Download Matter and Energy

UNIT 2:
MATTER AND ENERGY
Q1 TEST QUESTIONS:
1. What did you think of the test? (Easy/Hard/Impossible?)
a. How long did you study for this part?
b. What did you do to study?
2. What did you think of the candle task?
a. How long did you study for this part?
b. What did you do to study?
Warm-up:
Identify the following words as either matter or not
matter:
Desks
Happiness
Plates
Air
Glass
Laughter
Forces
Time
Feelings
Water
Sand
Helium
Energy
I. MATTER
Matter
Not Matter
I. MATTER
a. Matter: Anything that has mass
and takes up space.
b. Mass: the amount of matter (stuff)
something has
c. Substance: Matter that has a
uniform and definite composition
II. PHYSICAL PROPERTIES AND CHANGES
a. Physical Property:

Can be observed or measured without changing the
identity of the substance.
EX: Color, Mass, Volume, Melting Point (Name a
few more)
II. PHYSICAL PROPERTIES AND CHANGES
i.
Extensive Property:

Different with different amounts of a substance
EX: Mass, Volume
ii. Intensive Property:

The same no matter how much of a substance you
have
EX: Color, Melting Point
II. PHYSICAL PROPERTIES AND CHANGES
b. Physical Change:


A change that does not change the identity of the
substance
Changes the look, not the substance
EX: Melting, Crushing, Tearing (Name a few more)
II. PHYSICAL PROPERTIES AND CHANGES
i.
States of Matter: state changes are physical
changes
Deposition
Microscopic
Shape/Volume
Macroscopic
Solid
Liquid
Melting
Definite/
Definite
Gas (Vapor)
Evaporation
Indefinite/
Definite
Freezing
Indefinite/
Indefinite
Condensation
Sublimation
II. PHYSICAL PROPERTIES AND CHANGES

http://www.youtube.com/watch?v=v12xG80KcZw
&feature=related&safety_mode=true&persist_saf
ety_mode=1&safe=active
III. CHEMICAL PROPERTIES AND CHANGES
a. Chemical Property:

A substance’s ability to undergo changes that
transform it into a different substance
EX: Reacts with acid, Burns in air
III. CHEMICAL PROPERTIES AND CHANGES
b. Chemical Change:


A change that changes the substance you have
It is a chemically different substance after the
change
EX: Decomposing, Burning, Digesting
III. CHEMICAL PROPERTIES AND CHANGES
i.
Chemical Reactions
1. Writing Equations
2. Evidence
o Color Change
o Formation of gas (bubbles)
o Formation of solid (precipitate)
o Produce light/heat (energy)
CHEMICAL VS. PHYSICAL

Examples:
1.
melting point
2.
flammable
3.
density
4.
magnetic
5.
tarnishes in air
6.
rusting iron
7.
dissolving in water
8.
burning a log
9.
melting ice
10.
grinding spices
I. MATTER
b. Classifications of Matter
i. Mixture – made of multiple
substances that can be separated
by physical means.
EX: milk, air, chex mix, salad
dressing (name a few more!)
I. MATTER
1. Homogeneous Mixture –




Made of multiple substances
Appears to be one substance
All parts have the same composition and
properties.
Uniform throughout.
EX: salt water, hot
tea, air, steel,
name a few more!
I. MATTER
a. Solution –
• a homogeneous
mixture of two or
more substances in
a single phase.
• Solute –
Substance being
dissolved and
• Solvent –
substance doing
the dissolving
Ex: Salt water, air
I. MATTER
b. Alloy – a solid homogeneous mixture
Ex: Bronze – copper and tin, Steel – iron and
carbon, 14k gold – copper and gold,
Sterling Silver – silver and copper,
name a few more!
I. MATTER
2. Heterogeneous Mixture –
 Made of multiple substances whose parts can
be seen.
 Portions have different composition sand
properties.
 NOT uniform throughout
Ex: oil and
water, pizza,
mixed nuts,
name a few
more!
I. MATTER
**Why do some things mix?
 “like dissolves like”
 Polar dissolve polar
 Nonpolar dissolves nonpolar
 If substances don’t mix, they have
different polarities.
I. MATTER
ii. Pure Substance –
•
•
Constant composition that
is uniform throughout.
Can NOT be separated by
physical means
Ex: water,
oxygen, silver,
gold, sugar, salt,
name a few
more!
I. MATTER
1. Element – can not be broken down
into simpler, stable substances.
I. MATTER
a. Atom –

