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Unit 2:Matter and Energy
HonorsChemistry
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Guiding Questions
Why do substances boil or freeze at different temperatures? Why do we put salt on the roads in the winter?
Why does sweating cool us?
What is energy?
How do we measure energy?
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units: L, dm3, mL, cm3
Matter Introductory Definitions (…pull out your vocab!)
matter: anything having mass and volume
mass:
weight:
volume:
L3state of matter:
the amount of matter in an object
the pull of gravity on an object
the space an object occupies
solid, liquid, or gas
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Solid, Liquid, Gas
(a) Particles in solid (b) Particles in liquid (c) Particles in gas
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composition:
copper: water:
properties:
atom: a basic building block of matter
what the matter is made of
many Cu atoms many groups of2 H’s and 1 O
describes matter
what it looks like, smells like, etc.
how it behaves
~100 diff. kinds
Qualitative observations
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Lr103
No102
Md101
Fm100
Es99
Cf98
Bk97
Cm96
Am95
Pu94
Np93
U92
Pa91
Th90
Lu71
Tm69
Yb70
Er68
Ho67
Dy66
Tb65
Gd64
Eu63
Sm62
Pm61
Nd60
Pr59
Ce58
He2
Ne10
Ar18
Kr36
Xe54
Rn86
At85
I53
Br35
Cl17
F9
Po84
Te52
Se34
O8
Bi83
Sb51
As33
N7
Pb82
Tc43
Ta73
Hg80
Mt109
Hs108
Bh107
Sg106
Db105
Rf104
Ac89
La57
Hf72
W74
Re75
Os76
Ir77
Rh45
Ru44
Mo42
Nb41
V23
Li3
Fr87
Cs55
H 1
Na11
K19
Rb37
Mn25
Co27
Pd46
Au79
Cd48
Zn30
Cu29
C6
B5
Al13
S16
P15
Si14
Ge32
Sn50
Ag47
Pt78
= Internet link( )
Fe26
Ni28
Cr24
Ti22
Sc21
Zr41
Y39
Ga31
In49
Tl81
Mg12
Ca20
Sr38
Ba56
Ra88
Be4
Select an element
Other Physical DATA
The Periodic Table of Elements
Rg111
Ds110
Cp112
Uut113
Fl114
Uup115
Lv116
Uus117
Uuo118
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Elements contain only one type of atom
1. monatomic elements consist of unbonded, “like” atoms
e.g.,
2. polyatomic elements consist of several “like” atoms bonded together
diatomic elements:
Fe, Al, Cu, He
H2 O2 Br2 F2 I2 N2 Cl2
“HOBrFINCl = Hoberfinckle” “BrINClHOF = Brinklehoff”
others: P4 or S8
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Diatomic Elements, 1 and 7H2
N2 O2 F2
Cl2
Br2
I2
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allotropes: different forms of the same element inthe same state of matter
OXYGEN CARBON
oxygen gas
ozone
elementalcarbon graphite
diamond buckyball
(O2)
(O3)
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Allotropes of Carbon
Graphite
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Allotropes of Carbon
C60 & C70
“Buckyballs”“Buckytubes”
BuckminsterfullereneBuckminster Fuller was known for designing geodesic domes, like Epcot Center
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Allotropes of Carbon
Carbon nanotubes
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Allotropes of Carbon
GrapheneSuper strong and super conductive
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molecule: a neutral group of bonded atoms
Description Chemical Symbol Model
1 oxygen atom
1 oxygen molecule
2 unbonded oxygen atoms
1 phosphorus atom
1 phosphorus molecule
4 unbonded phosphorus
atoms
O
O2
2 O
P
P4
Elements may consist of either molecules or unbonded atoms
4 P
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Compounds
…contain two or more different types of atoms…have properties that are different from those of their constituent elements
Na (sodium):
Cl2 (chlorine):
explodes in water
poisonous gas
table salt (NaCl)
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Atoms can be altered onlyby _______ means
Molecules can be alteredby ________ means
(i.e., chemical reactions)
nuclear
chemical
e.g., Dehydration of sugar
C12H22O11(s) 12 C(s) + 11 H2O(g)
Electrolysis of water
2 H2O(l) 2 H2(g) + O2(g)
Atomic blast at Hiroshima
U
BaKr
neutron“bullet”
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Classifying Matter
(Pure) Substances …have a fixed composition
…have fixed properties
ELEMENTS COMPOUNDS
e.g., e.g., Fe, N2, S8, U H2O, NaCl, HNO3
Pure substances have a chemical formula
sulfur (S8) sodium chloride (NaCl)
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Mixtures two or more substances mixed together
…have varying composition
…have varying properties
The substances are NOT chemically bonded,and they… retain their individual properties
Tea, orangejuice, oceans,and air are all
mixtures
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Two Types of Mixtures
1. homogeneous: (or solution) particles are microscopic; sample has the samecomposition and properties throughout;evenly mixed
e.g.,
alloy: a homogeneous mixture of metals
e.g.,
Kool Aid
bronze (Cu + Sn) brass (Cu + Zn) pewter (Pb + Sn)
salt water
Oh Yeah!
