1. CRCT Matter Review

2. Distinguish between atoms and molecules
atom (page 313)
smallest unit of an element that maintains the properties of the element.

3. Two parts
nucleus (page 316) – tiny, extremely dense, positively charged, center of the atom
contains most of mass
electron cloud (page 317) – regions where electrons are likely to be found
contains most of volume
The atom is mostly empty space.

4. Particle
Symbol
Location
Charge
proton p+
nucleus 1+
neutron no
none (0)
electron e-
electron cloud 1-

5. Number of protons = number of electrons Identifies the element.
atomic number
Number of protons = number of electrons
Identifies the element.
Locate on the periodic table.
How many protons does carbon have?
How many electrons does carbon have?
What element has 20 protons?
What element has 16 electrons?

6. Answers How many protons does carbon have? (6)
How many electrons does carbon have? (6)
What element has 20 protons? (calcium)
What element has 16 electrons? (sulfur)

7. molecule
Two or more atoms bonded together

8. Describe the difference between pure substances (elements & compounds) and mixtures.

9. Substances cannot be broken down by physical changes.
Summarize
Substances cannot be broken down by physical changes.
Elements cannot be broken down (by physical or chemical means).
Compounds can be broken down by chemical reactions.
Mixtures (combination of two or more substances that are not chemically combined). They can be separated by physical changes.

10. What is this?
Find
an atom
a molecule
a compound

11. Can it be separated by physical means?
yes no
substance
mixture
Can it be separated by chemical means?
Is it uniform? no
yes no
yes
compound
element
homogeneous
heterogeneous
Aka: solution
Examples: colloid
suspension
Examples:
Examples:
Examples: alloy,

12. Describe the movement of particles in solids, liquids, gases and plasmas.

14. A change in state is a physical change. (Pages 74-79)
solid
melting
deposition
sublimation
freezing
condensation
liquid
gas
evaporation, boiling

15. Heating Curve warming the gas boiling (liquid & gas)
boiling point condensation point
boiling (liquid & gas)
melting point/ freezing point
warming the liquid
Temperature
melting (solid & liquid)
warming the solid
Time heating

16. plasma Add enough energy so some electrons are removed (free).
Positive atom fragments (ions) remain.

17. Distinguish between physical and chemical properties of matter
Physical properties can be observed directly without changing the identity of the matter.
Chemical properties cannot be observed directly without changing the identity of the matter.

18. Physical properties state of matter melting point boiling point
conductor - insulator
soluble – insoluble
ductile
malleable
brittle
texture
hardness
density
temperature

19. Chemical Properties reactivity Will it rust or tarnish?
Flammable or nonflammable? (Inflammable is not the antonym)
Combustible or incombustible?

20. Distinguish between physical and chemical changes in matter
Physical changes: identity of the matter does NOT change.
Chemical changes: identity of the matter changes.

21. physical changes
changes in state (melting, freezing, boiling, evaporation, condensation, sublimation, deposition)
cutting, chopping
crushing
sanding smooth
dissolving
clay changing shape

22. chemical change aka: chemical reaction burning/combustion
rusting/tarnishing
one substance  another substance

23. evidence of a chemical change
gas formation
solid (precipitate) formation
color change

24. Recognize that there are more than 100 elements and some have similar properties as shown on the Periodic Table of Elements.

25. PERIODIC TABLE DATA SHEET
 group, family (similar characteristics)
 period, series
Group number
&
name 1
alkali 2
alkaline
earth
3-12 transition element 13 14 15 16
17 halogen
18 noble gases
colorless odorless gases
Physical Characteristics
metals
nonmetals
metalloids
dull, brittle,
insulators
luster, conductors (heat & electricity),
ductile, malleable
metalloids
Si = semiconductor

26. Law of Conservation of Matter
Matter cannot be created or destroyed in an ordinary chemical or physical change.
mass at beginning = mass at the end.