1. Warm Up Define these terms: Mixtures Elements Compounds Heterogeneous
Pure substances
Homogeneous

2. Classification of Matter
Pure Substance
Mixture
Element
Compound
Heterogeneous
Homogeneous

3. Classification of Matter

4. Pure Substance Elements
Matter that can not be broken down into simpler substances under normal lab conditions
Contains only one kind of atom
Atom Molecule
Elements (symbols) Na, Au, C
Where can you find a list of all the elements?

5. Pure Substance Compounds
Can be separated into elements
Composed of two or more elements that combine in a chemical reaction
Combine in a fixed proportion
Examples – NaCl, H2O, Fe(NO3)3 + +

6. Which are elements and which are compounds?
Compounds contain more than one element. They always have the same composition, regardless of source (law of constant composition; law of definite proportions).

7. Mixtures Granite A blend or combination of two or more pure substances
Not chemically combined
Composition of mixtures is variable
Granite

8. Mixtures Heterogeneous
A heterogeneous mixture is one that does not blend smoothly throughout and in which the individual substances remain distinct.
Mixture with visibly different parts.
Sand + water
Salt + Pepper
M & M’s

9. Mixtures Homogeneous
A homogeneous mixture has constant composition throughout; it always has a single phase.
Mixture with no visibly different parts.
Sea water: H2O + NaCl
Air: N2 + O2 + CO2

10. Practice Classifying Matter
Make a list of 3 things (and their parts) found in the classroom. Classify these as
solid, liquid, or gas
pure substances or mixtures
homogeneous or heterogeneous
elements or compounds
Be prepared to share your classifications?

11. Classify Draw a picture that represents a pure compound. mixtures
pure substances
elements
compounds
Draw a picture that represents a pure compound.

12. Classify
Classify each of the following as, a homogenous or heterogeneous mixture, pure substance; element or compound.
CH4 (methane gas)
KMnO4 (potassium permanganate)
Co (cobalt)
Al + H2O (aluminum and water)
Draw atomic level pictures of each substance.

13. Law of Definite Proportions (% By Mass)
The mass of the compound is equal to the sum of the masses of the elements that make up the compound.
The ratio of the mass of each element to the total mass of the compound is a percentage called the percent by mass.

14. Review Questions Identify each of the following as an
example of a homogeneous mixture or a
heterogeneous mixture.
A. a pile of rusty iron filings
B. 70% isopropyl rubbing alcohol
C. Saltwater
D. Gasoline

15. Review Questions Identify each of the following as an
example of an element or a compound.
A. sucrose (table sugar, C6H12O6)
B. the helium in a balloon (He)
C. baking soda (sodium bicarbonate, NaHCO3)
D. a diamond (carbon, C)

16. Review Questions A 134.50-g sample of aspirin is made up
of 6.03 g of hydrogen, g of carbon,
and g of oxygen. What is the
percent by mass of each element in
aspirin?

17. Review Questions A 2.89-g sample of sulfur reacts with
5.72 g of copper to form a black
compound. What is the percentage
composition of the compound?

18. Calculate the % mass of each element in C6H12O6
Atomic mass of C = 12, H=1, O=16