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1
Molecules and Compounds
Read Chapter 3.
Study all examples and complete all
exercises.Complete all bold numberedproblems.
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2
Chapter 3 Outline
Molecular Formula
Molar Mass
Empirical and MolecularFormula
Nomenclature
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3
Compounds & Molecules
NaCl,salt
Buckyball, C60
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4
Compounds & Molecules
COMPOUNDS are a combination of 2 ormore elements in definite ratios by mass.
The character of each element is lost when
forming a compound.
MOLECULES are the smallest unit of acompound that retains the characteristics of
the compound.
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5
MOLECULAR FORMULAS
Formula for glycine isC2H5NO2 In one molecule there are
2 C atoms
5 Hatoms
1 Natom
2 Oatoms
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6
WRITING FORMULAS
Formula
HOCH2CH2OH
to show atom ordering
or in the form of a structural formula
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7
Molecular Modeling
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8
Molecular Modeling
Ball & stick Space-filling
Drawing of glycineC
H
H C
H
H
O
OHN
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9
Resources for
Molecular Modeling Oxford Molecular/CAChe Scientific
software on Saunders GeneralChemistry CD-ROM
Rasmol and Chime on the Internet See http://www.saundercollege.com
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10
ELEMENTS THAT EXIST
AS MOLECULESAllotrope ofC
Buckyball, C60
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11
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12
IONS AND IONIC COMPOUNDS
IONS are atoms or groups of atomswith a positive or negative charge.
Taking away an electron from an atom
gives a CATION with a positive
charge.
Adding an electron to an atom gives an
ANION with a negative charge.
F ti f
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13Formation ofCations & Anions
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14
Formation ofCations & Anions
A cation formswhen an atom
loses one or
more electrons.
An anion formswhen an atom
gains one or
more electrons
Mg --> Mg2+ + 2 e- F + e- --> F-
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15
PREDICTING ION CHARGES
In general
metals (Mg) lose electrons ---> cations
nonmetals (F) gain electrons ---> anions
Li1+ F1- LiF
MONATOMIC IONS
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16
Figure 3.7
Sn4+ Pb4+Also
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17
METALS
M ---> n e- + Mn+
where n = periodic group
Na+
Mg2+
Al3+
Transition metals --> M2+ or M3+
are most common
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18
NONMETALS
NONMETAL + n e- ------> Xn-
where n = 8 - Group number
C4- carbideN3- nitride
O2- oxide
F- fluoride
Bromine
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19
Groups of atoms with a charge.
(See back of periodic chart)
POLYATOMIC IONS
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20
Some Common
Polyatomic Ions
HNO3nitric acid
NO3
-
nitrate ion
21
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21
Some Common
Polyatomic IonsNH4
+
ammonium ion
One of the few commonpolyatomic cations
22S C
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22Some CommonPolyatomic Ions
CO32-
carbonate ion
HCO3-
bicarbonate ion
hydrogencarbonate
23
S C
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23
Some CommonPolyatomic Ions
PO43-
phosphate ion
CH3CO2-
acetate ion
24S C
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24
SO42-
Sulfate ion
SO32-
Sulfite ion
Some CommonPolyatomic Ions
25
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25
NO3-
Nitrate ion
NO2-
Nitrite ion
Some CommonPolyatomic Ions
26
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26
COMPOUNDS FORMED FROMIONS
CATION + ANIONCOMPOUND
Na+ + Cl- NaCl
A neutral compound requires equal
number of + and - charges.
27
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27
IONIC COMPOUNDS
NH4+
Cl-
ammonium chloride,NH4Cl
28
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28
Some Ionic Compounds
Ca2+ + 2 F- CaF2Calcium fluoride
Mg2+ + 2 NO3- Mg(NO3)2
Magnesiumnitrate
3 Fe2+ + 2 PO43- Fe3(PO4)2
Iron(II) phosphate
Calcium Fluoride
29
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29
Sample Questions Predict the charges for the ions formed
from:Se Ga
P Sr
Give the formula for each ion in Al2(SO4)3 Give the formula for the ionic compound
that forms between
Na and S
Ga and O
Ba and N
Answers
30
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30
Properties of Ionic CompoundsForming NaCl from Na and Cl2
A metal atom cantransfer anelectron to a
nonmetal. The resulting
cation and anionare attracted toeach other by
electrostatic
forces.
