electron geometry (eg) Mother structure of VSEPR molecular geometry (mg) Daughter Structure

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1 electron geometry (eg) Mother structure of VSEPR molecular geometry (mg) Daughter Structure Ch9 1) Which of the following represent the Lewis structure for N? 2) Which of the following represent the Lewis structure for Cl? 3) Which of the following represent the Lewis structure for Mg? 4) Which of the following represent the Lewis structure for Br? 5) Which of the following represent the Lewis structure for Ca2+? No valence electrons

2 2014Spring CHEM101 Ch9-10 Review Worksheet 6) Give the complete electronic configuration for Br-. 1s22s22p63s23p64s24p6 1s22s22p63s23p64s24d104p6 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s23d104p5 1s22s2p63s2p64s23d104p6 7) Give the complete electronic configuration for Ca2+. 1s22s22p63s24p6 1s22s22p63s23p6 1s22s22p63s23p5 1s22s23p64s25p6 1s22s2p63s2p6 8) Give the complete electronic configuration for S2-. 1s22s22p63s24p6 1s22s22p63s23p6 1s22s22p63s23p5 1s22s23p64s25p6 1s22s2p63s2p6 9) Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl RbBr > NaF > KCl NaF > KCl > RbBr KCl > NaF > RbBr NaF > RbBr > KCl RbBr > KCl > NaF 10) Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS MgO < CaO < SrS SrS < MgO < CaO SrS < CaO < MgO CaO < MgO < SrS CaO < SrS < MgO

3 11) Identify the shortest bond. single covalent bond double covalent bond triple covalent bond all of the above bonds are the same length 12) Identify the weakest bond. single covalent bond double covalent bond triple covalent bond all of the above bonds are the same strength 13) Identify the strongest bond. single covalent bond double covalent bond triple covalent bond all of the above bonds are the same strength 14) Identify the number of bonding pairs and lone pairs of electrons in water. 1 bonding pair and 1 lone pair 1 bonding pair and 2 lone pairs 2 bonding pairs and 2 lone pairs 2 bonding pairs and 1 lone pair 3 bonding pairs and 2 lone pairs 15) Identify the compound with the largest dipole moment in the gas phase.( calculate the electron negativity difference) Cl2 ClF HF LiF 16) Identify the compound with the smallest dipole moment in the gas phase. Cl2 ClF HF LiF

4 17) Choose the bond below that is most polar. H-I H-Br H-F H-Cl C-H 18) Choose the bond below that is least polar. P-F C-Br C-F C-I C-Cl 19) Choose the best Lewis structure for BeF2. 20) Choose the best Lewis structure for OCl2. 21) Choose the best Lewis structure for CH2Cl2.

5 2014Spring CHEM101 Ch9-10 Review Worksheet 22) Choose the best Lewis structure for XeI2. 23) Give the number of valence electrons for ICl ) Choose the best Lewis structure for ICl5.

6 2014Spring CHEM101 Ch9-10 Review Worksheet 25) Choose the best Lewis structure for SF4. 26) Choose the best Lewis structure for NO3.

7 27) Choose the best Lewis structure for SO ) Choose the best Lewis structure for PO4 3.

8 2014Spring CHEM101 Ch9-10 Review Worksheet 29) Draw the Lewis structure for CO3 2- including any valid resonance structures. Which of the following statements is TRUE? The CO3 2- ion contains one C O single bond and two C=O double bonds. The CO3 2- ion contains two C O single bonds and one C=O double bond. The CO3 2- ion contains three C O double bonds. The CO3 2- ion contains two C O single bonds and one C O triple bond. None of the above are true. 30) Using Lewis structures and formal charge, which of the following ions is most stable? OCN ONC NOC OCN ONC NOC None of these ions are stable according to Lewis theory. All of these compounds are equally stable according to Lewis theory. 31) Rank the following molecules in decreasing bond energy. Cl2 Br2 F2 I2 I2 > Br2 > Cl2 > F2 Cl2 > Br2 > F2 > I2 I2 > Cl2 > Br2 > F2 Cl2 > I2 > F2 > Br2

