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Chap2 Outline
2.1 What
is Matter? 2.2 How do
Matter and Energy Interact?
2.3
How is Matter Classified? 2.4
How are Substances Identified
2.5
How should Data be Reported? (Covered in Calculation
Unit)
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2.1
What is matter?
1.
describe matter by its properties.
2.
define mass, and state how to measure it.
3.
distinguish between chemical and physical properties, and give examples
of each.
4.
draw models to represent solids, liquids, and gases on the particle
level.
2.2
How do matter and energy interact?
1.
distinguish among kinetic, potential, and other forms of energy.
2.
apply the conservation of energy and matter to systems.
3.
describe the energy changes that accompany changes of state.
4.
describe energy transfers in chemical reactions.
2.3
How is matter classified?
1.
distinguish between pure substances and mixtures on the particle level.
2.
classify mixtures as heterogeneous or homogeneous.
3.
distinguish among atoms, elements and compounds.
4.
explain how compounds can be distinguished from mixtures.
2.4
How are substances identified?
1.
list five methods of separating the components of a mixture.
2.
list properties that can be used to identify a pure substance.
3.
calculate density and use density to identify pure substances.
4.
determine the identity of substances when given adequate information.
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Chemistry
Chapter 2 Notes - Matter and Energy
2-1
What is Matter?
2-2
How do matter and energy interact?
2-3
How is matter classified?
2-4
How are substances identified?
2-5
How should data be reported?
2-1 What
is matter?
Objectives:
SWBAT
1.
describe matter by its properties.
2.
distinguish between weight and matter.
3.
define mass, and state how to measure it.
4.
distinguish between chemical and physical properties, and give examples of
each.
5.
draw models to represent solids, liquids, and gases on the particle level.
A.
Matter: Anything that has mass and volume.
1.
Volume: The amount of space an object occupies.
2.
Mass: The quantity of matter in an object.
3.
Weight: The effect of gravity on an object.
a.
Mass is constant anywhere in the universe. Usually measured by
comparing with know masses (Balances).
b.
Weight changes depending upon the force of gravity. Usually measured
using springs to measure force (Scales).
B.
Properties of Matter:
1.
Physical Properties: Properties that can be observed without changing
the identity of the object.
a.
Extensive Properties: Physical Properties are dependent upon the
quantity of matter present. (Volume, Length, Heat, & Mass)
Intensive
Properties: A property that does not change when the quantity of
matter changes. Usually depends upon the identity of the object, not
the quantity. Many of these are some of the properties
we use to identify substances!
1)
Electrical Conductivity: Ability to carry a current.
2)
Heat Conductivity: Ability to carry heat.
3)
Density: The ration of mass to volume.
4)
Melting Point (Freezing Point): The temperature that liquids
change to a solid or from a solid to a liquid.
5)
Boiling Point (Condensation Point): The temperature that liquids
change to gases or gases change to liquids.
6)
Index of Refraction: The extent which transparent materials
"bend" light.
7)
Malleability: The ability to be hammered into thin sheets.
8)
Ductility: The ability to be drawn into a thin wire.
9)
Magnetism: The ability to be turned into a Magnet.
10)
Solubility: The ability to be dissolved into different solvents.
11)
Color: The wavelengths of light reflected by an object.
12)
Temperature: The average kinetic energy of a substance.
2.
Chemical Properties: Properties that can be observed only when
substances interact with other substances.
a.
Corrosion
b.
Flammability (Combustion, Burning)
c.
Electrolysis
d.
Effervescence
e.
Precipitation:
C.
Matter Changes: (Section 2-3 in book pg 44)
1.
Physical Change: A change that does not effect the identity of the
substance.
a.
Cutting paper, melting ice, shoveling dirt, bending metal, change of
state, dissolving substances, heating, etc.
b.
Changes of state: Kinetic Theory
2.
Chemical Change: A change that produces one or more new substances.
a.
Evidence of Chemical Changes:
1)
Change in intensive properties.
2)
Gases being formed without heating.
3)
Precipitate forming.
4)
Change in color.
