States of Matter and Law

Solid

The molecules that make up a solid are arranged in regular, repeating patterns. They are held firmly in place but can vibrate within a limited area.

Liquid

The molecules that make up a liquid flow easily around one another. They are kept from flying apart by attractive forces between them. Liquids assume the shape of their container.

Gas

The molecules that make a gas fly in all directions at great speeds. They are so far apart that the attractive forces between them are insignificant.

Plasma

At very high temps of stars, atoms lose their electrons. The mixture of electrons and nuclei that results is the plasma state of matter.

Meniscus

Graduated cylinder water and fluids form meniscus. Downward curved surface of fluid. Read at bottom point of meniscus.

Kinetic Molecular Theory

Describes and explains the behavior of solids and liquids and gases

molecules or crystals that make up solids are held together by…

ionic or strong covalent bonding

The attractive intermolecular forces between atoms, ions, or molecules in solids are very…

strong

solids have ? shapes and definite volumes and are not ? to any extent

definite compressible

types of solids

crystalline and amorphous

crystalline solid

a solid in which atoms, ions, or molecules exist in a regular, well-defined arrangement. They exhibit sharp/ definite melting points.

all have crystal lattice structures

examples of crystalline solids

ionic solids, molecular solids (diamond, salt, ice (water), cooper)

amorphous solid

a solid that does not have much order in its structure. particles are close together, and have little freedom to move. They are not arranged in a regular pattern and melt over a range of temps.

amorphous solid examples

rubber, glass, plastic, oil

crystal lattice

3d structural arrangement of atoms in a solid. made up of unit cells

unit cell

the simplest repeating unit is a crystal lattice

ionic solid type

networks of pos and neg ions held together by strong ionic bonds (ion- ion attraction)

ionic solid type properties and examples

poor conductor of heat and electricity

high melting points

hard and brittle

dull surface

table salt, chalk

molecular solid type

group of molecules held together by relatively weak IMF

molecular solid type properties and examples

poor conductor of heat and electricity

low melting points

soft

dull surface

water, sugar

covalent network solid type

network of atoms held together by strong/ covalent bonds

covalent network solid type properties and examples

poor conductor of heat and electricity

high melting points

hard and brittle

dull to shiny surfaces

graphite and diamond

metallic solid type

network of atoms held together by metallic bonds

metallic solid type properties and examples

good conductor of heat and electricity

varying melting points

varying hardness

lustrous surface

ductile and malleable

copper, zinc, and iron

stronger forces =

more energy needed= high melting point

weak forces=

less energy needed= lower melting point

liquids are often made up of molecules that contain ? bonds and have relatively strong ?

covalent

intermolecular forces

the ? of the molecules is random, unlike that of the solid state in which the molecules are regular

arrangement

the atoms and molecules that make up liquids have more freedom of movement than do those in ?

solids

liquids have no definite ? but do have definite ? and they are not easily compressible

shape

volume

two main properties of liquids

surface tension and viscosity

surface tension

elastic like force existing at the surface of a liquid and is caused by cohesion

cohesion

the intermolecular forces shared between neighboring particles. the surface particles have no particles above them, so they exhibit a stronger attractive force upon their neighbor on the surface.

viscosity

defined as a liquid’s resistance to flow. as the intermolecular forces of attraction become stronger within a liquid, the viscosity is increasing.

different liquids will have different viscosities because of differences in the strength of their ??

intermolecular forces

temperature can also affect viscosities

as temp increases, the viscosity of a liquid decreases

cause of frequent collisions between gas particles

gases consist of molecules that are in continuous random motion. due to this motion there are frequent collisions between neighboring gas particles

diffusion of gas molecules

constant random motion= diffusion of gas molecules from high to low concentration

kinetic energy of gas molecules during collisions with constant temperature

temp of gas constant= avg kinetic energy constant

energy is transferred between molecules but no energy is lost because collisions are perfectly elastic

the higher the temp of gas=

higher the avg kinetic energy and avg speed

pressure conversions

1atm= 101.3Kpa=760torr=760mmHg

1000pa=1Kpa

kinetic

movement or energy in motion (or motion)

elastic collision

no kinetic energy is lost or gained. kinetic energy can be transferred between colliding particles but total does not change

temperature (t)

measure of kinetic energy of gas particles in sample of matter

diffusion

movement of one material to another. goes from a high concentration to low concentration

pressure (p)

force exerted on a surface per unit area

for gases, this variable is the force of collisions as gas particles strike the walls of the container

volume (v)

this variable if the empty space the gas particles travel through

changes in this variable results in shorter or longer distances between the gas particles

number of particles (n)

this variable represents the number of gas particles present. for physical processes the variable is constant. it may change if theres chemical reaction

standard temp

0.00C= 273.15K

absolute zero temp

0K =-273.15C no motion or heat

pressure measurements

1atm= 101.3kPa= 760torr= 760mmHg

100Pa= 1kPa

boyles law formula

p1v1=p2v2

ST AND SP

273.15K and 101.3Kpa

boyles law define

pressure of a gas is inversely proportional to its volume at a constant temperature.

charles law define

temp and volume have direct relationship

charles law formula

v1/t1=v2/t2

gay lussac law define

temp and pressure have direct relationship

gay lussac law formula

p1/t1=p2/t2

combined gas law

pressure, volume, and temperature of a gas are related, and it combines Boyle's, Charles's, and Gay-Lussac's laws into one equation

combined gas law formula

p1v1/t1=p2v2/t2

ideal gas law define

representation of relationship between moles, pressure, volume, and temp

idea gas formula

PV=nRT

according to KMT of an ideal gas

gas molecules have insignificant volume

no attractive forces between molecules

molecules move in perfect straight lines

collisions are perfectly elastic (do not lose energy)

Endothermic process

Absorbs heat energy from surroundings
Requires energy input to occur
Surroundings feel colder because heat is taken in

examples of endothermic processes

Melting – solid state to liquid state
Vaporization – liquid state to gas state
Sublimation – solid state to gas state

Exothermic process

Releases heat energy into surroundings
Energy is given off as heat
Surroundings feel warmer because heat is released

examples of exothermic processes

Freezing/ solidification/ crystalization- liquid state to solid state
Condensation – gas state to liquid state
Deposition – Gas state to solid state

kinetic energy

energy of motion or movement of particles

explain kinetic energy

higher the ke, more part

motion energy described by temp of substance

if temp is changing= ke is changing

solid-liquid-gas= increase in ke and particles moves faster. this requires an input/ addition of energy (heat)

potential energy

energy of interactions or IMFs of particles

explain pe

higher the pe, weaker the IMFs

energy of interaction described by its state of matter

substance is changing= pe changing

solid-liquid-gas= increase in pe and the IMFs between particles weakened. this requires input/ addition of energy (heat)

melting/ fusion

solid to liquid

sublimation

solid to gas

freezing/ solidification/ crystallization

liquid to solid

evaporation/ vaporization (boiling)

liquid to gas

deposition

gas to solid

condensation

gas to liquid

change of state/ phase

transformation of one state/ phase of matter to another

heat

transfer of energy

heat content of material changes during phase change the temp does not