solids, liquids, gases ch 16 09-10. objectives 16-1 explain the 3 states of matter based on the...

Solids, Liquids, GasesCh 16

09-10

Objectives 16-1 Explain the 3 states of matter based on the

arrangement of particles, movement of particles, shape and volume.

16-2 Explain and apply Gas Laws. 16-3 Determine the viscosity of a liquid. 16-4 Create a phase change graph. 16-5 Explain a phase change graph. 16-6 Define sublimation. 16-7 Complete density problems.

Phases of MatterAKA: states of matter

Section 1

Objectives 16-1 Explain the 3 states of matter based on

the arrangement of particles, movement of particles, shape and volume.

16-4 Create a phase change graph. 16-5 Explain a phase change graph. 16-6 Define sublimation. 16-7 Complete density problems.

Kinetic Theory DEF: explanation of how particles

in matter behave.1. All matter composed of small

particles2. Particles in constant motion3. Particles collide with each other

and walls of container

Thermal EnergyDEF: Total kinetic and potential

energy of particles Temperature

DEF: measure of the average kinetic energy of the particles in a substance.

Solids

DEF: State of matter that has a definite shape and definite volume.

Particle arrangement Tightly packed together

Particle movement Vibrate in place

Picture

Particle movement Vibrate in place

Examples

SaltPlasticIceDiamondWaxDigital watch screens

LiquidsDEF: State of matter that has a no

definite shape, but definite volume.Particle arrangement

Loosely packed

Picture

Particle movement Slide past each other

Melting point - When a solid gains enough energy to break the structure holding it together

Heat of fusion - energy needed to change a solid to a liquid

GasesDEF: State of matter that has no

definite shape or no definite volume

Particle arrangementWidely spread out

Picture

Particle movement Move freely – don’t touch each

other much

Other info

Expand to fill whatever container they are in.

Heat of Vaporization Energy needed to change a liquid to a gas at its boiling point

Solid Liquid Gas

Shape DefiniteNot

definiteNot

definite

Volume Definite DefiniteNot

definite

PlasmaDEF: State of matter made up of

positively and negatively charged particles

The most common form of matter in the universe.

Plasma ExamplesNeon signs, fluorescent bulbs,

lightning bolts, Northern lights, fire, stars.

Phase Change GraphsShows the temperatures at which

substances change from solids to liquids, liquids to gases

Can show time or energy needed to make the changes

Phase changes - Adding energy

Phases Change Example

Solid liquid Melting Ice water

Liquid Gas Boiling Water steam

Solid Gas SublimingDry ice CO2

Gas

Phase changes – Giving Off energy

Phases Change Example

Liquid solid Freezing water ice

Gas liquid Condensing steam water

Gas solid DepositingWater vapor

frost

Phase change Graph

Water Phase Change Graph

DensityDEF: amount of mass in a

certain volume.

Circle Formula

Variable Units

m = mass g

D = densityLiquids – g/ml

Solids – g/cm3

V = volumeLiquids - ml

Solids - cm3

What is the density of a 140g block of plastic whose volume is 200mL?

What is the density of a piece of iron that has a mass of 59.8g and a volume of 2.08 cm3?

Steel has a density of 7.8 g/cm3. What must the volume of 33.3 g of steel be?

Granite has a density of 4.7 g/cm3. What is the mass of 46.8 cm3 of granite?

Floating VS Sinking

Water’s density is 1g/mL.Objects density < 1 will float in waterObjects density > 1 will sink. in water

Gas Laws

Sections 2 - 3

Objectives 16-2 Explain and apply Gas Laws. 16-3 Determine the viscosity of a liquid.

Viscosity – DEF: Resistance to flow

High viscosity slow moving

EX: cold syrup, molasses, cold magma

Low viscosity fast moving

EX: water, hot magma, bubble soap

PressureDEF: Amount of force exerted

per unit areaUnits

Pascals (Pa)Atmospheres (atm)

Relationships

Higher altitude = lower pressureLower altitude = higher pressureDeeper under water = higher

pressure

Thermal expansion in gases is involved with two different gas laws.Boyle’s LawCharles’ Law

Boyle’s LawDEF: The pressure a gas exerts on

the walls of its container is inversely related to the volume of the container.

Relationship IndirectConstants Temperature

VariablesPressure

Pascals (Pa) kiloPascals (kPa) OR atmospheres (atm)

VolumeL, mL, cm3

FormulaP1V1 = P2V2

Ways to rememberTeeter-totterBoyle watches PV

Real life examplesPopping a balloonSyringe and marshmallowScuba diving

Try One! – Boyles’ Law The initial pressure on a balloon is 35kPa

and the starting volume is 2L. If the final pressure is 10kPa, what is the final volume?

Charles’ LawDEF: The volume of a gas is

directly related to the temperature of the gas.

Relationship directConstants Pressure

Variables - units must be the sameVolume

L, mL, cm3 Temperature

K - kelvinFormula

T1V2 = T2 V1

Ways to rememberWindow washerCharles watches TV

Real life examplesHelium balloonAerosol canScuba tank in a hot car

Try one! – Charles’ Law If the original temperature was

5K and the final was 15K, how much did the volume increase from 20L?