Covalent Bonding & Molecular Compounds. Multiple Choice Review. Slide 1 / 109. Slide 2 / 109. Slide 3 / 109. aluminum, oxygen

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1 Slide 1 / 109 ovalent onding & Molecular ompounds Multiple hoice Review 1 Which pair of elements is most apt to form a molecular compound with each other? Slide 2 / 109 aluminum, oxygen magnesium, iodine sulfur, fluorine potassium, lithium barium, bromine 2 The correct name for SO is. Slide 3 / 109 sulfur oxide sulfur monoxide sulfoxide sulfate sulfite

2 3 The correct name for l 4 is. Slide 4 / 109 carbon chloride carbon tetrachlorate carbon perchlorate carbon tetrachloride carbon chlorate 4 The correct name for N 2 O 5 is. Slide 5 / 109 nitrous oxide nitrogen pentoxide dinitrogen pentoxide nitric oxide nitrogen oxide 5 The name of Pl 3 is. Slide 6 / 109 potassium chloride phosphorus trichloride phosphorous(iii) chloride monophosphorous trichloride trichloro potassium

3 6 The name of the binary compound N 2 O 4 is. Slide 7 / 109 nitrogen oxide nitrous oxide nitrogen(iv) oxide dinitrogen tetroxide oxygen nitride 7 The correct name for H 2 O is. Slide 8 / 109 hydrogen oxide hydrogen(ii) oxide dihydrogen oxide dihydrogen monoxide hydrogen dioxide 8 The correct name for XeF 4 is. Slide 9 / 109 monoxenon pentafluoride xenon pentafluoride xenon tetrafluoride monoxenon tetrafluoride xenon fluorate

4 9 The correct name for P 2 O 5 is. Slide 10 / 109 phosphorus oxide phosphorus pentoxide diphosphorus oxide phosphate diphosphorus pentoxide 10 The name of l 3 is. Slide 11 / 109 boron chloride boron trichloride monoboron chloride trichloro boron monoboron trichloride 11 The name of the binary compound S 2 is. Slide 12 / 109 carbon sulfide monocarbon disulfide carbon disulfide carbon sulfate carbon disulfate

5 12 The type of compound that is most likely to contain a covalent bond is. Slide 13 / 109 one that is composed of a metal and a nonmetal a solid metal one that is composed of only nonmetals held together by the electrostatic forces between oppositely charged ions There is no general rule to predict covalency in bonds. 13 There are paired and unpaired electrons in the Lewis symbol for a Nitrogen atom. Slide 14 / 109 4, 2 2, 4 2, 3 4, 3 0, 3 14 In the Lewis symbol for a sulfur atom, there are paired and unpaired electrons. Slide 15 / 109 2, 2 4, 2 2, 4 0, 6 5, 1

6 15 In the Lewis symbol for an Iodine atom, there are paired and unpaired electrons. Slide 16 / 109 4, 2 4,1 2, 5 6, 1 0, 5 16 There are unpaired electrons in the Lewis symbol for an oxygen atom. Slide 17 / The only noble gas without eight valence electrons is. Slide 18 / 109 r Ne He Kr ll noble gases have eight valence electrons.

7 18 How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell? Slide 19 / How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? Slide 20 / double bond consists of pairs of electrons shared between two atoms. Slide 21 /

8 21 covalent bond between the same two atoms is the longest. Slide 22 / 109 single double triple they are all the same length. strong 22 s the number of covalent bonds between two atoms increases, the distance between the atoms and the strength of the bond between them. Slide 23 / 109 increases, increases decreases, decreases increases, decreases decreases, increases is unpredictable 23 What is the maximum number of double bonds that a hydrogen atom can form? Slide 24 /

9 24 What is the maximum number of double bonds that a carbon atom can form? Slide 25 / In which of the molecules below is the carboncarbon distance the shortest? Slide 26 / 109 H 2 = H 2 H H H 3 H 3 H 2 = = H 2 H 3 - H 2 - H 3 26 Of the bonds N, = N, N the N bond is. Slide 27 / 109 strongest/shortest strongest/longest weakest/shortest weakest/longest intermediate in both strength and length

