Ch08-Testbank

1、Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical BondingA)MgB)MgC)MgD)Mg8.1 Multiple-Choice and Bimodal Questions1) There are _ paired and _ unpaired electrons in the Lewis symbolfor a phosphorus atom.A) 4, 2B) 2, 4C) 2, 3D) 4, 3E) 0, 3Answer: CDiff: 1Page Ref: Sec

2、. 8.12) In the Lewis symbol for a fluorine atom, there are _ paired and _unpaired electrons.A) 4, 2B) 4,1C) 2, 5D) 6, 1E) 0, 5Answer: DDiff: 1Page Ref: Sec. 8.13) Based on the octet rule, magnesium most likely forms a _ ion.E) MgAnswer: ADiff: 1Page Ref: Sec. 8.1Chemistry, 11e (Brown/Lemay/Bursten/M

3、urphy)Chapter 8: Basic Concepts of Chemical BondingA) 0B) 1C) 2D) 4E) 3Answer: CDiff: 1Page Ref: Sec. 8.14) Based on the octet rule, phosphorus most likely forms a _ ion.A) P3B) P3C) P5D) P5E) P+Answer: BDiff: 1Page Ref: Sec. 8.15) Based on the octet rule, iodine most likely forms an _ ion.A) I2B) I

4、4C) I4D) IE) IAnswer: EDiff: 1Page Ref: Sec. 8.16) There are _ unpaired electrons in the Lewis symbol for an oxygen atom.Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingA) Ne3S 2B) Ne3S 23P1C) Ne3S 23P3D) Ne3P 2E) Ne3S 23P6Answer: EDiff: 1Page Ref: Sec. 8.1ion

5、?7) How many unpaired electrons are there in the Lewis structures of aN 3A) 0B) 1C) 2D) 3E) This cannot be predicted.Answer: ADiff: 1Page Ref: Sec. 8.128) How many unpaired electrons are there in anO ion?A) 0B) 1C) 2D) 3E) This cannot be predicted.Answer: ADiff: 1Page Ref: Sec. 8.19) The electron co

6、nfiguration of the phosphide ion (P3 ) is _Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingA) O, SeB) SrC) NaD) BrE) Sr, O, SeAnswer: BDiff: 1Page Ref: Sec. 8.110) The halogens, alkali metals, and alkaline earth metals have _ valenceelectrons, respectively.A)

7、7, 4, and 6B) 1, 5, and 7C) 8, 2, and 3D) 7, 1, and 2E) 2, 7, and 4Answer: DDiff: 2Page Ref: Sec. 8.111) The only noble gas without eight valence electrons is _A) ArB) NeC) HeD) KrE) All noble gases have eight valence electrons.Answer: CDiff: 1Page Ref: Sec. 8.112) Which of the following would have

8、to lose two electrons in order to achieve a noble gas electron configuration?O Sr Na Se BrChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical Bonding26A) Ar3S 23p6B) Ar3S 23p2C) Ne3S 23p2D) Ne3S 23p6E) Kr3S 22p 6Answer: DDiff: 1Page Ref: Sec. 8.213) Which of the followin

9、g would have to gain two electrons in order to achieve a noble gas electron configuration?O Sr Na Se BrA) BrB) SrC) NaD) O, SeE) Sr, O, SeAnswer: DDiff: 1Page Ref: Sec. 8.114) For a given arrangement of ions, the lattice energy increases as ionic radius and as ionic charge _.A) decreases, increasesB

10、) increases, decreasesC) increases, increasesD) decreases, decreasesE) This cannot be predicted.Answer: A Diff: 1 Page Ref: Sec. 8.2215) The electron configuration of the S ion is _Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: BDiff: 1Page Ref: Sec.

