1. Matter is anything that has mass and takes up space.
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PROPERTIES OF MATTER
Matter is anything that has mass and takes up space.
Mass of an object is the amount of matter the object contains.
Matter that has a uniform and definite composition is called a substance
Pure substances contain only one kind of matter
Non example: lemonade
Discussion with shoulder buddy on why lemonade is not an example.
Identify the characteristics of matter and substances
Differentiate among the three states of matter
Define physical properties of substances

3. Diagrams of Matter

4. substance ELEMENTS COMPOUNDS
Substances that can be separated into simpler substances only by chemical means.
Made up of 2 or more different elements that are combined chemically in a set ratio
Separating a compound requires energy such as heat or electricity.
Example: salt, baking soda, sugar
The simplest forms of matter that can exist under normal laboratory conditions
Represented by a unique chemical name and chemical symbols
Organized on the periodic table
Examples: oxygen, hydrogen, and carbon

5. PRACTICE: Elements and their symbols
Sulfur , ________
_______________, N
Silicon, _____
_________________, K
Phosphorous, _______
______________, He

6. MIXTURE
Mixture is a combination of two or more pure substances in which each pure substance retains its individual chemical properties
Most everyday matter occurs as a mixture
Composition of mixtures is variable
Substances tend to mix naturally (hard to keep pure)
Can be separated by physical means

7. TYPES OF MIXTURES
Heterogeneous mixture is a mixture that does not blend smoothly throughout and in which the individual substances remain distinct
Ex. Salad dressing
Orange juice with pulp

8. Types of Mixtures
Homogeneous mixture is a mixture that has a constant composition throughout
It always has a single phase
If you cut two pieces, their composition will be the same.
Also referred to as a solution ex. Tea, metal alloy

9. Compare mixtures and substances
Create a Venn Diagram

10. Classify each of the following as homogeneous or heterogeneous mixture
Heterogeneous mixture , homogeneous mixture, or substance
Blood
Chocolate chip ice cream
Brass (a blend of copper and zinc)
Motor oil
Black coffee
Soda
Orange juice
Trail mix
Table salt
Tap water
Carbon dioxide
air
Raisin muffin

11. When would you use distillation?
Separating Mixtures
Distillation: a liquid is boiled to produce a vapor that is then condensed again to a liquid.
When would you use distillation?

12. Separating mixtures
Filtration is a technique that uses porous barrier to separate a solid into a liquid
Crystallization is a separation technique that results in the formation of pure solid particles of a substance from a solution containing the dissolved substance.
Example : rock candy
Produces highly pure solids

13. Separating Mixture
Sublimation is the process during which a solid changes to vapor without melting.
Ex. Dry ice
Chromatography is a technique that separates the components of a mixture dissolved in either a gas or a liquid based on the ability of each component to travel or to be drawn across the surface of a fixed substrate.

14. THINK and REFLECT
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
Sulfur and iron
Sand and salt
Gasoline and water
Aluminum and steel
Copper and silver

15. PROPERTIES OF MATTER
Physical property is a quality or condition of a substance that can be observed or measured without changing the substance’s composition
Examples: Color, solubility, odor, hardness, density, melting point, boiling point

16. PROPERTIES OF MATTER
Extensive properties are dependent on the amount of substance present.
Example: mass, length, and volume, amount of energy
Intensive properties are independent of the amount of substance present.
Example: density, scent, color, ability to conduct electricity and to transfer energy as heat, boiling point, melting point

17. Classify if the property is intensive or extensive property
Color
Smells like vanilla
Length
Boiling point
Ability to attract a magnet
Density
mass

18. PROPERTIES OF MATTER
Chemical Property is the ability or inability of a substance to combine with or change into one or more other substances.
Example: iron forming rust when combined with oxygen.

