True/False
Indicate whether the statement is true or
false.
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1.
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All samples of the same substance have the same density.
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2.
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Objects with a density greater than water will sink in water.
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3.
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Density can be expressed in g/ml or g/cm3.
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4.
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Absolute Zero, 0K = 273°C
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5.
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Compounds are two or more substances which are not chemically
comined
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6.
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The following graph shows a DIRECT relationship between Volume and
Pressure.
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7.
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Increasing the number of particles, heating, or decreasing volume will all cause
an increase in pressure.
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8.
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An isotope is an element with a positive or negative
charge.
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9.
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the resulting energy from electrons moving from lower to higher energy levels is
what causes the colored light that is produced in flame tests and neon lights.
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10.
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The modern periodic table (the one that we use now) is arranged in order of
increasing atomic number.
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11.
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Non-metals are located in the upper right hand side of the periodic
table.
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12.
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Ionic bonds are formed by the sharing of electrons.
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13.
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In a chemical reaction, the products are found on the left side of the
arrow.
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14.
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A precipitate forms when two aqueous solutions react to form a product that
cannot dissolve in water.
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15.
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Something that is insoluble will NOT dissolve in
water
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16.
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The solute is what dissolves the solvent in a solution.
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17.
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A pH value of 10 is considered to be neutral.
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Matching
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Match the energy level with the maximum number of electrons that it can
hold.
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18.
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the third evergy level
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19.
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the first energy level
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20.
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the second energy level
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Multiple Choice
Identify the choice that best completes the
statement or answers the question.
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21.
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Which of the following indicates a quantitative measurement?
a. | cold | c. | big | b. | 55.0 g | d. | yellow |
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22.
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Which of the following is a physical property?
a. | Melting point | c. | color | b. | density | d. | all of the
above |
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23.
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Which is the correct measurement for location marked by the arrow?
 a. | 60.25 | c. | 62.7 | b. | 62 | d. | 62.659 |
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24.
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What is the measurement 0.000 024 cm in proper scientific
notation?
a. | 2.40 x 10-5cm. | c. | 240 x 10-4cm.
| b. | 2.40 x 10-4 cm. | d. | 2.40 x 10-6cm. |
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25.
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An object has a mass of 18.5 kg. What is the mass of the
object in
grams? (1000 g = 1 kg)
a. | 1.85 x 104 g | c. | 185 x 10-1
g | b. | 18.5 x 103 g | d. | 1.85 x 10-4 g |
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26.
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What is the volume of the following rock?
 a. | 30 mL | c. | 70 mL | b. | 40 mL | d. | 10 mL |
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27.
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A group of students performed an experiment to calculate the mass of a
substance. The accepted value for the mass should be 2.85 grams. The group recorded the
following measurements after performing the experiment three times. Which statement correctly
describes the experimental data?Trial | Measurement | 1 | 2.01 | 2 | 3.05 | 3 | 2.75 | | |
a. | Precise but not accurate | c. | Accurate but not
precise | b. | Both accurate and precise | d. | Neither accurate nor precise |
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28.
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Silver, Copper and Oxygen are all:
a. | elements | c. | mixtures | b. | compounds | d. | metals |
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29.
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Which of the following is NOT a state of matter
a. | solid | c. | cold | b. | gas | d. | liquid |
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30.
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According to the Kinetic Molecular Theory, which of the following is not in
motion?
a. | solids | c. | gases | b. | liquids | d. | none of these are
correct. |
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31.
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Which of the following states of matter has the MOST amount of energy?
a. | solids | c. | gases | b. | liquids | d. | none of these have
energy. |
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32.
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The process by which particles gain enough energy at the surface of a
liquid to become a gas is known as?
a. | Evaporation | c. | Freezing | b. | Deposition | d. | Sublimation |
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33.
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Between which two points does thermal energy increase and
boiling occur for water?
 a. | A to B | c. | C to D | b. | B to C | d. | D to E |
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34.
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Accoriding to Boyle’s law, when volume decreases at a constant temperature
the following will happen:
a. | pressure stays the same | c. | pressure
increases | b. | pressure decreases | d. | none of the above |
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35.
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According to Bohr’s model of the atom, electrons must:
a. | not exist. | b. | be anywhere they want outside of the
nucleus. | c. | reside in the nucleus. | d. | move in “orbits” around the nucleus
like planets. |
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36.
