1. States of Matter and Energy

2. States of Matter

3. Physical Properties of Solids
**definite shape and volume**
Particles are low energy & have no freedom to change position.
Crystalline solids have an orderly arrangement of particles.
Amorphous solids particles have no particular order.

4. Crystalline vs. Amorphous

5. Physical Properties of Liquids
**Liquids change shape, but not volume**
The particles in a liquid move more rapidly than those of a solid.
The particles in a liquid can slide past each other, flowing freely. Liquids can take the shape of the container they are put into.

6. Properties of Liquids (Physical Science Only)
Buoyant force – The force caused by the pressure of a fluid against an object that is suspended. If the buoyant force of a fluid is greater than the force the object exerts on the fluid, the object floats. If it is less, the object sinks.
Archimedes Principle – The weight of a submerged or floating object is equal to the weight of the fluid it displaces .
Pascal’s Principle - When there is an increase in pressure at any point in a confined fluid, there is an equal increase at every other point in the container.

7. Physical Properties of Gases
**Gases are free to spread in all directions**
The particles of a gas move fast enough to break away from each other.
A gas expands to fill the available space - called diffusion.
A gas can also be compressed to a smaller volume (it causes the pressure to increase)
A gas is also the only state of matter with an odor (only gasses can enter your nose)

8. Gas Laws
Boyle’s Law- The gas law that states pressure and volume are inversely proportional. When the volume of a container of gas is increased, the pressure in the container decreases.
Charles’ Law- The gas law that states volume and temperature are directly proportional. When a gas is heated, it will expand if there is empty space.
Gay-Lussac’s Law- The gas law that states pressure and temperature are directly proportional. When a container of a fixed volume of gas is heated, the pressure inside the container increases.

9. Volume and Density
Solids tend to have the lowest volume, therefore having the greatest density
This is because of how close together particles are in a solid
Liquids are usually slightly less dense than solids and have a slightly larger volume
This is because their molecules are a little more spread out than in a solid.
Gasses have a much smaller density than liquids and a much larger volume
This is because the molecules of a gas are much more spread out than in a liquid or a solid

10. Physical Properties of Plasma
**Plasma is a state of high energy matter where atoms lose their electrons & become ions**
Plasma is the most common state of matter in the universe.
Plasmas conduct electric current, while gases do not. Stars, like the sun, are made of hydrogen in the plasma state.

11. Kinetic Theory
According to the kinetic theory, all matter is made of particles that are constantly in motion.
Because the particles are in motion, they have kinetic energy, or energy of motion.
Temperature is a measurement of average kinetic energy.
Higher temperatures indicate the particles moving faster.

12. Change of State
**Change of State: a physical change of a substance from one state to another**
The particles keep the same chemical identity- only their energy & arrangement changes.
Energy must be absorbed or released in any change of state.

13. Types of state changes

14. Laws of Conservation
The law of conservation of mass says that mass cannot be created or destroyed.
The law of conservation of energy states that energy cannot be created or destroyed.
For instance, when you drive a car, gasoline transforms its chemical energy into heat, used to move the car.

15. Types of Energy Potential Energy Kinetic Energy Chemical Energy
The amount of energy matter could potentially release in any form
Kinetic Energy
The amount of energy of an object in motion
Chemical Energy
The amount of energy stored in a chemical bond
Nuclear Energy
The amount of energy stored in the nucleus of an atom

16. Energy in Reactions When bonds are broken, energy is absorbed
energy is REQUIRED to break bonds
When bonds are formed, energy is released
This energy is stored in the chemical bonds as chemical energy and released during a reaction.

17. Exothermic Reactions

18. Endothermic Reactions

19. Periodic Table
The periodic table is an organized display of information about the elements.
There are patterns to the information which can make it possible to predict and understand both the physical properties and chemical properties of these elements.
Patterns of elemental properties reappear periodically, hence the name

20. Periodic Table Arrangement
The table is arrange by groups (columns) and periods (rows) Certain groups are called families because they all behave the same way

21. Families Group 1: Alkali Metals Group 2: Alkaline Earth Metals
Group 3-12: Transition Metals
Group 16: Chalcogens
Group 17: Halogens
Group 18: Noble Gases
Rare Earth Metals: Lanthanums
Radioactive Rare Earth Metals: Actinoids

22. Diatomic Elements Only found in nature as a pair
hydrogen (H2)
nitrogen (N2)
oxygen (O2)
fluorine (F2)
chlorine (Cl2)
bromine (Br2)
iodine (I2)
An easy way to remember the seven diatomic elements is that they form a seven on the periodic table