1. Matter: anything that has mass and takes up space
Mass: the amount of matter an object has
Weight: the force applied to an object by gravity
Substance: a sample that contains only one
kind of matter

2. States of matter Solid: matter that has - Definite shape and volume
- Particles packed tightly together
- No compressibility (incompressible)
Particles that move in a fixed position
(vibrate)

3. Liquids: matter that
- Particles are close but not in a fixed position
- Flows
- Takes the shape of its container
- Has a definite volume
- No compressibility (incompressible)

4. Gas: matter that
- Take the shape of its container
- Particles are farther apart
- Has no definite volume or shape
- Is easily compressed

5. Physical Property: a property that can be observed or measured without changing the substance’s composition
Ex: Color,
Temperature
Density
Odor
Hardness
State of matter

6. Physical Change: a change in a substance
which does not alter its chemical composition
- Freezing
- Melting
- Boiling
- Cutting
- Grinding
- Crumpling

7. Chemical Property: the ability of a
substance to react and form a new substance (observed only when there is a chemical change) (most chemical changes are not easily reversed)
Ex. Burning, rusting, rotting, corroding

8. Chemical Reactions
Chemical Reaction: one or more substances change into a new substance
Ex. Iron and oxygen react or make rust
Reactants: the starting substances in a
chemical reaction
Products: What you end up with in a
chemical reaction
HCl + NaOH → NaCl + H2O

9. How do you know if a chemical reaction is happening?
There are four indications of a chemical reaction. (not all indicators will be easy to see during every chemical reaction)
1. The production of a gas
2. A change in energy
3. A change in color
4. The production of a precipitate

10. Mixtures Mixtures: a physical blend of two or more substances
Heterogeneous Mixtures: mixtures that are not
uniform throughout or have more
than one phase
Ex. Oil and water, paint, chocolate chip
cookies, and salad

11. ALL MIXTURES CAN BE SEPERATED INTO THEIR INDIVIDUAL COMPONENTS!
Homogeneous Mixtures: a mixture that is
uniform throughout and only has
one phase
Ex. Lemonade, Koolaid, and Salt water
ALL MIXTURES CAN BE SEPERATED
INTO THEIR INDIVIDUAL COMPONENTS!

12. Elements and Compounds
Element: the simplest form of matter
- Can NOT be separated into simpler
substances through ordinary
chemical means
- They are the building blocks for all
substances
They are represented by one or two letter
symbols (C for Carbon, H for Hydrogen)

13. Compounds: two or more elements combined
- They can be separated into simpler
substances (the elements)
- They are represented chemical formulas
Ex. NaCl (salt) and H2O (water)

14. The Law of Conservation of Mass
Mass is never created nor destroyed in a chemical or physical change.
The mass of the products always equals
the mass of the reactants.

15. Intensive Properties: properties that do
not depend on the amount of matter present.
Ex. Melting point
Extensive Properties: properties that do depend
on the amount of matter present
Ex. mass

16. Qualitative and Quantitative Measurements
Qualitative Measurement: descriptive, non- numerical information
Quantitative Measurement: a numerical
measurement

17. How close is your measurement?
Accuracy: How close your measurement is
to the actual (accepted) measurement
Precision: a measure of how close a series of
measurements are to each other

18. Experimental Error
Experimental Error: How close the value you got in lab (the experimental value) is to the actual value (accepted value)
% Error = (Accept. Value – Exper. Value) x 100%
Accepted Value
In lab, I found that 1 ml of water has a mass of
1.32g. The accepted mass of 1ml of water
is 1g. What was my percent error?
%Error = (AV – EV) x 100% = (1g – 1.32g) x 100%
AV 1g= 32.0%