Solids, Liquids, & Gases

I. States of Matter (p.214-220)Kinetic Molecular TheoryFour States of MatterThermal Expansion

MATTER

Matter is….

Anything that has mass and volume Everything on the periodic table All solids, liquids, and gases

A. Kinetic Molecular Theory KMT

Tiny, constantly moving particles make up all matter.

The kinetic energy (motion) of these particles increases as temperature increases.

B. Four States of Matter Solids

low KE - particles vibrate but can’t move around

definite shape & volume crystalline - repeating geometric

pattern Ex. Snowflake, salt, ice

amorphous - no pattern Also called

NONCRYSTALLINE solids ex. glass, wax, plastics

B. Four States of Matter

Liquids higher KE - particles can

move around but are still close together

indefinite shape definite volume

Will flow and this can be described by VISCOSITY Viscosity is the resistance to flow Thicker liquids are more viscous than

thinner liquids

B. Four States of Matter

Gases high KE - particles can

separate and move throughout container

indefinite shape & volume Exert PRESSURE on the

sides of their container as the particles hit the sides

B. Four States of Matter Plasma

very high KE - particles collide with enough energy to break into charged particles (+/-)

gas-like, indefinite

shape & volume Most abundant type of matter in the

universestars, fluorescent

light bulbs, TV tubes

Bose Einstein Condensates

extremely low temperature fluids have properties that are not

completely understood such as their ability to spontaneously flow out of their containers

Only exist at temperatures close to absolute zero ( 0 K or - 273 ◦C )

C. Thermal Expansion Most matter expands when

heated & contracts when cooled.

Temp causes KE. Particles collide with more force & spread out.

EX: thermostats (bimetallic strip)

II. Changes in State (p.224-227)Phase ChangesHeating Curves

MATTER

A. Phase Changes

All phase changes are physical changes

Melting solid to liquid

Freezing liquid to solid

melting point = freezing point

A. Phase Changes

Vaporization (boiling) liquid to gas at the boiling point

Evaporation liquid to gas below the boiling point

Condensation gas to liquid

A. Phase Changes

Sublimation solid to gas EX: dry ice,

freeze drying, iodine

A. Phase Changes

B. Heating Curves

Kinetic Energy motion of particles related to temperature

Potential Energy space between particles related to phase changes

B. Heating Curves

Solid - KE

Melting - PE

Liquid - KE Boiling - PE

Gas - KE

B. Heating Curves

Heat of Fusion energy required to change from solid

to liquid some attractive forces are broken

B. Heating Curves

Heat of Vaporization energy required to change from liquid

to gas all attractive forces are broken EX: steam burns, sweating, and… the

drinking bird

HEATING CURVE

Properties of Matter

Matter can be identified by its PROPERTIES (characteristics).

Some properties are shared by lots of matter; some are unique and can be used to identify different types of matter. These special or unique properties are called CHARACTERISTIC PROPERTIES.

PHYSICAL PROPERTIES

PHYSICAL PROPERTIES are properties you can observe without changing the identity of the substance.

Examples: color, shape, size, mass, weight, state, boiling and freezing points, magnetism, tensile strength (stretch), viscosity, malleability (pounded into sheets), density

Physical Properties can be SPECIFIC or GENERAL

Specific: can be used to IDENTIFY an object, UNIQUE or “special”

General: not enough DETAIL to identify an object

PHYSICAL CHANGE

A PHYSICAL CHANGE is a change that does not affect an object’s identity

Examples: breaking into pieces, changing shape, freezing, melting, boiling

USUALLY can be reversed

When substances change STATES, their identity does not change.

As of 1995, 5 states of matter had been identified

CHEMICAL PROPERTIES CHEMICAL PROPERTIES are

properties that indicate whether an object can undergo a chemical change.

Examples: flammable, corrosive, explosive, light sensitive, heat sensitive

** Chemical properties cannot be tested without changing the substance chemically!!!**

CHEMICAL CHANGES

CHEMICAL CHANGES, also called reactions, involve the changing of one substance into another.

Examples: rusting, burning, digesting, cooking, photosynthesis

Chemical changes usually cannot be REVERSED.

However, when a chemical reaction takes place the MASS NEVER changes! The mass of the products always EQUALS the mass of the reactants.

This is a scientific law called the: LAW OF CONSERVATION OF MASS or MATTER