5)
Energy produced or absorbed.
a)
Change in temperature. **Burning**
b)
Production of light.
c)
Production of sound. **Explosion**
Exp
2A: Chemical or Physical Change Lab
Pg
39 1-4 (5 is story link)
Pg
66 #1-9
2-2 Energy
in Reactions
Objectives:
SWBAT
1.
distinguish among kinetic, potential, and other forms of energy.
2.
apply the conservation of energy and matter to systems.
3.
describe the energy changes that accompany changes of state.
4.
describe energy transfers in chemical reactions.
A.
Potential Energy (PE): Stored Energy.
B.
Kinetic Energy (KE): Energy in Motion. KE = ½ mv2
1.
Law of Conservation of Energy: Except for
nuclear reactions, energy is neither created nor destroyed. The total
amount of energy is constant.
a.
The total energy of a system is equal to the potential energy +
kinetic energy.
C.
Temperature: A measurement of the motion of molecules. Temperature measures
the intensity (concentration) of heat.
D.
Heat: Measures the total thermal energy of a system. Heat depends on both
the quantity of matter and the heat storage capacity (Specific Heat) of
matter.
1.
Difference between Heat and Temperature:
a.
These are related, but are not the same.
b.
Temperature is a reflection of the heat energy of a system, but is a
measurement of the heat concentration or intensity.
c.
The amount of heat is the total amount of energy of a system and is
dependent on:
1)
The temperature of the matter.
2)
The mass of the matter.
3)
The heat storage capacity (Specific Heat) of the matter.
2.
Temperature Scales
a.
C (1.8) + 32 = F
b.
F –32 (.555) = C
Demo:
Burn Steel Wool
E.
Distinguish between the quantities and intensities of energy?
Transparency:
1.
Which of the following has the most heat? Temperature?
a.
A cup with 50 mL of water at 20 C
b.
A cup with 50 mL of water at 20 C
2.
Which of the following has the most heat? Temperature?
a.
A cup with 50 mL of water at 20 C
b.
A bucket with 50 mL of water at 20 C
3.
Which of the following has the most heat? Temperature?
a.
A full bucket of water at 20 C
b.
A full cup of water at 20 C
4.
Which of the following has the most heat? Temperature?
a.
A cup with 50 mL of water at 25 C
b.
A cup with 50 mL of water at 20 C
5.
Which of the following has the most heat? Temperature?
a.
A cup with 100 mL of water at –150C
b.
A cup with 100 mL of water at –100 C
6.
Which of the following has the most energy?
a.
A cup with 50 mL of water at 20 C
b.
A cup with 50 mL of water at 70 C
7.
Which has the most energy?
a.
A cup with 100 mL of water at 20 C
b.
A cup with 50 mL of water at 20 C
8.
Which of the following has the most energy?
a.
A cup with 50 mL of water at 20 C
b.
A cup with 50 mL of alcohol at 20 C
F.
Kinetic Theory: States of Matter
G.
Chemical Reactions:
1.
For Chemistry when you describe heat and temperature do not use terms
like hot, cold, cool, etc. Remember that heat is measuring the total
amount of energy, while temperature measures the intensity of heat. Cold
is the absence of heat.
2.
If we pour together two reactants and observe temperature going up what
is happening?
a.
/---->Difference = 50 kJ given off as heat
b.
Reactants 100 kJ -----------> Products 50 kJ
3.
Exothermic Change: Energy is released to the surroundings (usually in
the form of heat). Temperature usually increases, -D H.
4.
If we pour together two reactants and observe that the temperature
dropped, what is happening?
a.
Difference is taken from environment -------\
1)
Reactants 125 kJ ---------> Products 200 kJ
5.
Endothermic Change: Energy is absorbed from the surroundings (usually in
the form of heat). Temperature decreases, +D H.
Need
to develop a Heat/Temperature Distinguishment Lab
Pg
43 # 6-7 (8 is Story Link)
Pg
45 9-11
Pg
66 # 10 - 21
2-3
How is
matter classified?
Objectives:
SWBAT
1.
distinguish between pure substances and mixtures on the particle level.
2.
classify mixtures as heterogeneous or homogeneous.
3.
distinguish among atoms, elements and compounds.
4.
explain how compounds can be distinguished from mixtures.
A.
Mixtures and pure substances:
1.
