Chemistry The Central Science, 12e (Brown et al：化学中心科学（Brown等人，12E

Chemistry The Central Science, 12e (Brown et al：化学中心科学（Brown等人，12E Chapter 8 Basic Concepts of Chemical Bonding Multiple-Choice Questions 1) Which ion below has a noble gas electron configuration? 2+A) Li 2+B) Be 2+C) B 2+D) C -2 E) N 2) Which of the following has eight valence electrons? 4+A) Ti B) Kr -C) Cl +D) Na E) all of the above 3) Which of the following does not have eight valence electrons? +A) Ca +B) Rb C) Xe -D) Br E) All of the above have eight valence electrons. 4) Lattice energy is __________. A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase B) the energy given off when gaseous ions combine to form one mole of an ionic solid C) the energy required to produce one mole of an ionic compound from its constituent elements in their standard states D) the sum of ionization energies of the components in an ionic solid E) the sum of electron affinities of the components in an ionic solid 5) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii __________. A) increases, decrease, increase B) increases, increase, increase C) decreases, increase, increase D) increases, increase, decrease E) increases, decrease, decrease 1 Copyright ? 2012 Pearson Education, Inc. The diagram below is the Born-Huber cycle for the formation of crystalline potassium fluoride. 6) Which energy change corresponds to the electron affinity of fluorine? A) 2 B) 5 C) 4 D) 1 E) 6 7) Which energy change corresponds to the first ionization energy of potassium? A) 2 B) 5 C) 4 D) 3 E) 6 108) The electron configuration [Kr]4d represents __________. +2 A) Sr +2 B) Sn +2 C) Te +1 D) Ag +1 E) Rb 9) Using the Born-Haber cycle, the ΔH? of KBr is equal to __________. f A) ΔH?[K (g)] + ΔH?[Br (g)] + I(K) + E(Br) + ΔH ffllattice B) ΔH?[K (g)] - ΔH?[Br (g)] - I(K) - E(Br) - ΔH ffllattice C) ΔH?[K (g)] - ΔH?[Br (g)] + I(K) - E(Br) + ΔH ffllattice D) ΔH?[K (g)] + ΔH?[Br (g)] - I - E(Br) + ΔH ffllattice E) ΔH?[K (g)] + ΔH?[Br (g)] + I(K) + E(Br) - ΔH ffllattice 10) 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 table B) a solid metal C) one that is composed of only nonmetals D) held together by the electrostatic forces between oppositely charged ions E) There is no general rule to predict covalency in bonds. 2 Copyright ? 2012 Pearson Education, Inc. 11) In which of the molecules below is the carbon-carbon distance the shortest? A) HC=H 22 B) H–C?C–H C) HC–CH 33 D) HC=C=CH 22 E) HC–CH–C H 323 12) Which of the following has the bonds correctly arranged in order of increasing polarity? A) Be-F, Mg-F, N-F, O-F B) O-F, N-F, Be-F, Mg-F C) O-F, Be-F, Mg-F, N-F D) N-F, Be-F, Mg-F, O-F E) Mg-F, Be-F, N-F, O-F 13) There are __________ valence electrons in the Lewis structure of CHCHCl. 32A) 14 B) 12 C) 18 D) 20 E) 10 14) There are __________ valence electrons in the Lewis structure of CHOCHCH.323A) 18 B) 20 C) 26 D) 32 E) 36 15) In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons. A) 2, 2 B) 4, 2 C) 2, 4 D) 0, 6 E) 5, 1 -16) In the nitrite ion (NO), __________. 2 A) both bonds are single bonds B) both bonds are double bonds C) one bond is a double bond and the other is a single bond D) both bonds are the same E) there are 20 valence electrons 17) The oxidation number of iron in FeO is __________. 23 A) -2 B) +1 C) +3 D) +2 E) -3 3 Copyright ? 