Matching (Value 22)
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Match each item with the correct statement below. a. | electronegativity | f. | periodic law | b. | ionization energy | g. | cation | c. | atomic
radius | h. | period | d. | metal | i. | group | e. | transition
metal | j. | electrons |
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1.
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type of element that is a good conductor of heat and electric current
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2.
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horizontal row in the periodic table
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3.
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type of ion formed by Group 2A elements
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4.
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ability of an atom to attract electrons when the atom is in a compound
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5.
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vertical column in the periodic table
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6.
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energy required to remove an electron from an atom
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7.
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type of element characterized by the presence of electrons in the d
orbital
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8.
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A repetition of properties occurs when elements are arranged in order of
increasing atomic number.
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Match each item with the correct statement below. a. | monatomic ion | f. | cation | b. | acid | g. | binary compound | c. | base | h. | anion | d. | law of definite proportions | i. | polyatomic ion | e. | law of multiple
proportions |
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9.
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compound composed of two different elements
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10.
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consists of a single atom with a positive or negative charge
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11.
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tightly-bound group of atoms that behaves as a unit and carries a net
charge
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12.
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produces a hydrogen ion when dissolved in water
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13.
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atom or group of atoms having a positive charge
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14.
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atom or group of atoms having a negative charge
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15.
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produces a hydroxide ion when dissolved in water
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Match each item with the correct statement below. a. | halide ion | e. | valence electron | b. | octet rule | f. | coordination number | c. | ionic
bond | g. | metallic
bond | d. | electron dot structure |
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16.
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a depiction of valence electrons around the symbol of an element
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17.
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an electron in the highest occupied energy level of an atom
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18.
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the number of ions of opposite charge surrounding each ion in a crystal
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19.
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the force of attraction binding oppositely charged ions together
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20.
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Atoms react so as to acquire the stable electron structure of a noble
gas.
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21.
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an anion of chlorine or other halogen
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22.
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the attraction of valence electrons for metal ions
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Multiple Choice (Value 55)
Identify the choice that best completes the statement or answers
the question.
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23.
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What element in the second period has the largest atomic radius?
a. | potassium | c. | carbon | b. | lithium | d. | neon |
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24.
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How many energy sublevels are in the second principal energy level?
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25.
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The atomic number of an element is the total number of which particles in the
nucleus?
a. | electrons | c. | protons | b. | protons and electrons | d. | neutrons |
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26.
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What distinguishes a substance from a mixture?
a. | Mixtures can be separated physically, while compounds cannot. | b. | Mixtures are
groupings of elements, and compounds are not. | c. | Substances are compounds, and mixtures are
not. | d. | Samples of the same substance can have different intensive
properties. |
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27.
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Which of the following elements is in the same period as phosphorus?
a. | nitrogen | c. | oxygen | b. | carbon | d. | magnesium |
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28.
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Which step in the scientific method requires you to use your senses to obtain
information?
a. | designing an experiment | c. | stating a
theory | b. | making an observation | d. | revising a hypothesis |
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29.
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What is the formula of the ion formed when phosphorus achieves a noble-gas
electron configuration?
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30.
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What is the formula for hydrosulfuric acid?
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31.
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Which of the following electron configurations gives the correct arrangement of
the four valence electrons of the carbon atom in the molecule methane (CH  )?
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32.
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Which electron configuration of the 4f energy sublevel is the most
stable?
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33.
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What do chemical symbols and formulas represent, respectively?
a. | elements and ions | b. | atoms and mixtures | c. | compounds and
mixtures | d. | elements and compounds |
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34.
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What is the relative mass of an electron?
a. | 1/1840 the mass of an alpha particle | c. | 1/1840 the mass of a neutron +
proton | b. | 1/1840 the mass of a hydrogen atom | d. | 1/1840 the mass of a C-12
atom |
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35.
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Which of the forces of molecular attraction is the weakest?
a. | hydrogen bond | c. | single covalent bond | b. | dipole interaction | d. | dispersion |
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36.
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What are the weakest attractions between molecules?
a. | hydrogen forces | c. | Van der Waals forces | b. | covalent forces | d. | ionic forces |
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37.
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Which of the following covalent bonds is the most polar?
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38.
