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1.
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An atom of lithium-7 has an equal number of
a. | electrons and protons | c. | positrons and neutrons | b. | positrons and
protons | d. | electrons and
neutrons |
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2.
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The H3O+ ion concentration of a solution
is 1 x 10-4 M. This solution is
a. | basic and has a pH of
10 | c. | acidic and has a pH of
10 | b. | acidic and has a pH of
4 | d. | basic and has a pH of
4 |
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3.
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An atom is electrically neutral because the
a. | ratio of the number of neutrons to the number of electrons is
1:1. | b. | ratio of the number of neutrons to the number of protons is 2:1. | c. | number of protons
equals the nubmer of electrons. | d. | number of protons equals the number of
neutrons. |
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4.
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What is the formula mass of calcium nitrate,
Ca(NO3)2?
a. | 70.0 g | c. | 102 g | b. | 164 g | d. | 150 g |
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5.
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Which kind of bond is formed when two atoms share electrons to form a
molecule?
a. | metallic | b. | ionic | c. | covalent | d. | electovalent |
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6.
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What is the pH of a 0.01 M
solution of KOH?
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7.
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Which of the following atoms have the largest atomic radius?
a. | barium (Ba) | c. | magnesium (Mg) | b. | chlorine (Cl) | d. | iodine (I) |
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8.
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What is the percent mass oxygen in acetone (C3H6O)?
a. | 1.00 % | b. | 10.3 % | c. | 62.0 % | d. | 27.6
% |
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9.
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What is the total number of molecules in 1.0 mole of Cl2 (g)?
a. | 35 | c. | 70 | b. | 6.02 x 1023 | d. | 12 x
1024 |
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10.
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Which of the following models best represents the shape of a compound
with trigonal planar geometry?
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11.
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In a solution, litmus paper
turned blue. The pH of this solution could be
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12.
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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. | 6.92 x 10-31 J | c. | 5.10 x 10-19
J | b. | 2.59 x 10-40 J | d. | 3.90 x 10-7 J |
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13.
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Which pair of elements form an ionic bond with each other?
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14.
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What is the Lewis dot structure for nitogen trifluoride (NF3)
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15.
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Given a pH of 3.8, which of the
following is true?
a. | has a slightly basic
pH | c. | contains more H+ ions than
OH- | b. | can be neutralized by a strong acid | d. | Contains more OH- ions than H+
ions |
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16.
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How many moles of CH4 are contained in 96.0 grams of
CH4?
a. | 16.0 moles | c. | 6.00 moles | b. | 12.0 moles | d. | 3.00 moles |
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17.
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According to the Arrhenius definition, a substance that is classified as an acid
will always produce _______ in solution
a. | F-(aq) | b. | H+(aq) | c. | I-(aq) | d. | K+(aq) |
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18.
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In theory, how many grams of
H2O can be produced
according to the above information? (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. | 7.17
grams | c. | 1.98
grams | b. | 3.96 grams | d. | 1.50 grams |
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19.
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Which of the following is a correct Lewis dot structure for potassium
chloride?
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20.
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The correct formula for sodium oxide is
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21.
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Which of the following atoms has six valence electrons?
a. | silicon (Si) | c. | argon (Ar) | b. | sulfur (S) | d. | magnesium (Mg) |
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22.
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Which of the following is an example of a physical change?
a. | burning gasoline | c. | breaking glass | b. | rusting of iron | d. | lighting a match
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23.
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When the
reaction
is completely balanced using smallest whole numbers, the
coefficient of H2O will
be
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24.
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Which sample of matter is a pure substance?
a. | hydrochloric acid solution (HCl + H2O) | c. | salt water (NaCl +
H2O) | b. | ammonia gas (NH3) | d. | air (O2, N2,
CO2) |
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25.
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What formula represents lead (II) phosphate?
a. | Pb2(PO4)3 | c. | PbPO4 | b. | Pb3(PO4)2 | d. | Pb4PO4 |
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26.
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The bonds present in nitrogen dioxide (NO2) are
a. | ionic | c. | covalent | b. | metallic | d. | van der Waals |
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27.
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Which subatomic particles are located in the nucleus of a neon atom?
a. | protons and electrons | c. | electrons and protons | b. | electrons and
neutrons | d. | protons and
neutrons |
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28.
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Which is the correct name of the compound with the formula
NH4NO2?
a. | ammonia nitrate | c. | ammonium nitrite | b. | ammonium nitrate | d. | ammonia nitrite |
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29.
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Which graph shows the
pressure-temperature realationship expected for an ideal gas?
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30.
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What is the name for the compound FeS
a. | iron (II) sulfate | c. | iron (II) sulfide | b. | iron (III) sulfide | d. | iron (III)
sulfate |
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31.
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Carbon reacts with chlorine to form CCl4. What is the name of
this compound?
a. | tetracarbon chloride | c. | carbon 4-chloride | b. | carbon tetrachloride | d. | 1-carbon
4-chloride |
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32.
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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. | 4.42 x 10-3 J | c. | 2.96 x 10-19
J | b. | 1.33 x 10-18 J | d. | 1.48 x 10-18 J |
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33.