9 32) Use the bond energies provided to estimate ΔH rxn for the reaction below. PCl3(g) + Cl2(g) PCl5(l) ΔH rxn =? Bond Bond Energy (kj/mol) Cl-Cl 243 P-Cl kj -419 kj -662 kj -67 kj -905 kj 33) Use the bond energies provided to estimate ΔH rxn for the reaction below. CH3OH(l) + 2 O2(g) CO2(g) + 2 H2O(g) ΔH rxn =? Bond Bond Energy (kj/mol) C-H 414 C-O 360 C=O 799 O=O 498 O-H kj -91 kj -486 kj -392 kj +206 kj 34) Use the bond energies provided to estimate ΔH rxn for the reaction below. XeF2 + 2 F2 XeF6 ΔH rxn =? Bond Bond Energy (kj/mol) Xe-F 147 F-F kj +159 kj -660 kj +176 kj -270 kj Ch10 35) Give the approximate bond angle for a molecule with an octahedral shape

10 Spring CHEM101 Ch9-10 Review Worksheet 36) How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3 37) How many of the following molecules are polar? PCl5 COS XeO3 SeBr2 electron geometry (eg) VSPER Mother structure geometry 38) Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3. eg=tetrahedral, mg=trigonal planar, sp2 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=tetrahedral, mg=trigonal pyramidal, sp3 eg=trigonal pyramidal, mg=tetrahedral, sp3 eg=trigonal planar, mg=trigonal planar, sp2 39) Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O. eg=tetrahedral, mg=bent, sp3 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=tetrahedral, mg=trigonal pyramidal, sp3 eg=bent, mg=bent, sp2 eg=trigonal planar, mg=trigonal planar, sp2 40) Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4. eg=tetrahedral, mg=tetrahedral, sp3 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3

11 eg=octahedral, mg=square planar, sp3d2 eg=octahedral, mg=octahedral, sp3d2 eg=trigonal bipyramidal, mg=seesaw, sp3d 41) Give the approximate bond angle for a molecule with an octahedral shape ) Determine the electron geometry (eg) and molecular geometry (mg) of CO3 2. eg=tetrahedral, mg=tetrahedral eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=bent eg=trigonal planar, mg=trigonal planar eg=tetrahedral, mg=trigonal planar 43) Determine the electron geometry (eg) and molecular geometry (mg) of SiF4. eg=tetrahedral, mg=trigonal pyramidal eg=octahedral, mg=square planar eg=trigonal bipyramidal, mg=trigonal pyramidal eg=tetrahedral, mg=bent eg=tetrahedral, mg=tetrahedral 44) Determine the electron geometry (eg) and molecular geometry (mg) of PF5. eg=trigonal bipyramidal, mg=trigonal bipyramidal eg=octahedral, mg=octahedral eg=trigonal bipyramidal, mg=tetrahedral eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=octahedral 45) Determine the electron geometry (eg) and molecular geometry (mg) of CO2. eg=tetrahedral, mg=tetrahedral eg=linear, mg=trigonal planar eg=trigonal planar, mg=bent eg=linear, mg=linear eg=trigonal planar, mg=trigonal planar 46) Determine the electron geometry (eg) and molecular geometry (mg) of ICl3. eg=trigonal planar, mg=trigonal planar eg=trigonal bipyramidal, mg= T-shape eg=trigonal planar, mg=bent eg=trigonal bipyramidal, mg=see-saw

12 eg=tetrahedral, mg=trigonal pyramidal 47) Determine the electron geometry (eg) and molecular geometry (mg) of XeF2. eg=trigonal bipyramidal, mg=bent eg=linear, mg=linear eg=tetrahedral, mg=linear eg=trigonal bipyramidal, mg=linear eg=tetrahedral, mg=bent 48) Determine the electron geometry (eg) and molecular geometry (mg) of XeF4. eg=tetrahedral, mg=tetrahedral eg=linear, eg=linear eg=tetrahedral, mg=bent eg=trigonal bipyramidal, mg=tetrahedral eg=octahedral, mg=square planar 49) Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons. C1 = tetrahedral, C2 = linear C1 = trigonal planar, C2= bent C1 = bent, C2 = trigonal planar C1 = trigonal planar, C2 = tetrahedral C1 = trigonal pyramidal, C2 = see-saw 50) Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF3 OF2 PF4+ PF3 < OF2 < PF4+ OF2 < PF3 < PF4+ OF2 < PF4+ < PF3 PF4+ < OF2 < PF3 PF4+ < PF3 < OF2 51) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule.

13 N2O NCl3 NO2 NCl3 > NO2 > N2O NO2 > N2O > NCl3 N2O > NO2 > NCl3 NCl3 > N2O > NO2 N2O > NCl3 > NO2 52) How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3 53) Determine the electron geometry (eg), molecular geometry (mg), and polarity of PCl3. eg=tetrahedral, mg=bent, polar eg=trigonal planar, mg=trigonal planar, nonpolar eg=linear, mg=linear, nonpolar eg=tetrahedral, mg=trigonal pyramidal, polar eg=trigonal pyramidal, mg=trigonal pyramidal, polar 54) Determine the electron geometry, molecular geometry and polarity of SF6. eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar eg=tetrahedral, mg=tetrahedral, polar eg=trigonal bipyramidal, mg=see-saw, polar eg=octahedral, mg=trigonal bipyramidal, nonpolar eg=octahedral, mg=octahedral, nonpolar 55) Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3. eg=trigonal planar, mg=trigonal planar, nonpolar eg=tetrahedral, mg=trigonal pyramidal, polar eg=trigonal planar, mg=trigonal pyramidal, polar eg=trigonal bipyramidal, mg=trigonal planar, nonpolar eg=octahedral, mg=tetrahedral, nonpolar 56) Place the following in order of increasing dipole moment. I < II = III I. BCl3 II. BIF2 III. BClF2

14 II < III < I I < II < III II < I < III I < III < II 2014Spring CHEM101 Ch9-10 Review Worksheet 57) Place the following in order of decreasing dipole moment. III > I > II II > I > III I > III > II II > III > I I = III > II I. cis-chcl=chcl II. trans-chcl=chci III. cis-chf=chf 58) Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3. eg=tetrahedral, mg=trigonal planar, sp2 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=tetrahedral, mg=trigonal pyramidal, sp3 eg=trigonal pyramidal, mg=tetrahedral, sp3 eg=trigonal planar, mg=trigonal planar, sp2 59) Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O. eg=tetrahedral, mg=bent, sp3 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=tetrahedral, mg=trigonal pyramidal, sp3 eg=bent, mg=bent, sp2 eg=trigonal planar, mg=trigonal planar, sp2 60) Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4. eg=tetrahedral, mg=tetrahedral, sp3 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=octahedral, mg=square planar, sp3d2 eg=octahedral, mg=octahedral, sp3d2 eg=trigonal bipyramidal, mg=seesaw, sp3d 61) Give the hybridization for the O in OF2. sp sp3 sp2 sp3d sp3d2

15 62) Give the hybridization for the S in SO3. sp sp3 sp2 sp3d sp3d2 63) Give the hybridization for the Br in BrO4. sp sp3d2 sp3d sp3 sp2 64) Give the hybridization for the S in SF6. sp sp2 sp3 sp3d sp3d2 65) Give the hybridization for the Br in BrF5. sp3d2 sp3d sp3 sp2 sp 66) Give the hybridization for the Br in BrCl3. sp3d2 sp3d sp3 sp2 sp 66) How many of the following molecules have sp2 hybridization on the central atom? 4 3 HCN SO2 OCl2 XeCl2

16 Spring CHEM101 Ch9-10 Review Worksheet 67) Use the molecular orbital diagram shown to determine which of the following is most stable. F2 F2 2 + Ne2 2 + O2 2 + F2 2

17 68) Use the molecular orbital diagram shown to determine which of the following are paramagnetic. O2 2 Ne2 2 + O2 2 + F2 2 + None of the above are paramagnetic.

18 69) Use the molecular orbital diagram shown to determine which of the following are paramagnetic. B2 2 + B2 2 N2 2 + C2 2 B2