Chapter 6 Chemical Bonding
1. Define electronegativity.
2. How does electronegativity vary as the atomic number of an element increases within
the same period of the periodic table?
3. How is the strength of a bond between two elements in a molecule related to their
electronegativities?
4. What is the difference between an ionic and a covalent bond?
5. How is the character of a bond (ionic or covalent) between two elements related to
their electronegativities?
6. Referring to electronegativit.ies, in your text, arrange the following
compounds in order of increasing ionic character of their bonds:
LiBr,
KCI,
KI,
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. What force holds the two ions together in an ionic bond?
9. What is the meaning of the valence or charge of an element that forms an ionic bond?
H. Cannon, C. Clapper and T. Guillot
Klein High School
Chemical Bonding
10. Given the electron configurations for the following neutral atoms, predict the
oxidation number each is most likely to have.
Element Configuration
Oxidation number
2 2
6 2
A
1s 2s 2p 3s
B
1s22s22p63s1
C
1s22s22p6
D
1s22s22p5
E
1s22s22p1
11. Write the correct formula for each of the following combinations of elements from
question 13. (If no reaction occurs, write none)
a. B and D
b. E and D
c. A and D
d. A and C
12. Underline the atom in each of the following pairs that has the lower electronegativity.
a. Li
Na
b. Cs Rb
c. Cs Ba
d. Cl Br
e. Fe Ni
f. S
Cl
13. List four general characteristics of compounds that have ionic bonds
14. Bonds between the which of the following pairs are
Al—Cl
K—F
Ba—Cl
15.
N—O
S—O
Fe—O
List three general characteristics of compounds formed entirely by covalent
compounds.
_________________________
________________________________
________________________________
16.
List three characteristics of metals.
___________________________________
___________________________________
___________________________________
17.
How does the bonding of atoms in a metal differ from the
bonding in a nonmetal?
6-2
HC/CC/TG KHS
Chemical Bonding
6-3
HC/CC/TG KHS
Chemical Bonding
Chapter 6 Bonding Worksheet
1) A chemical bond between atoms results
from the attraction between electrons
and what else?
a. neutrons
b. isotopes
c. protons
d. valence electrons
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
5) What type of chemical bond results
from the electrostatic attraction
between positive and negative ions?
a. ionic bond
b. metallic bond
c. polar covalent bond
d. nonpolar covalent bond
7. ________
8. ________
9. ________
10. ________
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
6) In a crystal of an ionic compound, each cation
is surrounded by what?
a. molecules
b. positive ions
c. dipoles
d. negative ions
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 ionic compound?
11. Name two elements that form compounds that are exceptions to the octet rule.
12.
13.
14.
15.
How does the energy of the crystal lattice formed in an ionic compound compare
with the energy of the neutral atoms involved in its formation?
a. higher in potential energy
b. lower in potential energy
c. equal in potential energy
d. unstable
____ What type of energy best represents the strength of an ionic bond?
____ What type of bonding holds a polyatomic ion together?
____ What type of forces holds two atoms together in an ionic bond?
6-4
HC/CC/TG KHS
Chemical Bonding
Metallic Bonds
1) Which of the following best describes
the valence electrons in metals?
a. attached to particular positive ions
b. shared by all surrounding ions
c. immobile
d. involved in covalent bonding
3) How does the strength of metallic
bonds vary moving from left to right in
any row of the periodic table?
a. increases
b. decreases
c. remains the same
2) Which of these best explains why
metals are malleable while ionic
crystals are brittle?
a. chemical bonds
b. London dispersion forces
c. heats of vaporization
d. polarity
4) How does drawing a metal into a wire
affect the metallic bonds?
a. break easily
b. break with difficulty
c. do not break
d. become ionic bonds
5.
Use the concept of electron configuration to explain why the number of valence
electrons in metals tends to be less than the number in most nonmetals.
6.
How does the behavior of the electrons in metals contribute to the distinctive
properties of metals?
a. luster
b. conductivity
c. malleability
d. ductility
Complete the following table
Components
Overall charge
Conductivity
Melting point
Hardness
Malleability
Ductility
Metallic
7.
9.
11.
13.
15.
17.
19.
Ionic
8.
10.
12.
14.
16.
18.
20.