2012 Pearson Education, Inc. 18) To convert from one resonance structure to another, __________. A) only atoms can be moved B) electrons and atoms can both be moved C) only electrons can be moved D) neither electrons nor atoms can be moved E) electrons must be added 19) For resonance forms of a molecule or ion, __________. A) one always corresponds to the observed structure B) all the resonance structures are observed in various proportions C) the observed structure is an average of the resonance forms D) the same atoms need not be bonded to each other in all resonance forms E) there cannot be more than two resonance structures for a given species For the questions that follow, consider the BEST Lewis structures of the following oxyanions: ----- (i) NO (ii) NO (iii) SO2 (iv) SO2 (v) BrO 23343 20) There can be four equivalent best resonance structures of __________. A) (i) B) (ii) C) (iii) D) (iv) E) (v) 21) In which of the ions do all X-O bonds (X indicates the central atom) have the same length? A) none B) all C) (i) and (ii) D) (iii) and (v) E) (iii), (iv), and (v) 22) Based on the octet rule, boron will most likely form a __________ ion. 3- A) B 1+ B) B 3+ C) B 2+ D) B 2- E) B 23) Which of the following does not have eight valence electrons? - A) Cl B) Xe +4 C) Ti +1 D) Rb +1 E) Sr 4 Copyright ? 2012 Pearson Education, Inc. 24) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. -A) PO3 4 B) SiF 4 C) CF 4 D) SeF 4 E) NF 3 25) The central atom in __________ does not violate the octet rule. A) SF 4 B) KrF 2 C) CF 4 D) XeF 4 -E) ICl 4 26) Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl? 2 A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. B) There aren't enough electrons. C) That would result in more than eight electrons around beryllium. D) That would result in more than eight electrons around each chlorine atom. E) That would result in the formal charges not adding up to zero. 27) Bond enthalpy is __________. A) always positive B) always negative C) sometimes positive, sometimes negative D) always zero E) unpredictable 28) Of the bonds C–N, C=N, and C?N, the C–N bond is __________. A) strongest/shortest B) strongest/longest C) weakest/shortest D) weakest/longest E) intermediate in both strength and length 5 Copyright ? 2012 Pearson Education, Inc. 29) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________. A) increases, increases B) decreases, decreases C) increases, decreases D) decreases, increases E) is unpredictable 30) Based on the octet rule, magnesium most likely forms a __________ ion. 2+A) Mg 2-B) Mg 6-C) Mg 6+D) Mg -E) Mg 3-31) The electron configuration of the phosphide ion (P) is __________. 2A) [Ne]3s 2lB) [Ne]3s3 P 23C) [Ne]3s3 P 2D) [Ne]3 P 26E) [Ne]3s3 P 32) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively. A) 7, 4, and 6 B) 1, 5, and 7 C) 8, 2, and 3 D) 7, 1, and 2 E) 2, 7, and 4 33) The only noble gas without eight valence electrons is __________. A) Ar B) Ne C) He D) Kr E) All noble gases have eight valence electrons. 34) Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br A) Br B) Sr C) Na D) O, Se E) Sr, O, Se 6 Copyright ? 2012 Pearson Education, Inc. 235) What species has the electron configuration [Ar]3d? 2+A) Mn 2+B) Cr 3+C) V 3+D) Fe +E) K 2+36) What is the electron configuration for the Co ion? 16A) [Ar]4s3d 7B) [Ar]3d 5C) [Ar]3d 29D) [Ar]4s3d 210E) [Ne]3s3p 37) The formula of palladium(IV) sulfide is __________. A) PdS 24 B) PdS 4 C) Pd4 S D) PdS 2 E) PdS 22 38) A nonpolar bond will form between two __________ atoms of __________ electronegativity. A) different, opposite B) identical, different C) different, different D) similar, different E) identical, equal -39) The ion ICI has __________ valence electrons. 4 A) 34 B) 35 C) 36 D) 28 E) 8 40) The Lewis structure of PF shows that the central phosphorus atom has __________ nonbonding and 3 __________ bonding electron pairs. A) 2, 2 B) 1, 3 C) 3, 1 D) 1, 2 E) 3, 3 7 Copyright ? 2012 Pearson Education, Inc. 41) The formal charge on carbon in the molecule below is __________. A) 0 B) +1 C) +2 D) +3 E) -1 8 Copyright ? 2012 Pearson Education, Inc.