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Which of the following are found inside the nucleus?
a. | protons | b. | neutrons | c. | electrons | d. | a and
b | e. | a
and c |
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37.
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The number of protons in an atom is always the same as it’s
a. | mass number | c. | isotope number | b. | atomic number | d. | nuetrons |
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38.
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Atoms are neutral when:
a. | protons and neutrons are equal | c. | protons and electrons are
equal | b. | neutrons and electrons are equal | d. | none of these are
correct. |
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39.
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24. Which of the following combinations describes an ion with a positive two
charge?
a. | 1 protons; 0 neutrons; 2 electrons | c. | 20 protons; 20 neutrons; 18
electrons | b. | 15 protons; 16 neutrons; 15 electrons | d. | 11 protons; 12 neutrons; 10
electrons |
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40.
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An atom’s mass number is the total of the:
a. | protons and neutrons | c. | protons and electrons | b. | neutrons and
electrons | d. | protons, neutrons
and electrons |
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41.
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Two neutral isotopes of the same element have a different number of:
a. | protons | b. | neutrons | c. | electrons | d. | a and
b | e. | a
and c |
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42.
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Which pair of symbols correctly represents two isotopes of the same
element?
a. |
 | c. |
 | b. |
 | d. | none of these represent
isotopes. |
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43.
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Which is the net charge on a particle that consists of 11 protons, 12
neutrons, and 10 electrons?
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44.
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Which is the mass number on a particle that consists of 11 protons, 12
neutrons, and 10 electrons?
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45.
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Which is the number of electrons in the Mg2+ ion?
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46.
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Lithium has an atomic mass of 6.9. which is the best explanation for
this?
a. | all lithium atoms have 6.9 mass units in their nuclei. | b. | The weighted average
of all lithium isotopes is 6.9. | c. | all lithium atoms have a mass of
6.9. |
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47.
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The amount of time that it takes for 1/2 of the mass of a radioactive isotope to
decay is known as a radioisotope’s:
a. | decay time | c. | half time | b. | radioactive time | d. | half life |
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48.
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The strongest type of radiation is known as:
a. | beta radiation | c. | alpha radiation | b. | gamma radiation | d. | delta radiation |
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49.
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Complete the following alha decay of Uranium-238
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50.
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Dimitri Mendeleev was known for his work on:
a. | I’ve never heard of him. | c. | the discovery of the
proton. | b. | his model of the atom | d. | the first periodic table. |
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51.
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Which of the following elements is most similar in properties to Nitrogen,
N?
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52.
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The energy level of the valence shell ist he same as the ________ that an
element can be found in.
a. | period number | c. | atomic number | b. | mass number | d. | group number |
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53.
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Element number 37 is a(n):
a. | halogen | c. | alkali metal | b. | transition metal | d. | alkaline earth
metal |
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54.
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Which of the following is a transition metal?
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55.
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Which of the following elements are BOTH noble gases?
a. | N and Ne | c. | Ne and Xe | b. | Cl and F | d. | H and He |
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56.
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From the top of the column 1 to the bottom of column 1 on the periodic
table:
a. | atomic radius decreases | c. | reactivity
decreases | b. | atomic mass decreases | d. | atomic radius increases |
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57.
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Which element will have the same number of electrons as
Ar when it forms a bond?
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58.
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Which of the following is the correct number of valence electrons for Ca?
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59.
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Which of the following has a full set of valence electrons?
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60.
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How does K achieve a stable octet?
a. | it gains 1 electron | c. | it loses 1 electron | b. | it gains 7 electrons | d. | it does not do
anything |
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61.
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w does an ionically bonded compound such as, potassium chloride
(KCl) formed?
a. | A potassium atom loses an electron to chlorine to form an ionic
bond. | b. | a chlorine atom loses seven electrons to form a cation and potassium atom gains seven
electrons to form an ionic bond. | c. | potassium and chlorine do not form a
bond. |
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62.
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Which of the following is true for ionic compounds?
a. | high melting and boiling points | c. | usually solid at room
temperature | b. | conduct electricity in water | d. | all of the
above |
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63.
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In an ionic compound of potassium oxide, the potassium ion has a charge
of 1+ and the oxide ion has a charge of 2-. Which of the following is the
formula for potassium oxide?
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64.
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A structural formula with a triple covalent bond will have how many dashes
between two atoms?
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65.
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What is the name of LiF?
a. | lithium fluoride | c. | lithium monofluoride | b. | monolithium monofluoride | d. | Monolithium
fluoride |
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66.
