MR. SURRETTE VAN NUYS HIGH SCHOOL
CHAPTER 18 : ELECTRONEGATIVITY AND POLARITY
WORKSHEET SOLUTIONS
1. Atoms that share electrons evenly form __________ bonds.
1A. covalent
2. Atoms that share electrons unevenly form __________ bonds.
2A. polar
3. Atoms that transfer electrons form __________ bonds.
3A. ionic
4. Dipoles are found in __________ substances.
4A. polar
5. Out of the following choices, __________ has the greatest electronegativity value.
(A) tungsten
(B) rubidium
(C) arsenic
(D) hydrogen
(E) chlorine
6. Out of the following choices, __________ has the greatest electronegativity value.
(A) chlorine
(B) iodine
(C) fluorine
(D) phosphorus
(E) strontium
7. Out of the following choices, __________ has the greatest electronegativity value.
(A) potassium
(B) boron
(C) sulfur
(D) oxygen
(E) barium
8. Predict the type of bond created when four hydrogen atoms bond with one carbon atom.
8A. covalent
9. Predict the type of bond created when two hydrogen and one oxygen atom form water.
9A. polar
10. Predict the type of bond created when two silicon and one oxygen atom form SiO2.
10A. polar
11. Predict the type of bond created when two gallium and three oxygen atoms form Ga2O3.
11A. polar
12. Predict the type of bond created when one carbon and four fluorine atoms form CF4.
12A. polar
13. Draw the LDS diagram for argon.
13A.
14. Complete the following steps and construct the LDS diagram for beryllium oxide.
14a. Draw LDS diagrams for beryllium and oxygen.
A.
14b. Show the transfer of electrons that forms beryllium oxide.
A.
14c. Draw the LDS diagram for beryllium oxide.
A.
15. Two oxygen and one carbon atom combine to form carbon dioxide. Complete the following steps to construct the structural diagram for CO2.
15a. Draw the LDS diagrams for oxygen and carbon.
A.
15b. Show the sharing of electrons to form carbon dioxide.
A.
15c. Draw the LDS diagram for carbon dioxide.
A.
15d. Draw the structural diagram for carbon dioxide.
A.
CHAPTER 18 :
POLARITY AND ELECTRONEGATIVITY
QUIZ SOLUTIONS
1. Atoms that share electrons unevenly form __________ bonds.
1A. polar
2. Atoms that transfer electrons form __________ bonds.
2A. ionic
3. Dipoles are found in __________ substances.
3A. polar
4. Out of the following choices, __________ has the lowest electronegativity value.
(A) chlorine
(B) rubidium
(C) arsenic
(D) hydrogen
5. Out of the following choices, __________ has the lowest electronegativity value.
(A) chlorine
(B) iodine
(C) fluorine
(D) phosphorus
6. Out of the following choices, __________ has the lowest electronegativity value.
(A) potassium
(B) boron
(C) sulfur
(D) oxygen
7. Predict the type of bond created when two fluorine atoms form F2.
7A. covalent
8. Predict the type of bond created when one calcium and one oxygen atom form CaO.
8A. ionic
9. Predict the type of bond created when two chlorine atoms form Cl2.
9A. covalent
10. Predict the type of bond created when one potassium and one chlorine atom form KCl.
10A. ionic
11. Predict the type of bond created when one carbon and four fluorine atoms form CF4.
11A. polar
12. Predict the type of bond created when two boron and three oxygen atoms form B2O3.
12A. polar
13. Draw the LDS diagram for fluorine.
13A.
14. Lithium and fluorine combine. Provide the LDS diagram for this compound.
14A.
15. Hydrogen and nitrogen combine to form ammonia. Provide the LDS diagram for this compound.
15A.
16. Aluminum and oxygen combine. Provide the LDS diagram for this compound.
16A.
(1) Aluminum has a + 3 charge.
(2) Oxygen has a - 2 charge.
(3) In order for the aluminum and oxygen charges to balance, cross-multiply the charges:
Al x 2 = 2 aluminum atoms.
O x 3 = 3 oxygen atoms.
(4) This makes the possible compound: Al2O3
(5) Double-check the charges on Al2O3:
Aluminum: + 3 x 2 = + 6.
Oxygen: - 2 x 3 = - 6.
Net charge : 0
(6) Number of available electrons for Al2O3:
Aluminum: Al x 2 = (3 e-) x 2 = 6 e-
Oxygen: O x 3 = (6 e-) x 3 = 18 e-
Total electrons : 24 e-
16A. (continued...)
(7) Aluminum atom: 3 valence electrons. Aluminum is a metal. It shares six electrons within compounds (it donates three from itself and accepts three from other atoms).
(8) Oxygen atom: 6 valence electrons. Oxygen is a non-metal. It surrounds itself with eight electrons (the octet rule).
(9) One possible LDS diagram for Al 2 O 3:
17. Boron and sulfur combine. Provide the LDS diagram for this compound.
17A.
(1) Boron has a + 3 charge.
(2) Sulfur has a - 2 charge.
(3) In order for the boron and sulfur charges to balance, cross-multiply the charges:
B x 2 = 2 boron atoms.
S x 3 = 3 sulfur atoms.
(4) This makes the possible compound: B2S3
(5) Double-check the charges on B2S3:
Boron: + 3 x 2 = + 6.
Sulfur: - 2 x 3 = - 6.
Net charge : 0
(6) Number of available electrons for B2S3:
Boron: B x 2 = (3 e-) x 2 = 6 e-
Sulfur: S x 3 = (6 e-) x 3 = 18 e-
Total electrons : 24 e-
(7) Boron atom: 3 valence electrons. Boron is a metal. It shares six electrons within compounds (it donates three from itself and accepts three from other atoms).
(8) Sulfur atom: 6 valence electrons. Sulfur is a non-metal. It surrounds itself with eight electrons (the octet rule).
(9) One possible LDS diagram for B 2 S 3:
18. Magnesium and nitrogen combine. Provide the LDS diagram for this compound.
18A.
(1) Magnesium has a + 2 charge.
(2) Nitrogen has a - 3 charge.
(3) In order for the magnesium and nitrogen charges to balance, cross-multiply the charges:
Mg x 3 = 3 magnesium atoms.
N x 2 = 2 nitrogen atoms.
(4) This makes the possible compound: Mg3N2
(5) Double-check the charges on Mg3N2:
Magnesium: + 2 x 3 = + 6.
Nitrogen: - 3 x 2 = - 6.
Net charge : 0
(6) Number of available electrons for Mg3N2:
Magnesium: Mg x 3 = (2 e-) x 3 = 6 e-
Nitrogen: N x 2 = (5 e-) x 2 = 10 e-
Total electrons : 16 e-
(7) Magnesium atom: 2 valence electrons. Magnesium is a metal. It shares four electrons within compounds (it donates two from itself and accepts two from other atoms).
(8) Nitrogen atom: 5 valence electrons. Nitrogen is a non-metal. It surrounds itself with eight electrons (the octet rule).
(9) One possible LDS diagram for Mg 3 N 2:
CHEMISTRY PAGE 6