1. Matter and Temperature
Chapters: 2,3 and 14

2. 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

3. 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…

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

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

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

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

8. 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

9. 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

10. 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)

11. Matter and Energy Matter- anything that has mass and volume
4 states: solids, liquids, gases, plasma
Energy- ability to do work:
Potential
Kinetic

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

13. Temperature and Kinetic Energy
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

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

15. 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

16. 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)

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

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

19. 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

20. Changes of State Releasing Energy
Condensation- gas to liquid
Freezing- liquid 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)

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

22. 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

23. 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

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

26. Heat Transfer A B 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 A
10ºC B

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

28. 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
◦C = F – 32.0
1.8

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

30. Specific Heat T E = cmΔ Specific Heat (Cp)
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
E =energy
c = specific heat
m = mass
delta T = temp. change T

31. 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

32. 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

34. 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

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

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

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

38. 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

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

40. 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

41. 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 = 500N²

42. 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

43. Bernoulli’s Principle
Fluid pressure decreases as speed increases

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

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

46. 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

47. 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

48. Gay-Lussac’s Law P₁ = P₂ T₁ T₂
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

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