Unit 17: Review All the Things. Part I. LPChem1415 Groups of similar elements have special names:
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Transcript of Unit 17: Review All the Things. Part I. LPChem1415 Groups of similar elements have special names:
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Unit 17: ReviewAll the Things.
Part I
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LPChem1415
Groups of similar elements have special names:
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LPChem1415
# valence electrons increases, left to right:1 2 3 4 5 6 7 8
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LPChem1415
Valence Electrons & Stability
Main Group Ion Charges1+
2+ 3+4± 3- 2- 1-0
Positive charge means electrons were REMOVED. Negative charge
means electrons were ADDED.
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LPChem1415
Ionic Nomenclature: Roman NumeralsFe2 (CO3)3 = iron ( ? ) carbonate
Fe2 (CO3)3 2-
6-
( ) 3
= 06+
( )2 +3+
Iron (III) carbonate
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C. Molar Conversionsmolar mass
(formula mass)
(g/mol)
MASSIN
GRAMS
MOLESNUMBER
OFPARTICLES
Avogadro6.02 1023
(particles/mol)
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C. Molar Conversionsmolar mass
(formula mass)
mass (grams) FM
MASSIN
GRAMS
MOLESNUMBER
OFPARTICLES
Avogadro6.02 1023
Particles Avogadro= moles =
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A. Molarity 1. Concentration of a solution.
solution of literssolute of moles(M)Molarity
total combined volume
substance being dissolved
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B. Molality 1. Concentration of a solution.
solvent ofkg solute of moles(m)Molality
Mass of solvent
substance being dissolved
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What is the percent composition of Cu2S?
Copper: 2(63.55) / 159.16 =
Cu2S has a molar mass of:
A. Percentage Composition
2(63.55) + 32.06 = 159.16
0.7986 = 79.86 % Cu
Sulfur: 1(32.06) / 159.16 = 0.2014 = 20.14 % S
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C. Johannesson
B. Empirical Formula
C2H6
CH3
reduce subscripts
Smallest whole number ratio of atoms in a compound
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C. Johannesson
B. Empirical Formula1. Find mass (or %) of each element.
2. Find moles of each element.
3. Divide moles by the smallest # to find subscripts.
4. When necessary, multiply subscripts by 2, 3, or 4 to get whole #’s.
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C. Johannesson
B. Empirical Formula Find the empirical formula for a
sample of 25.9% N and 74.1% O.
25.9 g 1 mol14.01 g
= 1.85 mol N
74.1 g 1 mol16.00 g
= 4.63 mol O
1.85 mol
1.85 mol
= 1 N
= 2.5 O
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C. Johannesson
B. Empirical Formula
N1O2.5Need to make the subscripts whole
numbers multiply by 2
N2O5
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C. Johannesson
C. Molecular Formula “True Formula” - the actual number
of atoms in a compound
CH3
C2H6
empiricalformula
molecularformula
?
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C. Johannesson
C. Molecular Formula1. Find the empirical formula.2. Find the empirical formula mass.3. Divide the molecular mass by the
empirical mass.4. Multiply each subscript by the
answer from step 3.
nmass EFmass MF
nEF
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C. Molecular Formula The empirical formula for ethylene
is CH2. Find the molecular formula if the molecular mass is 28.1 g/mol?
28.1 g/mol14.03 g/mol
= 2.00
empirical mass = 14.03 g/mol
(CH2)2 C2H4
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C. Johannesson
A.Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change
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C. Johannesson
B.Law of Conservation of Mass mass is neither created nor destroyed
in a chemical reaction
4 H
2 O
4 H
2 O4 g 32 g
36 g
total mass stays the same atoms can only rearrange
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C. Johannesson
C. Chemical Equations
A+B C+DREACTANTS PRODUCTS
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C. Johannesson
Al + CuCl2 Cu + AlCl3
Al
Cu
Cl
1 1
1 1
2 3
2
3
6
3
33 2
C. Balancing ExampleAluminum and copper(II) chloride react to form copper and aluminum chloride.
2
2
6
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D. Stoichiometry Problems How many moles of KClO3 must
decompose in order to produce 9 moles of oxygen gas?
9 mol O2 2 mol KClO3
3 mol O2
= 6 mol KClO3
2KClO3 2KCl + 3O2 ? mol 9 mol
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D. Stoichiometry Problems How many grams of silver will be
formed from 12.0 g copper?
12.0g Cu
1 molCu
63.55g Cu
= 40.7 g Ag
Cu + 2AgNO3 2Ag + Cu(NO3)2
2 molAg
1 molCu
107.87g Ag
1 molAg
12.0 g ? g