19. Classify the following as physical or chemical properties
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 -39C
Water has a density of 1.00g/cm3
Blue gray color
brittle
Reacts vigorously with fluorine

20. STATES OF MATTER
All matter that exists naturally on Earth can be classified as solid, liquid, or gas.
The other state of matter is plasma formed in lightening bolts and in stars.

22. Practice Solid, liquid, or gas Nitrogen Diamond Oxygen Mercury
Cooking oil
Clay
Neon
Bromine
Silver
Hydrogen
In which state of matter do the following exist at room temperature?

23. THINK
Fingernail polish remover (mostly acetone) is a liquid at room temperature. Would you describe acetone in the gaseous state as a vapor or a gas?
Justify your answer

24. THINK PAIR SHARE
Compare the properties of solids, liquids, and gases. Make a table that describes shape, volume, compressibility, and structure to share with the class.
ILLUSTRATION AND DIAGRAMMING TIME!!!

25. Physical Change
A change which alters a substance without changing its composition is a physical change. Example: cutting paper, chopping wood, and freezing water.
What is a physical change?

26. What is a chemical change?
A process that involves one or more substances changing into new substances
New substances formed in the reaction have a different composition and different properties from the substances before the reaction
Ability of a substance to undergo a chemical reaction
What is a chemical change?

27. Evidence of a Chemical Reaction
A chemical reaction always produces a change in properties.
Change in temperature
Gas produced
Precipitate formed
Change in color
Change in odor
How do we know a chemical change has taken place?

28. Chemical Change/chemical Reactions
In chemical reactions, the starting substances are called reactants, and the substances formed are called products.
What are the reactants and products?
Iron + Sulfur Iron Sulfide

29. CREATE A T-CHART of Chemical and Physical changes
CREATION TIME
CREATE A T-CHART of Chemical and Physical changes

30. THINK PAIR SHARE
State the difference between a physical change and a chemical change, and list three likely indications that a chemical reaction has occurred. Which indication is most suggestive of a chemical reaction?

31. Classify the following changes as physical or chemical?
Physical or chemical change
Cookies are baked
Water boils
Salt dissolves in water
A firefly emits light
Milk spoils
A metal chair rusts
Bending a piece of wire
Burning coal
Cutting glass

32. How does mass behave in a chemical reaction?
Conservation of Mass
The law of conservation of mass states that mass is neither created or destroyed during a chemical reaction.
Mass of the reactants equals the mass of the products.
How does mass behave in a chemical reaction?

33. Conservation of Mass
When ammonium nitrate (NH4NO3) breaks down explosively, it forms nitrogen gas (N2), oxygen gas (O2), and water (H2O). When 40 grams of ammonium nitrate explode, 14 grams of nitrogen, and 8 grams of oxygen are formed. How many grams of water are formed?
Mass of reactants = mass of products

34. Practice: conservation of mass
In the complete reaction of g of Sodium with g of Chlorine. What mass of sodium chloride is formed?

35. PRACTICE: Conservation of mass
Hydrogen and oxygen react chemically to form water. How much water would be formed if 4.8g of hydrogen reacted with 38.4 grams of oxygen?

36. PRACTICE: conservation of mass
A 12.2 g sample of X reacts with a sample of Y to form 78.9 g of XY. What is the mass of Y that reacted?

37. THINK: Conservation of mass
When powered iron is left exposed to air, it rusts. Explain why the rust weighs more than the original powered iron?

38. Law of Definite Proportions
The law of definite proportions states that a compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample.
The mass of the compound is equal to the sum of the masses that make up the compound.

39. Percent by mass
The percent by mass is the ratio of the mass of each element to the total mass of the compound expressed as a percentage
Percent by mass =
Percent by mass is obtained by dividing the mass of the element by the mass of the compound and then by multiplying this ratio by 100 to express it as a percentage.

40. EXAMPLE:
A 78.0 g sample of an unknown compound contains12.4g of hydrogen. What is the percent by mass of hydrogen in the compound?

