Name: __________________________________ Date: ______________ Block: ______
Ionic bonding practice
How many valence electrons do each of the following elements have?
1)
2)
3)
4)
carbon
selenium
xenon
potassium
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Which of the following ions are likely to be formed? Circle one:
5) N+5
6) He+
7) F-1
yes
yes
yes
no
no
no
8) Al+2
9) P-3
10) Mg+2
yes
yes
yes
no
no
no
Write the formula which result from combining the following ions:
11) K+1 and Br-
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12) Li+1 and O-2
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13) Ca+2 and Cl-1
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14) Al+3 and S-2
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15) Fe+2 and S-2
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16) Na+1 and NO3-1
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17) Na+1 and SO4-2
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18) NH4+1 and CO3-2
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19) Fe+3 and CrO4-2
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20) Al+3 and PO4-3
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Determine the formulas and charges of the cations
and anions in the following ionic compounds.
Cation
Anion
21)
CsCl
________
________
22)
CaF2
________
________
23)
NaOH
________
________
24)
Ca(OH)2
________
________
25)
KNO3
________
________
26)
Fe(NO3)2
________
________
27)
Fe2O3
________
________
28)
Al2(SO4)3
________
________
29)
CaCO3
________
________
30)
FeO
________
________
31) For each of the following pairs of elements, use the periodic table
to decide the charge on both the cation and anion and determine the
formula of the compound(s) formed in each case. When writing the
formulas put the cation first.
Elements
Compound formula
Mg
Br
K
S
Cl
Al
S
Cu+1
Zn+2
F
O
Cu+2
Co+2
Co+3
aluminum
oxygen
calcium
iodine
32) Explain why oxygen is a fairly reactive element while neon is not.
33) Explain why beryllium loses electrons when forming ionic bonds,
while sulfur gains electrons.
34) Explain why fluorine and chlorine have similar reactive qualities (the
word “valence” should be somewhere in your answer!)