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
Hetero or Homo Mixture
1. Dish Soap:________________
2. A Rock: ________________
3. Stainless Steel:________________
Why?
4. Brewed Coffee: ________________
5. Sand: ________________
6. Oatmeal: ________________
7. Dust Free Air: ________________
8. Rusty Metal: _________________
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.
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) =
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.
10.
II. Venn Diagram
Element
Both
Compound
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?