1. This slide show has been prepared under fair use exemption of the U. S
This slide show has been prepared under fair use exemption of the U.S. Copyright Law and are restricted from further use.

2. Physical &Chemical Properties

3. Physical & Chemical Topics
Physical properties
Chemical properties
Rule of thumb
Matter

4. Physical Property Observable property
Observed without changing the identity of the substance
Substance remains the same
Only appearance changes
Ex. State, color, size, melting point, boiling point, solubility

5. Physical Change Alters a substance without changing its composition.
Physical property changes but substance remains same.
can be “easily” undone
Ex. cut, bend, phase change, solubility,density

6. Examples of Physical Change
Cut
Phase change

7. Chemical Property
Describes how a substance changes into a new substance.
Describes a substance’s ability to change.
Example - flammability (ability to burn)

8. Chemical Change
Changing one substance into a new & different substance.
Process by which substance changes
Starting substance = reactant
Ending substance (new) = product
ex. burning, respiration, digestion, rusting, baking a cake

9. Examples of Chemical Change
Baking bread
Rusting
Respiration
Digestion
Burning

10. Take time to complete the Physical vs. Chemical Worksheets

11. Identify at least 1 physical and chemical property
Salt
Sugar
Baking soda
Corn starch
Rubbing alcohol
Water

12. Matter anything with mass and volume
mass – measure of the amount of matter.
volume – how much space it takes up.

13. Matter - Anything with mass and volume
Examples of matter
Chair
Person
Book
Examples of not matter
Light
Heat

14. Matter
Is air matter?

15. Atom
Smallest unit of an element that maintains the properties of that element.
building block of all matter
fundamental particle
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16. Element made of only one kind of atom
simplest form of matter that can exist under normal conditions
cannot be separated into simpler substances under normal conditions
approx 90 naturally occurring (others artificial)

17. Periodic Table

18. Charlene Marsh
5/23/2019
Compound
Compound - substance made from the atoms of two or more elements chemically bonded.
Molecules – smallest unit of a compound
Topics
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19. Pure Substances elements and compounds made of only one kind of matter
same throughout
same everywhere
in world
has a formula/symbol
ex. sugar (C12H22O11),
copper (Cu)

20. On notes page answer the question What are the two types of pure substances? Then identify the 8 substances.

21. Which type of pure substance?
Sodium (Na)
Water (H2O)
Iron (Fe)
Baking Soda (NaHCO3)
Carbon dioxide (CO2)
Nitrogen (N2)
Oxygen (O2)
Hydrochloric acid (HCl)

22. Classification of Matter

23. Mixtures variable composition (any proportion)
physical blend of two or more pure substances
variable composition (any proportion)
matter that can be physically separated
Parts not chemically bonded.
Can vary with location
No formula
ex. air, forest, beef stew, gold jewelry

24. Classification of Matter

25. Mixture
Stop and complete Substance vs. Mixture worksheet PSc.2.1 problems 1-20

26. Heterogeneous Mixture
heterogeneous – not uniform composition
two or more groups
ex. tossed salad, milk straight from the cow

27. Homogenous Mixture uniform composition evenly distributed
ex. salt water, Kool-Aide, gold jewelry.

28. Classification of Matter

29. Colloid mixture between homogeneous and heterogeneous.
particles do not settle
appears cloudy
scatters light
Tyndall effect

30. Tyndall Effect

31. Classification of Matter
Take 5 minutes to complete: Homogeneous vs. Heterogeneous Worksheet PSc.2.1 problems 21-35

32. Solubility
The amount of a substance that dissolves in a given quantity of a solvent at a given temperature to produce a saturated solution is its solubility.
Unit = grams solute / 100 g solvent

33. NCDPI Reference tables for Physical Science (adopted 2000) Solubility Curve
Once you determine that a substance will dissolve consult the solubility curve to determine how much of it will dissolve at a given temperature.
For example after adding 37 grams of NaCl to 100 ml of tap water no more will dissolve. Any additional salt settles to the bottom.
This is no longer on the reference tables. It will be included with a question as needed.

34. solidifying as dissolving.
Saturated
Same amount of solid
solidifying as dissolving.
Saturated solution – contains the maximum amount of solute for a given amount of solvent at constant temperature.
This is “ON THE LINE”.

35. Saturation
Unsaturated – a solution that contains less solute than a saturated solution. (Less than it could hold.)
Under the line
Supersaturated – a solution which contains more solute than it should be able to hold at a given temperature.
This is ABOVE the line
this is how rock candy is made
“extra” is all the solute dissolved greater than that which is expected for a saturated solution.

36. Practice problem using Solubility Curve
How much KNO3, potassium nitrate, will dissolve in 100 grams of water saturated at 70oC?

37. Practice problem using Solubility Curve
At 70oC 135g of KNO3 would dissolve.

38. Rate of Solution How fast a solute will dissolve depends on:
Size of solute particles
Since dissolving occurs on the surface, increasing surface area (power) allows more solvent to reach more solute and speeds dissolving.
Agitation/stirring
Moves solute away from solid so solvent can reach more solute.
Temperature
For solids a warmer solvent moves faster and farther apart thus increases rate of dissolving.
However, for gas solutes, as temperature of solvent increases the solubility of a gas decreases.

39. Solubility Curve problems
At this time stop and complete the solubility curve problems.

40. Reference page
Arbor Scientific. (2002). Retrieved July 22, 2003 from
Petrucci, R., Harwood, W., Herring, G. (2000). Retrieved July 22, 2003 from General Chemistry: Principles and Modern Applications Web site:
PowerMasters Motorsports Academy, curriculum samples, chemistry basics. ( ). Retrieved July 22, 2003 from Web site:
University of Cambridge, Department of Engineering, Materials Group. (2002). Retrieved July 22, 2003 from Web site: