Matter Physical and Chemical Properties 1
Matter Physical and Chemical Properties 1. Matter vs. Energy The universe is made up of matter and energy. Matter: –Has mass and takes up space (volume)
Dec 25, 2015
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MatterPhysical and Chemical
Properties
1
Matter vs. Energy
• The universe is made up of matter and energy.
• Matter:– Has mass and takes up space (volume)– Is usually a “thing”
• Energy:– Does not have mass or take up space– Energy moves matter!!!!!!
• ** Energy is the ability to make things move. Light, heat, sound, motion, and electricity are all forms of energy.
2
Properties of Matter• Property -characteristic that
distinguishes one type of matter from another– Chemical– Physical
• Specific property – a property that allows for the ID of matter
• For 2 separate samples of matter to be the same kind of matter, they have to have all the same specific properties
3
Extensive/Intensive
Intensive – Does not depend on the amount of material
Examples: temperature, density, boiling point
Extensive – Depends on the amount of material
Examples: mass and volume
4
Physical Properties
• Physical property- any property of matter that can be observed or measured without changing the identity of the matter
• Examplescolor shapetaste
densitystate/phasemalleability
D = M V
5
Volume and Density
• Volume= length X width X height• Density= mass (g) volume (mL or cm3)
• 1 mL = 1 cm3
Which is more dense?6
Physical Properties• States of matter:
– Bose-Einstein
– Solid – Liquid– Gas– Plasma
(Newest State)
7
States of Matter
Solid - fixed shape and volume and particles close together so rigid structure - particles vibrate only – no movement
Liquid - fixed volume & takes shape of container - particles farther apart than solid - little order - particles can move around
Gas - takes volume and shape of container - particles are far apart - random motion of particles
Physical Properties of Fluids
• Viscosity- the resistance of a fluid to flowing.
• Viscousmaple syrup (cold especially!)
• Not viscouswater
9
Physical Properties of Solids
• Malleable- able to be hammered or pressed out of shape without breaking
• This is a property of many metals
10
Chemical Properties
• Chemical property- property of matter that describes a substance based on its ability to change into a new substance
• Examplesflammability
reactivity with vinegarreactivity with oxygenreactivity with water
Iron + Oxygen Iron oxide (rust)
2Fe + 3O2 Fe2O311
Let’s Do It!!! Label your paper 1-5Chemical or Physical Property?Chemical vs. Physical Property
video1. Paper is white
2. Boiling point of H2O is 100oC
3. Zinc reacts with hydrochloric acid and creates hydrogen gas
4. Nitrogen does not burn
5. Sulfur smells like rotten eggs
Physical Property
Physical Property
Physical Property
Chemical Property
Chemical Property
12
Reference-Comparing Physical and Chemical
PropertiesSubstance/Matter Physical Property Chemical Property
Helium Less dense than air Nonflammable
Wood Grainy texture Flammable
Baking soda White powder Reacts with vinegar to produce bubbles
Powdered sugar White powder Does not react with vinegar
Rubbing alcohol Clear liquid Flammable
Red food coloring Red color Reacts with bleach and loses color
Iron Malleable Reacts with oxygen
13
Changes in Matter
• Matter is constantly changing• There are two types of changes in
matter:– Chemical– Physical
14
Physical Changes
• Physical change- a change in shape, size, color, or state a change without a change in chemical composition– Examples
tearing paper cutting your hair change in state
• Some mixtures can be separated based on their physical properties
Physical changes are
not indicative of a chemical reaction
15
Let’s Do It!!!
• Get with a partner• Google “Harcourt Mixtures Lab”
and click on the link for “The Mixtures Lab” and read the info on the left.
• Draw the chart from the lab in your notes. You have 15 minutes
• The Mixtures Lab• Online stopwatch 16
Chemical Changes• Chemical change- a change in which a
substance becomes another substance having different properties– A change that is not reversible using
ordinary physical means – Changes that usually cause, heat, sound,
light, odor, fizzing/foaming, color changes– Examples
mixing vinegar & baking sodaburning a piece of wood
soured milk
A chemical analysis is the only 100% way to know a
chemical change has occurred.