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The type of formula that uses dashes to represent bonds is known as what type of
formula? Example:
 a. | math formula | c. | dash formula | b. | structure formula | d. | dot formula |
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67.
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How many oxygens are shown in the formula?:
Mg3(PO4)2
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68.
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What is the molar mass of NaOH?
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69.
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Complete the following statement of equality: 1 mol N = _?_ grams N = 6.02 x 1023 N
atoms
a. | 14 | b. | 7 | c. | 0 | d. | none of these |
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70.
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What is the mass of 2 moles of He atoms?
a. | 2 g | c. | 8 g | b. | 4 g | d. | 1.20 x 1024
g |
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71.
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Which of the following has the greatest mass?
a. | 1 mol of Ag | c. | 1 mol of Au | b. | 1 mol of Al | d. | 1 mol of Ar |
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72.
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The percentage composition of carbon in CH4 is about 75%. What ist
he percentage of hydrogen in this compound?
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73.
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The approximate mass of one silicon atom is about equal to:
a. | one half the mass of one nitrogen molecule (N2) | b. | the mass of one
nitrogen atom (N) | c. | the mass of one nitrogen molecule
(N2) |
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74.
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To calculate the Molarity of a solution, you mus calculate:
a. | liters per grams. | c. | moles per liters. | b. | grams per liters. | d. | iters per
moles. |
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75.
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According to the law of conservation of mass, the total mass of the
reactants are
a. | always more than the total mass of the products. | b. | always less than the
total mass of the products. | c. | sometimes more and sometimes less than the
total mass of the products. | d. | always equal to the total mass of the
products. |
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76.
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In this equation, which are the reactant(s)?
 a. |
Mg only | c. | Mg + 02 | b. | Mg0 only | d. | 02 only |
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77.
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Which is the name of the kind of solid substance formed in this
figure?
 a. | aqueous | c. | coordinate complex | b. | precipitate | d. | synthesis |
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78.
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In the reaction represented by the equation N2 + 3H2
® 2NH3, what is the mole ratio of hydrogen to ammonia?
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79.
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For the reaction represented by the equation C + 2H2
®
CH4,
how many moles of hydrogen are required to produce 4 mol of methane,
CH4?
a. | 3 mol | b. | 4 mol | c. | 8 mol | d. | 1
mol |
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80.
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Which describes the function of a catalyst?
a. | It speeds up a reaction. | c. | It makes a reaction
exothermic. | b. | It slows down a reaction. | d. | It makes a reaction endothermic. |
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81.
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The coefficients in a chemical equation represent the
a. | masses, in grams, of all reactants and products. | b. | relative numbers of
moles of reactants and products. | c. | number of atoms in each compound in a
reaction. | d. | number of valence electrons involved in the reaction. |
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82.
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What type of chemical reaction releases energy to it’s
surroundings?
a. | endothermic | b. | exothermic | c. | both endothermic and
exothermic | d. | neither endothermic nor exothermic |
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83.
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Which type of chemical reaction is shown?
 a. | double replacement | c. | synthesis | b. | combustion | d. | decomposition |
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84.
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Which type of reaction is Al + O2
® Al2O3?
a. | synthesis | c. | single replacement | b. | decomposition | d. | combustion |
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85.
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What are the correct coefficients when this equation is balanced?
____K
+ ____Br2 ®
____KBr
a. | 1, 1, 1 | c. | 2, 1, 2 | b. | 1, 2, 1 | d. | 2, 1, 1 |
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86.
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Which type of chemical reaction would this be classified as always producing
carbon dioxide and water like the following:
C3H8
+ O2 ® CO2 +
H2O
a. | synthesis | c. | combustion | b. | double replacement | d. | decomposition |
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87.
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How many grams of hydrogen will be required to produce 32.0 grams of methane
from reacting 24 grams of carbon? given:
Hint: plug in the numbers
C +
2H2 ® CH4
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88.
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What mass of methane is produced when 36.0 grams of carbon react with 12 grams
of hydrogen?
given:
C + 2H2
® CH4
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89.
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When an acid is mixed with a base, __________________ occurs.
a. | a physical change | c. | neutralization | b. | acidification | d. | nothing |
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90.
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The following can be indications of an exothermic chemical change during a
reaction where NO HEAT IS ADDED.
a. | bubbles and gas form | c. | both of these | b. | heat is produced | d. | neither of
these |
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