Phases & Behavior of Matter

Review Everything in the universe is either matter or energy. Physical Science is the study of matter and energy. Matter is anything that has mass and takes up space.

Kinetic Theory of Matter All matter is composed of small particles (atoms). These particles are in constant motion. These particles are colliding with each other and the walls of their container.

Kinetic Energy Kinetic Energy is the energy of motion. Temperature is the measurement of the KE in an object. So, the more KE the higher the temp. As the particles in an object gain KE, the temperature goes up.

Solids Particles are closely packed together. Most are geometric. There are bonds between atoms/mol. Rigid shapes. Definite shape. Definite volume.

Liquids Particles in a liquid have more KE than particles in a solid. Liquid particles have enough KE to overcome the forces that hold them together. The particles can now move past one another. (flow) Definite volume No Definite shape. Viscosity

Gases fill their container. Clip Gases Gas particles have more KE than liquid particles. They have enough energy to break all bonds and escape the liquid state. No definite Shape No definite Volume. Gases fill their container.

Plasma Most common state of matter in the universe Extremely high temperatures. Contains positively and negatively charged particles

Artificially produced plasmas Terrestrial plasmas Lightning Artificially produced plasmas Those found in plasma displays, including TVs Inside fluorescent lamps (low energy lighting), neon signs

Thermometers Work because of thermal expansion. Because mercury expands and contracts uniformly, it was used in thermometers.

Gases exert pressure on their container

Pressure: The amt of force exerted per unit of area. Gases exert pressure by colliding with things Other particles of gas Sides of the container Objects within the area of the gas, like you. 

Boyle’s and Charles’ Law Both deal with gases. Boyle’s Law As the volume decreases, the pressure increases. Charles’ Law As the temperature decrease, the volume of a gas decreases.

Boyle’s Law P1V1 = P2V2 If you decrease the volume, the pressure will increase ( no Δt)

Boyle’s Law P1 V1 = P2 V2 P1 V1 = P2 V2 A volume of helium occupies 11.0 L at 98.0 kPa. What is the new volume if the pressure drops to 86.2 kPa? P1 V1 = P2 V2 (98.O kPa) (11.0 L) = (86.2 kPa) (V2) (98.O kPa) (11.0 L) = (V2) (86.2 kPa) (V2)=12.5 L

Charles’ Law If you increase the temperature, the volume will increase

Charles’ Law V1/T1 = V2/T2

Charles’ Law

Charles’ Law V1 = T1 V2 T2 = V2 = 0.24 L What would be the resulting volume of a 2.0 L balloon at 25.0˚C that was placed in a container of ice water at 3.0˚C? V1 = T1 V2   T2 2.0 L V2 25.0˚C 3.0˚C = V2 = 0.24 L

Viscosity Resistance to flow