Name:___________________________________
Date:_______________ Period:___
Review Chemistry I Honors
Unit 6: Ionic Compounds – Bonding and Nomenclature
1. Positive ions are called ______________. Negative ions are called ______________.
2. Why do chemical bonds form between atoms? (or…Why don’t atoms just stay single?)
3. In an ionic bond, electrons are
shared / transferred / connected
between atoms. (circle one)
4. An ionic bond is a chemical bond caused by electrostatic _________________________ between
______________ and _____________ that is formed by ____________________________ electrons
between atoms.
Ionic bonds form between ____________ and ____________. (metals, nonmetals, metalloids)
5. Circle the ionic compounds listed below.
CaSO4
CH4
CO2
BaCl2
NH3
KNO3
LiOH
6. How did you know which compounds in Question 5 above were ionic?
7. For the pairs of elements listed below, circle pairs that would likely form ionic bonds.
C and H
Na and F
Hg and Ag
Mg and S
N and C
K and O
8. What are binary ionic compounds? _____________________________________________________
_________________________________________________________________________________
9. Binary ionic compounds typically end with the suffix –_____.
10. A “formula unit” is the simplest or lowest ____________ of ___________ in an ionic compound.
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11. How do each of the following atoms achieve a stable octet?
(circle gain or lose and write in a number of electrons)
O will gain / lose ___ electrons
Li will gain / lose ___ electrons
N will gain / lose ___ electrons
12. List the oxidation number and group name for the following groups of elements.
Group 1
___
name: ___________________________
Group 2
___
name: ___________________________
Group 16 (6A) ___
name: _chalcogens_________________
Group 17 (7A) ___
name: ___________________________
13. List 3 physical properties of ionic compounds:
1. _____________________________________________
2. _____________________________________________
3. _____________________________________________
14. Determine the total number of atoms in each formula listed below.
Li3PO4
____
Ba(NO3)2
____
15. Determine the total number of ions in each formula listed below.
Li3PO4
____
Ba(NO3)2
____
16. Which of the following compounds contains the Sn4+ ion?
A. Sn2Br
B. SnCI
C. SnI2
D. SnO2
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17. Name the following compounds. (some compounds may need a Roman numeral)
(refer to a list of polyatomic ions if necessary)
MgI2
________________________
Fe2O3
________________________
Al(NO3)3
________________________
NH4Br
________________________
CuCO3
________________________
KHCO3
Ba(C2H3O2)2
________________________
SnCl4
________________________
________________________
18. Write a formula for the following chemical compounds. (refer to a list of polyatomic ions if necessary)
copper(I) oxide
______________
ammonium nitrate
______________
potassium phosphate ______________
iron(III) sulfide
______________
calcium hydroxide
______________
lead(II) iodide
______________
aluminum sulfate
______________
nickel(II) bromide
______________
19. Draw a Lewis Dot diagram for each the following ionic compounds.
NaF
CaCl2
K2S
20. What is the oxidation number of the unknown element X in the compound MgX2 ?
A. 1–
B. 2–
C. 1+
D. 2+
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KEY
1. Positive ions are called cations. Negative ions are called anions.
2. The formation of chemical bonds results in the formation of a more stable electron configuration (in
some cases, an octet) for atoms.
3. transferred
4. An ionic bond is a chemical bond caused by electrostatic _attraction_ between
__cations___ and __anions__ that is formed by __transferring__ electrons
between atoms.
Ionic bonds always from between __metals__ and __nonmetals_. (metals, nonmetals, metalloids)
5. CaSO4, BaCl2, KNO3, LiOH
6. a metal bonded to a nonmetal
7. Na & F , Mg & S , K & O
8. Ionic compound consisting of only two different elements
9. –ide
10. ratio (or combination) , ions
11. O gain 2 electrons
Li lose 1 electron
12. Group 1: 1+ (alkali metals)
Group 16: 2–
N gain 3 electrons
Group 2: 2+ (alkaline earth metals)
Group 17: 1– (halogens)
13. Ionic compounds:
-are crystalline solids at room temperature
-have high melting points
-conduct an electric current in the molten (liquid) state or in solution (dissolved in water)
14. Li3PO4 : 8 atoms Ba(NO3)2 : 9 atoms
15. Li3PO4 : 4 ions
Ba(NO3)2 : 3 ions
16. D. SnO2
17. MgI2
Al(NO3)3
CuCO3
Ba(C2H3O2)2
magnesium iodide
aluminum nitrate
copper(II) carbonate
barium acetate
18. copper(I) oxide
potassium phosphate
calcium hydroxide
aluminum sulfate
19.
[ ]-
Cu2O
K3PO4
Ca(OH)2
Al2(SO4)3
Fe2O3
NH4Br
KHCO3
SnCl4
iron(III) oxide
ammonium bromide
potassium bicarbonate
tin(IV) chloride
ammonium nitrate
iron(III) sulfide
lead(II) iodide
nickel(II) bromide
NH4NO3
Fe2S3
PbI2
NiBr2
[K]+
[K]+
20. A. 1–
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