17
Chemical Changes
• Chemical reaction- the process by which a chemical change occurs
• Types of chemical reactions– Synthesis (creating)– Decomposition (separating)– Combustion (burning)– Displacement/Replacement
(switching of atoms)
18
Chemical Changes• During chemical
changes, atoms are rearranged, and chemical bonds are broken and reformed
• One or more substances change to produce one or more different substances
O2H2
What does H2 & O2 gas
create?
19
Let’s Do It!!!!Label your paper 1-5
Chemical or Physical Change?1. Bending a Paper Clip
2. Baking a cake
3. The sublimation of carbon dioxide
4. Crushing an aluminum can
5. Vinegar and baking soda combining to create salt and water
Physical Change
Chemical Change
Chemical Change
Physical Change
Physical Change
20
Changes are either…. Endothermic – absorbing
energy • ex. boiling water
• Exothermic - releasing energy
ex. burning a candle
21
Nuclear Changes/Reactions
• A new substance is formed by changes in the atoms themselves - not just by rearranging the atoms.
22
Nuclear Reactions
• The TOTAL of mass plus energy is conserved.
• Mass + Energy of reactants =Mass + Energy of products
• Matter can change into energy and energy can change into matter.
23
Einstein’s Equation
• E = mc2
• Einstein is saying that matter and energy are different forms of the same thing!• c =(3.00 x 1010 cm/sec)2
24
How much energy can be obtained by completely converting 1.00g of
matter into energy?• E = mc2
• E = (1.00g) (3.00 x 1010 cm/sec)2
(after adjusting units)
• E = 21,500,000,000,000 calories
25
This means……
• SMALL amounts of matter convert to
LARGE amounts of energy
26
Reaction Laws
• Law of Conservation of Energy – in chemical and physical reactions, energy is conserved(not created or destroyed)
• Law of Conservation of Mass – in chemical and physical reactions, mass is conserved (not created or destroyed)
27
Law of Conservation of Mass
Chemical EquationH + O H2OReactants Products
Mass of Reactants = Mass of Products
Example: H + O H2O 5.0g + 5.0g = ?
10.0g28
ReviewChemical vs. Physical Changes
video 7 min• Number your paper from 1-5 and
answer the following questions• Which of these is a metric unit?
– A. pounds– B. cups– C. liters– D. inches
29
Review
• C• 2. Which of these is the symbol for
the metric unit micro?– A. M– B. m– C. ρ– D. μ
30
Review
• D• 3. Which of these is a physical
property?– A. density– B. reaction to water– C. combustibility
31
Review
• A• 4. Which of the following is a
chemical property? – A. reaction to acid– B. odor– C. temperature– D. color
32
Review
• A• 5. If 59 g of NaCl is produced in a
creaction, how much Cl was combined with 23 g of Na? Na + Cl NaCl– A. 36– B. 36 g– C. 79 g– D. 23 g 33
Review
• B
34
Composition of Matter• All matter has a composition, what it’s
made of• Different kinds of composition are:
– Pure substances- matter with a fixed composition that can’t be separated physically• Element • Compound
– Mixture- can be separated physically • Solutions• Colloids• Mechanical mixture 35
Classification is based on physical and chemical properties-Reference
Matter
Mixture Pure substance
Homogeneous(Solution)
Heterogeneous Element Compound
Metal Metalloid Nonmetal
Pure Substances• Element- made up of one
kind of atom and can’t be broken down intosimpler substancesby physical or chemical means
• 90 occur naturally on Earth 29 were synthesized (made) by scientists
• C, N, O, Na, H, Au (gold), etc.
