1. Matter-Properties and Changes
I will distinguish between physical and chemical properties
I will classify matter by composition: element, compound or mixture
I will identify observable characteristics of chemical reactions
I will explain the fundamental law of conservation of mass

2. Properties of Matter
I will identify the characteristics of a substance
I will distinguish between physical and chemical properties
I will differentiate among the physical states of matter

3. Substances Matter that has a uniform and unchanging composition
Aka pure substance
Example 1
Table Salt
Always 100% sodium chloride
Example 2
Water
H2O
NOT AN EXAMPLE
Sea water
Samples vary by location
Amount of salts, water, dissolved substances

5. Physical Properties
A characteristic that can be observed or measured WITHOUT changing the sample’s composition
Density
Color
Odor
Taste
Hardness
Melting point
Boiling point

6. Examples-Physical Properties
Salt (sodium chloride)
Forms solid white crystals at room temperature
Unique salty taste
Oxygen
Colorless
Gas at 25 degrees Celsius
Melting point -218 degrees Celsius
Boiling point -183 degrees Celsius
Density g/cc

7. Extensive Properties Dependent upon the amount of substance present
Examples
Mass
Volume
Length
Weight

8. Intensive Properties
Independent of the amount of the substance present
Examples

9. Chemical Properties
The ability of a substance to combine with or change into one or more other substances
And/Or
The inability of a substance to change into another substance
Example
Iron forms rust when combined with air
Iron + Nitrogen (at room temperature) = no chemical change

10. Observing Properties of Matter
Every substance has its own unique set of physical and chemical properties
May vary depending on conditions of immediate environment
Room temperature, standard pressure, etc.
Example
Copper
Physical Properties
Chemical Properties
Reddish brown
Shiny
Malleable (easily shaped)
Ductile (drawn into wire)
Conducts heat/electricity
Density 8.92 g/cc
Melting Point 1085 ℃
Boiling Point 2570 ℃
Forms green copper carbonate compound when in contact w/ moist air
Forms new substances when combined with nitric and sulfuric acids
Forms a deep blue solution when in contact with ammonia

12. States of matter PHYSICAL PROPERTY!!!!! Solid Liquid Gas Plasma
FUN FACT: (only occurs
naturally on Earth in the
form of lightening bolts!)
PHYSICAL PROPERTY!!!!!

13. Solids A form of matter that has its own definite shape and volume.
Examples
Wood
Iron
Paper
Sugar
Particles are VERY tightly packed
Will only expand SLIGHTLY when heated
Does NOT conform to shape of container
Incompressible
Volume stays the same
Example
Wax (moldable) but volume doesn’t change

14. Liquids Virtually incompressible
Tend to expand when heated
Liquid Particles
NOT rigidly held in place
less closely packed than solids
Are able to move past each other
A form of matter that flows, has constant volume, and takes the shape of its container
Examples
Water
Blood
Mercury

15. Gases
A form of matter that flows to CONFORM to the shape of its container and fills the ENTIRE volume of its container
Examples
Neon
Lighted signs
Methane
Cooking
Air
Mixture of gases
Particles are VERY far apart
EASILY compressed
A substance NATURALLY in the gaseous state at room temperature
RELATED TERMS
Vapor
The gaseous state of a substance that is a SOLID or LIQUID at room temperature
Example
steam

16. Quick Think
Describe the characteristics that identify a sample of matter as being a substance.
Classify each of the following as a physical or chemical property
Iron and oxygen form rust
Iron is more dense than aluminum
Magnesium burns brightly when ignited
Oil and water do not mix
Mercury melts at -39 ℃
Using what you know about the compressibility of gases, explain why the oxygen in a SCUBA tank is compressed.
Create a table that describes the three common states of matter in terms of their shape, volume, and compressibility.

17. Quick Think- Check
The sample of matter must have a uniform and unchanging composition to be a substance.
Properties
Chemical (rust)
Physical (density)
Chemical (burning)
Physical (mixing)
Physical (melting) point)
Particles of gas are spaced apart and are easily compressed. Therefore, it is possible to put a significant volume of oxygen in the tank, which allows the diver to remain under water longer!
Solid
Liquid
Gas
Definite volume
Fills volume of container
Definite shape
Fills container shape
Takes shape of container
Incompressible
Virtually incompressible
Compressible

18. Changes in Matter
I will define physical change and list several common physical changes
I will define chemical change and list several indications that a chemical change has taken place
I will apply the law of conservation of mass to chemical reactions

