Chapter 7 Chemical Bonding
1. Define electronegativity.
2. How is the strength of a bond between two elements in a molecule related to their
electronegativities?
3. What is the difference between an ionic and a covalent bond?
4. How is the character of a bond (ionic or covalent) between two elements related to
their electronegativities?
5. Referring to electronegativit.ies, in your text, arrange the following compounds in
order of increasing ionic character of their bonds:
LiBr,
SO2,
Ca3P2,
LiF
7. Referring to Tables of electronegativities in your text, classify each of'
the following bonds as either ionic: (I) or covalent (C)
a. A1-O
f. N-O
b. Al-S
g. Na-S
c. Bi-CI
h. P-O
d. Bi-O
i. S-O
e. C- Cl
j. Ti-Br
8. List four general characteristics of compounds that have ionic bonds
9. Bonds between the which of the following pairs are covalent or ionic?
Al—Cl
K—F
N—O
S—O
H. Cannon, C. Clapper and T. Guillot
Klein High School
Chemical Bonding
Ba—Cl
10.
Fe—O
List three general characteristics of compounds formed entirely by
covalent bonds.
11. List three characteristics of metals.
12. How does the bonding of atoms in a metal differ from the bonding in a
nonmetal?
13. Indicate whether each property listed below is characteristic of ionic (I),
covalent (C), or metallic (M) bonding More than one letter may be used
for each answer.
__ a. Shape of solid can be changed by pounding.
__ b. Not electrically conducting in solid phase
__ c. Electrically conducting in all phases
__ d High melting points
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Chemical Bonding
Chapter 7 Bonding Worksheet
1) A chemical bond between atoms
results from what?
a. transfer of electrons
b. sharing of electrons
c. attraction of oppositely
charged ions
d. all of the above
3) As the electronegativity
difference between two atoms
bonded together increases, the
percentage of what else
increases?
a. ionic character
b. covalent character
c. metallic character
d. electron sharing
7. ________
8. ________
9. ________
10. ________
11.
12.
2) What makes up a covalent bond?
a. a shared electron
b. two different ions
c. an octet of electrons
d. a shared electron pair
4) Which of the following would describe
the electronegativity of an atom with a
strong attraction for the electrons they
share with another atom?
a. high electronegativity
b. low electronegativity
c. zero electronegativity
d. Lewis electronegativity
What do we call the electrons involved in forming a chemical
bond?
If a bond’s character is more than 50% ionic, what type of bond is
formed?
If a bond’s character is more than 50% ionic, what can we say
about the electronegativity difference between the two atoms?
What is an example of an molecular compound?
____ What type of bonding holds a polyatomic ion together?
____ What type of forces holds two atoms together in an ionic bond?
Complete the following table
Components
Overall charge
Conductivity
Melting point
Structure of compound
Solubility in water
Covalent
7.
9.
11.
13.
15.
17.
Ionic
8.
10.
12.
14.
16.
18.
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Chemical Bonding
Covalent Compounds
Name the following Compounds
Write formulas for the following
1. ClO2
2. sulfur dioxide
3. N2O5
4. carbon dioxide
5. CCl4
6. carbon monoxide
7. N2O3
8. dinitrogen monoxide
9. PCl5
10. diphosphorus pentasulfide
11. P4O10
12. dinitrogen tetroxide
13. PCl3
14. tetraphosphorus decoxide
15. SF6
16. sulfur trioxide
17. CS2
18. dinitrogen pentoxide
19. SO3
20. trihydrogen nitride
21. sulfur hexafluoride
22. dinitrogen trioxide
23. disulfur dichloride
24. disulfur decafluoride
25. diboron tetrabromide
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Chemical Bonding
Write the formulas for the following:
1. sodium hydroxide
16. antimony (V) phosphide
2. lithium bromide
17. potassium phosphate
3. aluminum bicarbonate
18. plumbic perchlorate
4. ferrous oxide
19. stannous fluoride
5. dinitrogen pentoxide
20. nickel (III) phosphide
6. chromium (II) nitrate
21. carbon tetrachloride
7. chromium (VI) oxide
22. ammoniun sulfite
8. mercury (II)chloride
23. iron (III) oxalate
9. gold (III) oxide
24. arsenic trichloride
10. aluminum bicarbonate
25. carbon monoxide
11. cupric sulfide
26. calcium chloride
12. nickel (III) phosphide
27. cobalt (II) iodide
13. carbon tetrahydride
28. sulfur dioxide
14. aluminum carbide
29. ferric oxide
15. titanium (llI) phosphate
30. titanium (IV)phosphate
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Unit Name
Exercise #
Covalent and Ionic Bonding Lab
Two of the characteristics that differentiate covalently bonded compounds from ionically
bonded compounds are solubility and melting point. In this investigation, you will test
these two properties of different compounds in order to predict the type of bonding
present in each.
Given the following compounds:
potassium dichromate K2Cr2O7
Para dichlorobenzene C6H4Cl2
nickel (II) sulfate
NiSO4
butanol
C4H9O
silicon dioxide
SiO2
Test the solubility in water by adding some of the chemical to a test tube containing
about “two fingers” of water and report the solubility qualitatively as “soluble”,
“insoluble”, or “partly soluble”.
Test the approximate melting point by placing a small amount of each of the solid
compounds in a test tube and heating gently with a Bunsen burner. Note: Some of the
chemicals may decrepitate (explode) upon strong heating, so increase the temperature
gradually.
If the compound melts below room temperature record “low”. If it melts easily under
moderate heat, record “moderate”. If it melts or clumps together only under extreme
heat, record “high”. If it never melts, record “very high”.
In your conclusion, state your assessment of the composition of the compounds with
regard to metallic or nonmetallic makeup and whether the bonding is ionic or covalent.
Questions:
1. Did you heat the butanol? Why or why not?
2. Why is it difficult to decide the bonding for silicon dioxide?
3. Assume you have never heard of CO2, but you have a periodic table. Compare
CO2 to SiO2. What type of bonding do you predict for CO2?
___________ Why?__________
4. Characterize the usual solubility, melting point and composition for ionically and
covalently bonded compounds.
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