118
Uuo117
Uus116Uuh(292)
115
Uup(288)
114
Uuq(289)
113
Uut(284)
112Uub(285)
111
Rg(272)
110
Ds(269)
109
Mt(268)
108
Hs(269)
107
Bh(264)
106
Sg(266)
105
Db(262)
104
Rf(261)
103
Lr(262)
88
Ra(226)
87
Fr(223)
86
Rn(222)
85
At(210)
84
Po(209)
83
Bi208.980
82
Pb207.2
81
Tl204.383
80
Hg200.59
79
Au196.967
78
Pt195.078
77
I r192.217
76
Os190.23
75
Re186.207
74
W183.84
73
Ta180.95
72
Hf178.49
71
Lu174.967
56
Ba137.327
55
Cs132.905
54
Xe131.29
53
I126.904
52
Te127.60
51
Sb121.760
50
Sn118.710
49
I n114.818
48
Cd112.4
47
Ag107.868
46
Pd106.42
45
Rh102.906
44
Ru101.07
43
Tc(98)
42
Mo95.94
41
Nb92.906
40
Zr91.224
39
Y88.906
38
Sr87.62
37
Rb85.468
36
Kr83.80
35
Br79.904
34
Se78.96
33
As74.922
32
Ge72.61
31
Ga69.723
30
Zn65.39
29
Cu63.546
28
Ni58.69
27
Co58.933
26
Fe55.845
25
Mn54.938
24
Cr51.996
23
V50.942
22
Ti47.87
21
Sc44.956
20
Ca40.078
19
K39.098
118
Uuo117
Uus116Uuh(292)
115
Uup(288)
114
Uuq(289)
113
Uut(284)
112Uub(285)
111
Rg(272)
110
Ds(269)
109
Mt(268)
108
Hs(269)
107
Bh(264)
106
Sg(266)
105
Db(262)
104
Rf(261)
103
Lr(262)
88
Ra(226)
87
Fr(223)
86
Rn(222)
85
At(210)
84
Po(209)
83
Bi208.980
82
Pb207.2
81
Tl204.383
80
Hg200.59
79
Au196.967
78
Pt195.078
77
I r192.217
76
Os190.23
75
Re186.207
74
W183.84
73
Ta180.95
72
Hf178.49
71
Lu174.967
56
Ba137.327
55
Cs132.905
54
Xe131.29
53
I126.904
52
Te127.60
51
Sb121.760
50
Sn118.710
49
I n114.818
48
Cd112.4
47
Ag107.868
46
Pd106.42
45
Rh102.906
44
Ru101.07
43
Tc(98)
42
Mo95.94
41
Nb92.906
40
Zr91.224
39
Y88.906
38
Sr87.62
37
Rb85.468
36
Kr83.80
35
Br79.904
34
Se78.96
33
As74.922
32
Ge72.61
31
Ga69.723
30
Zn65.39
29
Cu63.546
28
Ni58.69
27
Co58.933
26
Fe55.845
25
Mn54.938
24
Cr51.996
23
V50.942
22
Ti47.87
21
Sc44.956
20
Ca40.078
19
K39.098
102
No(259)
101
Md(258)
100
Fm(257)
99
Es(252)
98
Cf(251)
97
Bk(247)
96
Cm(247)
95
Am(243)
94
Pu(244)
93
Np(237)
92
U238.029
91
Pa231.036
90
Th232.038
89
Ac(227)
70
Yb173.04
69
Tm168.934
68
Er167.26
67
Ho164.930
66
Dy162.50
65
Tb158.925
64
Gd157.25
63
Eu151.964
62
Sm150.36
61
Pm(145)
60
Nd144.24
59
Pr140.908
58
Ce140.116
57
La138.906
102
No(259)
101
Md(258)
100
Fm(257)
99
Es(252)
98
Cf(251)
97
Bk(247)
96
Cm(247)
95
Am(243)
94
Pu(244)
93
Np(237)
92
U238.029
91
Pa231.036
90
Th232.038
89
Ac(227)
70
Yb173.04
69
Tm168.934
68
Er167.26
67
Ho164.930
66
Dy162.50
65
Tb158.925
64
Gd157.25
63
Eu151.964
62
Sm150.36
61
Pm(145)
60
Nd144.24
59
Pr140.908
58
Ce140.116
57
La138.906
12
Mg24.305
11
Na22.990
4
Be9.012
3
Li6.941
12
Mg24.305
11
Na22.990
4
Be9.012
3
Li6.941
1
H1.008
1
H1.008
2
He4.003
2
He4.003
18
Ar39.948
17
Cl35.453
16
S32.066
15
P30.974
14
Si28.086
13
Al26.982
18
Ar39.948
17
Cl35.453
16
S32.066
15
P30.974
14
Si28.086
13
Al26.982
10
Ne20.180
9
F18.998
8
O15.999
7
N14.007
6
C12.001
5
B10.811
10
Ne20.180
9
F18.998
8
O15.999
7
N14.007
6
C12.001
5
B10.811
1
2
3
4
5
6
7
1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18
Lanthanides
Actinides
37