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Two Types of Mixtures (cont.)2. heterogeneous:
different composition and properties in thesame sample; unevenly mixed
e.g.,
suspension: settles over time
e.g.,
tossed salad
raisin bran
paint snowy-bulb gifts
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MATTER
Chart for Classifying Matter
PURE SUBSTANCE MIXTURE
ELEMENT COMPOUND
HOMOGENEOUS
HETEROGENEOUS
Has a chemical formula Has NO chemical formula
Made of 1 element Made of 2 or more different elements
Unevenly mixed
Uniform or evenly mixed throughout (a solution)
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Alike DifferentDifferent
Topic Topic
Double Bubble Mind Map
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Mixture vs. Compound
Mixture
FixedComposition
Bonds between
components
Can ONLY beseparated by
chemical means
VariableComposition
No bondsbetween
components
Can beseparated by
physical means
Alike Different
Contain two or more
elements
Can beseparated
intoelements
Involvesubstances
Compound
Different
Topic Topic
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Contrast…
24K GOLD 14K GOLD
24/24 atoms are gold
element
pure gold
14/24 atoms are goldmixture of gold & other metals
Auhomogeneous mixturee.g., Au + Cu
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Every sample of NaCl tastes the same, melts at the same temp., and is 39.3% Na and 60.7% Cl
by mass.
Compound Composition
All samples of a given compoundAlways have the same composition
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Phosgene gas (COCl2) is 12.1% carbon,16.2% oxygen, and 71.7% chlorine bymass. Find # of g of each element in254 g of COCl2.
C:
O:
Cl:
254 g (0.121) = 30.7 g C
254 g (0.162) = 41.1 g O
254 g (0.717) = 182 g Cl
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= 0.828
A sample of butane (C4H10) contains 288 g carbonand 60. g hydrogen. Find…
A. …total mass of sample
B. …% of each element in butane
C. …how many g of C and H are in a 24.2 g sample
288 g C + 60 g H
82.8% C17 % H
= 348 g
g 348
C g 288% C =
= 0.17g 348
H g 60.% H =
C:
H:
24.2 g (0.828) = 20.0 g C
24.2 g (0.17) = 4.2 g H 24.2 g
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A 550 g sample of chromium (III) oxide (Cr2O3)has 376 g Cr. How many grams of Cr and Oare in a 212 g sample of Cr2O3?
68.4% Crg 550Cr g 376
% Cr =and
31.6% O
Cr:
O:
212 g (0.684) = 145 g Cr
212 g (0.316) = 67 g O
chromium (III) oxide
100 %
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A sample of bronze contains 68 g copper and 7 g tin
A. Find total mass of sample
B. Find % Cu and % Sn
C. How many grams of each element does a 346 g sample of bronze contain?
68 g Cu + 7 g Sn = 75 g
90.7% Cug 75Cu g 68
% Cu = and 9.3% Sn
We don’t know! (Bronze is a mixture and isn’t necessarily
always 90.7% Cu and 9.3% Sn.)
However, assuming these % are correct…
Cu: 346 g (0.907) = 314 g Cu (and 32 g Sn)
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Separating Mixtures …involves physical means, or physical changes
1. sorting:
2. filter:
by color,shape,texture,etc.
particle sizeis different
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filtration in the chemistry laboratory
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filtration in the “real world”
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Separating Mixtures (cont.)
3. magnet:
4. chromatography:
one substance mustcontain iron
some substances dissolvemore easily than others
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Separating Mixtures (cont.)
5. density: “sink vs. float”
perhaps use a centrifuge
decant: to pouroff the liquid
blood after high-speed centrifuging
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Separating Mixtures (cont.) 6. distillation: different boiling points
heat source
thermometer
water in(cooler)
water out(warmer)
more-volatile substance
mixture
condenser
more-volatilesubstance, nowcondensed
(i.e., the onewith the lowerboiling point)
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No chemical reactionsare needed to separate mixtures;
substances are NOT bonded
dental amalgam
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Density how tightly packed the particles are
Density =
Typical units:
g/cm3 for solids g/mL for fluids
Vm D
volumemass m
V D
liquids and gases
Glass: liquid or solid?
