. | 164 g | b. | 70.0 g | d. | 102 g |
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70.
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An atom is electrically neutral because the
a. | number of protons equals the nubmer of electrons. | b. | ratio of the number
of neutrons to the number of protons is 2:1. | c. | ratio of the number of neutrons to the number
of electrons is 1:1. | d. | number of protons equals the number of
neutrons. |
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71.
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The correct formula for sodium oxide is
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72.
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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. | electrons and
protons | d. | protons and
electrons |
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73.
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Which of the following atoms has six valence electrons?
a. | magnesium (Mg) | c. | silicon (Si) | b. | sulfur (S) | d. | argon (Ar) |
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74.
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Which is the correct name of the compound with the formula
NH4NO2?
a. | ammonium nitrate | c. | ammonia nitrate | b. | ammonia nitrite | d. | ammonium
nitrite |
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75.
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According to the
Brønsted-Lowry definition, an acid is any species that can
a. | accept an
electron | c. | donate a
proton | b. | donate an electron | d. | accept a proton |
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76.
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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 combines with oxygen to form rust. | d. | Iron can be
flattened into sheets. |
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77.
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The gram molecular mass of Ca3(PO4)2 is
a. | 279 g | b. | 310 g | c. | 342 g | d. | 246
g |
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78.
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Which orbital notation shows the lowest energy arrangement of valence electrons
for 1s22s22p3?
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79.
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Which element within any given period of the Periodic Table would always have
the lowest first ionization energy?
a. | a noble gas | c. | a halogen | b. | an alkali metal | d. | an alkaline earth metal
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80.
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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. | AgCl | d. | NaNO3 |
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81.
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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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