19. Physical CHANGES Alter a substance WITHOUT changing its composition
Might result in dramatically different appearance (yet leave the composition of the substance unchanged)
Examples
Crunching up a piece of aluminum foil
Cutting a sheet of paper
Breaking a crystal
Phase changes (solid, liquid, gas)

20. Key words of Physical Changes
Bend
Grind
Crumple
Split
Crush

21. Chemical CHANGES
A process that involves one or more substances changing into a NEW substance
New substance
Formed in reaction
Different compositions — than original substance(s)
Different properties — than original substance(s)
Example
Fermentation of juice, sugars, and other ingredients (making wine)
Rusting of iron (a chemical combo of iron and oxygen)

22. Chemical CHANGES Commonly referred to as a chemical reaction Example
Reactants
Starting substances
Products
New substances
Example
Reactants = Iron, Oxygen
Product = rust

23. Key Words of Chemical Changes
Explode
Rust
Oxidize
Corrode
Tarnish
Ferment
Burn
Rot

24. The LAW of Conservation of Mass
Mass is neither created nor destroyed during a chemical reaction
Mass is conserved
Mass of Reactants = Mass of Products

25. Conservation of Mass Problem
Known
Mass mercury (II) oxide = 10.0g
Mass liquid mercury = 9.26g
Unknown
Mass formed oxygen = ? g
Mass Reactants = Mass Products
Mercury (II) oxide = Mercury + Oxygen
10.0g = 9.26g + ?
0.740 g of Oxygen formed

26. Quick Think
Describe the results of a physical change and 3 examples. Repeat with chemical change.
A friend tells you, “because composition does not change during a physical change, the appearance of a substance does not change.” Is your friend correct? Explain WHY?
Solve each of the following
In the complete reaction of g of sodium with g chlorine, what is the mass of the sodium chloride formed?
A 12.2 g sample of X reacts with a sample of Y to form 78.9 g XY. What way the mass of Y that reacted?

27. Quick Think-Check
During a physical change a substance is altered but its composition does not change. EX melting, freezing, boiling, bending, tearing
During a chemical change the composition of a substance IS altered. EX color change, odor, temperatures change, formation of gas or solid from a liquid.
The statement is false. Composition doesn’t change but a change in appearance often accompanies a physical change.
58.44g of sodium chloride
66.7 g of Y

28. Mixtures of Matter I will contrast mixtures and substances
I will classify mixtures as homogeneous or heterogeneous
I will list and describe several techniques used to separate mixtures

29. Mixtures A combination of two or more pure substances
Each pure substance retains its INDIVIDUAL chemical properties
Most everyday matter occurs as mixtures
Substances naturally tend to mix
It is very difficult to keep things pure

30. Mixture Examples Water and Sand Water Sand
Colorless liquid
Sand
Grainy solid
Doesn’t dissolve in water
Easily seen as two substances mixed
Water and Table Salt
Water
Colorless liquid
Table Salt
White crystal solid
Dissolves in water
NOT easy to see both substances individually
But if you boiled the water a white residue remains (salt!)

31. Types of Mixtures Heterogeneous Homogeneous Referred to as SOLUTIONS
Doesn’t blend smoothly throughout
Individual substances remain distinct
Examples
Water mixed with sand
Fresh orange juice
Pulp + Juice
Pizza
Dough + sauce + cheese + toppings
Homogeneous
Constant composition throughout
Always has a single phase
Examples
Water mixed with salt
Cough syrup
lemonade
Referred to as SOLUTIONS

32. Solutions Gas-Gas Gas-Liquid Liquid-Gas Liquid-Liquid Solid-Liquid
EX. Air is primarily a mixture of nitrogen, oxygen, and argon gases
Gas-Liquid
EX. Carbonated beverages contain carbon dioxide gas in solution
Liquid-Gas
Ex. Moist air contains water droplets in air (which is a mixture of gases)
Liquid-Liquid
Ex. Vinegar contains acetic acid in water
Solid-Liquid
Ex. Sweetened powder drink contains sugar and other solid ingredients in water
Solid-Solid
Ex. Steel is an alloy of iron containing carbon

33. Separating Mixtures Filtration Ex through filter paper
A technique that uses a porous barrier to separate a solid from a liquid
Ex through filter paper
Like coffee!
Used to filter heterogeneous mixtures composed of solids and liquids
Distillation
A separation technique that is based on differences in boiling points
A mixture is heated until the substance with the lowest boiling point boils to a vapor that can be condensed into a liquid and collected
Used to filter homogeneous mixtures

