Ruth Montag Chapter 10 Mastering Chemistry

10. Using the VSEPR model, the molecular geometry of the central atom in SO2 is ________. A. linear B bent C. tetrahedral D trigonal pyramidal E. trigonal planar

bent (b)

21. Give the hybridization for the C in HCN. A. sp3d B. sp2 C. sp3d2 D. sp3 E. sp

sp (e)

8. Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons. A. C1 = trigonal pyramidal, C2 = see-saw B. C1 = trigonal planar, C2= bent C. C1 = tetrahedral, C2 = linear D. C1 = trigonal planar, C2 = tetrahedral E. C1 = bent, C2 = trigonal planar https://drive.google.com/file/d/0B4_51_spvHBTblE2U2lPYXRhX0k/view?usp=sharing

C1 = trigonal planar, C2 = tetrahedral (d) (use link for answer)

15. What is the hybridization of the central atom of each of the following molecules? Drag the appropriate items to their respective bins.

COCl2= sp2 CCl4= sp3 PBr5= sp3d

9. 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. CS2 CF4 SCl2 A. SCl2 > CF4 > CS2 B. CS2 > CF4 > SCl2 C. CF4 > CS2 > SCl2 D. CS2 = SCl2 > CF4

CS2 > CF4 > SCl2 (b)

25. Determine whether each of the following molecules is polar or nonpolar. A. SiCl2F2 B. CO2 C. SeF6 D. IF5

SiCl2F2- polar CO2- nonpolar SeF6- nonpolar IF5- polar

22. Describe a sigma bond. A. p orbital overlapping with a d orbital B. s orbital overlapping with the side of a p orbital C. side by side overlap of d orbitals D. overlap of two d orbitals E. an attraction due to overlap of two orbitals along the internuclear axis

an attraction due to overlap of two orbitals along the internuclear axis (d)

11. Using the VSEPR model, the molecular geometry of the central atom in XeF4 is ________. A. square planar B. square pyramidal C tetrahedral B. trigonal bipyramidal D. seesaw

square planar (b)

23. A molecule containing a central atom with sp3 hybridization has a(n) ________ electron geometry. A. bent B. octahedral C. trigonal planar D. linear E. tetrahedral

tetrahedral (e)

3. Give the approximate bond angle for a molecule with a tetrahedral shape. A. 105° B. 180° C. 120° D. 90° E. 109.5°

109.5° (e)

13. Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3. A. eg=tetrahedral, mg=trigonal pyramidal, polar B. eg=octahedral, mg=tetrahedral, nonpolar C. eg=trigonal planar, mg=trigonal pyramidal, polar D. eg=trigonal planar, mg=trigonal planar, nonpolar E. eg=trigonal bipyramidal, mg=trigonal planar, nonpolar

eg=tetrahedral, mg=trigonal pyramidal, polar (a)

7. Determine the electron geometry (eg) and molecular geometry (mg) of XeF2. A. eg=tetrahedral, mg=linear B. eg=trigonal bipyramidal, mg=linear C. eg=trigonal bipyramidal, mg=bent D. eg=linear, mg=linear E. eg=tetrahedral, mg=bent

eg=trigonal bipyramidal, mg=linear (b)

2. Determine the electron geometry (eg) and molecular geometry (mg) of PF5. A. eg=trigonal planar, mg=octahedral B. eg=tetrahedral, mg=trigonal pyramidal C. eg=trigonal bipyramidal, mg=trigonal bipyramidal D. eg=trigonal bipyramidal, mg=tetrahedral E. eg=octahedral, mg=octahedral

eg=trigonal bipyramidal, mg=trigonal bipyramidal (c)

1. Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A. eg=tetrahedral, mg=trigonal planar B. eg=tetrahedral, mg=trigonal pyramidal C. eg=trigonal bipyramidal, mg= trigonal bipyramidal D. eg=trigonal planar, mg=bent E. eg=trigonal planar, mg=trigonal planar

eg=trigonal planar, mg=trigonal planar (e)

