State of Matter

Physical changes

a change that alters substance without changing its composition

Chemical Changes

A change in which one or more substances turn into a new substance

Examples of physical changes

freezing, boiling, and melting

Examples of chemical change

Decomposing, rusting, and burning

Physical property

A characterization that can be observed or measured without changing the samples composition

Physical properties has how many types of

2 types: intensive and extensive

What is intensive physical properties

dependent on what the substance is and not how much of it you have

What is extensive properties

Dependent on how much of a substance is present

Examples of intensive

Density

Examples of extensive

Mass, length, and volume

Chemical property

The ability of a substance to combine with or change into one or more other substances

Examples of chemical property

Iron forming rust

Copper turning green in air

Law of Conservation of Mass

Mass is neither created nor destroyed in a chemical reaction, it is conserved

Formula of Law of Conservation of Mass

Mass of Reactants = Mass of Products

How many types of Intermolecular Forces are there

3 types: London Dispersion Forces, Dipole-Dipole Forces, and Hydrogen Bond

London Dispersion Forces

Wear forces that result from temporary shifts in density of electrons in electron clouds

Dipole-Dipole Forces

Attractions between oppositely charged regions of polar molecules

Hydrogen bond

A special type of dipole dipole attractions that occur between molecules that contain hydrogen atom bonded to a small, highly electronegative atom, with at least one lone pair of electrons

What elements are usually hydrogen bonds

Oxygen, Fluorine, or Nitrogen

What type of molecules are Hydrogen bonds

Polar molecules

Matter

Anything that has mass and takes up space

3 main types of matter:

Solid, Liquid, and gas

Solid Properties

Have their own shape and have a definite volume and shape

Liquid properties

Definite volume

Takes the shape of the container

Gas properties

Have no definite shape or volume

They expand to fill the container

Vapor

Refers to gaseous state of a substance that is a solid or liquid at room temperature

Example of vapor

water

Kinetic Theory of gases

theory that explains properties of a gas

How many things does kinetic theory of gas assume

3 things

Gas particles are…

small particles situated by empty space

Gas particles are in…

constant, random, ratios motion with no attraction or repulsion's between particles

Collision are…

perfectly elastic (no kinetic energy lost, just transferred) and creates pressure

Heat

transfer of energy from an object or higher temperature to an object of lower temperature

Kinetic energy and temperature

directly proportional (one goes up so does the other)

Temperature unit

Kelvin (K)

Absolute zero (OK)

temperature when particle movement ceases

Melting point

temperature at which the forces that hold a solid together are broken and substance becomes a liquid

Boiling Point

Vapor pressure of liquid equals the atmospheric pressure

Vaporization

Liquid changes to a gas or vapor

Evaportation

vaporization only at the surface of a liquid

Sublimation

Solid changes to a gas without going to the liquid phase

Example of sublimation

dry ice

Phase changes that release energy

Heat flows from water to surroundings, particles lose energy

Freezing point

liquid to solid

Condensation

Gas becomes a liquid

Deposition

gas directly to a solid (opposite of sublimation)

Phase change diagram

What do the three slanted portions have in common

temperature change

What do the two straight lines have in common

constant temperature and phase change

Phase diagram

A graph of pressure versus temperature that shows in which phases a substance will exist under different conditions of temperature and pressure

triple point on phase diagram

Is the point on a phase diagram that represents the temperature and pressure at which all three phases of a substance can coexist.