1. Chapter 2
Matter

2. Overview Learn about the composition of matter
Learn the difference between elements and compounds
Distinguish between physical and chemical properties and changes
Distinguish between mixtures and pure substances
Learn 2 methods of separating mixtures

3. Did you ever wonder?... How do plants grow & why are they green?
Why is the sun hot?
Why does a hot dog get hot in a microwave?
Why does wood burn and rocks do not?
How does soap work?
Why does pop fizz?
What’s happening when iron rusts?
Why doesn’t aluminum foil rust?
How does a hair permanent work?

4. The Particulate Nature of Matter
Matter: the “stuff” the universe is composed of
Has mass and occupies space
Comes in many forms: the stars, your chair, brain tissue
Composed of tiny particles called atoms
Scanning tunneling microscope produces images of atoms
Can’t see with naked eye, similar to looking at beach from far away; can only see sand particles when you get close

5. Elements and Compounds
Atoms: all matter is composed of these tiny particles
Over 100 different atoms
Similar to words, all made from 26 different letters
All matter made from about 100 different atoms
Compounds: substances made by bonding atoms together in specific ways
Contain 2 or more different types of atoms
Same throughout
Molecule: made up of atoms that are “stuck” together

6. Atom Combinations

7. Elements
Some atoms can combine with like atoms to form molecules: H2 & O2
Carbon bonds forming large groups
Elements: substances that contain only one type of atom
Compound: always contains atoms of different elements (water = H2O)

8. Top Ten

9. Figure 2.5: The three forms of the element carbon: Diamond.

10. Figure 2.5: The three forms of the element carbon: Graphite.

11. Figure 2.5: The three forms of the element carbon: Buckminsterfullerene.

12. The States of Matter

13. Figure 2. 7: The three states of water: Solid
Figure 2.7: The three states of water: Solid. Solids: Rigid; have a fixed shape and volume

14. Figure 2.7: The three states of water: Liquid Liquid: has a definite volume but takes the shape of its container

15. Figure 2. 7: The three states of water: Gas
Figure 2.7: The three states of water: Gas. Gas: has no fixed volume or shape; uniformly fills any container

16. Physical and Chemical Properties and Changes
Physical Properties: Odor, color, volume, state, density, melting point, and boiling point
Chemical properties: refer to a substances ability to form new substances
Examples: wood burning, rusting of steel, digestion of food, growth of grass
Given substance changes to a fundamentally different substance or substances

17. Chemical vs. Physical change in water
Physical changes
solid → liquid → gas
Change of state: H2O molecules still present
Chemical change = electrolysis
water changed into different substances (water decomposes to hydrogen & oxygen)

18. Electrolysis, the decomposition of water by an electric current, is a chemical process.

19. Physical & Chemical Changes
Physical change involves a change in one or more physical properties, but no change in fundamental components of substance. Most common are changes in state.
Chemical change involves a change in the fundamental components of the substance. Chemical changes are called reactions.

20. Mixtures and Pure Substances
Mixture: something that has variable composition
Examples: soda, coffee, tap water, air
Composition of mixtures varies, but composition of compounds is always the same
Composition depends on how much of each component is used when mixture is formed
Can be separated into pure substances: elements and/or compounds

21. The composition of air.

22. Chart examining each substance of air.

23. Mixtures: Alloys Alloys: mixtures of metals
Many gold alloys: mixture of gold, copper, and silver
They are not compounds! (like water)
Composition varies

24. Figure 2.10: Twenty-four-karat gold is an element Eighteen-karat gold is an alloy Fourteen-karat gold is an alloy.

25. Homogeneous and Heterogeneous
Homogeneous mixture is the same throughout, & also called a solution
Examples: salt water, air, brass (mixture of copper and zinc)
Heterogeneous mixture contains regions that have different properties from other regions
Examples: sand/water mixture, rocky road ice cream, chocolate chip cookie dough

26. Representation of H2O molecules.

27. Distillation: Separation Process
Boil water (or other liquid)
Vaporizes (turns into gas = steam)
Condense (cool steam in tube) – turns back to liquid
Minerals are left behind
Pure water collected
Physical change

28. The solution is boiled and steam is driven off.

29. Salt remains after all water is boiled off.

30. No chemical change occurs when salt water is distilled.

31. Filtration: Separation Process
Pour mixture onto a mesh, such as filter paper
Liquid passes through, solid is left behind on filter paper

32. Filtration separates a liquid from a solid.

33. Separation of a sand-saltwater mixture.

34. Pure Substances Pure substances are either elements or compounds
Always have same chemical and physical properties

35. The organization of matter.

36. Setup to boil water.