10 27 Of the possible bonds between carbon atoms (single, double, and triple),. Slide 28 / 109 a triple bond is longer than a single bond a double bond is stronger than a triple bond a single bond is stronger than a triple bond a double bond is longer than a triple bond a single bond is stronger than a double bond 28 The ion Il 4 - has valence electrons. Slide 29 / The ion NO - has valence electrons. Slide 30 /

11 30 The Lewis structure of sh 3 shows nonbonding electron pair(s) on s. Slide 31 / This cannot be determined from the data given. 31 The Lewis structure of PF 3 shows that the central phosphorus atom has nonbonding and bonding electron pairs. Slide 32 / 109 2, 2 1, 3 3, 1 1, 2 3, 3 32 The Lewis structure of HN (H N) shows that has nonbonding electron pairs. Slide 33 / 109, 1 N, 1 H, 1 N, 2, 2

12 33 Of the following, cannot accommodate more than an octet of electrons. Slide 34 / 109 P s O S I 34 valid Lewis structure of cannot be drawn without violating the octet rule. Slide 35 / 109 NH 3 IF 3 PF 3 Sbl 3-1 NO 3 35 valid Lewis structure of cannot be drawn without violating the octet rule. Slide 36 / PO 4 PF 3 l 4 SeF 4 NF 3

13 36 The central atom in does not violate the octet rule. * Slide 37 / 109 SF 4 KrF 2 F 4 XeF 4 - Il 4 37 The central atom in violates the octet rule. Slide 38 / 109 NH 3 SeF 2 F 3 sf 3 H 4 38 valid Lewis structure of cannot be drawn without violating the octet rule. Slide 39 / 109 lf 3 Pl 3 SO 3 l 4 O 2

14 39 valid Lewis structure of cannot be drawn without violating the octet rule. Slide 40 / 109 NI 3 SO 2 Il 5 SiF 4 O 2 40 valid Lewis structure of cannot be drawn without violating the octet rule. Slide 41 / 109 NF 3 eh 2 SO 2 F 4 2- SO 3 41 The central iodine atom in the Il 4 - ion has non-bonded electron pairs and bonded electron pairs in its valence shell. Slide 42 / 109 2, 2 3, 4 1, 3 3, 2 2, 4

15 42 The central iodine atom in IF 5 has nonbonded electron pairs and bonded electron pairs in its valence shell. Slide 43 / 109 1, 5 0, 5 5, 1 4, 1 1, 4 43 The central Xe atom in the XeF 4 molecule has non-bonded electron pairs and bonded electron pairs in its valence shell. Slide 44 / 109 1, 4 2, 4 4, 0 4, 1 4, 2 44 Resonance structures differ by. Slide 45 / 109 number and placement of electrons number of electrons only placement of atoms only number of atoms only placement of electrons only

16 45 How many equivalent resonance forms can be drawn for O 3-2 (carbon is the central atom)? Slide 46 / How many equivalent resonance forms can be drawn for SO 2 without expanding octet on the sulfur atom (sulfur is the central atom)? Slide 47 / 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? Slide 48 /

17 48 How many different types of resonance structures can be drawn for the ion SO 3-2 where all atoms satisfy the octet rule? Slide 49 / In the nitrite ion NO 2 -,. Slide 50 / 109 both bonds are single bonds both bonds are double bonds one bond is a double bond and the other is a single bond both bonds are the same there are 20 valence electrons 50 The Lewis structure of the O 3-2 ion is. Slide 51 / 109

18 51 To convert from one resonance structure to another,. Slide 52 / 109 only atoms can be moved electrons and atoms can both be moved only electrons can be moved neither electrons nor atoms can be moved electrons must be added 52 For resonance forms of a molecule or ion,. Slide 53 / 109 one always corresponds to the observed structure all the resonance structures are observed in various proportions the observed structure is an average of the resonance forms the same atoms need not be bonded to each other in all resonance forms there cannot be more than two resonance structures for a given species 53 The basis of the VSPR model of molecular bonding is. Slide 54 / 109 regions of electron density on an atom will organize themselves so as to maximize s-character regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap atomic orbitals of the bonding atoms must overlap for a bond to form electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry

19 54 ccording to VSPR theory, if there are three electron domains in the valence shell of an atom, they will be arranged in a(n) geometry. Slide 55 / 109 octahedral linear trigonal bipyramidal 55 n electron domain could consist of. a. a nonbonding pair of electrons b. a single bond c. a multiple bond Slide 56 / 109 a only b only c only a, b, and c b and c 56 ccording to VSPR theory, if there are five electron domains in the valence shell of an atom, they will be arranged in a(n) geometry. Slide 57 / 109 octahedral linear trigonal bipyramidal

20 57 ccording to VSPR theory, if there are four electron domains in the valence shell of an atom, they will be arranged in a(n) geometry. Slide 58 / 109 octahedral linear trigonal bipyramidal 58 In the valence shell of an atom there are six electron domains. They will be arranged in a (an) geometry. Slide 59 / 109 hexagonal octahedral trigonal bipyramidal see-saw 59 Using the VSPR model, the electron-domain geometry of the central atom in F 3 is. Slide 60 / 109 linear trigonal bipyramidal octahedral

21 60 The electron-domain geometry of the central atom in OF 2 is. Slide 61 / 109 linear trigonal bipyramidal octahedral 61 The electron-domain geometry of the central atom in rf 3 is. Slide 62 / 109 linear trigonal bipyramidal octahedral 62 Using the VSPR model, the electron-domain geometry of the central atom in rf 4 - is. Slide 63 / 109 linear trigonal bipyramidal octahedral

22 63 The electron-domain geometry of is. Slide 64 / 109 H 4 PH 3 l 2 r 2 XeF 4 all of the above except XeF 4 64 The electron-domain geometry and the molecular geometry of a molecule of the general formula n are. Slide 65 / 109 never the same always the same sometimes the same not related mirror images of one another 65 The electron-domain geometry and the molecular geometry of a molecule of the general formula n will always be the same if. Slide 66 / 109 there are no lone pairs on the central atom there is more than one central atom n is greater than four n is less than four the octet rule is obeyed

23 66 For a molecule with the formula 2 the molecular shape is. Slide 67 / 109 linear or bent linear or linear or T-shaped T-shaped 67 Pl 5 has electron domains and a molecular arrangement. Slide 68 / 109 6, trigonal bipyramidal 6, 5, square pyramidal 5, trigonal bipyramidal 6, seesaw 68 The electron-domain geometry and molecular geometry of iodine trichloride are and, respectively. Slide 69 / 109 trigonal bipyramidal,, trigonal pyramidal trigonal bipyramidal, T-shaped octahedral, T-shaped,

24 69 Using the VSPR model, the molecular geometry of the central atom in XeF 2 is. Slide 70 / 109 linear bent trigonal pyramidal 70 Using the VSPR model, the molecular geometry of the central atom in l 3 is. Slide 71 / 109 linear bent trigonal pyramidal 71 Using the VSPR model, the molecular geometry of the central atom in F 4 is. Slide 72 / 109 linear bent trigonal pyramidal

25 72 Using the VSPR model, the molecular geometry of the central atom in SO 2 is. Slide 73 / 109 linear bent trigonal pyramidal 73 Using the VSPR model, the molecular geometry of the central atom in Nl 3 is. Slide 74 / 109 linear bent trigonal pyramidal 74 Using the VSPR model, the molecular geometry of the central atom in PF 5 is. Slide 75 / 109 square planar trigonal bipyramidal seesaw square pyramidal

26 75 The molecular geometry of is square planar. Slide 76 / 109 l 4 XeF 4 PH 3 XeF 2 Il 3 76 The molecular geometry of the S 2 molecule is. Slide 77 / 109 linear bent T-shaped 77 The molecular geometry of the SiH 2 l 2 molecule is. Slide 78 / 109 trigonal pyramidal octahedral T-shaped

27 78 The molecular geometry of the PHl 2 molecule is. Slide 79 / 109 bent trigonal pyramidal T-shaped 79 The molecular geometry of the Hl 3 molecule is. Slide 80 / 109 bent trigonal pyramidal T-shaped 80 The molecular geometry of the SF 2 molecule is. Slide 81 / 109 linear bent octahedral

