Name______________________________
Date________________________
Period________
CHAPTER 7 – CHEMICAL FORMULAS AND BONDING
IONIC COMPOUNDS
1.
What are the two types of bonds that will be discussed in this chapter?
2.
How do ionic bonds form?
3.
What do you call the positive ions?
4.
Quickly list a few properties of ionic compounds.
5.
We covered the octet rule in the last chapter, in your own words restate the octet rule.
6.
Besides cations and anions, there are 2 general types of ions listed in the book, list them and define them.
What do you call the negatives?
a.
7.
b.
What are the transition metals?
8.
What are the post-transition metals?
9.
Why do transition and post-transition metals have roman numerals after their names?
10.
In a chemical name how would you distinguish a Cu+ from a Cu+2?
11.
In this chapter you will not have to memorize the names and charges of any polyatomic ions (except hydroxide),
where can you find the names and charges of most of them? What is hydroxide?
12.
Looking at the chart on page 232, when fluorine becomes its most common ion (F -) is no longer called fluorine it is
now called fluor____. Therefore, when atoms become anions, you drop the ____ off the end and add _____.
13.
What is a binary ionic compound?
14.
How do you name binary ionic compounds?
15.
All ionic compounds are electrically _________________.
16.
How can the question above be true when ionic compounds consist completely of charged particles?
17.
What is the criss-cross method of writing chemical formulas?
18.
Use the criss-cross method of writing formulas for aluminum +3 ions and oxygen -2 ions.
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19.
Try the criss-cross method on sodium +1 ions and sulfur -2 ions.
20.
Try the criss-cross method on calcium +2 and phosphorous -3.
21.
Use the Preiodic Table to determine charges and then find the formula of the compound of lithium and nitrogen.
22.
Find the formula of the compound of barium and selenium.
23.
Find the formula of the compound of aluminum and bromine.
24.
Find the formula of the compound of magnesium and chlorine.
25.
Find the formula of the compound of iron forming a +2 ion and fluorine.
26.
Find the formula of the compound of titanium forming a +4 ion and nitrogen.
27.
Find the formula of the compound of nickel forming a +3 ion and chlorine.
28.
Find the formula of the compound of sodium and nitrate (NO3-).
29.
Find the formula of the compound of calcium and sulfate (SO42-).
30.
Find the formula of the compound of aluminum and carbonate (CO32-).
31.
Find the formula of the compound of ammonium (NH4+) and chlorate (ClO3-).
32.
Find the formula of the compound of copper forming a +2 ion and and chlorate (ClO3-).
33.
Find the formula of the compound of lithium and nitrate (NO3-).
34.
Find the formula of the compound of magnesium and phosphate (PO43-).
a.
Why does the phosphate compound need parentheses and the nitrate compound doesn’t?
b.
How many of each atom are there in the correct chemical formula of the compound formed?
35.
What number is not included in chemical formulas?
36.
How should Mg2O2 be written? Why?
37.
What is the definition of a hydrate?
38.
What is the name of something opposite of a hydrate?
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Jill was handed an assortment of index cards. Each index card had the chemical symbol for an ion written on it, as
shown below.
39.
40.
41.
42.
