quiz5 Flashcards

1. Based on valence bond theory, which statement best describes the electron geometry, bonding and hybridization of the central atom in carbon tetrachloride CCl4?
A. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp3 hybridization. The C-Cl bond is of σ-character.
B. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp2 hybridization. The C-Cl bond is of σ-character.
C. The electron geometry of carbon in carbon tetrachloride is tetrahedral with a sp3 hybridization. The C-Cl bond is of π-character.

2. Based on valence bond theory, which statement best describes the electron geometry and hybridization of the central atom(s) in acetylene C2H2?
A. The electron geometry of the 2 carbons in acetylene is tetrahedral with a sp3 hybridization.
B. The electron geometry of the 2 carbons in acetylene is trigonal planar with a sp2 hybridization.
C. The electron geometry of the 2 carbons in acetylene is linear with a sp hybridization.

3. Which statement best describe the structure of a carbonate anion CO32- ?
A. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a π-bond formed between a nonhybridized “C” p-orbital overlapping with an “O” p-orbital.
B. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are >120°. There is a π-bond formed between a nonhybridized “C” p-orbital overlapping with an “O” p-orbital.
C. The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are <120°. There is a π-bond formed

4. Based on valence bond theory, what is the hybridization of the central atom(s) in C2F4?
A. both carbons are sp3
B. one carbon is sp3 and the other carbon is sp2
C. both carbons are sp2

5. Which element contains triple covalent bonds?
A. oxygen
B. nitrogen
C. iodine

6. Explain how σ and π bonds are similar and how they are different.
A. Similarities: Both types of bonds result from overlap of atomic orbitals on adjacent atoms.

B. Differences: σ bonds are stronger and result from end-to-end overlap and all single bonds are σ bonds; π bonds between the same two atoms are weaker because they result from side-by-side overlap, and multiple bonds contain one or more π bonds (in addition to a σ bond).
C. C. Both A and B are correct.

7. How many σ and π bonds are present in the molecule HCN?
A. H C N  has one σ (H–C) and three π
B. H C N  has two σ (H–C and C–N) and two π
C. H C N  has two σ (H–C and C–N) and one π

8. Draw the Lewis structure for CO2, and predict the number of σ and π bonds for it.
A. Lewis structure of CO2 is , it has two σ and two π
B. Every single covalent bond is a sigma bond.
C.Every double covalent bond has both a sigma and a pi bond in it.
D. Every triple covalent bond has a sigma and two pi bonds in it.

9. Draw the Lewis structure for CO, and predict the number of σ and π bonds it has.
A. Lewis structure of CO is , it has two σ and two π
B. Lewis structure of CO is , it has one σ and two π
C. Lewis structure of CO is , it has two σ and one π

10. Give the shape that describes the hybrid orbital set sp2:
A. trigonal planar
B. trigonal bipyramidal
C. linear
D. octahedral

11. Give the shape that describes the hybrid orbital set sp3d:
A. trigonal planar
B. trigonal bipyramidal
C. linear
D. octahedral

12. Give the shape that describes the hybrid orbital set sp:
A. trigonal planar
B. trigonal bipyramidal
C. linear
D. octahedral

13. Give the shape that describes the hybrid orbital set sp3d2:
A. trigonal planar
B. trigonal bipyramidal
C. linear
D. octahedral

14. Give the shape that describes the hybrid orbital set sp3:
A. trigonal planar
B. trigonal bipyramidal
C. linear
D. tetrahedral

15. What is the hybridization of the central atom in BeH2?
A. sp
B. sp3d2
C. sp3
D. sp3d

16. What is the hybridization of the central atom in SF6?
A. sp
B. sp3d2
C. sp3
D. sp3d

17. What is the hybridization of the central atom in PO43– ?
A. sp
B. sp3d2
C. sp3
D. sp3d

18. What is the hybridization of the central atom in XeF4?
A. sp
B. sp3d2
C. sp3
D. sp3d

19. What is the hybridization of the central atom in PCl5?
A. sp
B. sp3d2
C. sp3
D. sp3d

20. Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino acid found in proteins. Lewis structure of this compound is shown below. What is the hybridization type of the nitrogen?

A. sp3
B. sp2
C. sp

21. Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino acid found in proteins. Lewis structure of this compound is shown below. What is the hybridization type of the sulfur?

A. sp3
B. sp2
C. sp

22. Identify the hybridization of the central atom in NO2
A. sp2
B. sp
C. sp3
D. sp3d

23. Predict the molecular geometry of XeF2 molecule by VSEPR.

A. bent
B. linear
C. tetrahedral

24. Predict the molecular geometry of SO3 molecule by VSEPR.

A. bent
B. trigonal planar
C. tetrahedral

26. Predict the geometry about the first carbon atom (on the left), determine the hybridization type of that carbon atom.

A. tetrahedral, sp3
B. trigonal planar, sp2
C. linear, sp

27. For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it is XeF2. Predict the shape of the molecules of the compound, what hybridization is consistent with the shape you predicted?

A. linear, sp3d hybridization
B. octahedral, sp3d2 hybridization
C. seesaw, sp3d hybridization
D. T-shaped, sp3d hybridization

28. Which of the following molecules are paramagnetic according to molecular orbital theory?
A. C2
B. F2
C. N2
D. O2
he oxygen atom to create a π bond.

29. For the carbonate ion, CO32– , which of the following is a correct description of its bonding?
A. In the structure, the carbon is sp2 hybridized, and each of the three sp2 orbitals overlaps with an oxygen orbital to create a σ bond. The unhybridized p orbital on the carbon atom overlaps with a p orbital on the oxygen atom to create a π bond.
B. In the structure, the carbon is sp3 hybridized, and each of the four sp3 orbitals overlaps with an oxygen orbital to create a σ bond.
C. In the structure, the carbon is sp hybridized, and each of the two sp orbitals overlaps with an oxygen orbital to create a σ bond. The unhybridized p orbitals on the carbon atom overlaps with a p orbital on t

30. Identify the hybridization of the central atom in CS2
A. sp2
B. sp
C. sp3
D. sp3d