30
31
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31
Electrostatic Forces
The oppositely charged ions in ionic
compounds are attracted to one another by
ELECTROSTATIC FORCES.These forces are governed by
COULOMBS LAW.
32
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32
Electrostatic Forces
COULOMBS LAW
As ion charge increases, the attractiveforce _______________.
As the distance between ions increases,
the attractive force ________________.This idea is important and will come
up many times in futurediscussions!
Force of attraction=(charge on+)(charge on-)
(distance between ions)2
33
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33
Importance of Coulombs Law
NaCl,Na+and Cl-,
m.p. 801 oC
MgO,Mg2+andO2-
m.p. 2800 oC
AlN, Al3+
and N3-
m.p. 2900o
C
34
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34
Names of Compounds
Rules for nomenclature arefound in section 3.5
STUDY them carefully!! We will be studying
nomenclature in the
laboratory in Experiment MA.
35
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35
Counting Atoms
Mg burns in air (O2) to
produce whitemagnesium oxide,MgO.
How can we figure outhow much oxide isproduced from agiven mass ofMg?
36
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36
Counting Atoms
Chemistry is a quantitative science
we need a counting unit.
The MOLE 1 mole is the amount of substance
that contains as many particles
(atoms, molecules) as there are in12.0 g of12C.
37
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37
Particles in a Mole
6.02 x 1023
Avogadros Number
Amedeo Avogadro
1776-1856
There is Avogadros number of
particles in a mole of any substance.
38
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38
Molein Chemistry is NOT:
An informer / spy
Dark spot on Cindy Crawfords upper lip
Rodent that burrows in the ground
A tunneling machine
Wave break
Spicy Mexican sauce
39
A l i i t
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39
A mole is a convenientmeasuring tool.
Pair Dozen Ream
Baseballs 2 baseballs 12 baseballs 13 baseballs500
baseballs
Pineapples2
Pineapples
12
Pineapples13 Pineapples
500
Pineapples
Calculators2
Calculators
12
Calculators 13 Calculators500
Calculators
Planets 2 Planets 12 Planets 13 Planets 500 Planets
Bakers Dozen
40
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0
Mole = mol =6.022 1023particles
Mole
Baseballs 6.022 1023 baseballs
Pineapples 6.022 1023 Pineapples
Calculators 6.022 1023 Calculators
Planets 6.022 1023 Planets
41
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Just as
1 doz eggs = 12 eggsor
1 mol of eggs = 6.022 1023 eggs
A mole is a Number
1 mol of H = 6.022 1023 atoms of H
1 mol of O = 6.022
1023
atoms of O1 mol of Al = 6.022 1023 atoms of Al
1 mol of Cr = 6.022 1023 atoms of Cr
42
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In chemistry, the mol is
more then just a number1 mol amu = 1.00 g
12 2411 1.661 1012
amu mass C g
43
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1 mol amu = 1.00 g
Proof:
1 mol = 6.022 1023
amu = 1.661
10-24
g
1 mol amu = (6.022 1023) (1.661 10-24g)= 1.00 g
44
M l M
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Molar Mass1 mol of12C
= 12.00 g of C= 6.02 x 1023 atoms
of C
12.00 g of12C is its
MOLAR MASS
Taking into account allof the isotopes of C,
the molar mass of C is12.011 g/mol
45
Molar Mass
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Molar Mass1 mol of12C = 12.00 g of C
= 6.02 x 1023
atoms of C12.00 g of12C is its MOLAR MASS
Taking into account all of the isotopes of
C, the molar mass of C is 12.011 g/mol
Find molar
mass fromperiodic
table
13
Al
26.9815
atomic number
symbol
atomic weight
46
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PROBLEM: How many molesare represented by 0.200 g ofMg?
