Matter and Temperature
Chapters: 2,3 and 14

Standards
• SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter
• SPS2a. Calculate density when given mass and volume
• SPS5. Students will compare and contrast the phases of matter as they relate to atomic and molecular motion
• SPS5a. Compare and contrast the atomic/molecular motion of solids, liquids, gases and plasmas
• SPS5b. Relate temperature, pressure and volume of gases to the behavior of gases

Classifying Matter
Matter: anything with mass and volume:
• Atom: smallest unit of an element
• Element: cannot be broken down into anything simpler (by chemical means) ex hydrogen, oxygen, carbon…

Classifying Matter
• Molecule: two or more different elements chemically bound; smallest unit of a compound
• Compound: made up of molecules
-formula ex NaCl

Pure Substances
• Fixed composition and definite properties ex: water, salt, nitrogen, oxygen

Mixtures
• combination of substances:
homogenous: parts are evenly distributed ex vinegar
heterogeneous: parts are not evenly distributed ex vegetables in a salad

Mixtures (cont’d)
• Miscible: can mix ex gasoline
• Immiscible: cannot mix ex oil and water

Physical Properties of Matter
• Physical Properties: can be observed without changing the identity of the substance ex melting point, boiling point , dissolving magnetism, ability to conduct electricity

Physical Properties (cont’d)
• mass: amount of matter in an object
• volume: amount of space an object takes up
• density: ratio between mass and volume
-D= m/V
-measured in g/cm3 or g/mL m
D V

Chemical Properties
• describes how a substance changes into another substance (cannot be reversed) ex flammability: ability to burn, reactivity: capacity to combine with another substance, rusting, effervescence
(bubbling)

Matter and Energy
Matteranything that has mass and volume
• 4 states: solids, liquids, gases, plasma
Energyability to do work:
• Potential
• Kinetic

Kinetic Molecular Theory
Kinetic Molecular Theory (KMT):
• All matter is made of constantly moving
particles (atoms, molecules)
• All particles have kinetic energy (KE)

Temperature and Kinetic Energy
Temperature
• measure of average kinetic energy
• the more KE an object has, the higher its temperature
Thermal energy = total KE; depends on:
• particle speed- faster particles have more KE
• number of particles- more particles have greater thermal energy

Thermal Energy Quiz
• Which beaker of water has more thermal energy?
B - same temperature, more mass
80ºC 80ºC
A B
400 mL
200 mL

States of Matter
1. solid: definite shape and volume
2. liquid: changes shape but not volume
3. gases: changes shape and volume
4 . plasma: no definite shape or volume and full of moving charged particles

Energy and Solids
Solids
• low KE - particles vibrate but can’t move around
• definite shape, volume:
*crystalline - repeating geometric pattern
*amorphous - no pattern (e.g. glass, wax)

Energy and Liquids
Liquids
• higher KE - particles can move, but are still close together
• indefinite shape, not volume
• flows-fluid

Energy and Gases
Gases
• high KE – particles move freely
• indefinite shape and volume
• flows- fluid

Energy and Plasma
Plasma
• very high KE- particles collide with enough energy to ionize (break into charged particles)
• lacks definite shape or volume
• can conduct electric current (unlike gases)
• most common state of matter

Changes of State Releasing Energy
• Condensationgas to liquid
• Freezingliquid to solid
• Temperature is constant during all changes in state of matter
(ex: If energy is added to ice, the temperature of ice will not rise until all the ice has melted)

Changes of State
• Sublimation Evaporation
Condensation
Melting
Freezing
• substance does not change during a phase change, but the energy does.

Changes of State Requiring Energy
• Melting Point: temperature at which a substance changes from a solid to a liquid
• Boiling Point: temperature at which a substance changes from a liquid to a gas

Energy Transfer Methods
• Conduction: when objects in direct contact are unequal in temperature
• Convection: occurs in fluids (liquids or gases)
-convection currents: rise and fall of fluids due to temperature differences (plate tectonics, wind)
• Radiation: transfer of energy by EM waves; no physical contact

Energy Transfer
• Heat: thermal energy that flows from a warmer material to a cooler material (energy transfer)
-measured in joules (J)

Heat Transfer
Why does A feel hot and B feel cold?
 Heat flows from A to your hand = hot.
 Heat flows from your hand to B = cold.
80ºC 10ºC
A B

Energy Transfer
• Conductor: material that can transfer energy easily as heat ex metals
• Insulator: material that cannot transfer energy easily ex. plastic, foam, wood

Temperature Scales
• T conversions:
• Fahrenheit: water boils- 212◦ F water freezes- 32◦F
• Celsius: water boils- 100 ◦ C water freezes- 0 ◦ C
◦F = 1.8C + 32.0
◦C = F – 32.0
1.8

