 Anything that has mass & take up space Mass = measurement of the amount of matter an object contains Chemistry = the study of matter & the changes that it undergoes

 Quantitative – numerical information how much how little how big how small

 Qualitative – descriptive information condition, color, size, shape, odor, texture

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Physical Properties – a characteristic that can be observed or measured w/out changing the identity of a substance

ex. color, odor, taste, hardness, density, melting/boiling points, state of matter

 States of Matter – the physical forms in which all matter  exists on Earth

Solid  def. shape & volume  shape independent of container  particles are packed together Liquid  def. volume  shape depends on container  particles can move freely Gas  indefinite volume & shape  particles move quickly & spread apart

Physical Changes – a change that occurs in the physical appearance of a substance, but does not change its identity breaking, splitting, grinding, cutting, crushing Ex. melting, boiling, freezing, evaporating, dissolving, condensing

 COLOR  STATE OF MATTER AT GIVEN TEMPERATURE SOLID, LIGUID, GAS  MELTING POINT  BOILING POINT  DENSITY (mass per unit volume)  SOLUBILITY  ELECTRICAL CONDUCTIVITY Does it conduct or is it an insulator?  MALLEABILITY How easily can it be deformed?  DUCTILITY How easily can it be drawn into a wire?  VISCOSITYHow susceptible is a liquid to flow?

4. Chemical Properties – relates to a substances ability to undergo changes that transform it into a different substance  easiest to see when a chemical is reacting Chemical changes – a change that produces matter with a different composition than the original matter ex. burning, rotting, rusting, reacting, cooking, digestion, respiration

 BURN  ROT  RUST  DECOMPOSE  FERMENT  EXPLODE  CORRODE

 EVOLUTION OF A GAS  FORMATION OF PRECIPITATE (two clear solutions when combined form solid)  RELEASE OF ABSORPTION OF ENERGY  COLOR CHANGE

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 A combination of 2 or more types of matter  Each component keeps its own identity & properties  Components are only physically mixed & can be separated using physical means

Heterogeneous mixture a mixture in which the substances are not evenly distributed

Homogeneous mixture – a mixture or ‘solution’ in which the substances are evenly distributed

Phase – used to describe any part of a sample with uniform composition & properties Homogeneous mixture 1 phase Heterogeneous mixture 2 phases

1. Filtration – a technique that uses a porous barrier to separate a solid from a liquid Can you think of any common applications?  ‘Plays’ on differences in physical properties

2. Distillation – a technique that can be used to physically separate most homogeneous mixtures based on differences in the boiling points of the substances involved

3. Chromatography – a technique that is used to physically separate the components of a mixture based on the tendency of each component to travel or be drawn across the surface of another material

 Every sample has same: ◦ characteristic properties ◦ composition  Are made of: ◦ one type of atom: element  Ex: iron, gold, oxygen ◦ 2 or more types of atoms: compound  Ex: salt, sugar, water

 Simplest form of matter that has its own unique set of properties  Can not be separated into simpler substances by physical or chemical means  Each element is made up of a single type of atom ex. hydrogen, nitrogen, lead

 A substance that contains 2 or more elements chemically combined in a fixed proportion  Properties are different than the individual elements ex. Glucose (sugar) Glucose – sweet, white solid Carbon – black, tasteless solid Oxygen – colorless, tasteless gas Hydrogen – colorless, tasteless gas

 Physical methods do not work  Recall… Chemical changes – a change that produces matter with a different composition than the original matter

 Chemical Symbol each element is represented by a one- or two-letter symbol Trends: 1 st letter = always capitalized 2 nd letter = always lowercase Subscripts = indicate the relative proportions of the elements in a compound H K Au H2OH2O C 6 H 12 O 6 Hydrogen Potassium GoldWaterGlucose

 The process by which the atoms of one or more substances are rearranged to form different substances  Occurrence can be indicated by changes in temperature, color, odor, & physical state  Also known as a chemical change  Chemical properties can only be observed when a substance undergoes a chemical change

The process of photosynthesis is a chemical reaction in which light energy, carbon dioxide and water, are transformed to create glucose and oxygen.

The photosynthetic chemical reaction can be shown by writing out the element symbols for each compound. Reactants  substances to the left of the arrow  ‘ingredients’  CO 2 and H 2 O Products  substances to the right of the arrow  ‘what is made’ or produced  C 6 H 12 O 6 and O 2

1. Transfer of energy Energy may be given off in the form of heat or light 2. Change in color Substances may ‘brown’ Indicators  How can you tell whether a chemical change has taken place?

3. Precipitate A solid that settles out of a liquid mixture 4. Gas production Indicated by the formation of ‘gas bubbles’

 During any chemical reaction, the mass of the products is always equal to the mass of the reactants + O 2 + CO 2 + H 2 O vapor

 Conservation of mass also applies to physical changes… 10g of ice 10g of liquid H 2 O

Law of Conservation of Mass  In any physical or chemical change, mass is conserved  i.e. Mass is neither created or destroyed