Exam Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In which set of elements would all members be expected to have very similar chemical properties? A) N, O, F B) Ne, Na, Mg C) Na, Mg, K D) S, Se, Si E) O, S, Se
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2) Which element would be expected to have chemical and physical properties closest to those of fluorine? A) O B) Fe C) S D) Cl E) Ne
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3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar. A) Hundʹs rule B) nuclear charge C) azimuthal quantum number D) paramagnetism E) diamagnetism
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4) In which orbital does an electron in a phosphorus atom experience the greatest effective nuclear charge? A) 2p B) 1s C) 3p D) 2s E) 3s
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5) The atomic radius of main-group elements generally increases down a group because __________. A) the principal quantum number of the valence orbitals increases B) effective nuclear charge decreases down a group C) effective nuclear charge increases down a group D) effective nuclear charge zigzags down a group E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases
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6) The effective nuclear charge of an atom is primarily affected by __________. A) nuclear charge B) orbital radial probability C) outer electrons D) inner electrons E) electrondistribution
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7) __________ is isoelectronic with argon and __________ is isoelectronic with neon. A) Cl- , Cl+ B) Ne- , Kr+ C) Ne- , Ar+ D) Cl- , F-
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7) E) F+, F-
8) Which equation correctly represents the first ionization of phosphorus? A) P (g) + e- → P- (g)
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B) P (g) → P- (g) + eC) P- (g) → P (g) + eD) P+ (g) + e- → P (g) E) P (g) → P+ (g) + e9) Which of the following correctly represents the second ionization of phosphorus? A) P- (g) + e- → P2- (g)
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B) P+ (g) + e- → P (g) C) P (g) → P+ (g) + eD) P+ (g) → P2+ (g) + eE) P+ (g) + e- → P2+ (g) 10) Chlorine is much more apt to exist as an anion than is sodium. This is because __________. A) chlorine has a greater ionization energy than sodium does B) chlorine is bigger than sodium C) chlorine has a greater electron affinity than sodium does D) chlorine is a gas and sodium is a solid E) chlorine is more metallic than sodium
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11) Sodium is much more apt to exist as a cation than is chlorine. This is because __________. A) chlorine has a greater electron affinity than sodium does B) chlorine is a gas and sodium is a solid C) chlorine is more metallic than sodium D) chlorine has a greater ionization energy than sodium does E) chlorine is bigger than sodium
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Consider the following electron configurations to answer the questions that follow: (i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5 12) The electron configuration belonging to the atom with the highest second ionization energy is __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v)
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13) The electron configuration that belongs to the atom with the lowest second ionization energy is __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v)
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14) The electron configuration of the atom with the most negative electron affinity is __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v)
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15) Which one of the following is a metalloid? A) Ge B) Br C) S
15) D) C
E) Pb
16) Consider the general valence electron configuration of ns2 np5 and the following statements: (i) Elements with this electron configuration are expected to form -1 anions. (ii) Elements with this electron configuration are expected to have large positive electron affinities. (iii) Elements with this electron configuration are nonmetals. (iv) Elements with this electron configuration form acidic oxides. Which statements are true? A) (ii) and (iii) B) (i), (iii,) and (iv) C) (i) and (ii) D) (i), (ii), and (iii) E) All statements are true.
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17) Hydrogen is unique among the elements because __________. 1. It has only one valence electron. 2. It is the only element that can emit an atomic spectrum. 3. Its electron is not at all shielded from its nucleus. 4. It is the lightest element. 5. It is the only element to exist at room temperature as a diatomic gas. C) 1, 2, 3, 4 D) 2, 3, 4 A) 3, 4 B) 1, 2, 3, 4, 5
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E) 1, 3, 4
18) Of the elements below, __________ is the most metallic. A) Na B) K C) Mg
E) Al
18) D) Ar
Consider the following electron configurations to answer the questions that follow: (i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5 19) The electron configuration of the atom that is expected to have a positive electron affinity is __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v)
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20) Which of the following statements is NOT true? A) Cations are larger than the atoms from which they are formed. B) The atomic radius decreases from left to right through a period of elements. C) The metallic character of elements decreases from left to right through a period of elements. D) The ionization energy increases from left to right through a period of elements. E) The atomic radius increases down the periodic table.
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21) Which of the following occurs for the representative elements going left to right across the period? A) electronegativity decreases B) the outer electrons are held more weakly C) forces of attraction between electron and nucleus increase because nuclear charge increase D) atomic size increases E) none of these
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22) Choose the orbital diagram that represents the ground state of N. A)
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B)
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23) Choose the valence orbital diagram that represents the ground state of Zn. A)
B)
C)
D)
E)
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24) Choose the valence orbital diagram that represents the ground state of Sr 2⁺. A)
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B)
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25) Choose the valence orbital diagram that represents the ground state of Se 2 ⁻. A)
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B)
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SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 26) Why is the first ionization energy of sulfur smaller than the first ionization energy of phosphorus?
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27) Why does the size of the transition elements stay roughly the same as you move across a period?
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MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 28) Why is the electron affinity so positive for the noble gas elements? A) The noble gas elements are diatomic elements. B) The added electron would have to go into a new shell. C) The added electron would have to be added into the half -filled p subshell. D) The added electron would have to be added into the p subshell. E) Electrons canʹt be added to gases. 29) Choose the species from which one electron could most easily be removed. A) K B) K+ C) Cl D) Ar 30) Among the alkali metals, cesium reacts more rapidly than sodium because: A) cesium has more protons B) cesium has more neutrons C) the valence electron of cesium is at a greater average distance from the nucleus D) cesium has a higher atomic weight E) cesium has more electrons
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29) E) Ca+ 30)
Answer Key Testname: UNTITLED1
1) E 2) D 3) B 4) B 5) A 6) D 7) D 8) E 9) D 10) C 11) D 12) A 13) B 14) E 15) A 16) B 17) A 18) B 19) B 20) A 21) C 22) C 23) B 24) E 25) D 26) When sulfur loses one electron, it take on a particularly stable, half -filled p subshell. The removal of this first electron therefore requires less energy than the removal of an electron from phosphorus initially half-filled p subshell. 27) The electrons added as the transition element increase in atomic number are NOT being added to the outermost shell. They are being added to an inner shell where they shield the outer electrons from nuclear charge. The number of outermost electrons are constant. For each electron added across the period, an additional proton is also added. This keeps the effective nuclear charge roughly constant as the transition elements increase in atomic number within a given period. Therefore, the size of the transition elements within a period stay roughly constant. 28) B 29) A 30) C
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