34. Separating Mixtures Crystallization Chromatography
Technique results in the formation of pure particles of a substance
From a solution containing dissolved particles
Ex rock candy
From a sugar solution
Often have to add just a little more than what the solution can possibly hold to get the crystals to come out of solution
Produces HIGHLY PURE solids
Chromatography
Technique that separates the components of a mixture (mobile phase) on the basis of the tendency of each to travel or be drawn across another surface (stationary stage)
EX. Soaking up a liquid with paper towel

35. Quick Think How do Mixtures and Substances differ?
Classify each of the following as either heterogeneous or homogeneous mixtures
Orange juice (with pulp)
Tap water
Steel (blend of iron/carbon)
Air
Raisin muffin
Applying Concepts
Describe the separation technique that could be used to separate each of the following mixtures
Two colorless liquids
A non dissolving solid mixed with a liquid
Red and blue marbles of the same size and mass

36. Quick Think-Check Two colorless liquids (distillation)
A non dissolving solid mixed with a liquid (filtration)
Red and blue marbles of the same size and mass (by hand!)
Substance = Matter that has a uniform and unchanging composition
Mixture = A combination of two or more pure substances. Each pure substance retains its INDIVIDUAL chemical properties.
Orange juice (heterogeneous)
Tap water (homogeneous)
Steel (blend of iron/carbon) (homogeneous)
Air (homogeneous)
Raisin muffin (heterogeneous)

37. Elements and Compounds
I will distinguish between elements and compounds
I will describe the organization of elements on the periodic table
I will explain how all compounds obey the laws of definite and multiple proportions

38. Element
A pure substance that cannot be separated into simpler substances by physical or chemical means
Each element has its own unique chemical name and symbol
Earth has 91 naturally occurring elements EX
Copper
Oxygen
gold

39. Periodic Table
1869
Russian Chemist Dmitri Mendeleev
First version –based on masses
Blank spots for undiscovered elements
Organizes the elements into periods (rows) and groups or families (columns)
Elements in the same group have similar chemical and physical properties

41. Compounds
A combination of two or more different elements that are combined chemically
Most substances are compounds Ex
Water
Salt
Sugar
Aspirin
Approximately 10 million known compounds
About new ones developed/discovered per year

42. Dirt, blood,
milk
Lemonade, gasoline, steel
Salt, baking soda, sugar
Oxygen, gold, iron

43. Compounds Can be broken down into simpler substances by chemical means
Often requires external energy to separate
Ex heat or electricity
Ex separate water into hydrogen and oxygen using electrolysis
More stable than the elements that make them up (in general)

44. Compounds
Have DIFFERENT properties than those of the elements that make it up
Ex water = clear liquid, hydrogen/oxygen clear gases
Ex sodium chloride = white, unreactive solid that flavors many foods you eat, sodium = highly reactive element that fizzes and burns when added to water, chlorine = poisonous pale green gas
VIDEO CLIP-ELEMENTS VS COMPOUNDS

45. Law of DEFINITE Proportions
Regardless of the amount, a compound is ALWAYS composed of the same elements in the same proportion by mass
bag sugar = 42.2% carbon, 6.50% hydrogen, 51.30% oxygen
sugar cane = 42.2% carbon, 6.50% hydrogen, 51.30% oxygen
SAME COMPOUND (SUCROSE) !
Conversely, compounds with DIFFERENT mass proportions MUST be DIFFFERENT compounds

46. Percent by Mass (%)
𝒎𝒂𝒔𝒔 𝒐𝒇 𝒆𝒍𝒆𝒎𝒆𝒏𝒕 (𝒑𝒂𝒓𝒕) 𝒎𝒂𝒔𝒔 𝒐𝒇 𝒄𝒐𝒎𝒑𝒐𝒖𝒏𝒅 (𝒘𝒉𝒐𝒍𝒆) X 100 = percent by mass (%)
% by mass demonstration
Practice Problems
A 78.0 g sample of an unknown compound contains 12.4 g of hydrogen. What is the Percent by mass of hydrogen in the compound?
Two unknown compounds are tested. Compound A contains g of hydrogen and g of oxygen. Compound B contains 2.0 g of hydrogen and 32.0 g of oxygen. Are the compounds the same?
All you know about 2 unknown compounds is that they have the same percent by mass of carbon. Is that enough information to be sure the two compounds are the same?

47. Law of MULTIPLE Proportions
Can compounds that are composed of the same elements differ from each other?
YES, different compounds have different mass compositions
When different compounds are formed by a combo of the same elements, different masses of one element with the same relative mass of the other element in a ratio of small whole numbers
Ratios compare the relative amounts of any items or substances