1. Bill Nye Discovery Video
Atoms in an aluminum can
Properties of Matter
Temperature Misconceptions (Heat Capacity)

2. Matter and Energy

3.  I. What is matter?
Matter can be defined as anything that ____ _____________________. Therefore, all matter has a _____ and a ______.
The building blocks of matter are atoms and
molecules.
• An atom is _________________________ ____________________________________.
• An element is a _____________________ __________________.
→ Cannot be ___________; simplest form of matter
Give three examples of elements:
has mass and takes up space
mass
volume
the smallest unit of an element that maintains the properties of that element
pure substance made of
only one kind of atom
broken down

4. • A compound is a substance that is made from
Give three examples of compounds:
• A molecule is the ________________________ __________________________________
_____________________.
the atoms of two or more elements that are chemically bonded
smallest unit of an element or compound that retains all the properties of that element or compound

5. 1. Extensive Property – a property that
A. Describing Matter
1. Extensive Property – a property that
depends on the ______ of matter in a sample.
Examples:
2. Intensive Property – a property that
depends on the ____ of matter in a sample,
not the amount of matter.
To identify an unknown substance,
______________ are examined.
amount
mass, volume
type
melting point, density
many properties

6. Properties can be divided into two groups:
a. physical property- ________________ _________________________________ _________________
Examples:
→ A physical change ________________ _____________________________ ____________________
a characteristic that can be observed or measured without changing the identity of the substance.
boiling point, malleability,
texture
Check out Table S!
is a change in a
substance that does not change the
identity of the substance.
cutting, melting, boiling

7. Properties can be divided into two groups:
b. chemical property- relates to a substances ability to ______________ that will transform it into _______________.
Examples: ability of charcoal to _____, the ability of iron to ____.
→ A chemical change is a change in which ___________________ are converted into _________________.
Examples: charcoal burning
-charcoal (carbon) plus oxygen yields carbon dioxide. 
undergo changes
another substance
burn
rust
one or more substances
different substances

8. Chemical changes are often written as ________,
* Chemical changes are often written as ________, with the _________ (undergoing the change) and ________ (substances formed)
clearly identified:
reactions
reactants
products
carbon + oxygen
carbon dioxide
(reactants)
(product)

10. B. Classification of Matter
Pure Substance- Element or _________; Composition is ______________ sample.
Mixture- A __________________________ ________;
→ a homogeneous mixture is ________ ________________; also called a _______.
Example:
→ a heterogeneous mixture is _____ _______ throughout sample;
compound
same throughout
physical blend of more than one substance
uniform throughout sample
solution
salt water
NOT
uniform
Ice Cream Blizzard

11. 1. Separating Mixtures - based on differences in physical properties
( )
Filtration – separates a ________________ in a _____________ mixture.
Ex. Brewed coffee
Distillation – used to separate a mixture of
_________ based on their ____________
______.
density, boiling point, melting point
solid from the liquid
heterogeneous
different boiling
points
two liquids

12. What is the difference between an element and a compound?
Checkpoint
What is the difference between an element and a compound?
__________________________________________________________
How many different elements are in a water molecule? ______ A molecule of carbon dioxide? _______
How do physical properties and chemical properties differ? __________________________________________________________
Classify each as a physical change(P) or a chemical change (C):
ripping a sheet of paper _____ melting a piece of wax ____ burning a log _____
Identify the following as a homogeneous mixture, a heterogeneous mixture, or a pure substance:
Sand on a beach __________ iodine ________________
Apple juice _____________ chicken noodle soup ___________
Separating Mixtures Activity

13. Unit 2- Part 2:The Flow of Energy
Law of Conservation of Energy – _____ ___________________________________
________________________
→ Energy can only change forms.
I. Heat and Temperature
Thermochemistry is the study of the _______ ____________ that accompany chemical reactions or physical changes.
Temperature is a measure of the _________ ____________ of the particles in a sample of matter.
in any
chemical or physical process, energy is
neither created nor destroyed.
changes in heat energy
average kinetic energy

14. →The greater the avg. kinetic energy, the ___________________.
* Absolute Zero - point at which all molecular motion stops; has never been reached!
greater the temperature
Unit
Fahrenheit
Celsius
Kelvin
Symbol ºF ºC K
Conversion
(9/5)ºC + 32 --
Freezing Point of Water
Boiling Point of Water
212
100
Body Temperature
98.6 37
310
Room Temperature
~68 25
298
Absolute Zero*
-460
-273
ºC + 273 32
273
373

15. Convert the following:
98.6 ºF to ºC b. 84ºC to K
c. -5.6ºC to ºF d. 210ºF to K

16. A. The ability to measure temperature is based on __________.
* Heat (q) is the sum total of the ______
_______ of the particles in a sample of
matter, and measured in ______ (or kJ) .
Heat always flows from areas of _______________, to areas of ______________.
Example: If a hot brass bar is placed in a room-temperature glass of water, the heat will flow from __________, to ________, until both are ________ __________.
heat transfer
kinetic
energies
Joules
high concentration
low concentration
the brass bar
the same temperature
the water

17. What is the flow of energy when an ice cube is
placed in a warm glass of water?
A calorie (cal) is the _____________ needed to raise the temperature of _________________.
→ How many calories are needed to raise
one gram of water 8°C?
→ How many calories are needed to raise two grams of water 4°C?
quantity of heat
1 gram of water 1°C

