1. Unit 2 Lesson #1 Types of Matter

2. Matter Anything that has mass & take up space
Mass = measurement of the
amount of matter an object
contains
Chemistry = the study of matter & the changes that it undergoes

3. Classifying Matter Quantitative – numerical information
how much, how little,
how big, how small
Qualitative –
descriptive information
condition, color, size,
shape, odor, texture

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

5. Pure Substances Every sample has same: Are made of:
1. Characteristic properties
2. Composition
Are made of:
1. one type of atom: element
Ex: iron, gold, oxygen
2. Two or more types of atoms: compound
Ex: salt, sugar, water

6. Which are pure substances?

7. Element
Simplest form of matter that has its own unique set of properties
Can not be separated into simpler substances by physical or chemical means
Each element is made up of a single type of atom
ex. hydrogen, nitrogen, lead

8. Compound
A substance that contains 2 or more elements chemically combined in a fixed proportion (Law of Definite Proportion) Ex.
2. Properties are different than the individual elements
ex. Glucose (sugar)
Glucose – sweet, white solid
Carbon – black, tasteless solid
Oxygen – colorless, tasteless gas
Hydrogen – colorless, tasteless gas

9. Breaking Down Compounds
Physical methods do not work
Recall…
Chemical changes – a change that produces matter with a different composition than the original matter

10. Symbols & Formulas Chemical Symbol
each element is represented by a one- or two-letter symbol H K Au
H2O
C6H12O6
Hydrogen
Potassium
Gold
Water
Glucose
Trends:
1st letter = always capitalized
2nd letter (for an element) = always lowercase
Subscripts = indicate the relative proportions of the elements
in a compound

11. Mixtures 1. A combination of 2 or more types of matter
2. Each component keeps its own identity & properties
3. Components are only physically mixed & can be separated using physical means
Cinnamon & Sugar
Chicken noodle soup
Air

12. Types of Mixtures 1. Heterogeneous mixture -
a mixture in which the substances are not evenly distributed
Oil & vinegar
Salad
Ice tea with ice

13. a mixture or ‘solution’ in which the substances are evenly distributed
2. Homogeneous mixture –
a mixture or ‘solution’ in which the substances are evenly distributed
Water
Kool-Aid
Stainless Steel

14. Phase – used to describe any part of a sample
Phase – used to describe any part of a sample with uniform composition & properties
Homogeneous mixture
Heterogeneous mixture
1 phase
2 phases

15. Practice Examples: Type of Matter graphite pepper sugar (sucrose)
paint
soda
Type of Matter
element
hetero. mixture
compound
solution

16. Separating Mixtures ‘Plays’ on differences in physical properties
1. Filtration – a technique that uses a porous barrier to separate a solid from a liquid
Can you think of any common applications?

17. 2. Distillation – a technique that can be
2. Distillation – a technique that can be used to physically separate most homogeneous mixtures based on differences in the boiling points of the substances involved

18. 3. Chromatography – a technique that is
3. Chromatography – a technique that is used to physically separate the components of a mixture based on the tendency of each component to travel or be drawn across the surface of another material

19. Crystallization
Separation technique that results in the formation of pure solid particles from a solution containing the dissolved substance
As one substance evaporates, the dissolved substance comes out of solution and collects as crystals
Produces highly pure solids
Rocky candy is an example of this

20. Practice Examples: Answers: tea muddy water fog saltwater
Italian salad dressing
Answers:
Solution
Heterogeneous

21. Substances vs. Mixtures

22. Unit 2 Lesson #2 Properties of Matter

23. Properties of Matter
1. Extensive – a property that depends on the amount of matter in a sample
ex. mass, volume, amount of energy
2. Intensive – a property that depends on the type (or identity) of matter in a sample
ex. hardness, density, boiling point, electrical conductivity
Substances – matter that has uniform & unchanging composition have identical intensive properties… Why?
because every sample has the same composition

24. Extensive vs. Intensive
Answers:
intensive
extensive
Examples:
boiling point
volume
mass
density
conductivity

25. 3. Physical Properties – a characteristic that can be observed or measured w/out changing the identity of a substance
ex. color, odor, taste, hardness, density, melting/boiling points,
state of matter
States of Matter – the physical forms in which all matter
exists on Earth

26. Can you identify these 3 states?
Solid
def. shape
& volume
shape independent of container
particles are packed together
Liquid
def. volume
shape depends
on container
particles can
move freely
Gas
indefinite volume &
shape
particles move quickly
& spread apart

27. Chemical Properties Chemical Property
describes the ability of a substance to undergo changes in identity
any of the properties of matter that may only be observed and measured by performing a chemical change or chemical reaction.
Ex. heat of combustion, reactivity with water, pH

28. Properties of Copper

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

30. Unit 2 Lesson #3 Changes in Matter

31. Phase Changes All Physical Changes Evaporation = Liquid -> Gas
Condensation =
Melting =
Freezing =
Sublimation =
Liquid -> Gas
Gas -> Liquid
Solid -> Liquid
Liquid -> Solid
Solid -> Gas
All Physical Changes

32. Physical Changes
Physical Change – a change that occurs in the physical
appearance of a substance, but does not change its identity
Ex. melting, boiling, freezing, evaporating, dissolving, condensing
breaking, splitting, grinding, cutting, crushing

33. Chemical Changes
Chemical Properties – relates to a substance’s ability to
undergo changes that transform it into a different
substance easiest to see when a chemical is reacting
Chemical changes – a change that produces matter with a
different composition than the original matter
ex. burning, rotting, rusting, reacting, cooking, digestion, respiration

34. The process of photosynthesis is a chemical reaction in which light energy, carbon dioxide and water, are transformed to create glucose and oxygen.

35. The photosynthetic chemical reaction can be shown by writing out the element symbols for each compound.
Reactants
substances to the left of the
arrow
‘ingredients’
CO2 and H2O
Products
substances to the right of
the arrow
‘what is made’ or produced
C6H12O6 and O2

36. Did a Chemical Reaction Occur?
1. Ammonium Chloride + Water 2. Sodium Bicarbonate + Calcium Chloride 3. Sodium Bicarbonate + Acetic Acid

37. Recognizing Chemical Changes
How can you tell whether a chemical change
has taken place?
1. Transfer of energy
Energy may be given off
in the form of heat or light
2. Change in color
or odor
Substances may
‘brown’ Indicators

38. 3. Precipitate
A solid that settles
out of a liquid mixture
4. Gas production
Indicated by the formation
of ‘gas bubbles’

39. Did a Chemical Reaction Occur?
1. Ammonium Chloride + Water
NH4Cl(s) + H2O(l) + Heat ----> NH4 + (aq) + Cl -(aq) + H2O(l)
2. Sodium Bicarbonate + Calcium Chloride
NaHCO3(s) + CaCl2(s) ----> CaCO3(s) + NaCl(aq) + HCl (aq)
3. Sodium Bicarbonate + Acetic Acid
NaHCO3(s) + CH3COOH(aq) ----> NaCH3COO-(aq) + CO 2(g) + H2O(l)

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

41. Law of Conservation of Matter
During any chemical reaction, the mass of the products is always equal to the mass of the reactants
+ O2
+ CO2
+ H2O vapor

42. I. Law of Conservation of Mass
Although chemical changes occur, mass is neither created nor destroyed in a chemical reaction
Mass of reactants equals mass of products
massreactants = massproducts
A + B  C

43. Conservation of mass also applies to physical changes…
10g of liquid H2O
10g of ice