Matter
Can NOT be separated
by physical means
Can NOT be separated
by chemical means
Particle
Diagram
CAN be Separated by
PHYSICAL means
Separated by chemical
means, only
Particle
Diagram
Same
composition
throughout
Particle
Diagram
Different
composition
throughout
Particle
Diagram
Elements vs. Compounds
Element = ___________________________________________________________________
Compound = ___________________________________________________________________
Rules for writing element symbols:
1) ______________________________________
2) ______________________________________
1. Circle all the elements and underline the compounds below.
2. On the line provided, record the number of different symbols within the species.
CO
Mg
___
Co
___
C2H5OH ___
Al(CN)3
___
Cl2
___
H2SO4
___
He
___
NI3
___
O2
___
___
NaCl
___
___
I
___
C
___
____
H2O
Cu
Questions:
1) Does each compound have the same number of symbols? ____
2) For each ELEMENT above, how many total symbols are listed? __
3) What is the minimum number of symbols that must be present in order for a species to be
considered a compound? __
Understanding Compound Formulas:
Within a compound, you may see subscripts. These subscripts tell you the number of each type of
atom that is present.
Example:
# carbon atoms __
# oxygen atoms __
If there are parentheses present around two or more atoms, the subscript applies to all atoms within the
parentheses.
Example:
# aluminum atoms __
# carbon atoms __
# nitrogen atoms __
If one of the atoms within the parentheses has a subscript, you multiply this number by the number outside
of the parentheses.
Example:
# of iron atoms: ____
# of sulfur atoms: ______
# of oxygen atoms: ____
Particle Diagrams
•
Elements: __________________________________________________________________________
___________________________________________________________________________________
•
Diatomic Elements: _________________________________________________________________
•
Br2, I2, N2, Cl2, H2, O2, F2
•
Compounds: ________________________________________________________________________
•
Mixtures: __________________________________________________________________________
Identify as element, diatomic element, compound, mixture of elements, mixture of compounds, or mixture of
elements and compounds
_________________________
_____________________
_____________________
_____________________
__________________
______________________
______________________
Separation of Matter
Separation Apparatus
Filtration
Watch Glass Evaporation
Crucible Evaporation
Type of
Separation
(Physical or
Chemical)
Description of
Technique
What types of
matter will it
separate?
Separation of Matter
(continued)
Distillation
Chromatography
On the other hand → _____________________ requires reacting
a sample with something else in order to turn it into a completely
different compound
Properties of Matter
_________________ are the constants about a substance; can use our
senses to observe them; do not require chemical analysis
Example: ______________________________________________
o Extensive Property: a property that depends on how much
material you are dealing with
Ex: _________________________________________
o Intensive Property: a property that does not depend on how
much material you are dealing with (help identify matter; a
constant about that particular type of matter)
Ex:
__________________________________________________
Chemical properties include behaviors substances adhere to when they
__________ with other substances
Examples:
Guided Practice: Identify the following as being intensive, extensive, or chemical
properties.
____________ 1. The mass of copper wire is 255 g.
____________ 2. The boiling point of ethyl alcohol is 77°C.
____________ 3. Baking soda reacts with vinegar to make carbon dioxide gas.
____________ 4. The density of mercury is 13.6g/mL.
____________ 5. The solubility of sodium chloride in water is 40g/100mL of water.
Physical vs. Chemical Changes
Matter is always changing. Ice in your drink melts. Wood in your fire burns.
Physical Change – a change that does NOT alter the chemical properties of a
substance (example: ______________, ______________); change in size or
shape; ____________________________
*PHYSICAL processes can be reversed ________________________
Example: ________________________________
Chemical Change – a reaction in which the composition of a substance is
changed (example: __________); properties _______________________
Signs of a chemical reaction:
Guided Practice:
Change of Matter
Burning toast
Making ice cubes
Lighting a candle
Spoiling Milk
Making Kool-aid
Physical or Chemical
Phases of Matter
Characteristics
Volume
Shape
Particle Arrangement
Solid
Liquid
Gas
Temperature and Density
Temperature: ____________________________________________________________
________________________________________________________________________
Formula (Table T)
Examples:
1) 100°C = ___________ K
2) 77 K = _____________ °C
3) 200°C = ___________K
4) 40°C = ___________K
5) 450K = __________°C
Density: ________________________________________________________________
Formula (Table T)
Examples
1) A copper penny has a mass of 3.1g and a volume of 0.35cm3. What is the density of
copper?
2) What is the volume of a pure silver coin that has a mass of 14g?
Uncertainty in Measurement
The degree of certainty determined by two factors
Precision - _______________________________________________________
Accuracy - _______________________________________________________
Practice
1) 3 groups of students measure the mass of a product of the same chemical
reaction. The groups recoded data of 8.83g, 8.84g and 8.83g. The known mass
of the product from that reaction is 8.60g. Are the students accurate or
precise?
2) Cheryl, Cynthia, Carmen, and Casey take target practice in PE. Assuming that
they were all aiming at the bulls eye, match each target with the proper
description.
1)
2)
3)
4)
Accurate and precise
Not precise, but one piece of data accurate
Precise but not accurate
Neither precise nor accurate
Percent Error
 Percentage error compares the absolute error to the size of what is being
measured.
Formula (Table T):
Measured value: value you “get”
Accepted value: value you “should get”
Practice:
1) A student determined in the laboratory that the percent by mass of water in
CuSO4 ∙ 5H2O is 40%. If the accepted value is 36%, what is the percent error?
2) A student found the boiling point of a liquid to be 80.4°C. If the liquids actual
boiling point is 80.6°C, what is the experimental percent error?