<?xml version="1.0"?><Settings><answerBulletFormat>Numeric</answerBulletFormat><answerNowAutoInsert>No</answerNowAutoInsert><answerNowStyle>Explosion</answerNowStyle><answerNowText>Answer Now</answerNowText><chartColors>Use PowerPoint Color Scheme</chartColors><chartType>Horizontal</chartType><correctAnswerIndicator>Checkmark</correctAnswerIndicator><countdownAutoInsert>No</countdownAutoInsert><countdownSeconds>10</countdownSeconds><countdownSound>TicToc.wav</countdownSound><countdownStyle>Box</countdownStyle><gridAutoInsert>No</gridAutoInsert><gridFillStyle>Answered</gridFillStyle><gridFillColor>0,0,0</gridFillColor><gridOpacity>100%</gridOpacity><gridTextStyle>Keypad #</gridTextStyle><inputSource>Response Devices</inputSource><multipleResponseDivisor># of Responses</multipleResponseDivisor><participantsLeaderBoard>5</participantsLeaderBoard><percentageDecimalPlaces>0</percentageDecimalPlaces><responseCounterAutoInsert>No</responseCounterAutoInsert><responseCounterStyle>Oval</responseCounterStyle><responseCounterDisplayValue># of Votes Received</responseCounterDisplayValue><insertObjectUsingColor>Blue</insertObjectUsingColor><showResults>Yes</showResults><teamColors>User Defined</teamColors><teamIdentificationType>None</teamIdentificationType><teamScoringType>Voting pads only</teamScoringType><teamScoringDecimalPlaces>1</teamScoringDecimalPlaces><teamIdentificationItem></teamIdentificationItem><teamsLeaderBoard>5</teamsLeaderBoard><teamName1></teamName1><teamName2></teamName2><teamName3></teamName3><teamName4></teamName4><teamName5></teamName5><teamName6></teamName6><teamName7></teamName7><teamName8></teamName8><teamName9></teamName9><teamName10></teamName10><showControlBar>Slides with Get Feedback Objects</showControlBar><defaultCorrectPointValue>100</defaultCorrectPointValue><defaultIncorrectPointValue>0</defaultIncorrectPointValue><chartColor1>187,224,227</chartColor1><chartColor2>51,51,153</chartColor2><chartColor3>0,153,153</chartColor3><chartColor4>153,204,0</chartColor4><chartColor5>128,128,128</chartColor5><chartColor6>0,0,0</chartColor6><chartColor7>0,102,204</chartColor7><chartColor8>204,204,255</chartColor8><chartColor9>255,0,0</chartColor9><chartColor10>255,255,0</chartColor10><teamColor1>187,224,227</teamColor1><teamColor2>51,51,153</teamColor2><teamColor3>0,153,153</teamColor3><teamColor4>153,204,0</teamColor4><teamColor5>128,128,128</teamColor5><teamColor6>0,0,0</teamColor6><teamColor7>0,102,204</teamColor7><teamColor8>204,204,255</teamColor8><teamColor9>255,0,0</teamColor9><teamColor10>255,255,0</teamColor10><displayAnswerImagesDuringVote>Yes</displayAnswerImagesDuringVote><displayAnswerImagesWithResponses>Yes</displayAnswerImagesWithResponses><displayAnswerTextDuringVote>Yes</displayAnswerTextDuringVote><displayAnswerTextWithResponses>Yes</displayAnswerTextWithResponses><questionSlideID></questionSlideID><controlBarState>Expanded</controlBarState><isGridColorKnownColor>True</isGridColorKnownColor><gridColorName>Yellow</gridColorName><AutoRec></AutoRec><AutoRecTimeIntrvl></AutoRecTimeIntrvl><chartVotesView>Percentage</chartVotesView><chartLabelsColor>0,0,0</chartLabelsColor><isChartLabelColorKnownColor>True</isChartLabelColorKnownColor><chartLabelColorName>Black</chartLabelColorName><chartXAxisLabelType>Full Text</chartXAxisLabelType></Settings> <?xml version="1.0"?><AllQuestions /> <?xml version="1.0"?><AllAnswers /> 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

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.

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.

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.

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?

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

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

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

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

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

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

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

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

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

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

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

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

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.

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.

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

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

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.

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.

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.

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.

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.

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

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.

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?

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

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

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?

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.

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

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

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

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

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

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

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?

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?

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

Practice: conservation of mass In the complete reaction of 22.99 g of Sodium with 35.45 g of Chlorine. What mass of sodium chloride is formed?

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?

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?

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?

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.

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.

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?

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?

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?

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.

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

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

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

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.

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

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

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

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?

Review Questions Magnesium combines with oxygen to form magnesium oxide. If 10.57 g of magnesium reacts completely with 6.96 g of oxygen, what is the percent by mass of oxygen in magnesium oxide?

Review Questions Express the following numbers in scientific notation. 34,500 2665 0.9640 789 75,600 0.002189

Review Questions Perform the following mathematic problems using the rules for significant figures. 2.015 + 3.1 +332.41 = 33 * 1.3021 = 1.34 /0.01 = 3444.12-3.222-122.2 =

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

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.

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.

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

Review Question Phosphorous combines with hydrogen to form phosphine. In this reaction, 108.3 g of phosphorous combines with excess hydrogen to produce 129.9 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?

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

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

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

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

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

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