Bonding
Unit 5 Page 1
Ionic Bonding Practice
1. 1 atom of lithium and 1 atom of fluorine
2. 1 atom of magnesium and 1 atom of oxygen
Formula Unit of Compound: _______________
Formula Unit of Compound: _______________
3. 1 atom of aluminum and 3 atoms of chlorine
4. 1 atom of calcium and 1 atom of sulfur
Formula Unit of Compound: _______________
Formula Unit of Compound: _______________
5. 1 atom of magnesium and ? atoms of bromine
6. 1 atom of potassium and ? atoms of chlorine
Formula Unit of Compound: _______________
Formula Unit of Compound: _______________
Bonding
Guided Practice
1. lithium fluoride
Unit 5 Page 2
Ionic Naming Practice
1. CaCl2
2. copper (II) chloride
2. FeCl3
3. lithium dichromate
3. Fe2(SO4)3
4. magnesium acetate
4. Na3PO4
5. sodium arsenate
5. KIO3
6. chromium (II) hydroxide
6. Cu(ClO4)2 ∙ 6H2O
7. lead (IV) sulfate
7. NaHSO4
8. magnesium sulfate heptahydrate
8. CuS2O3
9. ammonium nitrate
9. PbF2
Independent Practice
Formula to Name
Name to Formula
1. NaF
1. potassium fluoride
2. K2CO3
2. ammonium sulfate
3. MgCl2
3. magnesium iodide
4. Be(OH)2
4. copper (II) sulfite
5. SrS
5. aluminum phosphate
6. Cu2S
6. lead (II) nitrite
7. ZnI2
7. cobalt (II) selenide
8. Ca3(PO4)2
8. silver cyanide
9. NH4I
9. copper (II) bicarbonate
10. Mn(NO3)3
10. iron (II) oxide
11. FePO4
11. lithium cyanide
12. CoCO3
12. lead (IV) sulfite
13. HgCl
13. potassium permanganate
14. Fe2O3
14. vanadium (III) selenide
15. BeO
15. copper (II) chloride
Bonding
Unit 5 Page 4
Covalent Bonding Practice
Directions: Show how the atoms below would form covalent bonds by first drawing the neutral atoms and then
redrawing the molecule the atoms would form.
1. 2 atoms of hydrogen
2. 2 atoms of fluorine
3. 2 atoms of oxygen
4. 2 atoms of nitrogen
5. 4 atoms of hydrogen and 1 atom of carbon
6. 2 atoms of hydrogen and two atoms of carbon
Bonding
Unit 5 Page 5
Covalent Naming Practice
Guided Practice
1. bromine trioxide
11. CO2
2. tetrarsenic decoxide
12. CCl4
3. dinitrogen trioxide
13. PCl5
4. nitrogen triiodide
14. SeF6
5. sulfur hexafluoride
15. As2O5
6. phosphorus trichloride
16. XeF6
7. carbon monoxide
17. SO3
8. diphosphorus pentoxide
18. N2S4
9. dihydrogen monoxide
19. NI3
10. tetraphosphorous decoxide
20. P2O5
Independent Practice
1. dinitrogen monoxide
11. P4S3
2. sulfur trioxide
12. CBr4
3. iodine trichloride
13. N2O
4. phosphorus pentabromide
14. SeF6
5. carbon tetraiodide
15. B2Cl4
6. phosphorus trichloride
16. AsF5
7. dinitrogen trioxide
17. BF3
8. disulfur dichloride
18. P4S3
9. carbon diselenide
19. Cl2O7
10. dinitrogen pentoxide
20. CO
Bonding
Unit 5 Page 6
Polar vs Non-polar Covalent Practice
Directions: Show how the atoms below would form covalent bonds by first drawing the neutral atoms and then
redrawing the molecule the atoms would form. If the bonds are polar, indicate the direction of the dipole.
1. 2 atoms of nitrogen
Difference in electronegativity: ____________
Polar or Non-polar: _______________
3. 2 atoms of hydrogen and 1 atom of oxygen
2. 1 atom of hydrogen and 1 atom of chlorine
Example 1: CH4
C
H
H
H
H
N
A
S
Example 2: OF2
O
F
F
N
Difference in electronegativity: ____________
A
S or Non-polar: _______________
Polar
Example 3: CO2
4. 2 atomsCof sulfurOand 1 atom
O of carbon
N
A
S
Example 4: SF6
S F
F
N
F
F
F
Difference in electronegativity: ____________
A
Difference
in electronegativity: ____________
Polar or Non-polar: _______________
S or Non-polar: _______________
Polar
5. 4 atoms of hydrogen and 1 atom of carbon
6. 3 atoms of hydrogen and 1 atom of nitrogen
Example 5: SO22S
O
N
O
charge
A
S
Lewis
Structures
Practice: Draw
the Lewis Structures for
each compound
or ion listed
below.
Difference
in electronegativity:
____________
Difference
in electronegativity:
____________
Polar or Non-polar: _______________
Polar or Non-polar: _______________
F
Bonding
Unit 5 Page 8
Covalent Lewis Structure Practice
NH3
CCl4
SO3-2
C2H6
H2CO
N2
CO2
O2
NH4+1
PH3
Lewis Structures Practice: Draw the Lewis Structures for each compound or ion listed below.
SO4-2
SO2
OF2 (O in the middle)
HOOH
AsF3
HCN
COCl2 (everything attaches to C) (that says Cl,
NOT C I)
SiH4
H2S
PO4-3
Bonding
Unit 5 Page 12
IMF Practice
Guided/Independent Practice
Directions: Draw the Lewis structure for each of the following molecules, and draw dipoles where appropriate.
Indicate the type of intermolecular force for each (Dispersion, Dipole-Dipole, or Hydrogen Bonding).
HF
N2
1. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
2. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
NH3
H2O
3. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
4. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
CCl4
BF3
5. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
6. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
SF6
CF4
7. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
8. a. Is the molecule polar or non-polar? _________
b. Type of IMF __________________________
Bonding
Unit 5
Mixed Naming Practice
Identify the type of compound and write the name or formula.
1. Na2CO3________________________________
21. Dinitrogen trioxide_______________________
2. P2O5___________________________________
22. Nitrogen________________________________
3. NF3____________________________________
23. Lithium acetate__________________________
4. FeSO4__________________________________
24. Phosphorus trifluoride_____________________
5. SiO2___________________________________
25. Vanadium (V) oxide______________________
6. GaCl3__________________________________
26. Aluminum hydroxide_____________________
7. CoBr2__________________________________
27. Zinc sulfide_____________________________
8. B2H4___________________________________
28. Silicon tetrafluoride______________________
9. CO____________________________________
29. Silver phosphate_________________________
10. P4_____________________________________
30. Tetraphosphorus triselenide_______________
11. BBr3___________________________________
31. Potassium nitrite_______________________
12. Ca3(PO4)2_______________________________
32. Iron (II) phosphide______________________
13. C2Br6__________________________________
33. Disilicon hexabromide___________________
14. Cr(CO3)3_______________________________
34. Titanium (IV) nitrate____________________
15. Ag3P___________________________________
35. Diselenium diiodide____________________
16. IO2____________________________________
36. Copper (I) phosphate____________________
17. VO2___________________________________
37. Gallium oxide__________________________
18. PbS____________________________________
38. Tetrasulfur dinitride_____________________
19. CI4____________________________________
39. Phosphorus____________________________
20. N2O3___________________________________
40. Silicon trioxide_________________________