11、8.216) The principal quantum number of the electrons that are lost when tungsten forms a cation is _.A) 6B) 5C) 4D) 3E) 2Answer: ADiff: 1Page Ref: Sec. 8.217) Which one of the following species has the electron configurationAr3dA) Mn 2B)Cr 2C)V 3D)Fe3E) KAnswer: BDiff: 1Page Ref: Sec. 8.2218) What i

12、s the electron configuration for the Co ion?A)Ar4S 13d6B)Ar4S 03d705C)Ar4S 03d529D)Ar4S 23d922 10E)Ne3S 23p10Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: BDiff: 1Page Ref: Sec. 8.219) What is the electron configuration for the Fe ion?A)Ar4S 03d6B)Ar

13、4S 23d4C)Ar4S 03d8D)Ar4S 23d8E)Ar4S 63d2Answer: ADiff: 1Page Ref: Sec. 8.220) The formula of palladium(IV) sulfide is _A) Pd2S4B)PdS4C)Pd4SD)PdS2E) Pd2S2Answer: DDiff: 1Page Ref: Sec. 8.221) Elements from opposite sides of the periodic table tend to form _A) covalent compoundsB) ionic compoundsC) co

14、mpounds that are gaseous at room temperatureD) homonuclear diatomic compoundsE) covalent compounds that are gaseous at room temperature22) Determining lattice energy from Born-Haber cycle data requires the use ofA) the octet ruleChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of

15、 Chemical BondingAnswer: BDiff: 1Page Ref: Sec. 8.2B) Coulombs lawC) Periodic lawD) Hesss lawE) Avogadros numberAnswer: DDiff: 2Page Ref: Sec. 8.223) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell?A) 3B) 4C) 1D) 2E) 0Answer: BDiff: 1Page Ref: Se

16、c. 8.324) A _ covalent bond between the same two atoms is the longest.A) singleB) doubleC) tripleD) They are all the same length.E) strongChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingA) 0B) 1C) 2D) 3E) 4Answer: ADiff: 1Page Ref: Sec. 8.325) How many hydroge

17、n atoms must bond to silicon to give it an octet of valence electrons?A) 1B) 2C) 3D) 4E) 5Answer: DDiff: 1Page Ref: Sec. 8.326) A double bond consists of _ pairs of electrons shared between two atoms.A) 1B) 2C) 3D) 4E) 6Answer: BDiff: 2Page Ref: Sec. 8.327) What is the maximum number of double bonds

18、 that a hydrogen atom can form?Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical Bonding28) What is the maximum nu mber of double bonds that a carb on atom can form?A) 4B) 1C) 0D) 2E) 3An swer: DDiff: 1Page Ref: Sec. 8.329) In the molecule below, which atom has the

19、largest partial n egative charge ?ciIF-C -BrIrA) ClB) FC) BrD) IE) CAn swer: BDiff: 1Page Ref: Sec. 8.430) The ability of an atom in a molecule to attract electro ns is best qua ntified by theA) paramag netismB) diamag netismC) electro negativityD) electro n cha nge-to-mass ratioE) first ionization

20、potentialAn swer: CDiff: 1Page Ref: Sec. 8.4Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: BDiff: 1Page Ref: Sec. 8.231) Given the electronegativities below, which covalent single bond is most polar? Element:HCNOElectronegativity:2.12.5 3.0 3.5A) C-HB

21、) N-HC) O-HD) O-CE) O-NAnswer: CDiff: 1Page Ref: Sec. 8.432) Electronegativity _ from left to right within a period and _ fromtop to bottom within a group.A) decreases, increasesB) increases, increasesC) increases, decreasesD) stays the same, increasesE) increases, stays the sameAnswer: CDiff: 1Page

22、 Ref: Sec. 8.433) A nonpolar bond will form between two _ atoms of _electronegativity.A) different, oppositeB) identical, differentC) different, differentD) similar, differentE) identical, equalChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: BDiff: 1Pa

23、ge Ref: Sec. 8.234) The ion ICI 4 has _ valence electrons.A) 34B) 35C) 36D) 28E) 8Answer: CDiff: 1Page Ref: Sec. 8.535) The ion NO has _ valence electrons.A) 15B) 14C) 16D) 10E) 12Answer: EDiff: 1Page Ref: Sec. 8.536) The Lewis structure of AsH 3 shows _ nonbonding electron pair(s) on As.A) 0B) 1C)

24、2D) 3E) This cannot be determined from the data given.Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical Bonding37) The Lewis structure of PR shows that the central phosphorus atom has _nonbonding and _bonding electro n pairs.A) 2, 2B) 1,3C) 3, 1D) 1,2E) 3, 3An swer:

25、 BDiff: 1Page Ref: Sec. 8.538) The Lewis structure of HCN (H bon ded to C) shows that _has_nonbonding electro n pairs.A) C, 1B) N, 1C) H, 1D) N, 2E) C, 2An swer: BDiff: 2Page Ref: Sec. 8.539) The formal charge on carb on in the molecule below is _t I售o=c=oo=c=o*V tA) 0B) +1C) +2D) +3E) -1An swer: AD

26、iff: 1Page Ref: Sec. 8.5Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical Bondingwhere the Lewis structure of the40) The formal charge on nitrogen in NO 3 isA) -1B) 0C) +1D) +2E) -2An swer: CDiff: 2Page Ref: Sec. 8.5241) The formal charge on sulfur in SO4 ision is:

27、：0：.II .：o-s0：+ II -：0：A) -2B) 0C) +2D) +4E) -4An swer: BDiff: 2Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical BondingPage Ref: Sec. 8.542) In the Lewis structure of ClF, the formal charge on Cl is_and the formalcharge on F is _.A) -1,-1B) 0, 0C) 0, -1D) +1, -1E)

28、 -1, +1An swer: BDiff: 1Page Ref: Sec. 8.543) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is _.A) 0B) +1C) -1D) +2E) -2An swer: BDiff: 1Page Ref: Sec. 8.6244) How many equivale nt res onance forms can be draw n foCO3 - (carb on is the central atom)?A) 1B)

29、 2C) 3D) 4E) 0An swer: CDiff: 1Page Ref: Sec. 8.6Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical Bonding45) How many equivalent resonance forms can be drawn foSr O2 without expanding octet on the sulfur atom (sulfur is the central atom)?A) 0B) 2C) 3D) 4E) 1Answer:

30、 BDiff: 1Page Ref: Sec. 8.646) How many equivalent resonance structures can be drawn for the molecule of SO 3 without having to violate the octet rule on the sulfur atom?A) 5B) 2C) 1D) 4E) 3Answer: EDiff: 1Page Ref: Sec. 8.647) How many different types of resonance structures can be drawn for the io

31、n 2SO3 where all atoms satisfy the octet rule?A) 1B) 2C) 3D) 4E) 5Answer: ADiff: 2Page Ref: Sec. 8.648) Using the table of average bond energies below, theH for the reaction is _An swer: DDiff: 1Page Ref: Sec. 8.8H-CC-H(gH-CC-H(g + + 2Hl(2Hl(g g) )f f ICICC CIg)Ig)Bond:ACIH HC-C H-IC-IC-HD (kJ/mol):

32、839348299240413Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical Bonding kJ.A) +160B) -160C) -217D) -63E) +63An swer: CDiff: 1Page Ref: Sec. 8.849) Usi ng the table of average bond en ergies below, theH for the react ion is_kJ.H CCH (g) + H I (g)H2C CHI (g)Bond:ACC=

33、CH-IC-IC-HD (kJ/mol):839614299240413A) +506B) -931C) -506D) -129E) +12950) Usi ng the table of average bond en ergies below, theH for the react ion is_kJ.CO (g)+2H 2(g)H3C O H (g)Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical BondingAn swer: ADiff: 1Page Ref: Sec

34、. 8.8Bond:C-OC=OAOC-HH-HO-HD (kJ/mol):3587991072413436463A) +276B) -276C) +735D) -735E) -116An swer: EDiff: 1Page Ref: Sec. 8.851) Using the table of bond dissociation energies, the H for the following gas-phase reacti on is_kJ.BondD (kJ/mol)C-C卻卻c=cC-H41JH-Cl431C-Cl323A) -44B) 38C) 304D) 2134E) -38

35、Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical BondingH H H HI IH H - - C CC C HrHrHrHr52) Using the table of bond dissociation energies, the H for the following gas-phase reacti on is kJ.H H H HC=CC=CBandD 低JJmol)C-CC=C614C-H413H-Br珈匚-Br276A) 291B) 2017C) -57D)

36、-356E) -291An swer: CDiff: 1Page Ref: Sec. 8.8Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical Bonding53) Using the table of bond dissociation energies, the H for the following reaction is kJ.2HCl (g) F2 (g) 2HF (g) Cl2 (g)BandD (kj/mol)H-Cl4刃F-F155H-F567Cl-Cl沁A) -