28 81 The molecular geometry of the H 3 O + ion is. Slide 82 / 109 linear bent trigonal pyramidal octahedral 82 lf 3 has "T-shaped" geometry. There are non-bonding domains in this molecule. Slide 83 / The electron domain and molecular geometry of - ro 2 is. Slide 84 / 109,, trigonal pyramidal, linear, bent trigonal pyramidal, seesaw

29 84 The molecular geometry of the ro 3 - ion is. Slide 85 / 109 trigonal pyramidal bent T-shaped 85 The molecular geometry of the left-most carbon atom in the molecule below is Slide 86 / 109 trigonal bipyramidal octahedral T-shaped 86 The molecular geometry of the right-most carbon in the molecule below is. Slide 87 / 109 trigonal bipyramidal octahedral T-shaped

30 87 What is the molecular geometry of a molecule that has three bonding and two non-bonding domains? Slide 88 / 109 T-shaped Tetrahedral See-saw Square pyramidal Trigonal bipyramidal 88 onsider the following species when answering the following questions: Slide 89 / 109 (i) Pl 3 (ii) l 4 (iii) Tel 4 (iv) XeF 4 (v) SF 6 For which of the molecules is the molecular geometry (shape) the same as the VSPR electron domain arrangement (electron domain geometry)? (i) and (ii) (i) and (iii) (ii) and (v) (iv) and (v) (v) only 89 onsider the following species when answering the following questions: Slide 90 / 109 (i) Pl 3 (ii) l 4 (iii) Tel 4 (iv) XeF 4 (v) SF 6 Which of the molecules has a see-saw shape? (i) (ii) (iii) (iv) (v)

31 90 The ability of an atom in a molecule to attract electrons is best quantified by the. Slide 91 / 109 paramagnetism diamagnetism electronegativity electron change-to-mass ratio first ionization potential 91 lectronegativity from left to right within a period and from top to bottom within a group. Slide 92 / 109 decreases, increases increases, increases increases, decreases stays the same, increases increases, stays the same 92 Which covalent single bond is most polar? Slide 93 / 109 H N H O H O O N

32 93 nonpolar bond will form between two atoms of electronegativity. Slide 94 / 109 different, opposite identical, different different, different similar, different identical, equal 94 Of the molecules below, the bond in is the most polar. Slide 95 / 109 Hr HI Hl HF H 2 95 Of the bonds below, is the least polar. Slide 96 / 109 Na, S P, S, F Si, l Na, l

33 96 Which of the following has the bonds correctly arranged in order of increasing polarity? Slide 97 / 109 e F, Mg F, N F, O F O F, N F, e F, Mg F O F, e F, Mg F, N F N F, e F, Mg F, O F Mg F, e F, N F, O F 97 Which two bonds are most similar in polarity? Slide 98 / 109 O F and l F F and l F l l and I r I r and Si l l l and e l 98 Of the molecules below, only is polar. Slide 99 / 109 SbF 5 sh 3 I 2 SF 6 H 4

34 99 Of the molecules below, only is nonpolar. Slide 100 / 109 O 2 H 2 O NH 3 Hl Tel Of the molecules below, only is polar. Slide 101 / 109 l 4 H 4 SeF 4 Sil 4 O Of the molecules below, only is nonpolar. Slide 102 / 109 F 3 NF 3 IF 3 Pr 3 rl 3

35 102 The molecular geometry of the el 2 molecule is, and this molecule is. Slide 103 / 109 linear, nonpolar linear, polar bent, nonpolar bent, polar, polar 103 The molecular geometry of the PF 3 molecule is, and this molecule is. Slide 104 / 109, polar, nonpolar trigonal pyramidal, polar trigonal pyramidal, nonpolar, unipolar 104 Of the following molecules, only is polar. Slide 105 / 109 el 2 F 3 r 4 SiH 2 l 2 l 2

36 105 Of the following molecules, only is polar. Slide 106 / 109 l 4 l 3 Nl 3 el 2 l The molecular geometry of the HF 3 molecule is, and the molecule is. Slide 107 / 109 trigonal pyramidal, polar, nonpolar seesaw, nonpolar, polar seesaw, polar 107 The molecular geometry of the l 3 molecule is, and this molecule is. Slide 108 / 109 trigonal pyramidal, polar trigonal pyramidal, nonpolar, polar, nonpolar trigonal bipyramidal, polar

37 Slide 109 / 109