Jill formed ionic compounds using the index cards. She combined sodium and zinc
to form the compound Na2Zn. Is this a possible ionic compound? Why or why
not?
Jill then wrote the formulas for all the possible compounds that sodium could form
with the other ions. What formulas did she write?
PO4-3
Which monatomic ions in the cards to the right underwent oxidation to become the
ions listed on the cards? Which ones underwent reduction?
Zn
Jill also wrote formulas for the ionic compounds listed below. Identify whether
each formula is correct or incorrect. If the formula is incorrect, change it to make it
correct.
Al
a.
ZnCl3
b.
Al3O2
c.
Ca3(PO4)2
+2
Na
Ni
Reduction
Is
Gain (of e-)
+3
O-2
Losing
Electrons =
Oxidation
says
Gaining
Electrons =
Reduction
43.
To make salt (sodium chloride), we can take sodium metal (or a bunch of sodium atoms) and react them with a bunch
of chlorine molecules (chorine gas is 2 chlorine atoms stuck together, Cl2). Try to write the reaction for what is
happening.
44.
What is the difference between the sodium atoms on the left side of the equation versus the sodium atoms on the
right side in terms of charge? What’s the difference between the chlorines?
45.
If atoms lose electrons we say they are oxidized, if atoms gain electrons, they are reduced. So based on your answer
to the question above, did sodium undergo oxidation or reduction. What happened to chlorine?
46.
When your car rusts, the steel (which is mostly iron) reacts with oxygen from the air to form iron (III) oxide. Write
the chemical equation for this.
47.
Which element from the above reaction was oxidized? Which one underwent reduction?
Last Updated: 12/6/11
+2
Cl-
OXIDATION/REDUCTION (FROM ANOTHER CHAPTER)
Oxidation
Is
Loss (of e-)
+
Page 3/11
COVALENT COMPOUNDS
48.
In an ionic bond electrons are ______________________.
49.
In a covalent bond electrons are _______________________.
50.
A group of atoms is stuck together by a covalent bond is called a _________________________.
51.
To describe the composition of a molecular compound, chemists often use a _________________ formula.
52.
How does the above formula differ from an empirical formula?
53.
Explain how the octet rule helps explain why covalent bonds occur.
54.
Explain why ionic compounds are solids at room temperature, while covalent compounds are often gases or liquids?
55.
Why are covalently bonded molecular compounds never conductve?
56.
Study the flowcharts on the back of this page; ask the teacher any questions on any of the meanings.
COVALENT VS. IONIC COMPOUNDS
57.
You are on the planet Pluto and fall into a pool of liquid. Is the liquid probably an ionic or covalently bonded
compound? EXPLAIN.
58.
You are on the planet Mercury and find a solid hunk of rock. You try to melt it with a blow torch, but it won’t melt.
Is it probably Co(NO3)3 or C2N4O3? EXPLAIN.
59.
Contrast the typical physical states of ionic and covalent substances. Explain why they differ.
60.
You are swimming in a covalently bonded liquid substance. Lightning strikes the liquid and you get electrocuted.
What must be true about that liquid?
61.
Your friend says they are chewing a new ionically bonded chewing gum. What is wrong with that statement?
62.
Could wires be insulated with ionic compounds? Why would that be a problem if it got wet?
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NAME THESE COMPOUNDS THAT CONTAIN TRANSITION METALS (D-BLOCK METALS)
63. CuO
3rd Therefore the total charge
from the cations must be