The smallest unit of an element, that
maintains the chemical identity of that
element.
Element
HHHHHHHHHHHH
HHHHHHHHHHHH
HHHHHHHHHHHH
HHHHHHHHHHHH
Atom
H
I. MATTER
2. Compound –
•
•
Made of two or more types of atoms
Can be broken down into simpler substances
through chemical changes
NaCl (Table Salt)
Sucrose (table sugar)
I. MATTER
a. Molecule – the smallest unit of a
compound that maintains the
chemical identity of that compound.
Compound
Molecule
O
H
H
CONCEPT MAP:
WARM-UP:

Classify each type of matter:
CHEMICAL VS. PHYSICAL



http://www.youtube.com/watch?v=Ypwtjp0FSE&safety_mode=true&persist_safety_
mode=1&safe=active
http://www.youtube.com/watch?v=QL7V3L3dfDM
&safety_mode=true&persist_safety_mode=1&saf
e=active
http://www.quia.com/quiz/303980.html
IV. ENERGY
Energy: The ability to do work or
cause a change
b. Types of Energy:
i. Potential Energy: Energy of
position or composition
a.
ii.
Kinetic Energy: Energy of
motion
IV. ENERGY
i. Mechanical: Energy
due to an object’s
motion (kinetic) or
position (potential).

How does this picture
represent mechanical
energy?
EXAMPLES OF MECHANICAL ENERGY:
IV. ENERGY
ii.Electromagnetic: Light
energy


Includes energy from
gamma rays, x-rays,
ultraviolet rays, visible
light, infrared rays,
microwave and radio
bands
How do these pictures
show electromagnetic
energy?
THE ELECTROMAGNETIC SPECTRUM
IV. ENERGY
iii.

Electrical: Energy
caused by the movement
of electrons
Easily transported
through power lines and
converted into other
forms of energy
IV. ENERGY
iv. Chemical: Energy that
is available for release
from chemical reactions

The chemical bonds in a
matchstick store energy
that is transformed into
thermal energy when
the match is struck.
EXAMPLES OF CHEMICAL ENERGY:
IV. ENERGY
v.
Nuclear - Energy
stored in the nucleus
of an atom.
IV. ENERGY
vi.

Thermal – Heat energy
Heat: Energy transferred between
objects at different temperatures.
High Temperature

Heat
Low Temperature
Temperature: a measure of how fast
the particles are moving (kinetic
energy)
Hot = moving quickly
Cold = moving slowly
IV. ENERGY
1. Temperature is expressed using different scales…
Kelvin and Celsius
Relationship Between K and °C :
K = °C + 273
°C = K – 273
IV. ENERGY
Examples:
a. Convert from °C to K
i.
-37 °C
ii.
100 °C
b. Convert from K to °C
i.
273K
ii.
1200K
IV. ENERGY
d. Energy can be transferred between
a system and its surroundings
i. System: All components being studied at a
given time. EX: mixture in a beaker
ii. Surroundings: Everything outside the
system. EX: the beaker and air outside the
beaker
IV. ENERGY
e. Endothermic and Exothermic
Processes:
i.
Endothermic: a reaction that absorbs heat
(energy)
ii. Exothermic: a reaction that produces heat
(energy)
IV. ENERGY
Summary:
Relationship:
Surroundings
Feels:
Endothermic
System absorbs
energy from
surroundings
Cool/Cold
Exothermic
System releases
energy to
surroundings
Warm/Hot
V. LAW OF CONSERVATION OF MASS AND ENERGY
a. Definition:
MATTER can not be created nor
destroyed in a chemical reaction or
physical change.
ENERGY can not be created nor
destroyed in a chemical reaction or
physical change.
V. LAW OF CONSERVATION OF MASS AND ENERGY
o
If mass/energy is not created or
destroyed in a chemical reaction or
physical change, where does the
mass/energy go?
V. LAW OF CONSERVATION OF MASS AND ENERGY
o
o
Mass/Energy can be created/destroyed
in a nuclear reaction (Unit 5)
Einstein’s Equation:
E=mc2
o
What are the variables, E, m, and c?
o
What does this equation mean?