1. States of Matter

2. Kinetic Theory Definition: How particles in matter behave
All Matter is composed of small particles.
Particles are in constant random motion.
Particles collide with each other and walls of their containers

3. Thermal Energy Kinetic Energy
Definition: Total energy of a material’s particles; causes particles to vibrate in place.
Kinetic Energy
Definition: Temperature of the substance, or how fast the particles are moving.
- Lower Temperature: Slower Motion

4. Four States of Matter
Solid
Liquid
Gas
Plasma
Energy Level?

5. Solid Has a stable, definite shape Has a definite volume
Particles are packed closely together
Cannot move freely, can only vibrate
Energy and temperature are very low
Can only change their shape by force

6. Liquid Does not have a definite shape
Shape is determined by the container in which it is held
Volume is definite
Particles are farther apart than in solids, and can slide past each other easily
Energy and temperature, in comparison to a solid, are higher

7. Gas Has an indefinite, unstable shape
Volume is determined by the container that is closely sealed
Particles are far apart from each other, and can move around quickly
Energy and temperature are the higher than those of both solids and liquids
Gas

8. High Temperature gas with balanced positively and negatively charged particles.
Made up the most state in the universe
Examples: Fluorescent light, lightning, stars
Plasma 8

9. How particles behave….

10. Changes of State/Phase

11. Phase Changes Original State New State Names of Change Solid Liquid
Melting
Freezing
Gas
Evaporation
Condensation
Sublimation

12. Physical Change
Change that alters the substance without changing its chemical composition
Breaking, Bending, Cutting
Can be a reversible process
Examples:
Dissolving salt in water;
Denting a car bumper;
water to ice or vapor;
Glass break
Ice cream melts

13. Chemical Change
Occurs when one or more substance change into one or more new substance
Energy is released (exothermic) or absorbed (endothermic)
Indicator: Change in color and odor
Examples:
Burning candle,
Cooking
Melting sugar
Metal Rust
Food Disgetion
Photosynthesis

14. FLUID
Definition: A substance that can flow and take the shape of the container in which it is held.
Examples:
Liquids and Gases.

15. Liquid vs Gas Example /Property Liquid Gas Water Air Shape
No definite shape
Volume
No definite volume
Particles Arrangement
Close
Far apart
Energy binding particles
Strong
Weak

16. Properties of Fluid
Density
Pressure
Buoyancy
Viscosity

17. Density Mass (g or kg) Volume (liter, c.c. (cm3))
Definition: A measure of the mass of a substance per unit volume:
Does not dependent on size.
Density of a substance change as its phase change.
Usually solid being denser.
Mass (g or kg)
Volume (liter, c.c. (cm3))

18. Pressure Force (N) Area (cm2, m2)
Definition: Force exerted on a unit area of a substance.
Pressure changes Gas density, but NOT Liquids.
Thus, density can be used to identify a liquids (e.g. fancy drinks in layers)
SI Unit: Pascal (Pa)
Force (N)
Area (cm2, m2)

19. Pressure
Pascal’s principle – pressure applied to a fluid is transmitted throughout the fluid. Example: hydraulic machines.

20. Buoyancy
Definition: the ability of a fluid to exert an upward force on an object that is immersed in it.
Float
- Weight of object < Buoyant Force
- Density of object < Density of water
Sink – Weight of object > Buoyant Force

21. Buoyancy
How does an aircraft carrier made of steel (heavier than water) can stay afloat in the sea?
Clues: Density and Pressure

22. Viscosity Definition: A liquid’s resistance to flow
Determined by molecular structure
Increased temperature will lower viscosity.

23. Behavior of Gases
Pressure
Boyle’s Law
Charles’s Law
Gay-Lussac’s Law

24. Pressure Measured in units called pascal (Pa)
Collisions of particles in air result in atmospheric pressure.

25. Boyle’s Law Relates to pressure and volume
Volume decreases as pressure increases.
Pressure multiplied by volume is always equal to a constant if the temperature is constant.

26. Charles’s Law Relates to volume and temperature
At a constant pressure, volume increases as temperature increases.
At a constant pressure, volume decreases as temperature decreases.

27. Gay-Lussac’s Law
Relates pressure and temperature; at a constant volume, as temperature increases, pressure increases.