24. List the number of sigma bonds and pi bonds in a triple bond. A. 0 sigma, 1 pi B. 3 sigma, 0 pi C. 1 sigma, 2 pi D. 2 sigma, 1 pi

1 sigma, 2 pi (c)

16. Identify the number of electron groups around a molecule with sp2 hybridization. A. 2 B. 3 C. 1 D. 5 E. 4

3 (b)

17. Identify the number of electron groups around a molecule with a trigonal bipyramidal shape. A. 4 B. 5 C. 2 D. 1 E. 3

5 (b)

12. Which of the molecules below will be polar? CS2, BF3, SO2, CH3Br A. CS2 only B. CH3Br only C. Both BF3 and CH3Br D. Both SO2 and CH3Br

Both SO2 and CH3Br (d)

4. What are the electron and molecular geometries, respectively, for hydrogen sulfide, H2S? Hints A. Electron geometry is bent. Molecular geometry is tetrahedral. B. Electron geometry is linear. Molecular geometry is bent. C. Electron geometry is tetrahedral. Molecular geometry is linear. D. Electron geometry is tetrahedral. Molecular geometry is bent.

Electron geometry is tetrahedral. Molecular geometry is bent. (d)

6. What are the electron and molecular geometries, respectively, for iodine trifluoride, IF3? A. Electron geometry is trigonal bipyramidal. Molecular geometry is T-shaped. B. Electron geometry is octahedral. Molecular geometry is T-shaped. C. Electron geometry is trigonal bipyramidal. Molecular geometry is trigonal planar. D. Electron geometry is trigonal planar. Molecular geometry is trigonal bipyramidal.

Electron geometry is trigonal bipyramidal. Molecular geometry is T-shaped. (a)

26. Part A. PF3Cl2 is a nonpolar molecule. Based on this information, determine the F−P−F bond angle, the Cl−P−Cl bond angle, and the F−P−Cl bond angle. Enter the number of degrees of the F−P−F, Cl−P−Cl, and F−P−Cl bond angles, separated by commas (e.g., 30,45,90) Part B. Which statement best describes the polarity of CF2I2? a. The molecule is always polar. b. The molecule is always nonpolar. c. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar. Part C. Which statement best describes the polarity of SCl4Br2? a. The molecule is always polar. b. The molecule is always nonpolar. c. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.

Part A. 120, 180, 90 degrees Part B. The molecule is always polar. (b) Part C. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar. (c)

5. A. What is the value of the bond angles in CH4? Enter the bond angle of the molecule. B. What is the value of the smallest bond angle in ClF4−? Enter the smallest bond angle of the molecule. C. What is the value of the bond angles in BF3? Enter the bond angle of the molecule. D. What is the value of the bond angle in I3−?

Part A: 109.5 degrees Part B: 90 degrees Part C: 120 degrees Part D: 180 degrees

14. Determine the electron geometry, molecular geometry and polarity of N2O (N central). A. eg=tetrahedral, mg=linear, polar B. eg= linear, mg=linear, polar C. eg=tetrahedral, mg=bent, polar D. eg=trigonal planar, mg=bent, nonpolar E. eg=linear, mg=linear, nonpolar

eg= linear, mg=linear, polar (b)

18. Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O. A. eg=bent, mg=bent, sp2 B. eg=tetrahedral, mg=bent, sp3 C. eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 D. eg=trigonal planar, mg=trigonal planar, sp2 E. eg=tetrahedral, mg=trigonal pyramidal, sp3

eg=tetrahedral, mg=bent, sp3 (e)

20. Give the hybridization for the Br in BrO4-. A. sp2 B. sp C. sp3d D. sp3 E. sp3d2

sp3 (d) (and yes nineteen and both have the same answers)

19. Give the hybridization for the O in OF2. A. sp B. sp3d2 C. sp3d D. sp2 E. sp3

sp3 (e)