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1.
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Which set of procedures and observations indicates a chemical change
a. | Ethanol is added to an empty beaker and the ethanol eventually
disappears. | b. | A solid is gently heated in a crucible and the solid slowly turns to liquid.
| 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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2.
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Which of the following is an example of a physical change?
a. | lighting a match | c. | burning gasoline | b. | breaking glass | d. | rusting of iron |
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3.
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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. | 8.1 g/cm3 | b. | 2.7 g/cm3 | d. | 54
g/cm3 |
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4.
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Which statement describes a chemical property of iron?
a. | Iron can be flattened into sheets. | b. | Iron conducts electricity and
heat. | c. | Iron combines with oxygen to form rust. | d. | Iron can be drawn
into a wire. |
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5.
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Which sample of matter is a pure substance?
a. | air (O2, N2, CO2) | c. | hydrochloric acid solution (HCl +
H2O) | b. | ammonia gas (NH3) | d. | salt water (NaCl +
H2O) |
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6.
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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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7.
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Which subatomic particles are located in the nucleus of a neon atom?
a. | electrons and protons | c. | protons and neutrons | b. | electrons and
neutrons | d. | protons and
electrons |
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8.
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An atom is electrically neutral because the
a. | number of protons equals the nubmer of electrons. | b. | number of protons
equals the number of neutrons. | c. | ratio of the number of neutrons to the number
of electrons is 1:1. | d. | ratio of the number of neutrons to the number
of protons is 2:1. |
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9.
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An atom of lithium-7 has an equal number of
a. | electrons and neutrons | c. | positrons and neutrons | b. | electrons and
protons | d. | positrons and
protons |
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10.
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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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11.
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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. | 35.0 amu | b. | 35.5 amu | c. | 36.0 amu | d. | 37.0
amu |
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12.
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Which atom contains exactly 15 protons?
a. | phosphorous-32 | c. | oxygen-15 | b. | sulfur-32 | d. | nitrogen-15 |
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13.
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What is the total number of electrons present in an atom of  ?
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14.
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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. | 6.0 x 10- 7 m
| b. | 1.7 x 106 m | d. | 2.0 x 10-15 m |
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15.
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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. | 2.59 x 10-40 J | c. | 5.10 x 10-19
J | b. | 6.92 x 10-31 J | d. | 3.90 x 10-7 J |
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16.
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Beryllium is classified as
a. | an alkaline earth metal | c. | a transition metal
| b. | an alkali metal | d. | a noble gas |
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17.
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Which group contains elements with a total of four electrons in the outermost
energy level (valence shell)?
a. | Group 1A | b. | Group 2A | c. | Group 4A | d. | Group
6A |
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18.
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Which of the following atoms has a smallest atomic radius?
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19.
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Which element within any given period of the Periodic Table would always have
the lowest first ionization energy?
a. | an alkali metal | c. | an alkaline earth metal | b. | a
halogen | d. | a noble
gas |
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20.
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What trend can be seen as the atomic number increases in period 3?
a. | increasing atomic radius | c. | decreasing atomic
mass | b. | increasing electronegativity | d. | decreasing first ionization
energy |
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21.
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Which pair of elements form an ionic bond with each other?
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22.
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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. | a coordinate covalent bond | d. | an ionic bond |
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23.
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Which kind of bond is formed when two atoms share electrons to form a
molecule?
a. | ionic | b. | metallic | c. | electovalent | d. | covalent |
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24.
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The bonds present in nitrogen dioxide (NO2) are
a. | covalent | c. | metallic | b. | ionic | d. | van der Waals |
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25.
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Metallic bonds occur between atoms of
a. | fluorine | b. | neon | c. | sulfur | d. | copper |
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26.
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Which of the following atoms have the largest atomic radius?
a. | barium (Ba) | c. | iodine (I) | b. | chlorine (Cl) | d. | magnesium (Mg) |
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27.
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Which of the following atoms has six valence electrons?
a. | magnesium (Mg) | c. | sulfur (S) | b. | silicon (Si) | d. | argon (Ar) |
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28.
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1s22s22p63s23p64s1
is the electron configuration for which element?
a. | aluminum (Al) | c. | potassium (K) | b. | argon (Ar) | d. | calcium (Ca) |
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29.
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Which of the following elements has an electron configuration of
1s22s22p63s23p1?
a. | lithium | c. | phosphorous | b. | aluminum | d. | calcium |
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30.
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What is the Lewis dot structure for nitogen trifluoride (NF3)
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31.
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Which of the following is a correct Lewis dot structure for potassium
chloride?
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32.
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Which orbital notation shows the lowest energy arrangement of valence electrons
for 1s22s22p3?
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33.
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Which of the following models best represents the shape of a compound
with trigonal planar geometry?
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34.
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Which is the correct name of the compound with the formula
NH4NO2?
a. | ammonia nitrite | c. | ammonia nitrate | b. | ammonium nitrite | d. | ammonium
nitrate |
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35.
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The correct formula for sodium oxide is
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36.