6-5
HC/CC/TG KHS
Chemical Names and Formulas
Write the balanced ionic formulas:
Na +1
Mg +2
Fe +3
Pb +4
NH4 +1
Cl -1
O -2
P -3
OH -1
SO4 -2
PO4 -3
HSO3 -1
Cr2O7 -2
6-6
HC/CC/TG KHS
Chemical Names and Formulas
Draw dot diagrams for the following compounds:
1. Na + Cl
2. K + Br
3. Ba + F
4. Li + P
5. Mg + P
6. Ra + C!
7. Mg + S
8. Sr + 1
9. Cs + S
10. K + P
11. Ca + 0
12. Fr + F
13. Rb + 0
14. Ba + S
6-7
HC/CC/TG KHS
Chemical Names and Formulas
Binary Ionic Compounds
Write the formula for the following:
1. Sodium bromide
18.
Zinc phosphide
2.
Calcium oxide
19.
Chromium (III) oxide
3.
Manganese(II) oxide
20.
Antimony (V) sulfide
4.
Silver (I) Chloride
21.
Barium iodide
5.
Nickel(III)Bromide
22.
Potassium Sulfide
6.
Ferric Oxide
23.
Stannous oxide
7.
Cupric nitride
24.
Manganese (IV) fluoride
8.
Silver (I) oxide
25.
Zinc Sulfide
9.
Aluminum nitride
26.
Cobalt (II) iodide
10. Aluminum oxide
27.
Plumbous Chloride
11. Magnesium sulfide
28.
Mercury (I) oxide
12. Chromium (III)
phosphide
13. Zinc iodide
29.
Tin (IV) fluoride
30.
Iron (III) Chloride
14. Ferrous fluoride
31.
Tin (II) Sulfide
15. Lithium oxide
32.
Copper (I) Bromide
16. Cuprous sulfide
33.
Silver (I) iodide
17. Strontium nitride
Binary Ionic Compounds
*Name using the Latin system
6-8
HC/CC/TG KHS
Chemical Names and Formulas
1. chromium (II) oxide
21. CaBr2
2. strontium bromide
22. AlCl3
3. copper (I) sulfide
23. PbO2*
4. mercuric iodide
24. Co3N2
5. iron (II) sulfide
25. ZnO
6. ferrous fluoride
26. Mn3P4
7. potassium bromide
27. MgI2
8. cuprous oxide
28. AlP
9. iron (II) bromide
29. Fe2O3*
10. silver iodide
30. SnF2 *
11. plumbous phosphide
31. BaS
12. barium sulfide
32. MnO2
13. Lead (II) fluoride
33. NaCl
14. copper (II) chloride
34. HgO*
15. lead (IV) sulfide
35. SnCl4*
16. mercury (II) bromide
36. NiBr2
17. lithium chloride
37. AlI3
18. tin (IV) nitride
38. CuF*
19. mercury (I) nitride
39. B2S3
20. stannous chloride
40. Na2O
Ionic compounds Name the following compounds
1. NH4NO2
21. AgC2H3O2
6-9
HC/CC/TG KHS
Chemical Names and Formulas
2. Fe2(SO3)3
22. NaI
3. BaCl2
23. FeSO3
4. FeI2
24. Hg2Cl2
5. CsS
25. Pb(C2H3O2)4
6. Sn(NO3)4
26. NaOH
7. NaHCO3
27. KNO3
8. KCl
28. SrSO4
9. AlN
29. SrSO4
10. Ca3(PO4)2
30. MgSO4
11. Li2O
31. (NH4)3PO4
12. CrCl3
32. CuHCO3
13. Pb(NO3)2
33. CoCO3
14. Cu2S
34. SnSO3
15. Ca(C2H3O2)2
35. Na2CO3
16. Sb2S3
36. NH4CO3
17. Fe(C2H3O2)2
37. NaI
18. Ba(OH)2
38. (NH4)2SO4
19. Ag2SO4
39. Ca(C2H3O2)2
20. MgO2
40. ZnBr2
Naming Compounds
Write the name for:
6-10
HC/CC/TG KHS
Chemical Names and Formulas
1. Fe(NO2)2
11. KIO
2. (NH4)2SO4
12. LiCN
3. Ag2SO4
13. CuCl2
4. Zn(NO3)2
14. CuBr
5. NH4Br
15. Fe(NO3)2
6. BaCO3
16. FeCl3
7. Na3PO4
17. SnO2
8. K2CrO4
18. HgCO3
9. FeSO4
19. As(C2H3O2)3
10. (NH4)3PO4
20. NaClO2
Write the formula for:
1. sodium chlorite
11. ammonium dichromate
2. iron (III) perbromate
12. lead (II) acetate
3. calcium chlorate
13. iron (III) oxide
4. calcium hypochlorite
14. cobalt (II) nitrate
5. copper (II) chlorate
15. strontium nitrite
