1. The study of matter and the changes it undergoes
Chemistry
The study of matter and the changes it undergoes

2. UNIT 1: Properties Of Matter
Objectives:
Learn the states of matter and be able to describe them
Be able to classify matter
Investigate and describe the properties of matter.

3. Chemistry is...
The study of matter
C. Johannesson

4. Matter VS. Non-Matter Matter Non-Matter paper sound Heat electricity
water
electricity
Apples
Matter
paper
Heat
sound

5. Matter VS. Non-Matter Matter Non-Matter apples heat water electricity
sound
electricity
heat
Matter
paper
water
apples

6. Matter VS. Non-Matter
Describe the characteristics of the items you classified as matter
what do they have in common?
How are they different than the items you classified as non-matter?

7. Takes up space (volume)
Chemistry
Matter
Takes up space (volume)
Made up of atoms
Or molecules
Has Mass
C. Johannesson

8. Use the Kinetic Molecular Theory to describe
Four States of Matter
Energy
Phase Transition
Use the Kinetic Molecular Theory to describe
Particle Motion
C. Johannesson

9. Kinetic Molecular Theory
All matter is made up of particles
Particles of matter are always in motion.
The kinetic energy (speed) of these particles increases as temperature increases.
C. Johannesson

10. Four States of Matter
Solid
Liquid
Gas
Plasma

11. Solids Very low KE Fixed shape Fixed volume
Vibrate but do not move around
particles are tightly packed, usually in a regular pattern.
Fixed shape
Fixed volume

12. Liquids low KE Variable shape Fixed volume.
Particles vibrate & slide past each other but are still close together
ability to flow and be poured and to spread when a liquid is spilled.
Variable shape
Fixed volume.

13. Gases High KE Variable shape Variable volume
Particles vibrate, rotate, and move throughout the container
Variable shape
Variable volume

14. Plasma Very High KE Gas-like Variable shape Variable volume
Particles vibrate, rotate, and move around
Particles collide with enough energy to break into charged particles
Gas-like
Variable shape
Variable volume
Stars, fluorescent light bulbs, cathode ray tubes

15. Phase Transition
The change of a substance from one state of matter to another by the addition or removal of heat energy.

17. In Relation to the Kinetic Molecular Theory

18. At the phase transition point (for instance, boiling point) the two phases of a substance, liquid and vapor, have identical energies and are equally likely to exist.

19. Energy Changes in Matter
when any change occurs, energy is always involved
energy can be in different forms (light, heat, etc.)
energy is never destroyed or created (law of conservation of energy)

20. Energy Changes in Matter
Exothermic change- change that gives off energy (feels warm on outside)
Endothermic Change- change that uses up energy (feels cold on outside)

21. Classification of Matter
Objectives:
Differentiate between
pure substances
elements
compounds
mixtures
Heterogeneous
homogeneous mixtures.

22. Pure Substances Mixtures Classification Of Matter Elements Compounds
Page in Modern Cheistry
Pure Substances
Elements
Compounds
Mixtures
Heterogeneous
Homogeneous

23. Can it be physically separated?
MATTER
Can it be physically separated?
yes no
MIXTURE
PURE SUBSTANCE
Can it be chemically decomposed? no
yes
Is the composition uniform? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

24. Use your matter flowchart to classify these examples
element
hetero. mixture
compound
solution
Examples:
graphite
pepper
sugar(sucrose)
paint
soda

25. Pure Substances Element composed of one type of atom
EX: copper wire, aluminum foil
C. Johannesson

26. Pure Substances Compound
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)

27. Law of Definite Composition
Pure Substances
Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.

28. Two different compounds, each has a definite composition.
Pure Substances
For example…
Two different compounds, each has a definite composition.

29. Mixtures Variable combination of 2 or more pure substances.
Heterogeneous
Homogeneous

30. Mixtures particles don’t settle EX: rubbing alcohol Solution
homogeneous
very small particles
no Tyndall effect
Tyndall Effect
particles don’t settle
EX: rubbing alcohol

31. Mixtures Colloid heterogeneous medium-sized particles Tyndall effect
particles don’t settle
EX: milk

32. Mixtures Suspension heterogeneous large particles Tyndall effect
particles settle
EX: fresh-squeezed lemonade

33. Mixtures Examples: mayonnaise colloid muddy water suspension fog
saltwater
Italian salad dressing
colloid
suspension
solution

34. Mixtures are separated by differences in their physical property
Separating Mixtures
Mixtures are separated by differences in their physical property
Technique
Separates by
Filtration
Phase of matter
Decanting
Density
Distillation
Boiling point
Magnetism
Metals / non-metals

36. Properties of Matter Objectives:
identify and explain physical properties
density, melting point, boiling point, conductivity, and malleability
chemical properties
ability to form new substance
Distinguish between chemical and physical changes.

37. Properties of Matter
Physical
Intensive
Extensive
Chemical

38. Extensive vs. Intensive
Extensive Property
depends on the amount of matter present
Intensive Property
depends on the identity of substance, not the amount
C. Johannesson

39. Extensive vs. Intensive
Examples:
boiling point
volume
mass
density
conductivity

40. Physical vs. Chemical Physical Property Chemical Property
can be observed without changing the identity of the substance
Chemical Property
describes the ability of a substance to undergo changes in identity

41. Physical vs. Chemical physical chemical Examples: melting point
flammable
density
magnetic
tarnishes in air

42. Physical vs. Chemical Physical Change Chemical Change
changes the form of a substance without changing its identity
properties remain the same
Chemical Change
changes the identity of a substance
products have different properties

43. Physical Changes in Matter
change in a substance that doesn’t change the identity of the substance
Ex. grinding, cutting, melting, boiling
Can be reversible, or irreversible
Includes all changes of state (physical
changes of a substance from one state to another)

44. Chemical Changes in Matter
a change in which a substance is converted into a different substance
same as chemical reaction
doesn’t change the amount of matter present
reactants- substances that react
products- substances that form
Arrow points from the reactants to the new products

45. Physical vs. Chemical Signs of a Chemical Change (Reaction)
change in color or odor
formation of a gas (bubbling or fizzing)
formation of a precipitate (solid)
change in light or heat

46. Conservation of Mass
During any chemical reaction, the mass of the products is always equal to the mass of the reactants.
All the mass can be accounted for:
Burning of wood results in products that appear to have less mass as ashes; where is the rest?
Law of conservation of mass

47. In the pictures how do you know right away that a chemical change took place?
reactants
= product
43.43 g Original mass
= g Final mass

48. Physical vs. Chemical Examples: chemical physical rusting iron
dissolving in water
burning a log
melting ice
grinding spices
chemical
physical

49. The changes it undergoes
Chemistry
Chemistry
The study of matter
Its composition
Its structure
Its properties
The changes it undergoes
C. Johannesson