Chemistry deals with the properties of matter. Matter is anything that has mass and takes up space (volume) This and that fjalkdfja djfalkjdfa

Chemistry is the study of matter and the changes that it undergoes Chemistry and Matter Chemistry is the study of matter and the changes that it undergoes You depend on Chemicals everyday for: Cooking, Film, Laundry, Asprin

Any substance with a definite composition What is a Chemical? Any substance with a definite composition

Physical states of matter There are three states of matter Solids Liquids Gasses

States of Matter States of matter can be changed by a change in temperature or pressure Solid – definite shape and volume, particles slightly vibrate, incompressible, dense Liquid – no definite shape, definite volume, particles flow freely, slightly compressible, less dense Gas – no definite shape or volume, particles are not confined and move continuously, very compressible, least dense *vapor – gaseous state of a substance that is solid or liquid at room temp

Chemical reactions describe how matter behave. Chemical reaction: The process by which elements and/or compounds interact with one another to form new substances

Chemical reaction ------ Carbon dioxide + water + energy ----Sugar + oxygen Reactants Products

Exothermic reaction Rxn. in which energy is released Potassium permanganate & glycerol Potassium permanganate KMnO4, Glycerol C3H5(OH)3,

Endothermic reaction A reaction in which energy is absorbed barium hydroxide solid with ammonium chloride cause water to freeze.

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Matter Anything that has a mass and volume

Weight is the effect of Earth’s gravity on a mass Mass and Weight Weight is the effect of Earth’s gravity on a mass Mass - same no matter where an object is located Weight changes as the amount of gravity changes. 4

Units of Measurement SI units are metric system which uses seven base units The 4 you need to know now are meter, kilogram, second, Kelvin SI units range from very small to large measurements. Area , volume, pressure, weight are derived units - which means they are a combination of base units

Conversion for SI units KATHY HOW DOES MY DOG CATCH MICE K = Kilo H = Hecta D = Deca M = meter/liter/gram d = deci c = centi m = milli These are the common ones T = Tera G = Giga M = Mega K = Kilo ~ m = milli m = micro n = nano But we went both higher and lower ;~)

Jordan’s mnemonic device Tell Granny Melisa Kites Hovering Don’t make due ‘cause my mom’s napping

Conversion 1 foot = 12 inches 1 Km = 100 Hm 3 feet = 1 yard 1Km = 10 Dm 1 Km = 100 Hm 1 Km = 1000 m 1 m = 100 cm 1 m = 1000 mm 1 cm = 10 mm 1 foot = 12 inches 3 feet = 1 yard 1 inch = 2.54 cm 5280 feet = 1 mile

Making measurements Length – the straight line distance between any two points Mass – measure of the quantity of matter in an object Volume – a measure of space such as the capacity of a container Weight – the force with which gravity pulls on a quantity of matter

Physical Properties Can be observed without changing the composition of a substance Ex – size, shape, color, mass, volume, length, density, boiling point, melting point, freezing point, state of matter, hardness, smell, taste, Cutting, crushing, bending, dissolving

Chemical Properties Totally changes the identity of the substance; Only observed through chemical reactions Ex. Corrosive, combustible, ability to react with a substance, inability to react, explode, rust, oxidize, tarnish, ferment, rot, cook Indicators of a chemical rxn: temperature change, odor change, color change, formation of a precipitate, gas produced

What is the nature of matter Element – cannot be broken down into a simpler substance (ex: oxygen, hydrogen) Atom – smallest particle that has property of an element 21

Compound – made of more than one element (ex: water;h2o) Molecule – a neutral group of atoms held together by covalent bonds

Allotrope One of a number of different forms of an element Ex. O2 and O3; graphite, diamond, Buckyball, Bucky tube

Compounds Substance composed of two or more different elements Covalent vs. Ionic Acid and Base Organic or inorganic

Covalent Vs. Ionic Covalent compounds share electrons EX. Water, sugar and oxygen Ionic compound – compounds that has an electric charge. Ex. Table salt

Acid Vs. Base Acid: pH of less than 7 Base: pH of more than 7 Ex. Aspirin pH=2.7 Tastes sour Turns blue litmus paper red Base: pH of more than 7 Ex. Ammonia pH=11.6 Tastes bitter and feels slippery Turns red litmus paper blue Reacts with acid to produce salt

Organic Vs. Inorganic Organic compounds: contain carbon, hydrogen, oxygen and other trace elements Inorganic compound: generally do not have carbon

Chemical Formulas Tells what elements & how many atoms of each element are found in a substance Ex: Indigo = C16H10N2O2 Each molecule has 16 carbon atoms, 10 hydrogen atoms, etc… 28

Pure substance Any matter that has a fixed composition and definite properties (water) Pure substance such as water can not be broken down by physical action such as boiling, melting or grinding

Types of Mixtures Homogeneous – (same) mixture that is uniformly mixed Heterogeneous (different) – mixture where substances are not uniformly mixed 30

Heterogeneous and Homogeneous Heterogeneous Mixture – Like Sand in water Homogeneous Mixture – Like Salt in water

Miscible vs. Immiscible Miscible and immiscible refers to liquid Miscible - two liquids dissolve in each other Ex: Alcohol and water Immiscible – a heterogeneous mixture

Separating mixtures React a substance and remove it via filtration technique