41. Example: % by mass
1.0 g of hydrogen reacts completely with 19.0g of fluorine. What is the percent by mass of hydrogen in the compound that is formed?

42. Practice: % by mass
If 3.5 g of element X reacts with 10.5 g of element Y to form the compound XY, what is the percent by mass of element x in the compound? The percent by mass of element Y?

43. Practice: % by mass
Two unknown compounds are tested. Compound 1 contains 15.0g of hydrogen and 120.0g of oxygen. Compound 2 contains 2.0g of hydrogen and 32.0g of oxygen. Are the compounds the same? Explain.

44. Law of multiple Proportions
The law of multiple proportion states that when different compounds are formed by a combination of the same elements, different masses of one element combine with same fixed mass of the other element in a ratio of small whole numbers.
Example: water and hydrogen peroxide
H2O = 2:1
H2O2 = 2:2

45. REVIEW QUESTIONS
Describe a method that could be used to separate each mixture
Iron fillings and sand
Sand and salt
The components of ink
Helium and oxygen gases

46. Review Questions
Which of the following are the same and which are different? Justify your decision.
A substance and a pure substance
A heterogeneous mixture and a solution
A substance and a mixture
A homogeneous mixture and a solution

47. Correct the following statements
An element is a combination of two or more compounds
When a small amount of sugar is completely dissolved in water, a heterogeneous solution is formed.

48. Review Questions
Name the elements contained in the following compounds.
Sodium Chloride (NaCl)
Ammonia (NH3
Ethanol (C2H6O)
Bromine (Br2

49. Review Questions
What is the percent by mass of carbon in 44 g of carbon dioxide?

50. Review Questions
What is the percent by mass of oxygen in 44g of carbon dioxide?

51. Review Questions
A 25.3 g sample of an unknown compound contains 0.8g of oxygen. What is the percent by mass of oxygen in the compound?

52. Review Questions
Magnesium combines with oxygen to form magnesium oxide. If g of magnesium reacts completely with 6.96 g of oxygen, what is the percent by mass of oxygen in magnesium oxide?

53. Review Questions Express the following numbers in scientific notation.
34,500
2665
0.9640
789
75,600

54. Review Questions
Perform the following mathematic problems using the rules for significant figures. =
33 * =
1.34 /0.01 = =

55. Review Question Analyze
Is gas escaping from an opened soft drink an example of a chemical or physical change? Explain

56. Review Questions
List physical properties of eggs before and after they are cooked. Based on your observations, does a physical change or chemical change occur when eggs are cooked? Justify your answer.

57. Review Questions
You might have noticed that while eating ice cream on a hot day, some of the ice cream begins to melt. Is the observed change in the state of ice cream a physical or chemical change? Justify your answer.

58. Review Question Which states of matter are compressible?
Which states of matter are not compressible?
Explain.

59. Review Question
Phosphorous combines with hydrogen to form phosphine. In this reaction, g of phosphorous combines with excess hydrogen to produce g of phosphine. After the reaction, 11.0g of hydrogen remains unreacted. What was the initial mass of hydrogen before reaction? What mass of hydrogen is used in the reaction?

60. Review Questions
If you have 100 particles of hydrogen and 100 particles of oxygen, how many units of water can you form? Will you use all of the particles of both elements? If not, what will remain?
Hint: Chemical formula H2O

61. Review Questions Which of the following is not a chemical change?
Paper being shredded
Steel rusting
Charcoal burning
A newspaper yellowing in the sun

62. Review Questions
Which of these properties could not be used to distinguish between table salt and table salt?
Boiling point
Melting point
Density
color

63. Review Questions
The state of matter characterized by a definite volume and an indefinite shape is
Solid
Mixture
Liquid
Gas

64. Review Question Initial: final Reactant:_________ Product Mixture
Matter
compound

65. Review Questions Words: sentence Elements :_________ Reactant Theory
Compound
Substance