Pure substances: matter is composed of only one kind of atom or
compound.
a.
Elements: composed of the same type of atom.
1)
Elements are the simplest pure substances.
2)
Review: Chemical Symbols: First letter is capitalized,
all others are small!
3)
Elements may consist of single atoms or of groups of atoms
(molecules).
4)
Allotropes: different molecular forms of an element in the same
physical state. Examples:
a)
Oxygen: Nascent (O), Oxygen (O2) & Ozone (O3)
b)
Carbon: graphite, diamonds, bucky ball, buckytube, &
coal.
b.
Compounds/Molecules: a small group of atoms held together by a
chemical bond. These are pure substances usually composed of two or
more types of atoms (elements).
2.
Mixture: a collection of two or more pure substances physically mixed
together.
a.
Homogeneous:
Contains only one phase.
1)
Solutions: a homogeneous mixture that consists of substances
mixed on the scale of individual particles. Solutions are always
homogeneous.
b.
Heterogeneous:
Contains more than one phase. Mixtures are always heterogeneous.
1)
Phase: any part of a system that has uniform composition and
properties.
Homogeneous
Mixture |
Heterogeneous
Mixture |
Solutions |
Oil
& Vinegar |
Gasoline |
Salad |
Tea |
Bread
Dough |
Vinegar |
Plastic
Squeeze containers |
Sea
Water |
Concrete |
2)
It is very hard to tell the difference without laboratory
testing.
B.
Three principal differences between compounds and mixtures:
1.
Mixtures are never made of only a single compound.
2.
The properties of a mixture reflect the properties of the substances it
contains, but the properties of a compound often bear no resemblance to
the properties of the elements that compose it.
3.
Compounds have a definite composition by mass of their combining
elements (This is called the Law of Definite Proportions). The
iron-sulfur compound pyrite has a definite composition. The mass of
pyrite is always 46.55% iron and 53.45% sulfur. In contrast, substances
in a mixture can exist in any mass ratio.
C.
Predicting Properties of Homogeneous Mixtures
1.
Homogeneous Mixtures have intensive properties that are proportional to
their mixtures.
Experiment
2B: Properties of Homogeneous Mixtures
Need
to develop:
Need
worksheet:
Pg
51 #15-17 (18&19 Story Link)
Pg
67 #22-28
2-4 How
are substances identified?
Objectives:
SWBAT
1.
list five methods of separating the components of a mixture.
2.
list properties that can be used to identify a pure substance.
3.
calculate density and use density to identify pure substances.
4.
determine the identity of substances when given adequate information.
A.
Use Some Intensive Properties. Those intensive properties that depend upon
the structure of matter.
B.
Use Chemical Properties: These depend upon the identity of matter.
C.
Methods of separating mixtures:
1.
Mixtures can be separated by physical means using the differences in the
intensive properties of the materials of the mixture.:
a.
Filter (uses solubility)
1)
Solid & Liquid
2)
Sand & Gravel
3)
Sand & Salt
b.
Evaporation (uses heat to evaporate the solvent in a solution)
1)
Salt in water
c.
Distillation (uses the difference in boiling points)
1)
Water and alcohol
d.
Centrifuge (uses the difference in density)
e.
Decant (uses the differences in solubility & density
1)
Water and oil
f.
Chromatography (uses the difference in solubility)
Experiment
2D: Paper Chromatography
Experiment
2E: Murder In Opulance
Pg
57 #20-22 (23 Story Link)
Pg
67 #32-38
2-5 How
should data be reported?
A. Reliability
of measurements: Are measurements being recorded properly and made using
good laboratory techniques?
1.
Accuracy: the extent to which a measurement approaches the true value of a
quantity. Relate to the Chemical or Physical Change
Lab
2.
Precision: the degree of exactness of refinement of a measurement.
3.
Use the analogy of a bulls eye target to illustrate.
4.
Experiment 2A Accuracy
B.
Laboratory Equipment: In this class we will use the smallest division of the
scale of an instrument as the accuracy of the instrument.
C.
Standard Units.
D.
Graphing (see pg 800, Appendix B)
Pg
62 #24-31 (Significant Figures)
Pg
67 #39-52
Chapter
2 Review WS
Chapter
2 Review
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