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What is the name of the compound whose formula is
H2SO4?
a. | hydrosulfuric acid | c. | sulfuric acid | b. | hydrosulfurous acid | d. | sulfurous acid |
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37.
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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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38.
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What is the name for the compound FeS
a. | iron (II) sulfate | c. | iron (II) sulfide | b. | iron (III) sulfate | d. | iron (III)
sulfide |
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39.
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Carbon reacts with chlorine to form CCl4. What is the name of
this compound?
a. | carbon 4-chloride | c. | tetracarbon chloride | b. | 1-carbon 4-chloride | d. | carbon
tetrachloride |
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40.
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The gram molecular mass of Ca3(PO4)2 is
a. | 246 g | b. | 279 g | c. | 310 g | d. | 342
g |
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41.
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What is the total number of molecules in 1.0 mole of Cl2 (g)?
a. | 35 | c. | 6.02 x 1023 | b. | 70 | d. | 12 x
1024 |
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42.
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How many moles of CH4 are contained in 96.0 grams of
CH4?
a. | 3.00 moles | c. | 12.0 moles | b. | 6.00 moles | d. | 16.0 moles |
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43.
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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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44.
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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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45.
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When the
reaction
is completely balanced using smallest whole numbers, the
coefficient of H2O will
be
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46.
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The covalent bonds in water are
polar because
a. | H is more electronegative than
O. | c. | O is more electronegative than
H. | b. | O and H are equally
electronegative. | d. | water molecules are
cohesive. |
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47.
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Given the
reaction:
How many moles of C6H12O6 (s) are needed to
produce 24 moles of carbon dioxide?
a. | 4.0
moles | b. | 1.0
mole | c. | 24
moles | d. | 12
moles |
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48.
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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. | 1.98
grams | c. | 7.17
grams | b. | 1.50 grams | d. | 3.96 grams |
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49.
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Which graph shows the
pressure-temperature realationship expected for an ideal gas?
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50.
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Which temperature is the same
as -13 °C?
a. | 286 K | b. | 773 K | c. | 747 K | d. | 260 K |
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51.
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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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52.
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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. | 1.00 M | b. | 2.00 M | c. | 4.00 M | d. | 3.00 M |
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53.
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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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54.
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Which equation represents a
neutralization reaction?
a. | HNO3(aq) + KOH(aq) 
KNO3(aq) + H2O(l) | b. | 2 HCl(aq) + Zn(s)  ZnCl2(aq) +
H2(g) | c. | CaO(s) + H2O(l) 
Ca(OH)2(aq) | d. | H2SO4(aq) + CaCO3(aq) 
CaSO4(aq) + H2O(l)
+CO2(g) |
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55.
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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. | accept a proton | d. | donate a proton |
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56.
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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 OH- ions than H+
ions | b. | contains more H+ ions than OH- | d. | can be neutralized by a strong
acid |
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57.
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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. | I-(aq) | d. | K+(aq) |
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58.
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In the
reaction
an acid-base conjugate pair is
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59.
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In a solution, litmus paper
turned blue. The pH of this solution could be
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60.
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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
4 | c. | acidic and has a pH of
4 | b. | basic and has a pH of
10 | d. | acidic and has a pH of
10 |
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61.
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What is the pH of a 0.01 M
solution of KOH?
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62.
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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 = 4 to 5 | c. | Energy Level=
6 to 5 | d. | Energy Level = 5 to 2 |
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63.
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What is the maximum number of orbitals in the p sublevel?
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64.
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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 size of the nucleus | c. | an increase in number of
protons | d. | fewer electrons in the highest occupied energy level |
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65.
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Which of the following elements has the smallest atomic radius?
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66.
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As wavelength increases, what happens to Frequency and Energy?
a. | Both Increase | c. | Frequency increases, Energy decreases | b. | Both
Decrease | d. | Frequency
decreases, Energy increases |
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67.
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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. | Mostly
unreactive | b. | Solid at room temperature | d. | Solid at room temperature and mostly unreactive with strong
acids |
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68.
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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. | 1.97 x 1014
Hz | b. | 4.57 x 10-6 Hz | d. | 4.57 x 10-7 Hz |
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69.
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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. | 1.33 x 10-18 J | c. | 2.96 x 10-19
J | b. | 1.48 x 10-18 J | d. | 4.42 x 10-3 J |
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70.
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What is the formula mass of calcium nitrate,
Ca(NO3)2?
a. | 164 g | c. | 102 g | b. | 150 g | d. | 70.0 g |
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71.
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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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72.
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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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73.
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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. | 33.6 moles | b. | 1.50 moles | d. | 42.0 moles |
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74.
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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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75.
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Chemical equations must be balanced to satisfy
a. | the law of definite proportions. | b. | the law of multiple
proportions. | c. | the law of conservation of mass. | d. | Avogadro’s
principle. |
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76.
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What causes NH3 to have it’s shape, according to VSEPR
theory?
a. | the unusual location of the free electrons | b. | repulsive forces
between unshared pairs of electrons and bonds | c. | interaction between the fixed orbitals of the
unshared pairs of hydrogen | d. | ionic attraction and
repulsion |
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