How many atoms in this piece of Mg?
0.200 g
=
1 mole
24.3 g
0.00823 mole
0.00823 mole
=
6.02 x 1023 atom
1 mole
4.95 x 1021 atom
47
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MOLECULAR WEIGHTAND MOLAR MASS
Molecular weight is the sum
of the atomic weights of all atoms
in the molecule.
Molar mass = molecular weight
in grams
48
f
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What is the molar mass ofethanol, C2H6O?
1 mol contains
2 mol C (12.0 g C/1 mol) = 24.0 g C
6 mol H (1.0 g H/1 mol) = 6.0 g H
1 mol O (16.0 g O/1 mol) = 16.0 g O
TOTAL = molar mass = 46.0 g/mol
49
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Formula =C8H9NO2
Molar mass = 151.0 g/mol
Tylenol
50
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How many moles of alcohol arethere in a standard can of beer if
there are 21.3 g of C2H6O?
21.3 g=
1 mole
46.0 g0.463 mole
51
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How many molecules of alcoholare there in a standard can of
beer if there are 21.3 g of C2H6O?
0.463 mole
=
6.02 x 1023
molecule1 mole
2.79 x 1023 molecule
52
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How many atoms of C are therein a standard can of beer if
there are 21.3 g of C2H6O?
2.79 x 1023
molecule
=
2 atom C1 molecule
5.58 x 1023 atom C
Sample problems
53
Empirical and Molecular
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Empirical and MolecularFormulas
A pure compound always consists of thesame elements combined in the sameproportions by weight.
Therefore, we can express molecular
composition as PERCENT BYWEIGHT
Ethanol, C2H6O
52.2% C, 13% H,
34.8% O
54
Percent Composition
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Percent CompositionConsider some of the family of
nitrogen-oxygen compounds:NO2, nitrogen dioxide and closely
related, NO, nitrogen monoxide
(or nitric oxide)
Structure ofNO2 Chemistry of NO, nitrogen
monoxide (nitric oxide)
55
Percen
t Composition
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Percent CompositionConsider NO2, Molar mass = ?
What is the weight percent of N and of O?
Wt.%O =2(16.0g O per mole)46.0g
x 100%=69.6%
Wt.% N =14.0 g N
46.0 g NO2100% =30.4 %
56
Percen
t Composition
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Percent CompositionWhat are the weight percentages of N
and O in NO?
Wt. %O =16.0 g O
30.0 g NO100%=53.3%
Wt.% N =14.0 g N
30.0 g NO 100% = 46.7 %
57
Percent Composition
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Percent CompositionSamples Problems
1. Calculate the percent composition of H2O.
Wt. %O= 16.0g O
18.0 g H2O
100%= 88.9%
Wt.% H =2.0 g H
18.0 g H2O 100% = 11 %
58
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Percent CompositionSamples Problems
2. Calculate the percent O in NaOH.
Wt. %O 16.0g O
40.0 g NaOH100%40.0%
59
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Percent CompositionSamples Problems
3. Calculate the percent O and the
percent water in CuSO4.5H2O.
Wt. %O = 144.0g O249.6 g CuSO4 5H2O
100%= 57.69%
Wt. %H2O =90.0 g H2O
249.6 g CuSO4.5H2O
100%=36.1%
60
D t i i
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Determining
FormulasIn chemical analysis we determine
the % by weight of each element in agiven amount of pure compound and
derive theEMPIRICALor
SIMPLESTformula.
61
A compound of B and H is
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A compound of B and H is81.10% B. What is its empiricalformula?
81.10 g 1 mole
10.8 g
18.90 g 1 mole
1.0 g
B H
1.00 mole B 2.5 mole H
7.51 mole B 19 mole H
7.51 mole B 7.51 mole B
2.00 mole B 5.0 mole H
B2H
5
62
A compound of B and H is 81 10% B
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A compound of B and H is 81.10% B.
