1. Matter is anything that takes up space and has mass.

2. States of Matter Matter exists in three states: Solid Liquid Gas
Examples: rock, wood, chalk
Liquid
Examples: water, milk
Gas
Examples: oxygen, carbon dioxide

3. Properties of Matter Solids Have definite shape and volume
Particles are tightly packed
Particles can only vibrate
Incompressible

4. Properties of Matter Liquids Has a constant volume, shape can change
Takes the shape of the container
Particles move against each other (flow)
Very slightly compressible

5. Properties of Matter Gases (in gas form at room temp)
Completely fill the container
Particles are in constant, random motion
Particles are very far apart
Highly compressible

6. Particle Representation of Matter
Which one has the most energy?
The least energy?

8. Phase Changes of Matter

9. Properties of Matter
Intensive properties are independent of amount of substance present ex: color, smell, hardness, MP, BP, density, texture
Extensive properties depend on amount of substance. ex: mass, length, volume

10. Properties of Matter
Physical properties can be observed or measured without changing the chemical composition of substance. ex: odor, density, hardness, MP, BP, physical state, magnetism, compressibility

11. Properties of Matter
Chemical properties tell the ability of the substance to undergo reaction or not undergo reaction
Ex: sodium will react with water

12. Changes of Matter
Physical changes occurs without changing chemical composition of substance
Ex: melting, boiling, freezing, condensing, subliming, depositing, cutting, compressing

13. Changes of Matter
Chemical changes cause a substance(s) to form. Also called chemical reaction.
Ex: rusting, corroding, fermenting, decomposing, reacting, photosynthesis, combustion (burning)

14. Types of Matter
Pure substance has uniform consistency throughout. ex. elements & compounds
Elements can’t be separated into simpler substances by chemical or physical means. Contains 1 type of atom.
Compounds can be broken down by chemical means. Has 2 or more different types of atoms.

15. Types of Matter Mixtures contain 2 or more different pure substances.
Homogeneous mixtures have constant composition throughout. 1 phase. Also called solutions. ex: butter, smooth peanut butter
Heterogeneous mixtures do not have constant composition throughout. More than 1 phase. ex: chunky peanut butter

16. Matter Flowchart

17. Definitions
Reactants are the substances present at the beginning of a chemical reaction.
Products are the substances present at the end of a chemical reaction.
Ex: Sodium and chlorine react to form sodium chloride. Sodium, chlorine are reactants. Sodium chloride is product.

18. Evidence of Chemical Change
Color change
Formation of odor (smell)
Bubbles (formation of gas)
Solid (precipitate) formation
Temperature change (gets hot or cold)

19. Definitions
Endothermic reaction. The reaction gets cold; heat flows into the reaction.
Exothermic reaction. The reaction gets hot; heat flows out of the reaction. (fire)

20. The Law of Conservation of Mass or Matter
During a chemical reaction, matter is neither created nor destroyed.
Mass of reactants = Mass of products
Ex: When 48.6 g magnesium reacts with 32.0 g oxygen, how much magnesium oxide forms?

21. The Law of Definite Proportions
A compound is always composed of the same elements in the same proportion by mass.
% by mass = mass of element X 100
mass of compound

22. The Law of Definite Proportions
Example:
A compound contains g carbon and g oxygen. What are the % by mass of each element?

23. Percent Error
Sometimes in chemistry we don’t get the “maximum” or expected result. This can be due to many factors. Percent error indicates the accuracy of a measurement or calculation.

24. Percent Error
% Error = 𝑒𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙 𝑣𝑎𝑙𝑢𝑒 −𝑎𝑐𝑡𝑢𝑎𝑙 𝑣𝑎𝑙𝑢𝑒 𝑎𝑐𝑡𝑢𝑎𝑙 𝑣𝑎𝑙𝑢𝑒 x 100
“your value”
“from a literature
source or given”

25. Percent Error Example: An object has an actual mass of 35.0 g.
Toni massed the object at 34.0 g. Calculate
her percent error.

26. The Law of Multiple Proportions
When elements combine, they do so in a ratio of small whole numbers.
For example, carbon & oxygen react to form CO and CO2, but not CO1.3.

27. Separating Mixtures
Mixtures contain pure substances that can be separated based on their physical properties (solubility, BP, MP)

28. Filtration
Heterogeneous mixtures of solids & liquids can be separated by filtration.

29. Distillation
Homogeneous liquid mixtures can be separated by distillation which separates based on boiling point.

30. Crystallization
Separates solids from supersaturated solution.

31. Sublimation
Can be used to separate two solids from a mixture in which one substance sublimes.

32. Chromatography
Is used to separate compounds that have been dissolved in liquid or gas. Paper chromatography is shown below.