37、359B) -223C) 359D) 223E) 208An swer: ADiff: 1Page Ref: Sec. 8.8 8.2 Multiple-Choice Questio ns1) Which ion below has a noble gas electron configuration?A) Li2B)Be2C) B2D)C22E)NAn swer: BDiff: 1Page Ref: Sec. 8.1An swer: ADiff: 3Page Ref: Sec. 8.1Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8

38、: Basic Con cepts of Chemical Bonding2) Of the ions below, on ly _has a n oble gas electro n con figurati on.A)S3B)O2C) ID) KE)ClAn swer: EDiff: 1Page Ref: Sec. 8.13) Which of the follow ing has eight vale nee electr ons?A) Ti4B) KrC)ClD)NaE) all of the aboveAn swer: EDiff: 3Page Ref: Sec. 8.14) Whi

39、ch of the follow ing does not. have eight vale nee electr ons?A)CaB)RbC) XeD) BrE) All of the above have eight vale nee electr ons.Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: DDiff: 22Page Ref: Sec. 8.55) The chloride of which of the following meta

40、ls should have the greatest lattice energy?A) potassiumB) rubidiumC) sodiumD) lithiumE) cesiumAnswer: DDiff: 2Page Ref: Sec. 8.26) Lattice energy is _.A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phaseB) the energy given off when gaseous ions combine t

41、o form one mole of an ionic solidC) the energy required to produce one mole of an ionic compound from its constituent elements in their standard statesD) the sum of ionization energies of the components in an ionic solidE) the sum of electron affinities of the components in an ionic solidAnswer: ADi

42、ff: 1Page Ref: Sec. 8.27) In ionic bond formation, the lattice energy of ions _ as the magnitude of the ioncharges _ and the radii _.A) increases, decrease, increaseB) increases, increase, increaseC) decreases, increase, increaseD) increases, increase, decreaseE) increases, decrease, decreaseChemist

43、ry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical BondingAn swer: DDiff: 1Page Ref: Sec. 8.2The diagram below is the Born-H uber cycle for the formatio n of crystalli ne potassium fluoride.1 蛙卡FLE)8) Which en ergy cha nge corresp onds to the electr on affin ity of fluori n

44、e?A) 2B) 5C) 4D) 1E) 6An swer: CDiff: 1Page Ref: Sec. 8.29) Which en ergy cha nge corresp onds to the first ioni zatio n en ergy of potassium?A) 2B) 5C) 4D) 3E) 6Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: DDiff: 24Page Ref: Sec. 8.510) The electro

45、n configuration Kr4d 10 represents _A) Sr+2B) Sn+2C) Te+2D) Ag+1E) Rb+1Answer: DDiff: 3Page Ref: Sec. 8.211) Fe+2 ions are represented by _A) Ar3d 1B) Ar3d 4C) Ar3d 6D) Ar3d 104s1E) Ar3d 3Answer: CDiff: 4Page Ref: Sec. 8.212) Using the Born-Haber cycle, the Hf of KBr is equal to _Hf 癧癧Br (g)I1 (K)E(

46、Br)H latticeHf 癧癧Br (g)I1 (K)E(Br)H latticeHf 癧癧Br (g)I1 (K)E(Br)H latticeHf 癧癧Br (g)I1 E(Br)HlatticeHf 癧癧Br (g)I1 (K)E(Br)H latticeA)Hf癧K (g)B)Hf癧K(g)C)Hf 癧癧(g)D)Hf 癧癧(g)E)Hf 癧癧(g)Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: DDiff: 25Page Ref: Sec.

47、 8.5D) H2CC CH 2E) H3CCH 2 CH 313) The type of compound that is most likely to contain a covalent bond is _.A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic tableB) a solid metalC) one that is composed of only nonmetalsD) he

48、ld together by the electrostatic forces between oppositely charged ionsE) There is no general rule to predict covalency in bonds.Answer: CDiff: 1Page Ref: Sec. 8.314) In which of the molecules below is the carbon-carbon distance the shortest?A)H2C CH 2B) H C C HC)H3C CH 3Answer: BDiff: 1Page Ref: Se

49、c. 8.315) Of the atoms below, _ is the most electronegative.A) BrB) OC) ClD) NE) FChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: DDiff: 1Page Ref: Sec. 8.416) Of the atoms below, _ is the most electronegative.A) SiB) ClC) RbD) CaE) SAnswer: BDiff: 1Pa

50、ge Ref: Sec. 8.417) Of the atoms below, _ is the least electronegative.A) RbB) FC) SiD) ClE) CaAnswer: ADiff: 1Page Ref: Sec. 8.418) Which of the elements below has the largest electronegativity?A) SiB) MgC) PD) SE) NaChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical B

51、ondingAnswer: DDiff: 1Page Ref: Sec. 8.519) Of the molecules below, the bond in _ is the most polar.A) HBrB) HIC) HClD) HFE)H 2Answer: DDiff: 1Page Ref: Sec. 8.420) Of the bonds below, _ is the least polar.A) Na, SB) P, SC) C, FD) Si, ClE) Na, ClAnswer: BDiff: 1Page Ref: Sec. 8.421) Which of the fol

52、lowing has the bonds correctly arranged in order of increasing polarity?A)BeF, MgF, NF, OFB)OF, NF, BeF, Mg FC)OF, BeF, MgF, NFD)NF, BeF, MgF, O FE)MgF, BeF, N F, O FChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: DDiff: 28Page Ref: Sec. 8.522) Which t

53、wo bonds are most similar in polarity?A) O Fand Cl FB) B Fand Cl FC) Al Cland I BrD) I Br and Si ClE) Cl Cl and Be ClAnswer: ADiff: 2Page Ref: Sec. 8.423) The bond length in an HI molecule is 1.61 ? and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charg

54、e on I in HI?30 19(1 debye = 3.34 10 coulomb-meters ; ; e=1.6 10 coulombs )A)1.6 10 19B) 0.057C) 9.1D) 1E) 0.22Answer: BDiff: 5Page Ref: Sec. 8.424) Which of the following names is/are correct for the compoundTiO 2A) titanium dioxide and titanium (IV) oxideB) titanium (IV) dioxideC) titanium oxideD)

55、 titanium oxide and titanium (IV) dioxideE) titanium (II) oxideChemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: DDiff: 3Page Ref: Sec. 8.525) Which of the following names is/are correct for the compoundSnCl 4?A) tin (II) chloride and tin (IV) chlorideB)

56、 tin tetrachloride and tin (IV) chlorideC) tin (IV) tetrachlorideD) tin chlorideE) tin chloride and tin (II) tetrachlorideAnswer: BDiff: 1Page Ref: Sec. 8.426) The Lewis structure of N2H2 shows _A) a nitrogen-nitrogen triple bondB) a nitrogen-nitrogen single bondC) each nitrogen has one nonbonding e

57、lectron pairD) each nitrogen has two nonbonding electron pairsE) each hydrogen has one nonbonding electron pairAnswer: CDiff: 2Page Ref: Sec. 8.527) There are _ valence electrons in the Lewis structure of C3HCH2Cl.A) 14B) 12C) 18D) 20E) 10Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic

58、 Con cepts of Chemical Bonding28) In the Lewis symbol for a sulfur atom, there are _ paired and _unpaired electrons.A) 2, 2B) 4, 2C) 2, 4D) 0, 6E) 5, 1Answer: BDiff: 2Page Ref: Sec. 8.5Chemistry, 11e (Brow n/Lemay/Burste n/Murphy)Chapter 8: Basic Con cepts of Chemical BondingAn swer: ADiff: 2Page Re

59、f: Sec. 8.5229) The Lewis structure of the CO3 ion is _Chemistry, 11e (Brown/Lemay/Bursten/Murphy)Chapter 8: Basic Concepts of Chemical BondingAnswer: CDiff: 2Page Ref: Sec. 8.630) In the nitrite ion (NO 2-) , _.A) both bonds are single bondsB) both bonds are double bondsC) one bond is a double bond

60、 and the other is a single bondD) both bonds are the sameE) there are 20 valence electronsAnswer: DDiff: 2Page Ref: Sec. 8.631) Resonance structures differ by _A) number and placement of electronsB) number of electrons onlyC) placement of atoms onlyD) number of atoms onlyE) placement of electrons on