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Which of the following statements is NOT true about ions?
a. | Charges for ions are written as numbers followed by a plus or minus
sign. | b. | When a cation forms, more electrons are transferred to it. | c. | Cations are
positively charged ions. | d. | Anions are common among
nonmetals. |
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39.
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Which of the following is a chemical property?
a. | hardness | c. | color | b. | freezing point | d. | ability to react with
oxygen |
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40.
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What must be done to be certain that a chemical change has taken place?
a. | Check for the production of bubbles before and after the change. | b. | Check the
composition of the sample before and after the change. | c. | Demonstrate that a release of energy occurred
after the change. | d. | Demonstrate that energy was absorbed by the
reactants after the change. |
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41.
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How many valence electrons are transferred from the calcium atom to iodine in
the formation of the compound calcium iodide?
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42.
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What is the shape of a molecule with a triple bond?
a. | tetrahedral | c. | pyramidal | b. | linear | d. | bent |
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43.
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Atomic size generally ____.
a. | increases as you move from left to right across a period | b. | remains constant
within a period | c. | decreases as you move from left to right across a period | d. | decreases as you
move from top to bottom within a group |
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44.
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When naming a transition metal ion that can have more than one common ionic
charge, the numerical value of the charge is indicated by a ____.
a. | Roman numeral following the name | c. | suffix | b. | prefix | d. | superscript after the name |
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45.
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A substance that forms a vapor is generally in what physical state at room
temperature?
a. | gas | c. | liquid | b. | solid | d. | liquid or solid |
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46.
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Which subatomic particle plays the greatest part in determining the properties
of an element?
a. | proton | c. | neutron | b. | electron | d. | none of the
above |
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47.
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Of the elements Fe, Hg, U, and Te, which is a representative element?
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48.
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Of the following elements, which one has the smallest first ionization
energy?
a. | aluminum | c. | carbon | b. | silicon | d. | boron |
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49.
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Which of the following does NOT involve a physical change?
a. | decomposing | c. | mixing | b. | melting | d. | grinding |
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50.
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Which of the following elements has the smallest first ionization energy?
a. | calcium | c. | magnesium | b. | potassium | d. | sodium |
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51.
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Why is hydrogen bonding only possible with hydrogen?
a. | Hydrogen’s nucleus is electron deficient when it bonds with an electronegative
atom. | b. | Hydrogen is the only atom that is the same size as an oxygen
atom. | c. | Hydrogen is the most electronegative element. | d. | Hydrogen tends to
form covalent bonds. |
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52.
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What type of compound is CuSO  ? a. | polyatomic covalent | c. | polyatomic ionic | b. | monotomic ionic | d. | binary
molecular |
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53.
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What is the formula unit of sodium nitride?
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54.
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Select the correct symbol for an atom of tritium.
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55.
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Which element, when combined with fluorine, would most likely form an ionic
compound?
a. | lithium | c. | chlorine | b. | carbon | d. | phosphorus |
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56.
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The side-by-side overlap of p orbitals produces what kind of bond?
a. | beta bond | c. | sigma bond | b. | alpha bond | d. | pi bond |
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57.
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When paper turns yellow-brown upon exposure to sunlight, what type of change is
likely taking place?
a. | a physical change | b. | a chemical change | c. | neither a physical
change nor a chemical change | d. | both a physical change and a chemical
change |
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58.
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What causes the shielding effect to remain constant across a period?
a. | Electrons are added to different principal energy levels. | b. | The charge on the
nucleus is constant. | c. | The atomic radius increases.
| d. | Electrons are added to the same principal energy
level. |
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59.
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In which of the following sets is the symbol of the element, the number of
protons, and the number of electrons given correctly?
a. | Zn, 30 protons, 60 electrons | c. | In, 49 protons, 49
electrons | b. | F, 19 protons, 19 electrons | d. | Cs, 55 protons, 132.9 electrons |
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60.
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Which of the following is NOT an example of chemistry research in the main area
of energy?
a. | determining the usefulness of oil from soybean plants | b. | studying the effects
of insulation | c. | developing rechargeable batteries | d. | producing hook-and-loop
tape |
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61.
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The atomic number of an element is the total number of which particles in the
nucleus?
a. | protons and electrons | c. | protons | b. | electrons | d. | neutrons |
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62.
