1. Matter and Change

2. Matter Matter is anything that has mass and takes up space. Stuff!
There are three basic states of matter:
Solid (s) has definite shape and volume
Liquid (l) shape can change, still has definite volume
Gas (g) no definite shape or volume
Draw a representation of the states of matter here.

3. Phase Changes Matter can change from one state (or “phase” to another)
There are six possible phase changes. Energy is either absorbed or released.
Freeze, sublimate, condensation melt evaporate, deposition .
Deposition

4. Energy
The universe consists of matter and energy. Energy does not have mass or take up space.
Energy is involved when matter changes from one state to another.
Solid + Energy  Liquid “Melting”
Example:
Ice (s) + heat energy  Water (l)

5. Energy Changes
Endothermic- a process which requires, or absorbs energy. (Feels cold in chemical changes)
Ex: H2O (s) + energy  H2O (l)
Ex: Melting, evaporating, boiling
Ex: baking soda reacts with acid
Exothermic- a process which releases or gives off heat. (Feels hot in chemical reactions)
Gasoline burns and releases heat
Exercising muscles produces body heat
Ex: freeze, condensation

7. Classification of Matter
There are two kinds of matter:
Pure Substances (elements and compounds)
Mixtures
Elements- are pure substances
Can’t be broken down by ordinary means
Are found on the Periodic Table
Usually found as single atoms
Some gaseous elements exist as two atoms bonded together (The HOFBrINCl gases) like O2

8. Compounds Compounds- are also pure substances
Can be broken down by chemical reactions only
Are made up of two or more elements chemically combined, or “bonded”
Always have a chemical formula that doesn’t change
The compound has new properties, not the same as the original elements. .

9. Examples of Pure Substances
Elements:
Carbon
Oxygen
Gold
Neon
About 100 more!
(If you are not sure, check the periodic table.)
Compounds:
Water, H2O
Sodium chloride, NaCl
Hydrogen peroxide, H2O2
Methane, CH4
Baking Soda NaHCO3
Glucose C6H12O6
There thousands and thousands of known compounds!
(If it has a chemical formula, it’s a compound.)

10. Compare: Element, compound or mixture?

11. ANSWERS: Element, compound or mixture?

12. Mixtures Mixture- a physical combination of two or more substances.
A mixture can be separated by physical means
The components of the mixture retain (keep) their original properties
The composition can vary (for example. A mixture could be 50% A and 50% B, or it could be
only 30% A and 70% B.)

13. Examples of Mixtures Salt water ( H2O and NaCl)
Sugar water ( H2O and C12H22O11)
Air ( Nitrogen, Oxygen, and trace elements)
Brass ( copper and zinc combine to form an alloy)

14. Mixtures There are two kinds of mixtures. Homogeneous mixtures:
Appear uniform, or the same, throughout
Also known as solutions
Heterogeneous mixtures:
Not uniform in appearance or composition

15. Examples of Mixtures Heterogeneous: Soil Homogeneous:
Sand and water mixture
Sometimes you must look very closely, or even magnify to see the different parts.
Homogeneous:
Air
Salt water
Sugar water
Brass
Solutions

16. Separation of Mixtures
Mixtures can be separated by physical means. Physical means include:
Filtration separates components based on their size
Distillation separates components based on their different boiling points
Chromatography separates based on differences in solubility
Pictures of these on the next few slides…..

17. Filtration
Filtering apple cider

18. Distillation

19. Chromatography

20. Physical and Chemical Changes
Physical Change-
Is usually reversible (can be undone)
All phase changes are physical changes
List the six phase changes here:
(s)  (l) melting and (l)  (s) freezing
(l)  (g) evaporation (s) (g) Sublimation
(g)  (l) Condensation (g)  (s) Deposition
Dissolving is a physical change
Shape changes are physical changes (such as: tearing, bending, etc.)

21. Physical and Chemical Changes
Always produces a new substance
The new substance will have different properties
Evidence of Chemical Change
Color change
Bubbles of gas appear
A new solid forms (a “precipitate)
Temperature change

22. Chemical Changes Chemical Changes are also called chemical reactions.
Chemical reactions always produce a new substance:
Rusting
Burning
Cooking
Digesting
There are many more!

23. Chemical Reactions A + B ------------- > C
reactants yields products
Chemical reactions must obey the Law of Conservation of Mass:
The mass of the products must equal the mass of the reactants.
In other words, matter is neither created nor destroyed
5 grams of A + 5 grams of B yields grams of C

24. Properties A property is something you can observe or measure.
There are two types of properties, physical and chemical.

25. Physical Properties
Physical properties can be measured or observed without changing or destroying the sample
Examples of physical properties
Mass
Color
Density
Melting and boiling points
Ductility (can make wire)
and malleability (flexibility)

26. Physical Properties There are two types of physical properties
Extensive- these depend on the amount of the substance. (Mass, length, and volume)
Intensive- stay the same no matter what the amount of the substance is. (Color, density, conductivity, etc.)

27. Chemical Properties
Chemical Properties- how a substance reacts with other substances
Reacts with water
Reacts with oxygen
Reacts with whatever
Even if it doesn’t react, that is also a chemcial property
These are easy to recognize, always “React”

28. Chemical Properties Corrosive Flammability Oxidizes
Solid Oxidizer Test : measures the potential of a solid substance to increase the burn rate or intensity of a combustible substance
Nonflammable Clothing