Ch. 7 Multiple Choice

Name: _______________________

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Elements in the modern version of the periodic table are arranged in order of increasing __________. A) oxidation number B) number of isotopes C) atomic number D) atomic mass E) average atomic mass

1)

2) Which element would be expected to have chemical and physical properties closest to those of fluorine? A) Fe B) S C) Ne D) O E) Cl

2)

3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar. A) paramagnetism B) nuclear charge C) azimuthal quantum number D) Hund's rule E) diamagnetism

3)

4) In which orbital does an electron in a phosphorus atom experience the greatest effective nuclear charge? A) 1s B) 2p C) 2s D) 3p E) 3s

4)

5) Atomic radius generally increases as we move __________. A) down a group and from right to left across a period B) up a group and from right to left across a period C) up a group and from left to right across a period D) down a group; the period position has no effect E) down a group and from left to right across a period

5)

6) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? A) Si > P > Ar > Na > Mg B) Na > Mg > Si > P > Ar C) Ar > P > Si > Mg > Na D) Mg > Na > P > Si > Ar E) Ar > Si > P > Na > Mg

6)

7) The atomic radius of main-group elements generally increases down a group because __________. A) effective nuclear charge increases down a group B) effective nuclear charge zigzags down a group C) the principal quantum number of the valence orbitals increases D) effective nuclear charge decreases down a group E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases

7)

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8) Screening of the nuclear charge by core electrons in atoms is __________. A) more efficient than that by valence electrons B) less efficient than that by valence electrons C) essentially identical to that by valence electrons D) responsible for a general decrease in atomic radius going down a group E) both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group

8)

9) Which one of the following atoms has the largest radius? A) Cl B) O C) Ne

9) D) F

E) S

10) The effective nuclear charge of an atom is primarily affected by __________. A) electrondistribution B) orbital radial probability C) outer electrons D) inner electrons E) nuclear charge

10)

11) Which one of the following atoms has the largest radius? A) Sr B) Ca C) K

D) Y

E) Rb

11)

12) Which one of the following has the smallest radius? A) P B) Na C) Cl

D) Fe

E) Br

13) Which one of the following atoms has the largest radius? A) Sr B) Co C) I

D) Ba

E) Ca

12)

13)

14) Which one of the following elements has the largest atomic radius? A) Te B) Se C) Sb D) As

E) S

14)

15) Which one of the following elements has the largest atomic radius? A) B B) O C) Al D) F

E) P

15)

16) In which of the following atoms is the 2s orbital closest to the nucleus? A) P B) S C) Si D) Cl E) The 2s orbitals are the same distance from the nucleus in all of these atoms.

16)

17) In which of the following atoms is the 3s orbital closest to the nucleus? A) I B) Cl C) At D) Br E) The 3s orbitals are the same distance from the nucleus in all of these atoms.

17)

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18) Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? A) O < F < S < Ba < Mg B) O < F < S < Mg < Ba C) F < O < S < Mg < Ba D) F < O < S < Ba < Mg E) F < S < O < Mg < Ba

18)

19) __________ is isoelectronic with argon and __________ is isoelectronic with neon. A) Ne- , Ar+ B) Cl- , Cl+ C) Cl-, FD) Ne- , Kr+

19) E) F+, F-

20) Which of the following is an isoelectronic series? A) F-, Cl- , Br-, I-

20)

B) O2- , F- , Ne, Na+ C) S, Cl, Ar, K D) Si 2- , P2- , S2- , Cl2E) B5-, Si 4- , As3- , Te221) Which isoelectronic series is correctly arranged in order of increasing radius? A) K+ < Ca2+ < Ar < Cl-

21)

B) Cl- < Ar < K+ < Ca2+ C) Ca2+ < K+ < Cl- < Ar D) Ca2+ < Ar < K+ < ClE) Ca2+ < K+ < Ar < Cl22) Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? A) F < K < Br < Ge < Rb B) F < K < Ge < Br < Rb C) F < Br < Ge < Rb < K D) F < Br < Ge < K < Rb E) F < Ge < Br < K < Rb

22)

23) Of the choices below, which gives the order for first ionization energies? A) Cl > S > Al > Ar > Si B) S > Si > Cl > Al > Ar C) Al > Si > S > Cl > Ar D) Cl > S > Al > Si > Ar E) Ar > Cl > S > Si > Al

23)

24) Of the following atoms, which has the largest first ionization energy? A) Br B) I C) O D) C

E) P

25) Of the following elements, which has the largest first ionization energy? A) Sr B) Ba C) Ca D) Rb

E) K

26) Of the following elements, which has the largest first ionization energy? A) Sb B) As C) Se D) Ge

E) S

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24)

25)

26)

27) __________ have the lowest first ionization energies of the groups listed. A) Transition elements B) Alkaline earth metals C) Halogens D) Alkali metals E) Noble gases

27)

28) Which of the following has the largest second ionization energy? A) Al B) Na C) Mg D) P

E) Si

28)

29) Which of the following has the largest second ionization energy? A) Ge B) Ca C) Ga D) Se

E) K

29)

30) Which of the following correctly represents the second ionization of calcium? A) Ca+ (g) + e- → Ca2+ (g)

30)

B) Ca- (g) + e- → Ca2- (g) C) Ca+ (g) → Ca2+ (g) + eD) Ca (g) → Ca+ (g) + eE) Ca+ (g) + e- → Ca (g) 31) The ion with the smallest diameter is __________. A) ClB) O2C) F-

31)

32) Of the following species, __________ has the largest radius. A) Ar B) Rb+ C) Sr2+

D) Br-

E) I-

D) Kr

E) Br-

32)

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 33) The electron configuration belonging to the atom with the highest second ionization energy is __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v)

33)

34) 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)

34)

35) The electron configuration of the atom with the most negative electron affinity is __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v)

35)

36) 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)

36)

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37) An electron in a(n) __________ subshell experiences the greatest effective nuclear charge in a many-electron atom. A) 3s B) 3f C) 4s D) 3p E) 3d

37)

38) A tin atom has 50 electrons. Electrons in the __________ subshell experience the lowest effective nuclear charge. A) 3d B) 1s C) 5p D) 3p E) 5s

38)

39) In which orbital does an electron in a phosphorus atom experience the greatest shielding? A) 3s B) 2p C) 1s D) 3s E) 3p

39)

40) The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table. A) increase, increase B) increase, decrease C) decrease, increase D) decrease, decrease E) are completely unpredictable

40)

41) The __________ have the most negative electron affinities. A) transition metals B) alkali metals C) chalcogens D) alkaline earth metals E) halogens

41)

42) In general, as you go across a period in the periodic table from left to right: (1) the atomic radius __________; (2) the electron affinity becomes __________ negative; and (3) the first ionization energy __________. A) increases, increasingly, increases B) decreases, increasingly, decreases C) increases, increasingly, decreases D) decreases, decreasingly, increases E) decreases, increasingly, increases

42)

43) Most of the elements on the periodic table are __________. A) nonmetals B) liquids C) metals

43) D) gases

E) metalloids

44) The only noble gas that does not have the ns2 np6 valence electron configuration is __________. A) radon B) neon C) krypton D) helium E) All noble gases have the ns2np6 valence electron configuration.

44)

45) The first noble gas to be incorporated into a compound was __________. A) He B) Xe C) Kr D) Ne

45)

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E) Ar

Answer Key Testname: MC CH 7

1) C 2) E 3) B 4) A 5) A 6) B 7) C 8) A 9) E 10) D 11) E 12) C 13) D 14) C 15) C 16) D 17) C 18) C 19) C 20) B 21) E 22) D 23) E 24) C 25) C 26) E 27) D 28) B 29) E 30) C 31) C 32) E 33) A 34) B 35) E 36) B 37) A 38) C 39) E 40) A 41) E 42) E 43) C 44) D 45) B

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