6. cadmium iodate
16. tin (IV) oxide
7. chromium (III) sulfite
17. aluminum phosphate
8. bismuth (III) chromate
18. cobalt (II) hydroxide
9. barium nitrite
19. potassium permanganate
10. aluminum sulfate
20. Iron (II) sulfate
Write the name of the following compounds:
1. Ba(ClO3)2
12. HMnO4
6-11
HC/CC/TG KHS
Chemical Names and Formulas
2. Na3P
13. Mg(OH)2
3. KOH
14. HBr
4. K2SO3
15. CaSO4
5. Al2(C2O4)3
16. Ba(OH)2
6. NH4OH
17. Al(OH)3
7. Cu3(PO3)2
18. HMnO4
8. Li2CO3
19. H2CrO4
9. Ag3PO4
20. Au(OH)3
10. K2SO4
21. NaCN
11. KF
22. K2SO4
6-12
HC/CC/TG KHS
Chemical Names and Formulas
Naming Acids and Bases
Name the following compounds:
1. HF
13. HCl
2. HI
14. H2S
3. H3N
15. HBr
4. H3AsO4
16. H3AsO3
5. NaOH
17. H3BO3
6. H3PO4
18. H3PO3
7. HNO3
19. H3P
8. NH4OH
20. HClO3
9. H2Cr2O7
21. HC2H3O2
10. Ca(OH)2
22. H2SO3
11. H2SO4
23. HIO3
12.
HIO4
Write the formula for the following:
1. sodium hydroxide
2. barium hydroxide
3. potassium hydroxide
4. calcium hydroxide
5. ammonium hydroxide
6. iron (III) hydroxide
7. cobalt (II) hydroxide
8. gold (III) hydroxide
9. tungsten (IV) hydroxide
10. cesium hydroxide
11. copper (II) hydroxide
12. mercury (I) hydroxide
13
HC/CC/TG KHS
Chemical Names and Formulas
Write the formula of the following compounds:
1. hydrochloric acid
14. hypochlorous acid
2. ammonium hydroxide
15. gold (III) hydroxide
3. barium phosphate
16. phosphoric acid
4. hydroselenic acid
17. acetic acid
5. hydroiodic acid
18. oxalic acid
6. hydrophosphoric acid
19. perchloric acid
7. permanganic acid
20. chlorous acid
8. chloric acid
21. nitrous acid
9. sulfurous acid
22. nitric acid
10. chromic acid
23. phosphorus acid
11. cyanic acid
24. hydronitric acid
12. hydrofluoric acid
25. hydrosulfuric acid
13.
silicic acid
14
HC/CC/TG KHS
Naming Compounds
Lab #1
Naming Compounds Lab
Purpose: To gain practice in writing formulas and naming compounds.
Procedure: Using a spot plate as a reaction vessel, combine the first chemical and the
second chemical. Be careful to use the bottle with the correct formula of the chemical
named. Record any changes observed following the addition of the second chemical. Be
careful not to touch the dropper to the spot plate well. If you do, it will cross-contaminate
the reagent bottles. Each solution contains two ions, one positive and one negative. The
product that we are interested in will be formed by combination of the underlined ions in
the reactants.
Reactants
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
Formula
Pos.
ion
Neg
ion
Ppt
Color
Formula
Name
Copper (II) sulfate
Sodium sulfide
Copper (II) sulfate
Ammonium hydroxide
Aluminum iodide
Ammonium hydroxide
Potassium chromate
Ammonium hydroxide
Potassium chromate
Silver (I) nitrate
Potassium chromate
Lead (II) nitrate
Lead (II) nitrate
Sodium phosphate
Aluminum iodide
Sodium phosphate
Aluminum iodide
Lead (II) nitrate
Aluminum iodide
Silver (I) nitrate
Sodium phosphate
Silver (I) nitrate
Sodium sulfide
Silver (I) nitrate
6-15
HC/CC/TG KHS