1. Classification of Matter
I. Composition of Matter
Matter Flowchart
Pure Substances
Mixtures

2. Can it be separated by physical means?
A. Matter Flowchart
MATTER
yes no
Can it be separated by physical means?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be decomposed by chemical means? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element

3. B. Pure Substances Element matter composed of identical atoms
EX: copper

4. Periodic Table of Elements

5. B. Pure Substances Compound/ Molecule
matter composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
chemically combined
EX: salt (NaCl) or water (H2O)

6. Chemical Formulas
Shows how many atoms of each element are in the substance.
Example: C16H10N2O2 is a blue dye.
The number of atoms of each element is written after the element’s symbol as a subscript.
If only one atom is present, no subscript is needed.

7. Chemical Formulas You try. C12H22O11
How many atoms of each element are in this formula?
C is for carbon.
H is for hydrogen.
O is for oxygen.

8. C. Mixtures Variable combination of 2 or more pure substances.
Homogeneous Mixture (Solution)
even distribution of components
very small particles
particles never settle
EX: saline solution

9. C. Mixtures Heterogeneous Mixture uneven distribution of components
Can physically separate
Colloids and Suspensions
EX: granite

10. C. Mixtures Colloid medium-sized particles
Tyndall effect - particles scatter light (looks cloudy)
particles never settle
EX: milk

11. C. Mixtures Suspension large particles particles scatter light
particles will settle (needs to be shaken)
EX: fresh-squeezed lemonade

12. Law of Conservation of Mass and Energy
Mass cannot be created nor destroyed
Energy cannot be created nor destroyed; it can be transformed or transferred to other forms of energy.

13. MATTER Solids, Liquids, & Gases I. States of Matter
Kinetic Molecular Theory
Four States of Matter
Thermal Expansion

14. A. Kinetic Molecular Theory
KMT
Tiny, constantly moving particles make up all matter.
The kinetic energy (motion) of these particles increases as temperature increases.

15. B. Four States of Matter Solids
low KE - particles vibrate but can’t move around
definite shape & volume
crystalline - repeating geometric pattern
amorphous - no pattern (e.g. glass, wax)

16. B. Four States of Matter Liquids
higher KE - particles can move around but are still close together
indefinite shape
definite volume

17. B. Four States of Matter Gases
high KE - particles can separate and move throughout container
indefinite shape & volume

18. B. Four States of Matter Plasma
very high KE - particles collide with enough energy to break into charged particles (+/-)
gas-like, indefinite shape & volume
stars, fluorescent light bulbs, TV tubes

19. C. Thermal Expansion
Most matter expands when heated & contracts when cooled.
 Temp causes  KE. Particles collide with more force & spread out.
EX: thermostats (bimetallic strip)

20. II. Changes in State Phase Changes Heating Curves
MATTER
Solids, Liquids, & Gases
II. Changes in State
Phase Changes
Heating Curves

21. melting point = freezing point
A. Phase Changes
Melting
solid to liquid
Freezing
liquid to solid
melting point = freezing point

22. A. Phase Changes Vaporization (boiling)
liquid to gas at the boiling point
Evaporation
liquid to gas below the boiling point
Condensation
gas to liquid

23. A. Phase Changes Sublimation solid to gas
EX: dry ice, freeze drying, iodine

24. A. Phase Changes

25. B. Heating Curves Kinetic Energy motion of particles
related to temperature
Potential Energy
space between particles
related to phase changes

26. B. Heating Curves Gas - KE  Boiling - PE  Liquid - KE 
Melting - PE 
Solid - KE 

27. B. Heating Curves Heat of Fusion
energy required to change from solid to liquid
some attractive forces are broken

28. B. Heating Curves HEATING CURVE Heat of Vaporization
energy required to change from liquid to gas
all attractive forces are broken
EX: steam burns, sweating, and… the drinking bird
HEATING CURVE

29. Classification of Matter
II. Describing Matter
Physical Property
Physical Change
Chemical Change
Chemical Property

30. A. Physical Property
A characteristic of a substance that can be observed without changing its identity.
can be used to separate mixtures
EX: magnetism, density

31. B. Physical Change
A change in the form of a substance without changing its identity.
properties remain the same
reversible
can be used to separate mixtures
EX: dissolving, grinding

32. C. Chemical Change A change in the identity of a substance.
properties change
irreversible
Signs: color change, formation of a gas/solid, release of light/heat
EX: burning, rusting

33. D. Chemical Property
A characteristic that indicates whether a substance can undergo a specific chemical change.
EX: flammability, reactivity