Post on 28-Dec-2015
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?