Its empirical formula is B2H5. What is
its molecular formula?Is the molecular formula B2H5, B4H10,
B6H15, B8H20, etc.?
B2
H6
is one example of this class of compounds.
B2H6
63A compound of B and H is 81.10% B.
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A compound of B and H is 81.10% B.Its empirical formula is B2H5. What isits molecular formula?
We need to do an EXPERIMENT to find theMOLAR MASS.
Here experiment gives 53.3 g/mol.
Compare with the mass of B2H5 , 26.66 g/unit
Find the ratio of these masses.
mol1
HBofunits2=HBofg/unit26.66
g/mol3.5352
52
Molecular formula = B4H
10
64
Determine the formula of a
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Determine the formula of acompound of Sn and I using
the following data. Reaction of Sn and I2 is done using
excess Sn.
Mass of Sn in the beginning = 1.056 g
Mass of iodine (I2) used
= 1.947 g
Mass of Sn remaining
= 0.601 g
65
Ti d I di
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Find the mass of Sn that combined
with 1.947 g I2.
Mass of Sn initially = 1.056 g
Mass of Sn recovered = 0.601 g
Mass of Sn used = 0.455 g
Tin and IodineCompound
66
Tin and Iodine
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0.455 g 1 mole
118.7 g
1.947 g 1 mole
126.9 g
Sn I
1.00 mole Sn 4.01 mole I
0.0383 mole Sn 0.1534 mole I
0.0383 mole Sn 0.0383 mole Sn
SnI4
Tin and IodineCompound
67
More Problems
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More Problems2. Calculate the formula for the iron sulfide
that forms when 53.73g Fe react with
46.27 g of sulfur.
53.73 g 1 mole
55.8 g
46.27 g 1 mole
32.1 g
Fe S
1.00 1.50
0.963 1.44
0.963 0.963
Fe2S
3
2.00 3.00
68
More Problems
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More ProblemsCalculate the empirical formula a compound
containing 90.7% Pb and 9.33% O.
90.7 g 1 mole
207.2 g
9.33 g 1 mole
16.0 g
Pb O
1.00 1.33
0.438 0.583
0.438 0.438
Pb3O
4
3.00 3.99
69
More Problems
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More ProblemsCalculate the empirical formula for a
compound containing 36.5% Na, 25.4% S
and 38.1% O.
36.5 g 1 mole
23.0 g
25.4 g 1 mole
32.1 g
Na S O
2.01 1.00 3.01
Na2SO
3
38.1 g 1 mole
16.0 g
1.59 0.791 2.38
0.791 0.791 0.791
70
More Problems
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More ProblemsCalculate the empirical and molecular
formulas for nicotine, 74.0% C, 8.7% H and
17.3% N, with a molar mass of 160 g/mole.
74.0 g 1 mole
12.0 g
8.7 g 1 mole
1.0 g
C H N
4.98 7.0 1.00
17.3 g 1 mole
14.0 g
6.17 8.7 1.24
1.24 1.24 1.24
Empirical formula C5H7N
71
More Problems
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More Problems7. Calculate the empirical and molecular
formulas for nicotine, 74.0% C, 8.7% H and
17.3% N, with a molar mass of 160 g/mole.
Empirical formula C5H7N
Molecular formula C10H14N2
160= 2
81
72
Practice Problems
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Practice Problems
Names/Formulas
FeO
Pb(C2H3O2)2magnesium bromide
sodium chromate
calcium phosphate
ammonium carbonate
73
Practice Problems
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Practice Problems
(NH4)2SAs2O3
SO2silicon disulfide
As2S
5
dinitrogenmonoxide
74
Practice Problems
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Practice Problems
As2S3
dinitrogenpentoxide
silicon tetrabromidediphosphorus pentoxide
HBrO3
H3PO4(aq)
H2CO3
75
Practice Problems
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Practice Problems
Calculations
1. 26 g H2 is how many moles H2?
