Name: ____________________________ Period: _____ Date: ___________________________
Chapter 5: Compounds Pretest/Posttest
Not a whole lot of new vocabulary in this unit….
1. _____ another name for a charge on an ion
A. anion
B. cation
C. charge
D. covalent bond
E. diatomic molecule
F. ionic bond
G. metallic bond
H. nonpolar bond
I. oxidation number
J. polar bond
K. polyatomic ion
2. _____ when two or more atoms gain/lose
electrons when forming a compound
they form charged particles that are
attracted to each other. Happens
between metals and nonmetals.
3. _____ an element that always occurs in nature
with two atoms per molecule. There
are seven of them: N2, O2, F2, Cl2,
Br2, I2, and H2.
4. _____ an ion that has more than one atom to
it, but it acts like only one atom, e.g. OH-, SO42-, NH4+
5. _____ name for any ion with a negative charge
6. _____ a covalent bond in which the electrons are shared equally
7. _____ a bond between atoms of the same metal element, not between atoms of
different elements. It allows for many special properties.
8. _____ will be positive if the atom loses electrons or negative if it gains electrons
9. _____ bond in which atoms share electrons, between two nonmetals.
10. _____ name for any ion that has lost electrons and has positive charge
11. _____ a covalent bond in which the electrons are not shared equally; leads to
partial charges on the molecule
Determine the total number of atoms of each element in the following compounds.
12. C2H4
C = ________
H = ________
13. H3PO4
H = ________
P = ________
O = ________
14. Ni(OH)2
Ni = ________
O = ________
H = ________
15. Metals tend to _________________________ electrons, form _____________ ions
and can be found on the ___________ hand side of the periodic table.
16. Nonmetals tend to ____________________ electrons, form ______________
ions and can be found on the ____________ hand side of the periodic table.
17. – 18. Here is a periodic table. Draw the Lewis diagram and label the charge
(oxidation #) of each family. Skip 3 – 12.
Skip these for now.
19. ________________________ bonds form between metals and nonmetals when
electrons are _____________________.
20. _________________________ bonds form between two nonmetals when electrons
are ______________________.
Identify the following as ionic or covalent bonds.
21. ________________________ CO2
22. ________________________ (NH4)2O
23. ________________________ FeI3
Determine the charge on each metal ion in bold.
24. _________ Ag2O
25. _________ Fe2O3
26. _________ CuSO4
Use Lewis diagrams to show the bonding between the following atoms. Make sure to
use the correct method to show gaining, losing, or sharing.
27. Na + S
28. C + F
Write the name of the compound for each example given.
29. ___________________________ LiNO3
30. ___________________________ CaCl2
31. ___________________________ SBr2
Write the formula for each compound given.
32. ____________ magnesium iodide
33. ____________ diphosphorus trioxide
34. ____________ strontium sulfate
Balance the following chemical equations.
35.
_____ Fe + _____ Cl2  _____ FeCl3
36.
_____ H2 + _____ N2  _____ NH3
37.
_____ CaCl2 + _____ AgNO3  _____ AgCl + _____ Ca(NO3)2
Write and balance the following chemical equations.
38. Chlorine gas reacts with potassium bromide to form potassium chloride and
bromine.
39. Calcium oxide reacts with sulfur dioxide to form calcium sulfite.
Answer Key_
Name: __
Period: _____ Date: ___________________________
Chapter 5: Compounds Pretest/Posttest
Not a whole lot of new vocabulary in this unit….
I
1. __ __ another name for a charge on an ion
A. anion
B. cation
F__ when two or more atoms gain/lose
2. __
electrons when forming a compound
they form charged particles that are
attracted to each other. Happens
between metals and nonmetals.
C. charge
D. covalent bond
E. diatomic atom
F. ionic bond
G. metallic bond
with two atoms per molecule. There
are seven of them: N2, O2, F2, Cl2,
Br2, I2, and H2.
H. nonpolar bond
I. oxidation number
J. polar bond
K. polyatomic ion
E__ an atom that always occurs in nature
3. __
K__ an ion that has more than one atom to
4. __
it, but it acts like only one atom, e.g. OH-, SO42-, NH4+
A__ name for any ion with a negative charge
5. __
H__ a covalent bond in which the electrons are shared equally
6. __
G__ a bond between atoms of the same metal element, not between atoms of
7. __
different elements. It allows for many special properties.
C__ will be positive if the atom loses electrons or negative if it gains electrons
8. __
D__ bond in which atoms share electrons, between two nonmetals.
9. __
B__ name for any ion that has lost electrons and has positive charge
10. __
J__ a covalent bond in which the electrons are not shared equally; leads to
11. __
partial charges on the molecule
Determine the total number of atoms of each element in the following compounds.
12. C2H4
13. H3PO4
14. Ni(OH)2
2_
H = _3_
Ni = _1_
C=_
4_
P = _1_
O = _2_
H=_
4_
H = _2_
O=_
give away_ electrons, form _positive_ ions
15. Metals tend to _
left_ hand side of the periodic table.
16. Nonmetals tend to _take away_ electrons, form _negative_
ions and can be found on the _right hand_ hand side of the periodic
and can be found on the _
table.
17. – 18. Here is a periodic table. Draw the Lewis diagram and label the charge
(oxidation #) of each family. Skip 3 – 12.
Skip these for now.
ionic_ bonds form between metals and nonmetals when
electrons are _transferred_.
20. _covalent_ bonds form between two nonmetals when electrons
are _shared_.
19. _
Identify the following as ionic or covalent bonds.
covalent _ CO2
22. _both_ (NH4)2O (the bonds that hold N and H together are covalent. The
21. _
23. _
ionic _ FeI3
bonds that hold NH4 and O together are ionic. It is
considered to be an ionic compound)
Determine the charge on each metal ion in bold.
+2_ AgO
25. _+3_ Fe2O3
26. _+2_ CuSO4
24. _
Use Lewis diagrams to show the bonding between the following atoms. Make sure to
use the correct method to show gaining, losing, or sharing.
27. Na + S
28. C + F
Write the name of the compound for each example given.
lithium nitrate_ LiNO3
30. _calcium chloride_ CaCl2
31. _sulfur dibromide_ SBr2
29. _
Write the formula for each compound given.
MgI2_ magnesium iodide
33. _P2O3_ diphosphorus trioxide
34. _SrSO4_ strontium sulfate
32. _
Balance the following chemical equations.
35.
36.
37.
2_ Fe
_3_ H2
3_ Cl2  _2_ FeCl3
+ _____ N2  _2_ NH3
_____ CaCl2 + _2_ AgNO3  _2_ AgCl
_
+ _
Write and balance the following chemical equations.
+ _____ Ca(NO3)2
38. Chlorine gas reacts with potassium bromide to form potassium chloride and
bromine.
Cl2 + KBr  KCl + Br2 (unbalanced)
Cl2 + 2 KBr  2 KCl + Br2 (balanced)
39. Calcium oxide reacts with sulfur dioxide to form calcium sulfite.
CaO + SO2  CaSO3 (balanced)