Chapter 8 Study Guide: bonding…not James Bond




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Chapter 8 Study Guide: BONDing…not James Bond





  1. In the gaseous phase, which of the following compounds would be the most polar?

a) CsF

b) CsCl


c) NaCl

  1. NaF

  2. LiF




  1. Based on electronegativities, which of the following would you expect to be most ionic?

a) N2

b) CaF2

c) CO2

d) CH4

e) CF4


  1. Which of the following molecules has no dipole moment?

a) CO2

b) NH3

c) H2O

d) all


e) none


  1. Choose the molecule with the strongest bond.

a) CH4

b) H2O

c) NH3

d) HF


e) All are equal


  1. As indicated by Lewis structures, which of the following would probably not exist as a stable molecule?

a) CH3OH

b) CH2O

c) CH3O

d) C2H2

e) C3H4

Use the following to answer questions 6-8:


Draw the Lewis structures of the molecules below and use them to answer the following questions:

I.

BH3

II.

NO2-

III.

SF6

IV.

O3

V.

PCl5




  1. Which of the molecules obeys the octet rule?

a) I only

b) II and III

c) III and IV

d) I and IV

e) V


  1. How many of the molecules have no dipole moment?

a) 1

b) 2


c) 3

d) 4


e) They are all polar.


  1. Which of these molecules show resonance?

a) I, II

b) II, IV

c) II, V


  1. III, IV

  2. III, V




  1. This molecule contains a carbon atom with trigonal planar geometry.

a) CH3CHO

b) CO2

c) CH3Cl

d) C2H6

e) none of these


  1. This molecule shows the smallest number of lone pairs in its Lewis structure.

a) CH3CHO

b) CO2

c) CH3Cl

d) C2H6

e) All have zero lone pairs.


  1. When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that is found to have the empirical formula SCl. Which of the following could be the correct Lewis structure for this compound?

a)

b)

c)

d)

e) :


  1. In the Lewis structure for ICl2, how many lone pairs of electrons are around the central iodine atom?

a) 0

b) 1


c) 2

d) 3


e) 4
Use the following to answer questions 13-15:
Consider the following molecules.

I.

BF3

II.

CHBr3 (C is the central atom)

III.

Br2

IV.

XeCl2

V.

CO

VI.

SF4

Select the molecule(s) that fit the given statement.

  1. These molecules violate the octet rule.

a) I, II, IV

b) I, III, IV, VI

c) III, V, VI

d) I, IV, VI

e) I, II, IV, VI


  1. These molecules have a zero net dipole moment.

a) III, V

b) I, III, IV

c) III, IV, V

d) I, III, IV, VI

e) none of them


  1. These molecules are part of the AX5 family.

a) II, IV, VI

b) I, IV


c) IV, VI

d) VI only

e) none of them


  1. The hybridization of the central atom in XeF5+ is:

a) sp

b) sp2

c) sp3

d) sp3d

e) sp3d2


  1. The hybridization of the central atom in O3 is:

a) sp

b) sp2

c) sp3

d) sp3d

e) sp3d2


  1. Which of the following molecules contains a central atom with sp2 hybridization?

a)



b)

c)


d)


e)





  1. Consider the following Lewis structure:

Which statement about the molecule is false?

a) There are 10 sigma and 2 pi bonds.

b) C-2 is sp2 hybridized with bond angles of 120°.

c) Oxygen is sp3 hybridized.

d) This molecule contains 28 valence electrons.

e) There are some H–C–H bond angles of about 109° in the molecule.


  1. When a carbon atom has sp3 hybridization, it has

a) four  bonds

b) three  bonds and one  bond

c) two  bonds and two  bonds

d) one  bond and three  bonds

e) four  bonds


  1. Which of the following statements is (are) incorrect?

I.

The hybridization of boron in BF3 is sp2.

II.

The molecule XeF4 is nonpolar.

III.

The bond order of N2 is three.

IV.

The molecule HCN has two pi bonds and two sigma bonds.

a) All four statements are correct.

b) II is incorrect.

c) I and IV are incorrect.

d) II and III are incorrect.



e) II, III, and IV are incorrect.


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