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What causes NH3 to have it’s shape, according to VSEPR
theory?
a. | interaction between the fixed orbitals of the unshared pairs of
hydrogen | b. | the unusual location of the free electrons | c. | repulsive forces
between unshared pairs of electrons and bonds | d. | ionic attraction and
repulsion |
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34.
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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 = 5 to 1 | b. | Energy Level = 5 to
2 | c. | Energy Level= 6 to 5 | d. | Energy Level = 4 to
5 |
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35.
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Which of the following elements has the smallest atomic radius?
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36.
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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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37.
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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. | Ethanol is added to an empty beaker and the ethanol eventually
disappears. | c. | Large crystals are crushed with a mortar and pestle and become
powder. | d. | A cool, shiny metal is added to water in a beaker and rapid bubbling
occurs. |
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38.
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Given the
reaction:
How many moles of C6H12O6 (s) are needed to
produce 24 moles of carbon dioxide?
a. | 24
moles | b. | 1.0
mole | c. | 4.0
moles | d. | 12
moles |
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39.
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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. | 4.57 x 1014 Hz | c. | 4.57 x 10-7
Hz | b. | 4.57 x 10-6 Hz | d. | 1.97 x 1014 Hz |
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40.
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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. | Solid at room temperature | c. | Mostly
unreactive | b. | Gaseous at room temperature and highly reactive | d. | Solid at room temperature and mostly unreactive
with strong acids |
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41.
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The gram molecular mass of Ca3(PO4)2 is
a. | 310 g | b. | 246 g | c. | 279 g | d. | 342
g |
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42.
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Which of the following elements has an electron configuration of
1s22s22p63s23p1?
a. | phosphorous | c. | lithium | b. | calcium | d. | aluminum |
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43.
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What is the total number of electrons present in an atom of  ?
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44.
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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. | 2.50 mol | d. | 1.50 mol |
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45.
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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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46.
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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. | 8.1
g/cm3 | d. | 2.7
g/cm3 |
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47.
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What is the name of the compound whose formula is
H2SO4?
a. | sulfurous acid | c. | sulfuric acid | b. | hydrosulfurous acid | d. | hydrosulfuric
acid |
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48.
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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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49.
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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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50.
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As wavelength increases, what happens to Frequency and Energy?
a. | Frequency increases, Energy decreases | c. | Both Decrease | b. | Both
Increase | d. | Frequency
decreases, Energy increases |
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51.
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What is the maximum number of orbitals in the p sublevel?
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52.
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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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53.
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Which atom contains exactly 15 protons?
a. | oxygen-15 | c. | sulfur-32 | b. | phosphorous-32 | d. | nitrogen-15 |
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54.
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Metallic bonds occur between atoms of
a. | copper | b. | fluorine | c. | sulfur | d. | neon |
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55.
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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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56.
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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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57.
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Which type of bond is formed by the transfer of electrons from one atom to
another?
a. | an ionic bond | c. | a covalent bond | b. | a coordinate covalent bond | d. | a hydrogen bond |
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58.
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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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59.
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According to the
Brønsted-Lowry definition, an acid is any species that can
a. | donate an
electron | c. | accept an
electron | b. | donate a proton | d. | accept a proton |
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60.
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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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61.
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A neon sign is being made with 80 grams of neon. How many atoms are
contained the neon sign?
a. | 6.02 x 1023 atoms | c. | 2.40 x 1024
atoms | b. | 1.20 x 1024 atoms | d. | 4.80 x 1024
atoms |
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62.
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In the
reaction
an acid-base conjugate pair is
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63.
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1s22s22p63s23p64s1
is the electron configuration for which element?
a. | potassium (K) | c. | aluminum (Al) | b. | calcium (Ca) | d. | argon (Ar) |
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64.
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Given the balanced
equation:
AgNO3 + NaCl  NaNO3 +
AgCl
Which compound would
precipitate out of the reaction?
a. | AgCl | c. | NaNO3 | b. | NaCl | d. | AgNO3
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65.
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Beryllium is classified as
a. | an alkali metal | c. | a transition metal | b. | an alkaline earth metal | d. | a noble gas |
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66.
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Which of the following atoms has a smallest atomic radius?
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67.
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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. | 36.0 amu | b. | 35.0 amu | c. | 35.5 amu | d. | 37.0
amu |
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68.
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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. | 6.0 x 10- 7 m | d. | 1.7 x 106 m |
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69.
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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. | 0.25 M | c. | 0.33 M | d. | 1.0 M |
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70.
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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. | 42.0 moles | b. | 33.6 moles | d. | 1.50 moles |
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71.
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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. | an alkali metal | b. | a halogen | d. | an alkaline earth metal
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72.
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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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73.
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Chemical equations must be balanced to satisfy
a. | the law of conservation of mass. | b. | the law of definite
proportions. | c. | Avogadro’s principle. | d. | the law of multiple
proportions. |
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74.
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Which statement describes a chemical property of iron?
a. | Iron combines with oxygen to form rust. | b. | Iron conducts
electricity and heat. | c. | Iron can be flattened into
sheets. | d. | Iron can be drawn into a wire. |
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75.
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Which orbital notation shows the lowest energy arrangement of valence electrons
for 1s22s22p3?
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76.
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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. | 3.00 M | b. | 1.00 M | c. | 4.00 M | d. | 2.00 M |
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