1. Chapter 1 Matter & Change
1.2 Matter & Its Properties

2. Matter Matter- anything that has mass and takes up space.
Mass- measure of the amount of matter
Volume- amount of 3-D space an object occupies
COMPOUND
ELEMENT
ATOM
made from atoms of 2 or more elements
pure substance of only one kind.
smallest unit of an element that maintains the element’s properties

3. Properties
We use properties and characteristics to define and group substances.
Properties can be…. or
Intensive
Extensive
Does not depend on amount of matter present.
Melting & Boiling Points
Depends on amount of matter present.
Volume
Mass

4. Physical vs Chemical
Characteristics that can be observed without Δing the identity of the substance.
Relates to a substance’s ability to undergo Δs that transform it into different substances.
& Boiling Point
Rusting
& Burning

5. Physical Change
Physical Change- change that does not alter the identity of the substance.
Example:
State Change- changes between the 3 states of matter.
*Only a change in distance & interactions btw particles, not chemically altered.

6. Phase Differences
Solid- has definite volume & shape; particles packed in fixed positions.
Liquid- has definite volume & indefinite shape; particles close together but free-flowing.
Gas- has indefinite volume & shape; particles are at great distance from each other.
Plasma-high temperature, ionized phase of matter as found on the sun.

8. Chemical Change
Chemical Change/Reaction- when 1 or more substances are changed into DIFFERENT substances.
Example:
Carbon plus Oxygen yields (forms) Carbon Dioxide
Carbon Oxygen → Carbon Dioxide
Reactants
Products

9. Conservation of Matter & Energy
Even though the substances have changed & formed new substances, the amount of matter stays the same.
When physical and chemical changes occur, energy is involved. (heat/light) It can be absorbed or released but NEVER created. It just changes form.
Conservation of Energy

10. Classification of Matter
Matter can be divided into 2 general categories, mixtures & pure substances
Mixtures
More than 1 substance
Each component retains its own properties
Does NOT chemically combine.
Can be separated using physical properties

11. Separation Techniques
Decanting
Paper
Chromatography
Vaporization
Centrifuge
Filtration

12. Separation: Distillation

14. Two Types of Mixtures Heterogeneous Homogeneous
-not uniform throughout
-unevenly distributed
Homogeneous
-uniform in composition
-same proportions throughout
-often solutions
copper sulfate
malachite, a copper mineral

15. Pure Substances Element or compound
Same composition throughout (Homogeneous)
Fixed composition
Every sample has the exact same characteristic properties
Every sample has the exact same composition
See pg. 18- Lab Chemicals

17. Chapter 1 Matter & Change
1.3 Elements

18. Elemental Composition

19. The Periodic Table Vertical columns Groups or Families Horizontal rows
Periods
Each element in a Group has similar properties.
Properties change in a pattern across the Periods

20. The Periodic Table
Below the table, are two rows called the Lanthanide & Actinide series. They actually belong in the table after the second column, but that would make the table too long and awkward.

21. Metals Conduct electricity & heat Typically solids at room
temperature EXCEPT Hg
Malleable- can be
hammered/
rolled into sheets
Ductile- can be drawn into a wire
Have tensile strength- ability to
resist breaking when pulled
Found in columns 1- 13*

22. Nonmetals Poor conductors, Brittle Br is a liquid at room temperature.
C, P, Se, S & I are solids at room temperature.
Rest are gases at room temperature.
Fewer elements are nonmetals than metals
Found in columns 13* - 17

23. Metalloids/ Semimetals
Separate the metals & nonmetals
Have characteristics of both
Solids at room temp.
Important contribution- as semiconductors; Silicon
Found on the “stairs” between columns 13 – 17

24. Noble Gases Generally unreactive Gases at room temperature.
Found in Group 18

25. Former Names of Elements
L is Latin; G is Greek