2nd determine the Resulting
charge from all the anions
4th divide the total charge by
the number of cations


1st Determine the Charge on the
individual anion
Cu O
Cation
Anion
Name
64. Cu2O
3rd Therefore the total charge
from the cations must be


2nd determine the Resulting
charge from all the anions
4th divide the total charge by
the number of cations


1st Determine the Charge on
the individual anion
Cu2 O
Cation
Anion
Name
65. Cu2O3
3rd Therefore the total charge
from the cations must be


2nd determine the Resulting
charge from all the anions
4th divide the total charge by
the number ofcations


1st Determine the Charge on
the individual anions
Cu2 O3
Cation
Anion
Name
66. MnO2
3rd Therefore the total charge
from the cations must be


2nd determine the Resulting
charge from all the anions
4th divide the total charge by
the number of cations


1st Determine the Charge on
the individual anions
Mn O2
Cation
Anion
Name
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7-1 IONIC BONDING (WRITE THE CORRECT FORMULA FOR EACH OF THE FOLLOWING IONIC COMPOUNDS LISTED BELOW.)
Compound Name
Formula
Compound Name
nickel(II) nitride
67.
lithium nitride
68.
69.
lithium nitrite
70.
Nickel(II) nitrite
71.
lithium nitrate
72.
nickel(II) nitrate
ammonium chloride
74.
zinc(II) chloride
73.
(the only positive polyatomic ion)
(Roman numeral indicates the charge on the element)
75.
magnesium chlorite
76.
barium chloride
77.
magnesium chlorate
78.
silver(I) bromate
magnesium hydroxide
80.
gold(III) bromide
79.
(one of 2 polyatomic ions that end in –ide)
81.
iron(III) sulfite
82.
lithium bromide
83.
iron(III) sulfate
84.
potassium iodide
85.
chromium(III) sulfide
86.
copper(II) iodide
87.
magnesium phosphate
88.
potassium Iodate
magnesium hydrogen phosphate
90.
ammonium carbonate
92.
lithium acetate
89.
hydrogen phosphate is on the back of the PT
Formula
91.
magnesium dihydrogen phosphate
93.
Sodium bisulfate
94.
strontium thiocyanate
95.
calcium bicarbonate
96.
tin(IV) oxide
97.
sodium acetate
98.
99.
cobalt(II) fluoride
100.
sodium hypochlorite
101.
sodium phosphide
102.
calcium chromate
103.
potassium permanganate
104.
osmium (III) dichromate
105.
copper(II) sulfate pentahydrate
106.
barium hydroxide octahydrate
107.
Nickel (II) chloride hexahydrate
dihydrogen phosphate is on the back of the PT
(penta = 5, hydrate = H2O)
Last Updated: 12/6/11
CuSO4 • 5H2O
hydrogen cyanide
(one of 2 polyatomic ions that end in –ide)
108.
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7 –3 WRITE THE NAMES &/OR FORMULAS FOR EACH OF THE FOLLOWING
Ionic Compound Name
Formula
Compound Name
Formula
109.
FeCl
110.
CaS
111.
FeCl2
112.
CaSO3
113.
FeCl3
114.
CaSO4
115.
Fe2O
116.
NaClO
117.
FeO
118.
Na2CO3 • H2O
119.
Fe2O3
120.
CuSO4 • 5 H2O
121.
FeO2
122.
Na2CO3
123.
KOH
124.
BaF2
125.
LiI
126.
Cu(NO3)2
127.
AlF3
128.
AgI
129.
Iron(II) chloride
130.
Nickel(II) sulfate
131.
Magnesium oxide
132.
Zinc(II) phosphate
133.
Cobalt(II) nitrate
134.
Sodium nitride
135.
Magnesium sulfate
136.
Copper(I) carbonate
137.
Ammonium chloride
138.
Ammonium sulfate
139.
Chromium(III) phosphate
140.
Sodium Hypochlorite
141.
Barium hydroxide
142.
Magnesium sulfate heptahydrate
143.
Lead(II) sulfide
144.
Calcium sulfate dihydrate
Covalently Bonded Molecular Compounds
145.
CO
146.
ClO2
147.
CO2
148.
P4S3
149.
C2O
150.
NO
151.
C2O2
152.
SF4
153.
SiO2
154.
XeF4
155.
PCl3
156.
SbF5
157.
Silicon tetrafluoride
158.
Nitrogen trihydride (ammonia)
159.
Dinitrogen monoxide
160.
Sulfur dioxide
161.
Sulfur trioxide
162.
Dihydrogen monoxide (water)
163.
Dinitrogen pentoxide
164.
Carbon disulfide
165.
Iodine pentafluoride
166.
Carbon tetraiodide
167.
Sulfur hexafluoride
168.
Boron trichloride
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Fill in the following table of mixed IONIC and COVALENT compounds.
Compound Name
Formula
Compound Name