Temperature Scales (cont’d)
• Kelvin: based on absolute zero (-273.15 ◦C, when molecular energy is at a minimum)
theoretically, KE = 0 at absolute zero (but particles actually never stop moving!)
K = ◦C + 273.0
Tκ = Tс + 273

Specific Heat
• Specific Heat (C p
)
– amount of energy required to raise the temp. of 1 kg of material by 1 degree Kelvin
– units: J/(kg·K) or J/(kg·°C)
E = cmΔ T
E =energy c = specific heat m = mass delta T = temp. change

Specific Heat Practice
How much energy must be transferred as heat
To 200kg of water in a bathtub to raise the water’s temperature from 25◦C to 37◦C?
Given: Known: Solution:
ΔT= 37◦C - 25◦C E = cmΔ T E= 4186J x 200kg x 12K
ΔT= 12K kg·K m= 200kg E= 1.0 x 10⁴ kJ c= 4186 J

Law of Thermodynamics
• First Law of Thermodynamics: total energy used in any process is conserved
• Second Law of Thermodynamics: energy transferred as heat moves from higher T to a lower T
- energy decreases in all energy transfers
- entropy: measure of disorder within a system when left to itself

Heat Engines
• Heat engines: convert chemical energy to mechanical energy through combustion
- mechanical energy: transferred by work
- internal combustion: burns fuel inside engine; always generate heat

Fluids
• gases, liquids
• Exert pressure, bouyancy,
• 3 basic principles govern fluids: Archimedes’,
Pascal’s, and Bernoulli’s

Pressure
• Amount of force exerted on a given area pressure
 force area
• P = F
A
• SI unit = Pascal; 1P = 1N/m²
• Fluids exert pressure in all directions

Buoyant Force
• All fluids exert an upward buoyant force on matter
• Due to increased pressure with increased depth

Archimedes’ Principle
• Archimedes’ principle: buoyant force on an object in fluid is an upward force equal to the weight of the fluid that the object displaces

Buoyancy and Density
• Objects with D = 1.00g/cm³ or less will float

Pascal’s Principle
• Pascal’s principle: if pressure is increased at any point in a container, the pressure increases at all points by the same amount
• P₁ = P₂ or F₁ = F₂
A₁ A₂

Pascal’s Principle Practice
A hydraulic lift lifts a 19,000 N car. If the area of the small piston (A₁) equals 10.5 cm² and the area of the large piston (A₂) equals 400 cm², what force needs to be exerted on the small piston to lift the car?
Given: Known: Solution:
F₂ = 19,000N F₁ = F₂ F₁ = (F₂)(A₁)
A₁ = 10.5 cm² A₁ A₂ A₂
A₂ = 400 cm² F₁ = (19,000N)(10.5cm²)
F ₁ = ? 400cm
F₁ = 500N ²

Fluids in Motion
• Move faster in smaller areas than large ones
(think water through a partially blocked hose)
• Viscosity: the resistance of fluids to flow

Bernoulli’s Principle
• Fluid pressure decreases as speed increases

Behavior of Gases
Properties:
• Fill container
• Mix with each other
• Low density
• Compressible
(unlike solids or liquids, gases are mostly empty space)

Gas Laws
Describe how the behavior of gas is affected by:
• Pressure
• Volume
• Temperature
(laws help predict the behavior of gases under certain circumstances)

Boyle’s Law
• Boyle’s Law: volume and pressure of a gas are inversely related
• P₁V₁ = P₂V₂
P₁ = initial pressure
V₁ = initial volume
P₂ = final volume
V₂ = final volume
P
V

Boyle’s Law Practice
A cylinder has a volume of 7.5 L and contains a gas at a pressure of 100 kPa. If the volume changes to 11 L, what is the final pressure?
Given: Known: Solve:
P₁ = 100 P P₁V₁ = P₂V₂ P₂ = P₁V₁
V₁ = 7.5 L V₂
V₂ = 11 L P₂ = (100 kPa)(7.5 L)
P₂ = ? 11L
P₂ = 68 kPa

Gay-Lussac’s Law
• Gay-Lussac’s Law: pressure and temperature are directly related
• P₁ = P₂
T₁ T₂
P₁ =initial pressure
T₁ = initial temp
P₂ = final pressure
T₂ = final temp
P
T

Charles’ Law
• Charles’ Law: volume and temperature are directly related (at constant pressure) V₁ = V₂
• V₁ = V₂
T₁ T₂
V
T₁ = initial temp
V₁ = initial volume
T₂ = final temp
V₂ = final volume
T