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An -ate or -ite at the end of a compound name usually indicates
that the compound contains ____.
a. | fewer electrons than protons | c. | a polyatomic
anion | b. | only two elements | d. | neutral molecules |
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63.
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Which of the following can be observed only in a microscopic view?
a. | shape of a soybean plant | c. | X-ray of a knee
joint | b. | structure of a muscle cell | d. | foam insulation |
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64.
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A molecule with a single covalent bond is ____.
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65.
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Which of the following does NOT indicate that a chemical change may have taken
place?
a. | precipitate formation | c. | energy transfer | b. | gas production | d. | fracture
formation |
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66.
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How are chemical formulas of binary ionic compounds generally written?
a. | cation on left, anion on right | b. | anion on left, cation on
right | c. | subscripts first, then ions | d. | Roman numeral first, then anion, then
cation |
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67.
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In the chemical reaction in which sucrose is heated and decomposes to form
carbon dioxide and water, which of the following is a reactant?
a. | sucrose | c. | carbon dioxide | b. | heat | d. | water |
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68.
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Which of the following is true about the composition of ionic compounds?
a. | They are composed of cations only. | b. | They are formed from two or more nonmetallic
elements. | c. | They are composed of anions only. | d. | They are composed of anions and
cations. |
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69.
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Which of the following materials is a substance?
a. | gasoline | c. | stainless steel | b. | air | d. | silver |
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70.
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Which of the following best describes an example of pure chemistry?
a. | studying chemicals containing carbon | b. | finding an antidote for a new strain of
virus | c. | developing a cure for osteoporosis | d. | testing the effects of lower concentrations of
a drug on humans |
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71.
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What type of ions have names ending in -ide?
a. | only metal ions | c. | only anions | b. | only gaseous ions | d. | only cations |
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72.
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Which of the following is used for chemical symbols today?
a. | icons | c. | letters | b. | numbers | d. | drawings |
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73.
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In an s orbital, the probability of finding an electron a particular
distance from the nucleus does NOT depend on ____.
a. | direction with respect to the nucleus | c. | the Schrodinger
equation | b. | the electron energy sublevel | d. | a quantum mechanical
model |
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74.
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Which of the following groupings contains only representative elements?
a. | Cu, Co, Cd | c. | Al, Mg, Li | b. | Ni, Fe, Zn | d. | Hg, Cr, Ag |
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75.
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If E is the symbol for an element, which two of the following symbols represent
isotopes of the same element? a. | 3 and 4 | c. | 1 and 4 | b. | 2 and 3 | d. | 1 and 2 |
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76.
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In which of the following are the symbol and name for the ion given
correctly?
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77.
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What is the electron configuration of the oxide ion (O  )?
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Short Answer (Value 7)
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78.
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List the number of protons, neutrons, and electrons in  C.
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79.
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From which orbital in a lithium atom is an electron transferred to form Li  ?
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80.
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Write the formula for the compound barium oxide.
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81.
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What is the electron configuration of oxygen?
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82.
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Give the electron configuration for calcium the ion.
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83.
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What orbital is filled when iodine gains an electron to become a negative
ion?
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84.
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Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass
of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant?
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Numeric Response (Value 10)
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85.
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What is the usual charge on an ion from Group 7A?
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86.
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How many traditional areas of study can chemistry be divided into?
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87.
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How many electrons are present in the d sublevel of a neutral atom of
nickel?
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88.
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How many electrons are in the highest occupied energy level of copper?
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89.
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How many valence electrons are in bromine?
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90.
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Use the periodic table to determine the number of electrons in a neutral atom of
lithium.
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91.
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In how many physical states does water commonly exist?
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92.
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How many unshared pairs of electrons does the nitrogen atom in ammonia
possess?
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93.
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How many electrons are in an atom of gold?
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94.
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How many electrons are in the highest occupied energy level of a neutral
strontium atom?
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Completion (Value10)
Complete
each statement.
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95.
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1. Write IUPAC names for formulas and formulas
for IUPAC names.
a)
VBr5
b) cobalt(III)nitrate
c) Ni(OH)3
d) bismuth(III)silicate
e) FeO
f)
europium(II)tripolyphospate
g)
Fe(C17H35COO)2
h) tin(II)dichromate
i)
Mn3P4
j) uranium(VI)oxide
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