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To find volume, use…
1. a formula
water displacement
V = l ∙ w ∙ hV = p ∙ r2 ∙ h
V = ?
VfinalVinitial
Vobject = Vfinal – Vinitial
2.
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** Density of water =
The density of a liquid or solid is nearly constant,no matter what the sample’s temperature
1.0 g/mL = 1.0 g/cm3
Things that are “less dense” floatin things that are “more dense.”
D < 1 g/cm3
Density of gases is highly dependent on temperature
D < 1 g/cm3D > 1 g/cm3D < 1 g/cm3
(And things that are “more dense” sinkin things that are “less dense.”
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Ironwood Trees
• Several different varieties of hardwood trees, having densities between 1.34 and 1.49 g/cm3
• Most dense species is South African Ironwood (black ironwood)• Olea laurifolia• Found in Florida and
West Indies• D = 1.49 g/cm3
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Will Bowling Balls sink or float in H2O?
21.6 cm in diameterVsphere = 4/3 p r3
V = 4/3 p (10.8 cm)3
V = 5,276.7 cm3
If DBB > 1, it will sink If DBB < 1, it will float
Since the mass of a BB varies, let’s figure out at what mass it will sink v. float
m = (1.00 g/cm3)(5276.7 cm3)
m
V D
m = 5276.7 g
m = D V
…or 11.6 lbs
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Density Calculations
1. A sample of lead (Pb) has mass 22.7 g and volume 2.0 cm3. Find sample’s density.
Vm
D 3cm 2.0g 22.7
m
V D
2. Another sample of lead occupies 16.2 cm3
of space. Find sample’s mass.
33 cm 16.2
cmg
11.35 m = D V = 180
3cmg
= 11
g
V
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3cmg
3. A 119.5 g solid cylinder has radius 1.8 cm and height 1.5 cm. Find sample’s density.
1.5 cm
1.8 cm
m
V D
m
V = p r2 h
Vm
D
= p (1.8 cm)2(1.5 cm)
= 15.268
3cm 15.268
g 119.5 = 7.8
cm3
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4. A 153 g rectangular solid has edge lengths 8.2 cm, 5.1 cm, and 4.7 cm. Will this object sink in water?
8.2 cm
5.1 cm
4.7 cm
m
V D
Vm
D
(Find the object’s density and compare it to water’s density.)
m
V = l w h
= 8.2 cm (5.1 cm)(4.7 cm)
3cmg
= 196.55
3cm 196.55
g 153 = 0.78
cm3
< 1 No; it floats.
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Galilean Thermometer ProblemOn a cold morning, a teacher walks into acold classroom and notices that all bulbsin the Galilean thermometer are huddledin a group. Where are the bulbs? At thetop of the thermometer, at the bottom or elsewhere?
1. Bulbs have essentially fixed masses
and volumes. Therefore, each bulb has a relatively fixed density. 2. The surrounding liquid has a fixed
mass, but its volume is extremely
temperature-dependent.
D1
D2
D3
D4
D5
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D1
D2
D3
D4
D5
3. The density of the liquid can be written as…
liq
liqliq V
m D so…
…if the liquid is cold: …but if it’s hot:
mliq =
On a cold morning,where are the bulbs? AT THE TOP
Vliq
mliq Dliq=
VliqDliq
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•
Osmium
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Properties of Matter
CHEMICAL properties tell how a substance reacts with other substances
PHYSICAL properties can be observed without chemically changing the substance
EXTENSIVE properties depend on the amount of substance present
INTENSIVE properties do not depend on the amount of substance
ON
E O
F T
HE
SE
AND
ON
E O
F T
HE
SE
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P,
Examples:
electrical conductivity……………………..…
reactivity with water……………………….....
heat content (total energy)………………..…
ductile: can be drawn (pulled) into wire…..
malleable: can be hammered into shape…
brittle…………………………………………….
magnetism………………………………………
C,
P,
I
I
E
P, I
P, I
P, I
P, I
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Physical and Chemical PropertiesExamples of Physical Properties
Boiling point Color Slipperiness Electrical conductivity
Melting point Taste Odor Dissolves in water
Shininess (luster) Softness Ductility Viscosity (resistance to flow)
Volatility Hardness Malleability Density (mass / volume ratio)
Examples of Chemical Properties
Burns in air Reacts with certain acids Decomposes when heated
Explodes Reacts with certain metals Reacts with certain nonmetals
Tarnishes Reacts with water Is toxic
Ralph A. Burns, Fundamentals of Chemistry 1999, page 23Chemical properties can ONLY be observed during a chemical reaction!
