1. Matter: Properties and Changes
Chapter 3

2. What is Matter?
What everything is made of
Matter has mass and volume

3. (Pure) Substance Unchanging chemical composition
Elements and Compounds

4. Physical States of Matter
Properties of the States of Matter

5. Physical Properties
Can be determined without changing the nature of the substance

6. Intensive Property Does NOT depend on the amount
Extensive Property
Depends on the amount

7. Chemical Properties
Describe how matter reacts, or doesn’t react, with other kinds of matter

8. Properties and States of Matter
The properties of a substance can vary depending on its physical state

9. 3-2 Changes in Matter

10. Physical Changes Alters a substance without changing its composition
Also a change in State & dissolving

11. A Phase Change is a Physical Change
From one state to another

12. Chemical Changes
New substance(s) are formed

13. Evidence of Chemical Change

14. The Law of Conservation of Mass
Mass is neither created nor destroyed during a chemical reaction

15. 3-3 Mixtures of Matter

16. Mixtures Two or more substances (not chemically combined)
Each substance retains its individual chemical properties
The proportion can vary
Air, salt water, sugar water, tap water
Can be physically separated

17. Heterogeneous Mixture
Not evenly mixed
Soil, fruit salad

18. Homogeneous Mixture
The substances are distributed the same throughout (All samples will be the same make-up)
Called a solution. See page 81
Sugar or salt water

19. Alloy
A mixture of metals

20. Separating Mixtures
Physical processes based on the physical properties of the substances

21. Filtration
Use of a porous barrier (filter paper) to separate a heterogeneous mixture of a solid and a liquid

22. Decanting
Slowly pouring off a liquid and leaving the solid behind

23. Distillation Separate homogenous mixture by boiling
Different boiling points

24. Crystallization
A solid forms from a solution

25. Sublimation Solid to vapor
One solid sublimates while the other does not

26. Chromatography
Each component (colored ink) travels across the paper at different rates

28. 3-4 Elements and Compounds

30. Element
Can not be separated into smaller components by physical or chemical means
92 in nature
Name, symbol, atomic number
75% of the mass of universe is Hydrogen

31. What is the human body made of?

32. Dmitiri Mendeleev
Invented first periodic table

33. Mendeleev’s Periodic Table
Horizontal rows –
called periods
Vertical columns –
called groups/families
Elements in the same group have similar properties

34. Compounds
Made up of two or more different elements that are chemically combined
Eg. water and sodium chloride
Chemical formula, a specific ratio
Subscript

35. Separating Compounds into components
Usually requires energy (heat, electricity)
Electrolysis

36. Properties of Compounds
Different than the component elements
Eg. Water and salt

37. The Law of Definite Proportions
A chemical compound always contains the same elements in exactly the same proportions (by mass)
Deals with various amounts of the same compound
All compounds of a substance have the same chemical formula

38. Percent by Mass The percent mass of each element in a compound
Percent mass = mass of element x 100
mass of compound
See page 88
Different masses of a compound will have the same percent of each element

39. The Law of Multiple Proportions
When different compounds form from the same elements, they do so in a ratio of small whole numbers
Deals with different compounds made of the same element
Carbon dioxide and carbon monoxide