Unit 2 Notepack: Matter & Change
Name:________________________________
Period____
2-1 What is matter?
A. Matter: Anything that has _______and ______________.
B. Pure Substances: Matter that has fixed _______ _______ and definite _______ _______. Cannot be
broken down by _______ _______ means.
a. Element: a substance that cannot be __________________________________________
by chemical means.
i.e.
b. Compound: a substance made of __________________________________________
that are chemically combined.
i.e.
1. Every compound is _____________ _ from the__________ ____ that it contains.
i.e. Water: H2O
Physical Properties:
Chemical Properties:
Hydrogen: H2
Oxygen: O2
Physical Properties:
Physical Properties:
Chemical Properties:
Chemical Properties:
2. Molecule: The smallest unit of a substance that keeps _______ _______ _______ _______
_______ _______ of that substance.
3. Chemical formula: Shows the _______ _______ _______ in a compound. It also shows
_______ _______ _______ _______ _______ _______ are in the compound.
a. In the chemical formula _______ _______ shows how many _______ _______
_______ _______ are in the compound.
C16 H10 N2 O2
b. The large numbers in front of the chemical formula, called coefficients, show the
__________________________________________.
3 C16 H10 N2 O2
Try 1 Ca(ClO3)2 , called calcium chlorate
Now try 4 Ca(ClO3)2
 Practice Problems: Identify the name and number of molecules and atoms in the following substances.
1. How many atoms of each element are in CH4, methane?
2. How many atoms of each element are in AlCl3, aluminum chloride?
3. How many atoms of each element are in 4H2O, water?
4. How many atoms of each element are in 10 Fe3P2, iron phosphide?
5. How many atoms are in 6 Zn(NO3)2, zinc nitrate?
6. How many atoms are in Al2(SO3)3, aluminum sulfite?
C. Mixtures: Matter that has compositions that are not_______or _____________________. Mixtures
can be separated by _____________________into the _____________________that are mixed w/in
them.
a. Homogeneous Mixture: (homo = ______)The composition is the_____throughout.
a. Solid  Solid:
b. Liquid  Liquid:
c. Gas  Gas:
d. Solid (dissolves)  Liquid:
e. Gas (dissolves)  Liquid:
b. Heterogeneous Mixture: (Hetero = ______________) The composition is
______________ throughout.
a. Anytime more than one ______________exists in a mixture, it is considered heterogeneous b/c
“___________” states of matter are of __________ composition.
Question: Which three types of matter will always “look” homogeneous? Why.
 Practice Problems
Why?
Hetero or Homo Mixture
1. Dish Soap:________________
2. A Rock: ________________
3. Stainless Steel:________________
4. Saltwater: ______________
5. Pen ink: _______________
6. An Egg: ________________
7. Dust Free Air: ________________
8. Rusty Nail: _________________
Try these from the nuts, bolts, and paper clips lab. Make, draw, and identify as element, compound, or mixture
Bo = boltium atoms
Nu3
3 Nu
Nu2P3
2 Bo2Nu3
Nu(BoP4)2
P = paperclipium atoms
Nu = nutogen atoms
2-2 Properties of Matter
A. Physical Properties: Can be measured without ____________________________. Usually easy to
measure with ______________ or our ______________.
1. Measurable with our senses = ______________data:
2. Measurable with numbers = ______________ data:
B. Chemical Properties: Potential reactivity of substance with other substances.
1. Can only be measured by trying the ____________________________.
a. Common reactions tested for:
Table 2
Substance
Physical Property
Chemical Property
2-3 Changes of Matter
A. Physical Change: Affects one or more ______________ properties of a substance w/o
____________________________. Chemical properties are ________________________.
i.e.
1. More on Dissolving.
Solvent = Think water, the _______________. More of this, so it does the dissolving.
Solute = _______________, like sugar put in water. Less of this, so it gets dissolved.
2. Phase changes=
B. Chemical Changes: Occur when one or more substances are changed into ___________
____________________________ that have ____________________________.
i.e.
Chemical or Physical Property?
Chemical or Physical Change?
1. Tarnishes in Rain:_______________________
1. Lighting a firework: _____________________
2. Bends easily: _______________________
2. Boiling Pasta:_______________________
3. Decomposes: _______________________
3. Chewing gum: _______________________
4. Reusable/Recyclable: _______________________
4. Running your car: ______________________
5. Shiny______________________________
5. Rolling your bike: _______________________
6. Not Flammable: _______________________
6. Melting a crayon: _______________________
7. Perishable Food: _______________________
7. Rusting a nail: _______________________
8. Freezable Food: _______________________
8. Opening a can of pop: ____________________
C. Chemical equation: Describes the original beginning substances (called
)
using
chemical formulas. Then an arrow points to the newly created substances
(called
) using chemical formulas again.
(s) =
+=
(l) =
=
(g) =
∆=
(aq) =
H2 (subscripts) =
2 H2 = (Coefficients) =
Example:
a. Balancing Equations: The law of conservation of mass states that matter cannot be
________________ or _________________. So, the number of atoms reacting must equal the
number of atoms produces. However, a chemical change rearranges these atoms into new
__________________.
b. To balance equations, follow these steps.
1. Count atoms on each side of_________. They should be _________. If not, you need
to _________them.
2. Balance both sides by using ____________. Remember, they multiply through
everything inside of that compound. NEVER change _________.
3. Double check work.
Try These
____ KClO3  ____ KCl + ____ O2
____AlBr3 + ____ K2SO4  ____ KBr + ____ Al2(SO4)3
____ C3H8 + ____ O2  ____ CO2 + ____ H2O
Examples from class demos and life examples. Balance as well.
1.
2.
3.
4.
5.
6.
7.
8.
9.
2-4 Percent Yeild
1. What does Percent mean?
Example #1: What percent of this class is female?
2. What does Yield mean?
a. Example #2: As farmer had a 9 kilogram yield of grapes for wine making. What does this mean?
b. What if the farmer expected to grow 10 kilograms of grapes on the piece of land? Was this a good
year or bad year? How can we express that numerically?
3. What would % yield mean?
a. Show work calculating % yield or Example #2.
b. Example #3: What if the farmer had actually produced 11 kilograms instead? Was this a good year
or a bad year?
Show work for expressing it in % yield.
c. What is an error?
4. In the above examples #2 and #3, how much error did the farmer have?
a. Why is this an “absolute value”?
b. How can we calculate % error? What are we comparing it to?
2-5 Matter & Gas Pressure
A. Kinetic Theory:



Solids:
Liquids:
Gases:
Particle Spacing:
Particle Spacing:
Particle Spacing:
Energy:
Energy:
Energy:
Motion:
Motion:
Motion:
Shape:
Shape:
Shape:
Volume:
Volume:
Volume:
B. Four States of Matter: _____________________________________________
1. Solids: _______________ shape. _______________volume.
a. Particles are_______________and packed _______________. Therefore, they do not flow
around each other. Instead the_______________.
 Crystalline Solids: Particles are arranged in an ________________________pattern
 Amorphous Solids: Particles are _______________in an orderly fashion. This allows them
to slowly move around each other. These behave like ____________ _______________.
Examples: __________________________________________
2. Liquids: _______________shape. _______________volume.
a. Liquids will take the shape of _______________, but they maintain the ___________ __________________. Particles are _______________& packed______________ together. The
higher energy allows the particles to ____________around eachother.
b. Viscosity: A liquid’s _______________ to flow.
3. Gases: _______________shape. _______________volume.
c. Gases take the ______________________________They also occupy the__________
_______________of the container no matter how big or small it is. Particles are moving so
__________ they fly around and hit____________and ________________. This high energy
motion has overcome the forces that hold ____________________ together.
4. Plasma: _______________energy matter. A common example is the ____________.
a. Super high energy gas particles that _______________. This is why plasma TV’s work. The
_______________ in the gases acts like the old cathode ray tube. Other examples are;
b. Plasma is the ______________________________form of matter in the Universe.
2-6 Conservation of energy and matter during _____________________ and ____________________:
1. Matter cannot be ______________________________.
2. Energy cannot be ______________________________.
3. Only the _______________ of matter or energy can be changed.
4. Define Heat: Measure of _______________ of ___________ from an object of _________ energy to an
object of ________ energy.
5. Define Temperature: Measure of actual ___________ at a given _____________
6. System vs. Surroundings. The ________________ is the thing being observed or described. The
_________________ are everything else around this. We often measure the _________________ with a
thermometer or with our sences.
A. __________________ = Endo- means ___________. The system __________ energy from the
___________________. This feels ______________ to an observer.
a. i.e.
B. __________________= Exo- means _____________. The system ___________ energy to the
_________________. This feels ________________ to an observer.
a. i.e.
C. Energy and Phase Changes: During a phase change, all the energy goes to motion until phase
change is done. The temp does not change until the phase change is done.
Melting:
Diagram Example:

Freezing:
Diagram Example:

Evaporation/
Boiling:
Diagram Example:

Condensation:
Diagram Example:

Sublimation:

Diagram Example: