1. Chapter 1/2
Chemistry and Matter

2. What is Chemistry?
Chemistry is the study of matter and the changes that matter undergoes.
Because all things are made up of matter, chemistry affects all aspects of life.

3. Areas of Chemistry Organic Chemistry Inorganic Chemistry Biochemistry
Analytical Chemistry
Physical Chemistry

4. The Scientific Method Making Observation (leads to a question)
Developing a Hypothesis
Experiment (Test Hypothesis)
Conclusion (Develop Theory or Scientific Law)
Repeat experiment

5. Matter Matter: Anything that takes up space and has mass (inertia)
Mass: The measure of the amount of matter that an object contains
Properties of Matter: Describes the characteristics and behavior of matter, including the changes that matter undergoes

6. Matter The Macroscopic View of Matter
Matter that is large enough to be seen
The Submicroscopic View of Matter
So small that you cannot see it, even with the most powerful microscope
The Microscopic View of Matter
Small enough that a microscope is needed.

7. Extensive vs. Intensive
An extensive property is a property that depends on the amount of matter in a sample.
Ex. Mass, volume, length, etc.
An intensive property is a property that depends on the type of matter in a sample, not the amount of matter.
Ex. Color, Texture, density, etc.

8. Observations of matter
Qualitative: made without measurement
Ex. Color, texture, shape, etc.
Quantitative: made with measurement
Ex. Mass, volume, length, etc.

9. States of Matter SOLID LIQUID GAS
Solid: a form of matter with definite shape and volume
Liquid: a form of matter with a indefinite shape, but a definite volume
Gas: a form of matter with an indefinite shape and volume
SOLID
LIQUID
GAS
Freezing
Evaporation
Melting
Sublimation
Condensation

10. Mixtures
Mixture: A combination of two or more substances in which the basic identity of each substance is not changed.
Mixtures can be classified as heterogeneous or homogeneous
Heterogeneous Mixtures: A mixture that has a composition that is different throughout.
Ex. Cookie Dough ice cream
Homogeneous Mixtures: A mixture that has a composition that is the same throughout.
Ex. Lemonade (solutions)

11. AQUEOUS SUGAR SOLUTION
Solutions
A solution is made up of a solute and a
solvent
Solute: The substance being dissolved
Solvent: The substance doing the dissolving
When the solvent is water the solution is said to be ‘AQUEOUS” (an aqueous solution.) = +
SOLUTE
SOLVENT
SOLUTION = +
SUGAR
WATER
AQUEOUS SUGAR SOLUTION

12. Separating Mixtures
Differences in Physical properties can be used to separate mixtures.
Filtration: a process that separates a solid from a liquid in a heterogeneous solution.
Distillation: A liquid is boiled to produce a vapor which is then condensed into a liquid (used to separate a liquid from solids or to separate two liquids)

13. Elements vs. Compounds
Element: simplest form of matter that has a unique set of properties.
Compound: substance that contains two or more elements chemically combined
Compounds can be broken down into simpler substances by chemical means, elements cannot.

14. Symbols
Chemists use chemical symbols to represent elements, and chemical formulas to represent compounds
Ex. Sodium = Na, Chlorine = Cl
Ex. Sodium Chloride = NaCl

15. Matter MATTER MIXTURES PURE SUBSTANCES COMPOUNDS ELEMENTS
PHYSICAL CHANGES
HETEROGENEOUS
MIXTURES
HOMOGENEOUS
MIXTURES
COMPOUNDS
ELEMENTS
SALT, BAKING SODA,
SUGAR
OXYGEN, GOLD,
IRON
DIRT, BLOOD, MILK
SODA, GASOLINE,
AIR

16. = = Density MASS DENSITY VOLUME DENSITY
The amount of matter (mass) contained in a unit volume.
Measured in
grams
MASS =
DENSITY
VOLUME
Measured in
milliliters
MASS per VOLUME
-OR-
GRAMS PER MILLILITER =
DENSITY

17. Chemical vs. Physical Changes
Physical Property: a quality or condition of a substance that can be observed or measured without changing the substance’s composition
Ex. Solubility, melting point, boiling point, color, density, electrical conductivity, and physical state (solid, liquid, gas)
During a physical change, the composition of matter always remains the same.
Tearing, cutting, grinding
Change of state: boil, freeze, melt, and condense

18. Chemical vs. Physical Changes
Chemical Property: the ability of a substance to undergo a chemical change is called a chemical property
Ex. Flammable, corrosive, ability to rust
During a chemical change, the composition of matter always changes
Ex.. burn, rot, rust, decompose, ferment, explode, corrode
A chemical change is also called a chemical reaction.
Possible indicators of a chemical change include:
a transfer of energy
a change in color
the production of gas
or the formation of a precipitate

19. Chemical Reactions and Energy
the capacity to do work
All chemical changes involve some sort of energy change.
Energy is either given off ….“EXOTHERMIC”
Or….taken in…. “ENDOTHERMIC” 

20. Law of Conservation of Mass and Energy
The law of conservation of mass and energy states that both matter and energy cannot be created or destroyed in any process
IT’S THE LAW!!!

21. Energy Energy is the capacity to do work or produce heat
Kinetic Energy: Energy of Motion
Potential Energy: Energy of Position (stored energy)