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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

2. Particle Theory of Matter
Matter is anything that has mass and takes up space.
Chemistry is the study of matter and the changes it undergoes.
1. Matter is made up of tiny particles (Atoms & Molecules)
2. Particles of Matter are in constant motion.
3. Particles of Matter are held together by very strong electric forces
4. There are empty spaces between the particles of matter that are very large compared to the particles themselves.
5. Each substance has unique particles that are different from the particles of other substances.

3. Kinetic Molecular Theory
Gases are highly energetic. They move quickly and the particles are far apart.
Liquids are less energetic. The particles slide past each other and are closer together.
Solids have the least amount of energy. They are bunched tightly together and vibrate in place.

4. 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.

6. 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?

7. 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

9. substance COMPOUNDS ELEMENTS
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

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

11. Most everyday matter occurs as a 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

12. 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

13. It always has a single phase
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
Types of Mixtures

14. 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
Classify each of the following as homogeneous or heterogeneous mixture

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

16. Produces highly pure solids
Separating mixtures
Filtration is a technique that uses porous barrier to separate a solid from 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

17. 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.
Separating Mixture

18. A non-dissolving solid mixed with a liquid
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

19. 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
PROPERTIES OF MATTER

20. Physical Properties
A property is a characteristic or description of a substance that may help identify it.
Physical properties are observed using the senses (sight, smell, taste, touch and hearing) and measuring devices.
Physical properties can be determined without destroying the substance.

21. Quantitative vs. Qualitative Properties
Quantitative Properties
Qualitative Properties
Some of the properties scientists use to describe substances can be measured.
Quantitative properties are properties that can be associated with numbers.
A way to remember: Quantitative comes from the word quantity.
Many of the properties scientists use to describe substances cannot be measured.
Qualitative properties are properties that can be associated with words.
A way to remember: Qualitative comes from the word quality.

22. 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
PROPERTIES OF MATTER

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

24. Example: iron forming rust when combined with oxygen.
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.

25. Chemical Properties
A chemical property describes the behavior of a substance as it becomes a new substance.
Chemical Property
Description
Reaction of an acid with a base
Acids and bases will combine in a neutralization reaction.
e.g. Vinegar reacts with baking soda to produce carbon dioxide gas.

26. Chemical Properties
A chemical property describes the behavior of a substance as it becomes a new substance.
Chemical Property
Description
Flammability
How easily a substance will burn if ignited.
e.g. Gasoline burns easily if ignited.

27. Chemical Properties
A chemical property describes the behavior of a substance as it becomes a new substance.
Chemical Property
Description
Bleaching ability
The ability to break down pigment.
e.g. Hydrogen peroxide breaks down the pigment (color) in hair.

28. Chemical Properties
A chemical property describes the behavior of a substance as it becomes a new substance.
Chemical Property
Description
Corrosion
The ability of a chemical to corrode or rust.
e.g. Discarded batteries in landfill sites break down readily when they come in contact with groundwater.

29. 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

30. Physical and Chemical Changes
We experience physical and chemical changes everyday when we cook an egg, burn gasoline in the car, freeze water to make ice cubes or mix vinegar and oil to make salad dressing.

31. What is a 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?

32. Physical Change
In a physical change, the substance involved remains the same.
Most physical changes are easy to reverse.
Physical Change
Description
Changes of State
e.g. Melting, Freezing, Boiling

33. Physical Change Physical Change Description
Dissolving solids into liquids
e.g. dissolving salt (solute) into water (solvent), making Kool-Aid

34. 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?

35. Chemical Change
In a chemical change, the original substance is changed into one or more new substances.
The new substances have different properties from the original substance.
Most chemical changes are difficult to reverse.

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

37. Clues that a Chemical Change has occurred:
A new color appears.

38. Clues that a Chemical Change has occurred:
Heat or light is produced or absorbed.

39. Clues that a Chemical Change has occurred:
A solid material (a precipitate) forms in a liquid.

40. Clues that a Chemical Change has occurred:
Bubbles of gas are formed.

41. 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

42. 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
Classify the following changes as physical or chemical?

43. 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?

44. Mass of reactants = mass of products
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?
Conservation of Mass
Mass of reactants = mass of products

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

46. 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?

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

48. 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?

49. 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.

50. 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= 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 𝑥100
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.

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

52. 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?

53. 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?

54. 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.

55. 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

56. 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

57. 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

58. 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.

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

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

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

62. 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?

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

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

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

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

67. 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.

68. 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.

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

70. 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?

71. 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

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

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

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

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

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