1. Chemistry
Matter and Change

2. Chemistry is…
…the study of the composition, structure, and properties of matter and the changes it undergoes
C2H5OH O2  2 CO2 + 3 H2O + Energy
Reactants  Products

3. Matter Mass Anything that has mass and occupies space
A measure of the amount of matter

4. Atom Element The smallest unit of an element that maintains
the properties of that element
Element
A pure substance made of only one kind of atom

5. Compound A substance that is made from the atoms of two or
more elements that are chemically bonded.
Sucrose – C12H22O11
Sucrose is also known as table sugar, and is used to make Gummy Bears!

6. Properties of Matter Extensive properties
depend on the amount of matter that is present.
Extensive properties
Volume
Mass
Energy Content (think Calories!)
do not depend on the amount of matter present.
Intensive properties
Melting point
Boiling point
Density

7. Physical Change
A change in a substance that does not involve a change in the identity of the substance.
Example:
Phase Changes

8. Phase Differences
Solid – definite volume and shape; particles packed in fixed positions.
Liquid – definite volume but indefinite shape; particles close together but not in fixed positions
Gas – neither definite volume nor definite shape; particles are at great distances from one another
Plasma – high temperature, ionized phase of matter as found on the sun.

9. Three Phases

10. Copper Phases - Solid

11. Copper Phases - Liquid

12. Copper Phases – Vapor (gas)

13. Chemical Change
A change in which one or more substances are converted into different substances.
Heat and light are often evidence of a chemical change.

14. Classification of Matter

15. Separation of a Mixture
The constituents of the mixture retain their identity and may be separated by physical means.

16. Separation of a Mixture
The components of dyes such as ink may be separated by paper chromatography.

17. Separation of a Mixture
Distillation

18. Separation of a Compound The Electrolysis of water
Compounds must be separated by chemical means.
With the application of electricity, water can be separated into its elements
Reactant  Products
Water  Hydrogen + Oxygen
H2O  H O2

19. Period
The Periodic Table
Group or Family
Group or family
Period

20. Properties of Metals
Metals are good conductors of heat and electricity
Metals are malleable
Metals are ductile
Metals have high tensile strength
Metals have luster

21. Examples of Metals
Potassium, K reacts with water and must be stored in kerosene
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Zinc, Zn, is more stable than potassium
Mercury, Hg, is the only metal that exists as a liquid at room temperature

22. Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.
Nonmetals are poor conductors of heat and
electricity
Nonmetals tend to be brittle
Many nonmetals are gases at room temperature

23. Examples of Nonmetals
Microspheres of phosphorus, P, a reactive nonmetal
Sulfur, S, was once known as “brimstone”
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

24. Properties of Metalloids
Metalloids straddle the border between metals and nonmetals on the periodic table.
They have properties of both metals and nonmetals.
Metalloids are more brittle than metals, less brittle than most nonmetallic solids
Metalloids are semiconductors of electricity
Some metalloids possess metallic luster

25. Silicon, Si – A Metalloid
Silicon has metallic luster
Silicon is brittle like a nonmetal
Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B
Germanium, Ge
Arsenic, As
Antimony, Sb
Tellurium, Te