|9.||Which of the following molecules is polar?
|10.||Indicate the type of hybrid orbitals used by the central atom in TeF4.|
|11.||The hybridization of the O atom in CO2 will be|
|12.||The number of pi bonds in the molecule below is
13. Order the forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest .
a) dipole-dipole, London dispersion, ionic, and hydrogen-bonding
b) London dispersion, dipole-dipole, hydrogen-bonding, and ionic
c) hydrogen-bonding, dipole-dipole, London dispersion, and ionic
d) dipole-dipole, ionic, London dispersion, and hydrogen-bonding
e) London dispersion, ionic, dipole-dipole, and hydrogen-bonding
14. Which of the following would you expect to have the highest boiling point?
e) All of the above have the same boiling point.
15. The molecules in a sample of SO2 are attracted to each other by a combination of
a) London forces and H-bonding
b) H-bonding and ionic bonding
c) covalent bonding and dipole-dipole interactions
d) London forces and dipole-dipole interactions
e) none of these
16. When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction?
a) a hydrogen from one molecule and a hydrogen from the other molecule
b) a hydrogen from one molecule and an oxygen from the other molecule
c) an oxygen from one molecule and an oxygen from the other molecule
d) an oxygen and a hydrogen from the same molecule
e) two hydrogens from one molecule and one hydrogen from the other molecule
Chemical Bonding and Geometry
17. Which formula is matched with the correct number of valence electrons in the free (not bonded) central atom, bonds, and lone pairs in the molecule for the underlined atom?
a. SeH2; 6 valence electrons, 2 bonds, and 1 lone pair
b. SiCl4; 4 valence electrons, 4 bonds, and 0 lone pairs
c. FCl; 1 valence electron, 1 bond, and 0 lone pairs
d. SCl2; 6 valence electrons, 2 bonds, and 0 lone pairs
e. PH3; 4 valence electrons, 3 bonds, and 1 lone pair
18. The electron-dot structure for the species NH4O+ contains
a. 1 double bond and 4 single bonds
b. 5 single bonds and 3 lone pairs.
c. 5 single bonds and 2 lone pairs.
d. 5 single bonds and 1 lone pair.
e. 5 single bonds and zero lone pairs.
19. What is the hybridization of the carbon atom in CO2?
20. Which of the following molecules requires two resonance hybrid Lewis structures to account for the bonding?
21. Which of the following is the best electron-dot description for sulfur dioxide, SO2?
22. Which of the following compounds (or ions) contains an atom that does NOT follow the octet rule?
23. What is atom X in the Lewis structure of the following anion?
24. Which of the following statements is correct?
a. Covalent bonds usually involve two nonmetals and ionic bonds usually involve two metals.
b. Covalent bonds usually involve two metals and ionic bonds usually involve a metal and a nonmetal.
c. Covalent bonds usually involve a metal and a nonmetal and ionic bonds usually involve two nonmetals.
d. Covalent bonds usually involve two nonmetals and ionic bonds usually involve a metal and a nonmetal.
e. Covalent bonds usually involve two metals and ionic bonds involve two nonmetals.
25. The molecular structure of the IO3– ion is best described as:
a. bent or angular.
b. trigonal planar.
c. trigonal pyramidal.
d. trigonal bipyramidal.
26. The electron domain geometry of the AsF6– ion is octahedral. The hybrid orbitals used by the As atom for bonding are:
27. The F-B-F bond angle in BF3 is ____________.
28. The geometry associated with sp hybridization is:
c. trigonal biplanar
d. trigonal planar
29. Which series of elements is arranged in order of increasing electronegativity?
a. C, Si, P, As, Se
b. O, P, Al, Mg, K
c. Na, Li, B, N, F
d. K, Mg, Be, O, N
e. Li, Be, B, C, Ca
Use the following to answer questions 30-32:
Consider the representations below to answer the next three questions.
30. How many of the following statements are correct concerning drawing I?
|I.||Each molecule induces a dipole onto the next molecule in close proximity.|
|II.||The phenomenon shown is relatively weak and short-lived.|
|III.||All nonpolar molecules contains this type of interaction.|
|IV.||The forces that exist in this example are London dispersion forces.|