18. The quantity of heat being transferred depends on three things:
1. The ______ of the material changing temperature.
- _____ conducts heat much better than ______.
● The specific heat of a substance is the ___________________________________
________________.
Using your reference
tables, what is the unit
for specific heat?
nature
metal
plastic
amount of heat needed to raise one gram of
the substance 1°C
Substance
Specific Heat ( )
water (l)
4.18
ethanol (l)
2.44
calcium (s)
0.647
gold (s)
0.129

19. ☼ Heat affects the temperature of objects with
_______________ much less than the
temperature of those with _______________.
2. The _____ of the material changing temperature.
- It takes more heat to increase the temperature of a ______ block than it does to increase the temperature of a _____ block.
3. The ____ of the temperature change.
- _________ is needed to change the temperature of a liter of water 8°C than to change a liter of water 1°C.
high specific heat
low specific heat
mass
10cm3
1cm3
size
More heat

20. Combining these three factors, the amount of heat (q)
gained or lost with a change in temperature of a
substance can be found using the following
equation: q=
q = mCΔT m= C=
ΔT=
heat released or absorbed (Joules)
mass of substance
(grams)
specific heat capacity
(J/g●°C)
change in temperature
(°C)

21. The temperature of a 85.0 gram piece of copper alloy
increases from 30.0°C to 45.0°C when the copper
absorbs 523 J of heat. What is the specific heat of
the copper alloy?
How much heat will the same sample lose if it is cooled to 25 °C?
0.41 J/(gK)
697 J

22. What is the total number of Joules of heat energy
absorbed by 15 grams of water when it is heated
from 30 °C to 40 °C?
How many Joules of heat energy are released with
50 grams of water is cooled from 70 °C to 60 °C?
→ How many calories are released in the above example?

23. Change of state- a ______________ of a
II. States of Matter
Change of state- a ______________ of a
substance from one state of matter to another.
The three states of matter are indicated on the chart below:
physical change
State
Characteristic
Example
Shape
Volume
Molecular Arrangement
Solid (s)
Liquid (l)
Gas (g)
definite
definite
Close together; fixed
iron
indefinite
definite
Close together; flow
water
indefinite
indefinite
neon
Far apart; flow

24. The arrangement of molecules can be seen in the diagram below:
A. Although it may be difficult to imagine, the molecules in each state are in constant motion.
What happens when a drop of food color is placed on one side of a cup of water?
In which state do you think particles are moving the fastest? The slowest?

25. Compare the molecules in each state of matter:
Solid
Liquid
Gas
Speed of particles
Avg. KE of particles
Attraction among particles
Entropy (randomness)
Low Energy
High Energy

26. What happens when you add heat energy to solid
water (ice)?
What happens when you add heat energy to
liquid water?
Therefore, as ______________ to the different states of matter, they are able to _______
_____________________.
As heat is added, the molecules become so ________, that they overcome the
_____________ holding them together.
It melts into a liquid
It vaporizes into steam
energy is added
change into a new state of matter
energetic
attractive forces

27. Possible changes of state are shown below:
• Which terms are opposites? -

29. B. Heats of Vaporization and Fusion
1. Heat of Vaporization (Hv) – the heat necessary to
convert a given amount of a _____________
_______
It takes 40.7 kJ to vaporize 18 grams of water (2260 J/g)
How many kJ does it take to condense 18g of water?
→ Exactly the same as the quantity of heat ________ when the vapor
condenses (-ΔHcond).
liquid into a gas (vapor).
released

30. Vaporization and condensation occur at the same __________!!
Determining heat needed to vaporize/condense a
specific amount of liquid/gas
→ q = mHv
temperature

31. How much heat is absorbed when 24.8 g of H2O(l) at
100°C and kPa is converted to steam at 100°C?
How many kilojoules of heat are absorbed when 0.46 g
of chloroethane (C2H5Cl) vaporizes at its normal
boiling point? (Hvap = 26.4 kJ/mol)

32. 2. Heat of Fusion (Hf) – the heat necessary to convert a
given amount of a ____________________.
It takes 6.0 kJ to melt 18 grams of solid water (334 J/g).
How many kJ does it take to freeze 18g of water?
→Exactly the same as the quantity of heat is
released when the liquid solidifies (-ΔHsolid)
Fusion and melting occur at the same __________!!
a. Determining heat needed to melt/freeze a specific amount of solid/liquid → q = mHf
solid into a liquid
temperature

33. How many grams of ice at 0° C will melt if 2.25 kJ of heat are added?
How many grams of ice at 0°C could be melted by the addition of kJ of heat?

34. If heat is being added, why is the temperature constant?
The energy is being used to ____________ _____________.
Substances with high ____________ and ___________ have high __________________.
overcome the attractive forces
melting points
boiling points
intermolecular forces

35.  Checkpoint
What formula would you use if there is a change in temperature? _________________
Which state of matter has the strongest intermolecular forces? _________________
What formula would you use to determine how much energy it takes to convert a solid to a liquid? _______________________ From a gas to a liquid? ___________________
Does it take more energy to turn ice into liquid water or to turn liquid water into water vapor? Explain _____________________
Why do substances with strong intermolecular forces have higher melting and boiling points? _______________________