Physical Properties of Matter
• Matter: Anything that has _____________
and ____________________.
– Mass: Amount of ______________ in an object.
Instrument:
– Volume: Amount of ______________ an object
takes up.
Instrument:
Types of Matter
• Types of Matter:
1.) Pure Substances
2.) Mixtures
Link – Matching Game
Pure Substances
1.) Pure Substances – All samples have
the same composition and properties.
There are 2 types of Pure Substances:
1.) Element
2.) Compound
Pure Substances
a.) Element: A substance that cannot be
chemically broken down.
Eg. Periodic Table (Li, C, Be, . . . all)
Pure Substances
b.) Compound: A substance that can be
chemically broken down.
Eg.
1.) NH3  ____________ +_____________
2.) CO2  ____________ + _____________
Pure Substances - Compounds
2 types of Compounds:
– i.) Binary – A compound made from _____
different elements.
Eg. NH3, CO2, H2O
– ii.) Tertiary / Ternary – A compound made of
____ or more elements.
Eg. C6H12O6 (glucose), NaOH, KClO3
Pure Substances - Compounds
** The composition (or, % composition) of
compounds can never vary! **
(Composition is Constant).
Eg. H2O -------------- ratio: ____ mol H : ____ mol O
%H and %O must be the same in all
samples of H2O, regardless of mass!
Ex.1:
2 Samples of a Compound . . .
Sample 1
60% X
40% Y
Sample 2
14g X
6g Y
%X=?
Are Samples 1 and 2 the Same or Different Compound??? Explain.
Ex.2:
3 Samples of Compounds . . . Are they the SAME or DIFFERENT??? . . .
Method 1: %Composition
Sample 1
Sample 2
Sample 3
X
6g
30%
1.5g
Y
12g
60%
3.0g
Z
2g
10%
0.5g
Same or Different? Explain.
Ex.2: (Use data from previous problem)
3 Samples of Compounds . . . Are they the SAME or DIFFERENT??? . . .
Method 2: Ratios (X : Y : Z)
Sample 1
Original
Ratio
Reduce
Same or Different? Explain.
Sample 2
Sample 3
Ex.3:
3 Samples of Compounds . . . Are they the SAME or DIFFERENT??? . . .
Method 1: %Composition
Sample 1
Sample 2
Sample 3
X
12g
50%
3.5g
Y
4g
30%
2.5g
Z
2g
20%
1.0g
Same or Different? Explain.
Ex.3: (Use data from previous problem)
3 Samples of Compounds . . . Are they the SAME or DIFFERENT??? . . .
Method 2: Ratios (X : Y : Z)
Sample 1
Original
Ratio
Reduce
Same or Different? Explain.
Sample 2
Sample 3
Mixtures
2.) Mixtures: 2 or more substances
(“ingredients”) physically combined.
2 Types:
a.) Homogeneous Mixtures
b.) Heterogeneous Mixtures
Homogeneous Mixtures
a.) Homogeneous mixtures: uniform
composition and properties throughout
the sample.
Eg. glass, metal alloys, solutions, pure air
air = (21% O2, 75% N2, 4% Other)
** Must have same (equal) amounts of substance
throughout the entire mixture. **
Homogeneous Mixtures
** Solutions are Always homogeneous mixtures!!! **
Solution: A homogenous mixture consisting of a
solute dissolved in a solvent.
Eg. 1.) NaCl(aq)
(aq) = ______________
2.) Other solutions?
Link-Salt dissolving
Salt dissolving(2)
Heterogeneous Mixtures
Heterogeneous mixtures: No uniform
composition and properties throughout the
sample.
Eg. Soil, fog, cereal, salad, air (polluted).
Item
Iron
Pure Substance or Mixture?
Type of Matter
Orange juice
Magnesium chlorate
Vinegar
Hydrogen
Classroom
Paint (in can)
Gatorade
Compare / Contrast
Compounds
Elements
Mixtures
Breaks down
chemically
Pure Substance
Composition varies
Properties always
the same
Homogeneous
• Task: Draw 3 boxes.