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The formation of a mixture
The formation of a mixture
The formation of a compound
The formation of a compoundChemical Change
Chemical Change
Physical Change
Physical Change
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Physical & Chemical Changes
Limestone,CaCO3
crushing
PHYSICALCHANGE
Crushed limestone,CaCO3
heating
CHEMICALCHANGE
Pyrex
CO2
CaO
Lime andcarbon dioxide,
CaO + CO2
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Pyrex
O2
H2O
Pyrex
H2O2
Light hastens the decomposition of hydrogen peroxide, H2O2. The dark bottle in which hydrogen peroxide is usually storedkeeps out the light, thus protecting the H2O2 from decomposition.
Sunlight energy
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States of MatterLIQUID SOLID GAS
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
( ( ) )
vibrating translating;close together
translating quickly;far apart
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Changes in State Energy put into system
Energy removed from system
LIQUID GASSOLID
freezing condensation
deposition
sublimation
boilingmelting
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Energy the ability to do work
potential energy:
kinetic energy:
--
--
e.g.,
stored energy
stored in bonds between atoms
in food,
energy of motion
wiggling, translating,and rotating of particles
-- “hot” gas particles movefaster, have more KE
gasoline, batteries
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Law of Conservation of Energy:
2 H2 + O2 2 H2O
Eafter = Ebefore
+
+ energy
+WHOOF!
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For the combustion of acetylene…
PEreactants
PEproducts
KEstopper
heat, light, sound
EN
ER
GY
CO2 + H2OC2H2 + O2
Energy is conserved.
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Energy Changes
endothermic change: system absorbs heat
exothermic change: system releases heat --
--
Choose “endo” or “exo”…
water boiling
paper burning
steam condensing
CO2 subliming
water freezing
ice melting
beaker feels cold
beaker feels hot
ENDO
EXO
EXO
ENDO
EXO
ENDO
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R
P
En
erg
y endothermic exothermic
R
P
En
erg
yACTIVATION
ENERGY
(most chemical reactions) (photosynthesis)
CO2 + H2O + sunlight C6H12O6 + O2
C + O2 CO2
Reaction Coordinate Diagrams
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The Mole
Atoms are so small, it is impossible to count them bythe dozens, thousands, or even millions.
To count atoms, we use the concept of the mole
1 mole of atoms =
That is, 1 mole of atoms = _________ atoms
The mole is the SI unitfor “amount of substance.”
602,000,000,000,000,000,000,000 atoms
6.02 x 1023
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How Big is a Mole?
…about the size of a chipmunk,weighing about 5 oz. (140 g), andhaving a length of about 7 inches (18 cm).
I Meant, “How Big is 6.02 x 1023?” BIG.6.02 x 1023 marbles would cover theentire Earth (including the oceans)
…to a height of 2 miles.
6.02 x 1023 $1 bills stacked face-to-face
…and back …7.5 million times.
(It takes light 9,500 years to travel that far)
would stretch from the Sun to Pluto
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For any element on the Periodic Table,one mole of that element
(i.e., 6.02 x 1023 atoms of that element)has a mass in grams equal to the decimal
number on the Table for that element.
He2
4.003
Ne10
20.180
Ar18
39.948
Kr36
83.80
Xe54
131.29
Rn86
(222)
1 mole of (i.e., 6.02 x 1023) helium atomshas a mass of 4.0 grams.
1 mol Ne = 20.2 g1 mol Ar = 39.9 g1 mol Kr = 83.8 g
1 mol Xe = 131.3 g
1 mol Rn = 222 g
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1 mol = 6.02 x 1023 particles
MOLE(mol)
MASS(g)
Particle(atoms)
1 mol = molar mass (in g)
Island Diagram
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Island Diagram Problems
1. How many moles is 3.79 x 1025 atoms of zinc?
= 63.0 mol Zn( )1 mol6.02 x 1023 at.
3.79 x 1025 at.
2. How many atoms is 0.68 moles of zinc?
= 4.1 x 1023 at. Zn( )1 mol6.02 x 1023 at.
0.68 mol.
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3. How many grams is 5.69 moles of uranium?
5.69 mol( )1 mol238.0 g
= 1,354 g U= 1.35 x 103 g U
4. How many grams is 2.65 x 1023 atoms of neon?
( )1 mol
= 8.9 g Ne
20.2 g( )1 mol6.02 x 1023 at.
2.65 x 1023 at.
5. How many atoms is 421 g of promethium?
421 g( )1 mol145 g ( )1 mol
6.02 x 1023 at.
= 1.75 x 1024 at. Pm