Chem States of Matter

Physical Change

A change that alters a substance without changing properties.

Chemical Change

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

Physical Property

A characteristic that can be observed or measured without changing the samples composition(color, temperature, density).

Properties of matter(2)

Intensive and Extrusive

Extrusive

Dependent on how much of a substance is present. Ex: mass, volume, length

Intensive

Dependent on what the substance is and not how much of it you have. Ex: Density

Chemical Property

The ability of a substance to combined with or change into one or more substances. Ex: iron from rust, copper from air.

Law of Conservation of Mass

Mass is neither created nor destroyed in a chemical reaction, it is conserved. Mass of Reactants = Mass or Products

Intermolecular Forces(3)

London Dispersion Forces, Dipole-Dipole Forces, Hydrogen bonds

London Dispersion Forces

Weak forces that result from temporary shifts in density of electron clouds(weakest).

Dipole-Dipole Forces

Attractions between opposite charges regions of polar molecules(middle).

Hydrogen Bonds

A special type of dipole-dipole attraction that occurred between molecules that contain hydrogen atom bonded to a small, highly electronegative atom, with at least one lone pair of electrons. Usually oxygen(O), Florine(F), or Nitrogen(N). Always polar and the (strongest).

Matter

anything that has mass and takes up space(solid, liquid, gas).

Solid Properties

have a definite volume and shape.

Liquid Properties

Take the shape of the container, definite volume.

Gas Properties

Have no definite shape or volume, expand to fill the container.

Vapor

refers to gaseous state of a substance that is a solid or liquid at room temp. Ex: water

Kinetic Theory of Gases

1) Gas particles are small particles separated by empty space.

2) Gas particles are in constant, random, rapid motion with no attractions or repulsion’s between particles.

3) Collision are perfectly elastic and creates pressure(no kinetic energy lost, just transferred).

Heat

transfer of energy from an object of higher temperature to an object of lower temp.

Kinetic energy and temp are directly proportional (one goes up so does the other)

Temperature is measured in units (K) kelvins

At a temp of absolute zero (OK) particle moving ceases

Melting Point

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

Boiling Point

Vapor pressure of liquid changes to a gas or vapor

Vaporization

Liquid changes to a gas or vapor

Evaporation

Vaporization only at the surface of a liquid

Sublimation

Solid changes to a gas without going through the liquid phase. Ex: dry ice

Phase Changes that release energy

Freezing point(liquid to solid), condensation(gas becomes a liquid), deposition(gas directly to a solid).

A, C, E, temp change. B and D have a constant temp and phase change.

A-solid is warming, B-melting, C-liquid is warming, D-vaporization, E-vapor is warming

Phase diagram

Temp(Cº) + Pressure(atm). Triple Point: water can be all three. Left(solid)/Middle(liquid)/right(gas).