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