• Metal- properties: luster, reflects heat and light, good conductors of heat and electricity, malleable, ductile, all are solids except mercury (liquid)
• Nonmetal-properties: poor conductors of heat and electricity, brittle, not malleable or ductile, are solids, liquids and gases
• Metalloid- has some properties of metals and some properties of nonmetals
Elements
38
Pure Substances
• Compound- composed of two or more different elements
• The atoms are chemically combined so that the elements take on new identities and lose their original properties
Examples:H2O, CO2,CO, NO2,
39
Mixtures
• Mixtures- two or more substances that do not combine chemically, but remain the same individual substances; – Can be separated by physical means– Two types:
• Heterogeneous• Homogeneous
Based on the prefixes“hetero” and “homo,” what do you think are characteristics of thesetwo types of mixtures?
40
Heterogeneous Mixtures
• “Hetero” = different• Consists of visibly different substances
or phases (solid, liquid, gas) • Mechanical mixture- visibly not wholly
one• Example:
Trail Mix
Notice the visibly differentsubstances in these mechanical
mixtures
Pizza
41
Heterogeneous Mixtures
• Suspension- special type of heterogeneous mixture of larger particles that eventually settle
42
Heterogeneous Mixtures• Colloids- heterogeneous mixture with
particles that never settle– Milk and paint– Foggy appearance because its particles are
large enough to scatter light, unlike a solution
43
Homogeneous Mixtures
• “Homo” = same • Same uniform appearance and
composition throughout; maintain one phase (solid, liquid, gas)
• Commonly referred to as solutions• Example:
Salt WaterNotice the
uniformappearance
44
Homogeneous Mixtures• Solution- a mixture of two or more
substances that is identical throughout– Can be physically separated– Composed of solutes and solvents
the substance in the smallest amount and the one that dissolves in the solvent
the substance in the larger
amount that dissolves the solute
Colloids (milk, fog, jello) are considered solutions
Iced Tea Mix(solute)
Water(solvent)
Iced Tea(solution)
Salt water is considered a
solution. How
can it be physically separated?
45
ReviewSeparating Mixtures video
8min• Number your paper from 1-5 and
answer the following questions• Which of these is a metric unit?
– A. centiliters– B. cups– C. pounds– D. inches
46
Review
• A• 2. Which of these is a chemical
property?– A. density– B. reaction with water– C. color– D. length
47
Review
• B• 3. Which of these is a pure
substance?– A. pizza– B. tap water– C. aluminum
48
Review
• C• 4. Which of the following is a
homogenous mixture? – A. air– B. trail mix– C. soil– D. air with dust particles
49
Review• A Liquefy and then distill to
separate• 5. Which of these is a compound?
– A. – B. – C. – D.
A B C D50
Review
• D
51
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