1. PROPERTIES OF MATTER: PHYSICAL & CHEMICAL

2. Physical Properties
PROPERTY – ABILITY TO DO SOMETHING TYPES OF PHYSICAL PROPERTIES – * INTENSIVE – DO NOT DEPEND ON AMOUNT OF MATTER * EXTENSIVE – DEPEND ON AMOUNT OF MATTER

3. EXTENSIVE -
MASS, WEIGHT, VOLUME, & LENGTH

4. INTENSIVE -
TEXTURE, COLOR, ODOR, LUSTER (SHINY), MALLEABILITY (BEATEN INTO SHEETS), DUCTILITY (DRAWN INTO WIRES), CONDUCTIVITY (ALLOW ENERGY TO ELECTRICITY TO FLOW), HARDNESS (SCRATCHING), SOLUBILITY (DISSOLVE), MELTING/FREEZING/BOILING POINT, & DENSITY

5. COPPER ORE – COPPER – COPPER WIRE
SHEEP WOOL – REMOVED WOOL – DYED WOOL

6. DENSITY – AMOUNT OF MATTER IN A GIVEN SPACE
TOOLS – TRIPLE BEAM BALANCE, RULER OR GRADUATED CYLINDER UNITS – GRAMS PER CUBIC CENTIMETER (g/cm3) FORMULA – DENSITY = MASS/VOLUME D = M/V HOW TO FIND DENSITY – 1. MASS OUT OBJECT 2. FIND VOLUME OF OBJECT (l x w x h, displacement, or liquid in graduated cylinder) 3. CALCULATE – MASS DIVIDED BY VOLUME

8. CHEMICAL PROPERTIES *Reactivity with other chemicals
*Toxicity (Damage to Organism)
Talk Hg
*Flammability
*Combustion
*Oxidation states (rust/tarnish/rot)
*Chemical stability
*Types of chemical
bonds that will form

9. Physical vs. Chemical Change
Changing from one state to another is a
Physical Change.
If a new substance is formed it is a
Chemical Change. Molecular structure changes/rearranges.
Images are from

10. SIGNS OF PHYSICAL CHANGE SIGNS OF CHEMICAL CHANGE
CHANGED IS BASED ONLY ON PHYSICAL APPEARANCE
YOU CAN GET THE ORIGINAL SUBSTANCE BACK
STATE OF MATTER CHANGES
SIGNS OF CHEMICAL CHANGE
ODOR PRODUCED
CHANGE IN TEMPERATURE
COLOR CHANGE
BUBBLES FORMED
SOLID FORMED
SUBSTANCE DISAPPEARS

13. CHANGES OF STATE: MELTING – SOLID TO LIQUID * HOW: GAINS ENERGY
PARTICLES STRENGTH – STRONG/WEAK
ENERGY CHANGES – MORE/LESS = CHANGE IN STATE
ENERGY CAN BE FROM HEAT/PRESSURE
MELTING – SOLID TO LIQUID
* HOW: GAINS ENERGY
* WHAT HAPPENS: SPEED UP TO BECOME WEAKER TO SLIDE OVER EACH OTHER
MELTING POINT – TEMPERATURE TURNS TO LIQUID

14. FREEZING – LIQUID TO SOLID. HOW: LOSES ENERGY
FREEZING – LIQUID TO SOLID * HOW: LOSES ENERGY * WHAT HAPPENS: SLOW DOWN, GET CLOSER, STRONGER AND VIBRATE FREEZING POINT = TERMPERATURE TURNS TO SOLID FREEZING POINT = MELTING POINT E.G. – LIQUID STEEL LOSES ENERGY AND FORMS SOLID – PARTICLES SLOW DOWN, GET CLOSER, STRONGER AND VIBRATE

15. BOILING – LIQUID TO GAS. HOW: GAINS ENERGY
BOILING – LIQUID TO GAS * HOW: GAINS ENERGY * WHAT HAPPENS: SPEEDS UP, WEAKENS AND BREAK AWAY IN ALL DIRECTIONS * WHERE – THROUGHOUT THE ENERGETIC SUBSTANCE BOILING POINT – TEMPERATURE TURNS TO GAS

16. EVAPORATION – LIQUD TO GAS. HOW: GAINS ENERGY
EVAPORATION – LIQUD TO GAS * HOW: GAINS ENERGY * WHAT HAPPENS: SPEEDS UP, WEAKENS AND BREAKS AWAY IN ALL DIRECTIONS * WHERE: SURFACE OF SUBSTANCE

18. SUBLIIMATION – SOLID TO GAS. HOW: GAINS ENERGY
SUBLIIMATION – SOLID TO GAS *HOW: GAINS ENERGY *WHAT HAPPENS: SPEEDS UP, WEAKENS SKIPS LIQUID STATE AND BREAKS AWAY IN ALL DIRECTIONS

19. CONDENSATION – GAS TO LIQUID. HOW: LOSES ENERGY
CONDENSATION – GAS TO LIQUID *HOW: LOSES ENERGY *WHAT HAPPENS: SLOWS DOWN, STRENGTHENS, AND SLIDE PAST EACH OTHER

25. Balance Chemical Reactions
Chemical reactions can be represented by equations.
To show conservation of mass  Balance equations
Make sure there are the same number of each type of atom in the products and in the reactants
CaCO3  CaO + CO2

26. Balancing Equations CH4 + 2 O2 → CO2 + 2 H2O
No subscript or coefficient is understood to be 1.

27. Balancing Equations 1 C  1 C 4 H  4 H 4 O  4 O
CH4 + 2 O2 → CO2 + 2 H2O =
C1H4 + 2 O2 → C1O2 + 2 H2O1
1 C  C
4 H  H
4 O  O

28. Practice: N2 + H2  NH3 Balance the following equations:
H2O2  H2O + O2
N H2  NH3

29. Practice: Balance the following equation: P4 + O2  P4O6
*******GIZMO TIME