1. Matter

2. Matter Matter is anything that has mass and takes up space (volume)
Matter is made up of tiny particles called atoms
Atoms combine to form many different types of matter (curling iron, pizza, water, etc.)
Law of Conservation of Matter – matter can be neither created nor destroyed
(3 min)

3. Types of Matter Pure Substances Elements Compounds Impure substances
Homogeneous mixtures
Heterogeneous mixtures

4. Pure Substances Element – matter made up of one type of atom
Can be found on the periodic table
Compound – matter made up of two or more atoms CHEMICALLY bonded together
Can only be separated by chemical reactions

5. Impure Substances
Impure mixtures – two or more elements and/or compounds not chemically bonded
Can be separated by physical means
Homogeneous mixtures – uniform in composition; parts are not easily distinguished
Heterogeneous mixtures – components are not evenly distributed; parts can be identified

6. Separating mixtures Heterogeneous mixtures: filtration
Homogeneous mixtures: distillation (2 liquids), crystallization (evaporate), and chromatography

8. States of Matter Matter occurs in FOUR states Solid Liquid Gas Plasma
(flames, lightning,
Northern lights, sun)

9. STATES OF MATTER https://www.youtube.com/watch?v=KCL8zqjXbME (5 min)
LIQUID
PLASMA
SOLID
GAS
Tightly packed, in a regular pattern
Vibrate, but do not move from place to place
Close together with no regular arrangement.
Vibrate, move about, and slide past each other
Well separated with no regular arrangement.
Vibrate and move freely at high speeds
Has no definite volume or shape and is composed of electrical charged particles

10. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Solid to liquid
Melting
Heat goes into the solid as it melts.
Liquid to solid
Freezing
Heat leaves the liquid as it freezes.

11. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Liquid to gas
Vaporization, which includes boiling and evaporation
Heat goes into the liquid as it vaporizes.
Gas to liquid
Condensation
Heat leaves the gas as it condenses.
Solid to gas
Sublimation
Heat goes into the solid as it sublimates.

12. Properties of Matter
Matter has physical properties – characteristics that may be observed without changing the identity of the substance
Density, color, melting point, solubility
Matter has chemical properties – characteristics that cannot be observed without changing the identity of the substance
Flammability

13. Changes of Matter
Matter is not rigid and can change through physical or chemical means
Physical change – Change in a material that does not result in producing a new chemical (phase change, dissolving, cutting)
Chemical change – change in a material that results in a new chemical being formed (cooking, digestion)

14. Evidence of a chemical change
Form a gas Release of energy
Permanent color change Precipitate
New odor

15. Temperature Temperature and heat are NOT the same thing!
Temperature = average speed of particles
Units = oC, K, oF
Heat = a form of energy, can be used to make particles go faster
Units = joules (J), calories* (cal)
*1 cal = amount of heat needed to raise temp of 1 g of water by 1oC

16. Specific Heat Specific heat- aka heat capacity
The ratio of heat added to a system and the temp change of the system
How much heat you need to add to a substance to change its temp
Specific heat of liquid water = J/goC
or 1.00 cal/goC

17. Calories
If a metal absorbs 63.2 calories of heat, how many Joules of energy is this?
A) If a metal absorbs calories of heat, how many Joules of energy is this?

18. Law of Conservation of Energy
Law of Conservation of Energy – energy can be neither created nor destroyed (but can be transferred or transformed)

19. Energy Calculations (Q = m x c x ΔT)
Energy = specific heat x mass x change in temp
(Q = m x c x ΔT)
NOTE: mass in g, Temp in oC, Energy in J
This formula is slightly different in your book, but this is the one on the AP chemistry formula sheet
How much energy is required to raise the temp of 18g ice from -40oC to its normal melting point of 0oC? NOTE: look at page 329
Q = 18g x 2.03 J/goC x 40oC=
= 1500 J or 1.5 kJ

20. Energy Calculations
A) How much energy is needed to raise 18g of water from 0oC to 100oC? (s of H2O is J/goC)
B) A block of aluminum weighing 140. g is cooled from 98.4°C to 62.2°C with the release of joules of heat. From this data, calculate the specific heat of aluminum.