2. 4.25 x 1021 molecules NH3 is howmany grams NH3?
3. 1.5 x 102 formula units KClO3 is howmany moles KClO3
4. 0.0042 mole Fe2O3 is how manyformula units Fe
2
O3
?
5. 2.15 moles MgSO4.7H2O is how many g
MgSO4.7H2O?
76
Practice Problems
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Practice Problems
6. 25 molecules HBr is how many moleHBr?
7. .00002 g Sn is how many atoms Sn?
8. 7.25 mole H2S is how many g H2S?
9. 5.2 g Sr(OH)2is how many formulaunits Sr(OH)2?
10. How many moles of CCl4 will contain2.4 g of chlorine?
77
Practice Problems
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Practice Problems
11. 19 g of HNO3 contains howmany
a) molecules of HNO3? b) grams ofO?
12. Calculate the percentcomposition of NaCl.
13. Calculate the empirical and
molecular formulas for acompound containing 43.7g P and56.3g O, with a molar mass of 140g/mole.
78
Practice Problems Answers
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Practice Problems Answers
Iron(II) oxide, ferrous oxide
lead(II) acetate, plumbous acetate
MgBr2 Na2CrO4 Ca3(PO4)2
(NH4)2CO3 ammonium sulfidediarsenic trioxide sulfur dioxide
SiS2 As2S5 N2O
diarsenic trisulfide N2O5 SiBr4P2O5 bromic acid phosphoric acid
carbonic acid
79
Practice Problems Answers
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Practice Problems Answers1. 13 mole 2. 0.120 g
3. 2.5 x 10-22 mole 4. 2.5 x 1021 atom
5. 530. g 6. 4.2 x 10-23 mole
7. 1 x 1017 atom 8. 247 g
9. 2.6 x 1022 formula units
10. 0.017 mole
11. a) 1.8 x 1023 molecule
b) 14 g
12. 39.3%, 60.7% 13. C5H7N
14. P2O5
80
Sample Questions
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Sample Questions Predict the charges for the ions formed
from:
Se -2 Ga +3 Al3+
P -3 Sr +2 SO42-
Give the formula for each ion in Al2(SO4)3 Give the formula for the ionic compound
that forms between
Na and S Na2S
Ga and O Ga2O3
Ba and N Ba3N2
81
Sample Problems
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Sample Problems
1. 2.5 mole S = ? atom S2.5 mole
=
6.02 x 1023 atom
1 mole
1.5 x 1024 atom S
82
Sample Problems
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Sample Problems
2. 2.1 mole Zn = ? g Zn
2.1 mole=
65.4 g
1 mole140 g Zn
83
Sample Problems
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Sample Problems
3. 1.42 g Mg = ? atom Mg
1.42 g
=
1 mole
24.3 g
3.55 x 1022 atom
6.02 x 1023 atom
1 mole
84
Sample Problems
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Sample Problems
4. 125.2 g O2
= ? mole O2
125.2 g=
1 mole
32.0 g3.91 mole O2
85
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Sample Problems
1. 1.5 mole H2O = ? g H2O
1.5 mole=
18.0 g
1 mole27 g H20
86
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Sample Problems
2. 1.50 mole CCl4
= ? molecules CCl4
1.5 mole
=
6.02 x 1023 molecule
1 mole
9.03 x 1023 molecule
87
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Sample Problems
3. 1.25 mole CaCl2
= ? formula units CaCl2
1.25 mole
=
6.02 x 1023 formula unit
1 mole
7.52 x 1023 formula unit
88
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Sample Problems
4. 2.5 g K = ? g KOH
2.5 g K
=
1 mole K
39.1 g K
3.6 g KOH
1 mole KOH
1 mole K
56.1 g KOH
1 mole KOH
89
Sample Problems
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Sample Problems
5. 34.5 g CaCO3
= ? g O
34.5gCaCO3
=
1 moleCaCO3
100.1gCaCO3
16.5 g O
3 moleO
1 moleCaCO3
16.0 gO
1 moleO