In box #1, illustrate a Mixture of Copper (Cu) and Sulfur (S).
In box #2, illustrate a Compound of Cu and S.
In box #3, illustrate a different Compound of Cu and S.
KEY:
Cu = shaded circle
S = unshaded circle
Separating Mixtures
•
There are six (6) main methods used to
separate various types of mixtures:
1.
2.
3.
4.
5.
6.
Chromatography
Filtration
Evaporation
Magnetism
Separatory Funnel
Distillation
Separating Mixtures
• See handout on Separating Mixtures
Phases of Matter
1.) Solids
2.) Liquids
3.) Gases
Comparing Solids, Liquids, and Gases
Phase changes
Properties of Phases
Type
SOLID
LIQUID
GAS
Shape
Volume
Motion
of
Particles
Arrangement
of
Particles
Entropy
Symbol
KE = Kinetic Energy (energy in motion)
PE = Potential Energy (stored energy)
Entropy: The measure of randomness of a system
Low entropy = organized
High entropy = not organized (random)
Diagram of Each Phase
Solid
Liquid
Gas
Pattern
No Pattern
No Pattern
Phase Changes:
A.) solid  liquid  gas:
B.) gas  liquid  solid:
1.) Particles must speed up
1.) Particles must slow down
2.) Particles must spread apart
2.)
3.) KE increases
3.)
4.) PE increases
4.)
• Endothermic – Energy must be absorbed.
• Exothermic – Energy must be released.
Phase Changes
Type of Change
Name
Solid  liquid
Fusion
Liquid  gas
Solid  gas
Sublimation
Gas  liquid
Liquid  solid
Solidification
(or _________________)
Gas  solid
Deposition
Examples of Exothermic phase changes:
Type of Change
Name
Examples of Endothermic phase changes:
Type of Change
Name
Q: Which of the following phase changes
is endothermic?
1.
2.
3.
4.
H2O(l)  H2O(s)
H2O(g)  H2O(l)
H2O(l)  H2O(g)
H2O(g)  H2O(s)
Heating and Cooling Curves
Link: Heating Curve Tutorial
Link: Heating Curve Link
Link: Heating Curve of Water (Step-by-Step) (Link 2)
Link: Phase Changes (Notebook)
Joules
• Joules (J) – Unit for measurement of heat
1 Kilojoule (1 kJ) = ______ J
Heating Curve Graph Questions:
** The graph represents a heating curve of a
substance where heat is being added at a rate
of 100 Joules per minute (100 J/min.)**
1.) In the graph, where is the substance
a.) a solid only
b.) a liquid only
c.) a gas only
d.) existing both as a solid and liquid
e.) a liquid and a gas together
2.) What is the melting point temperature of the substance?
3.) What is the boiling point temperature of the substance?
4.) How long did the fusion of the substance take?
5.) How long did the vaporization of the substance take?
6.) How long did it take to completely melt the substance?
7.) How long did it take to completely boil the substance?
8.) How much heat was needed to melt the substance?
9.) How much heat was needed to boil the substance?
1.) In what region is the substance both a liquid and a gas?
2.) How much time does it take for the solid to melt (fuse)
completely? (start at 0)
3.) Name ALL regions where KE increases:
4.) What is the change in temperature from CD?
5.) What is the phase changing process at DE called?
What is it called at BC?
6.) Name the region (range) where any trace of liquid is
present.
Temperature
• Temperature – Measures the Average Kinetic
Energy (KE = energy in ___________).
(**Does NOT measure heat!**)
Eg. (Drawing) H20(l) molecules moving at speeds
of 40mph, 20mph, and 30mph.
What is the Average?
• Thermometer – Measures Temperature
**There are three (3) different units of measurement of temperature . . .
Measuring Temperature
Unit of
Measurement
Fahrenheit (◦F)
Celsius or
Centigrade (◦C)
Kelvin (K)
Water Freezing
Point
Water Boiling Point
Link: Comparing Fahrenheit, Celsius, and Kelvin
** Converting Celsius  Kelvin and Kelvin  Celsius:
**
◦C
= K – 273
K = _______________
Conversions
Kelvin (K)
0K
Celsius (◦C)
0◦C
100◦C
100K
1.) Heat ALWAYS flows from hot  cold.
** We “feel” cold when our body (loses / gains) heat.
** We “feel” hot when our body (releases / absorbs) heat.
Eg. 1.) Ice pack
2.) Heat pack / heating pad
2.) Heat continues to flow from hot  cold
until it reaches equilibrium (equal heat
on both sides), unless interrupted.
Eg. 10◦C beaker of water + 70◦C heated
stone
3.) ** Mass is important!** The more mass
there is, the more heat energy it can contain.
(Draw the following)
Eg. 1.
Which has more energy:
2g of H20 at 100◦C or 100g of H20 at 100◦C?
Eg. 2.
Which has more energy:
10ml of H20 at 50◦C or 10ml of H20 at 20◦C?
Law of Conservation of Energy
Law of Conservation of Energy: Energy
cannot be created or destroyed, but it can
change forms.
**The energy lost by one object (exothermic),
must be gained by another (endothermic).
ENERGY LOST = ENERGY GAINED
Law of Conservation of Energy
Eg.1: Describe what happens when you put your hand in cold water.
Hand
Cold Water
1.)
1.)
2.)
2.)
Law of Conservation of Energy
Eg.2: Light Bulb
Electricity  filament in light bulb  Light
** a lot of energy wasted as heat  it goes up and out.
Measurement of Heat Energy
(**refer to Table B)
q = mCΔT = Amount of heat given off or
absorbed in a reaction.
q = heat (in joules (J))
J = unit of measurement for heat
m = mass (in grams (g))
C = specific heat capacity of a substance (in J/g◦C)
ΔT = change in Temperature [t2 – t1] (in ◦C)
Δ = “Change in”
*NOTE: kJ = kilojoules.
1kJ = 1000J
(** know this conversion!)
• Calorimeter – instrument used to measure the
amount of heat given off in a reaction.
** NOT a thermometer (which measures the avg. KE!)
**Set up the equation q = mCΔT, using only the units for
each symbol . . .
Eg.1. How many joules are absorbed when 50.0g of
H2O are heated from 30◦C to 58◦C?
Law of Conservation of Energy
**NOTE: Heat is measured in joules (J).
The value (in J) is not a (-)-number because heat is
either lost (exothermic) or gained (endothermic).
For example,
1.)10g of water cools from 40◦C to 25◦C. How much heat was
used (lost)?
2.)10g of water warms up from 25◦C to 40◦C. How much heat was
gained?
3.) What is the difference between 1.) and 2.)?
Eg.2.(HW) p.51, #30-35.
Eg.3. When 2.00g of an unknown sample of a solid
absorbed 1000. J of energy, its temperature increased
from 30.0◦C to 48.0◦C. What is the specific heat
capacity (C) of the solid?
Eg.4. When 5.00g of water at 25.0◦C absorbs 900. J of
energy, what will its final temperature be?
*** q = mCΔT does not apply during phase
changes, because there is NO change in
temperature (no ΔT).***
**Refer to Heating Curve for phase change
illustration.
Calculating Heat Energy During Phase Changes:
** See Table B **
1.) Heat of Fusion (melting): The amount of
heat it takes to melt 1g of a substance at its
melting point.
Heat of fusion = J/g
q = (m)(heat of fusion) or, q = mHF
Heat of Fusion
• Eg.1. How many joules are required to melt
460g of ice at 0◦C?
Calculating Heat Energy During Phase Changes:
** See Table B **
2.) Heat of Vaporization (boiling): The amount
of heat it takes to boil 1g of a substance at its
boiling pt.
Heat of vaporization = J/g
q = (m)(heat of vaporization) or, q = mHV
Eg.1. How many joules are required to boil
460g of water at 100◦C?
Eg.2. Link – Calculate Heat Energy Worksheet
Eg.3. p.51 # 36,37
Activity:
1.) Draw a Heating Curve.
2.) Label the phase or phase change for each region.
3.) Label each region with the appropriate formula for
calculating heat (q=mCΔT; q=mHF; q=mHV)