Chapter 9: Chemical Bonds Study Guide
Multiple Choice—concept based and some problems
1. Of the following compounds, which is the most ionic?
(A)
(B)
(C)
(D)
(E)
SiCl4
BrCl
PCl3
Cl2O
CaCl2
2. The best explanation for the fact that diamond is extremely hard is that diamond
crystals
(A)
are made up of atoms that are intrinsically hard because of their electronic
structures.
consist of positive and negative ions that are strongly attracted to each other.
are giant molecules in which each atom forms strong covalent bonds with all of its
neighboring atoms.
are formed under extreme conditions of temperature and pressure.
contain orbitals or bands of delocalized electrons that belong not to single atoms
but to each crystal as a whole.
(B)
(C)
(D)
(E)
1999
Questions 14-17 refer to the following descriptions of bonding in different types of
solids.
(A) Lattice of positive and negative ions held together by electrostatic forces.
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces.
(D) Strong multiple covalent bonds (including bonds.) with weak intermolecular
forces
(E) Macromolecules held together with strong polar bonds.
14. Cesium chloride, CsCl (s)
15. Gold, Au(s)
16. Carbon dioxide, CO2(s)
17. Methane, CH4(s)
1994
Questions 21-23 refer to the following diatomic species.
(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2
21. Has the largest bond-dissociation energy
22. Has a bond order of 2
1994
28. The electron-dot structure (Lewis structure) for which of the following molecules
would have two unshared pairs of electrons on the central atom?
(A) H2S
(B) NH3
(C) CH4
(D) HCN
(E) CO2
3. Consider the carbon dioxide molecule, CO2, and the carbonate ion, CO32–.
(i) Draw the complete Lewis electron-dot structure for each species.
(ii) Account for the fact at the carbon-oxygen bond length in CO32– is greater than
the carbon-oxygen bond length in CO2.
4. When a covalent bond is formed between atoms of two different elements:
A) the bond is ionic;
B) both atoms attain an inert gas
configuration;
C) the electrons of the bond are shared equally between the two atoms;
D) the electrons of the bond spend more time in the vicinity of the more
electronegative element;
E) one atom is metallic.
5. Based on the formal charges, which is the predicted arrangement:
NOBr
BrNO
Types of bonding:
A) ionic
B) nonpolar covalent
E) metallic
NBrO
C) polar covalent;
D) coordinate covalent;
6._____ Which type of bond accounts for the high electrical conductivity of copper?
7._____ When an electron pair is shared equally between two atoms, what type of bond
exists?
8._____ What type of bond would be predicted in sodium oxide?
9._____ What type of bond would be expected to produce hydrogen selenide gas?
10. Which chemical compound has the HIGHEST bond dissociation energy?
a) O2
b) N2
c) Cl2
d) HF
Problems:
10. Draw ALL of the resonance structures for CO3-2.
11. Draw ALL of the resonance structures for O3.
12. Determine the O-F bond length in the chemical compound: OF2
13. Which element in each problem is the most electronegative?
a) Br, F
b) Br, Se
c) Cl, As
d) N, H
14. Draw Lewis structures for the following covalent molecules:
a) CH3OH
b) NH2OH
15. Draw the Lewis structures for both acetic acid AND acetate ion. Which structure has
resonance potential?
16. Using the following equation:
CH4 + Cl2
CH3Cl + HCl
Calculate the ΔH rxn
17. Hydrogen peroxide has an O-O bond length of 147.5pm and 2 O-H bonds with
lengths of 95.0pm. Draw the appropriate Lewis structure
**Look over the exceptions and be able to explain why a certain Lewis structure is
wrong or correct! **
**Look over concepts of metallic bonding **
**Review homework assignments/problems and look over AP questions. **