169.
Co2O3
170.
Mercury(I) chloride
171.
KMnO4
172.
Sodium hydride
173.
Calcium sulfide
177.
Copper(I) oxide
Rb2O
179.
181.
K2SO3
174.
Cl2O7
175.
Phosphorous trichloride
176.
Lithium sulfate
178.
Nitrogen trichloride
180.
Sodium hydroxide
SnF2
182.
183.
BaSO3
184.
Lead (IV) oxide
185.
NH4NO3
186.
Silver(I) cyanide
187.
Ru(NO3)3
188.
189.
Cesium bromide
190.
191.
Chlorine trifluoride
192.
193.
Chromium (III) carbonate
194.
Last Updated: 12/6/11
Formula
(NH4)(HSO4)
Cobalt(II) perchlorate
ClO7
Dihydrogen monoxide
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DETERMINING THE # OF ATOMS
For the following indicate the # of atoms represented.
195. 1 molecule of magnesium hydroxide
Mg
O
H
O
H
S
O
S
O
196. 2 molecules of magnesium hydroxide
Mg
197. 1 molecule of aluminum sulfate
Al
198. 5 molecules of aluminum sulfate
Al
199. 1 molecule of dinitrogen tetraoxide
N
O
200. 3molecules of dinitrogen tetraoxide
N
S
201. Al2O3
Al
O
Al
O
202. 2 Al2O3
203. CaCO3
Ca
C
O
Ca
C
O
Al
C
O
Al
C
O
C
H
O
C
H
O
204. 3 CaCO3
205. Al2(CO3)3
206. 2 Al2(CO3)3
207. C2H4O2
208. 4 C2H4O2
Last Updated: 12/6/11
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DETERMINING NAMES FROM FORMULAS
DETERMINE BOND TYPE
- If metal or ammonium present, then ionic
- Otherwise, Covalent
IONIC: Is the cation a transition
COVALENT: Is there
or post-transition metal?
more than 1 of the 1st
element?
YES: Determine the
charge
by
charge
balance from the anion,
then write the name
followed
by
roman
numerals indicating the
charge.
NO: Write the
name of the
element
or
ammonium.
Is it bound to a single
atom or polyatomic ion?
SINGLE ATOM: Use
the root & add –ide to
the end.
POLYATOMIC: Write the full
name of the polyatomic ion.
YES: Determine the
prefix & write the
name of the element.
NO: Just write
the name of the
element.
Write the root of the 2nd followed
by –ide & any necessary prefixes.
NUMERICAL
PREFIXES
1
mono2
di3
tri4
tetra5
penta6
hexa7
hepta8
octa9
nona10
deca-
For practice, go to http://chemistry2.csudh.edu/homeworkn7/hwintrocsn7.html
& click on “Nomenclature”, & then on “(161) Names to Formulas”
or on “(160) Formulas to Names”
or click on “Stoichiometry”, & then on “(130) Balancing Equations”
Last Updated: 12/6/11
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DETERMINING FORMULAS FROM NAMES
Determine Bond Type
- If a metal or ammonium present, then ionic - Otherwise, covalent -
IONIC: Is the cation a
COVALENT:
transition or post-transition metal?
YES, TRANSITION OR
POST-TRANSITION:
Write the symbol from
the Per. Table & the
charge from the name
(roman numeral in
parenthesis).
NO,
AMMONIUM:
Write NH4+.
NO: Elements,
Write the element
symbol & charge
obtained from the
Per Table.
Is the anion a single type of non-metallic
element (ends in –ide except for hydroxide
& cyanide) or a polyatomic ion (ends in –
ate or –ite)?
SINGLE ELEMENT:
Write down the element
symbol & its ionic
charge from the
periodic.
POLYATOMIC:
Remember or look up the
formula & charge for the
polyatomic ion and write
it down.
Do the charges cancel each other out?
YES:
Just erase all the
charges and leave
the elements written
the way they are
Last Updated: 12/6/11
Find the non-metallic elements’
symbols from the periodic table.
Note the 2nd elements’ name will
have been modified with –ide at the
end.
NO:
Use charge balance (criss-cross rule) to
determine the quantities of cations & anions
present in the formula. Reduce as necessary.
If >1 polyatomic ion required, put
parenthesis around the polyatomic ion
formula & charge, and put the subscript
outside the parenthesis.
Write the formula
using the symbols
and appropriate
subscripts based on
the prefixes from the
name.
NOTE – no prefix
means 1 of that
element.
NUMERICAL
PREFIXES
1
mono2
di3
tri4
tetra5
penta6
hexa7
hepta8
octa9
nona10
deca-
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