Workplace Hazardous Materials Information System Why Is It .

Workplace Hazardous Materials InformationSystem Why is it important?

CLASS A: COMPRESSED GASThis class includes compressed gases,dissolved gases, and gases liquefied bycompression or refrigeration.CLASS B: FLAMMABLE ANDCOMBUSTIBLE MATERIALThis class includes solids, liquids, andgases capable of catching fire in thepresence of a spark or open flame undernormal working conditions.CLASS C: OXIDIZING MATERIALThese materials increase the risk of fire ifthey come in contact with flammable orcombustible materials.

CLASS D: POISONOUS AND INFECTIOUS MATERIALDivision 1: Materials Causing Immediate and Serious ToxicEffectsThese materials can cause death or immediate injury when aperson is exposed to small amounts. Examples: sodium cyanide,hydrogen sulphideCLASS D: POISONOUS AND INFECTIOUS MATERIALDivision 2: Materials Causing Other Toxic EFFECTSThese materials can cause life-threatening and serious longterm health problems as well as less severe but immediatereactions in a person who is repeatedly exposed to smallamounts.CLASS D: POISONOUS AND INFECTIOUS MATERIALDivision 3: Biohazardous Infectious MATERIALThese materials contain an organism that has been shown tocause disease or to be a probable cause of disease in persons oranimals.

CLASS E: CORROSIVE MATERIALThis class includes caustic and acid materialsthat can destroy the skin or eat through metals.Examples: sodium hydroxide, hydrochloric acid,nitric acidCLASS F: DANGEROUSLY REACTIVE MATERIALThese products may self-react dangerously (forexample, they may explode) upon standing or whenexposed to physical shock or to increased pressure ortemperature, or they emit toxic gases when exposedto water.

What is Chemistry and Matter?Chemistry is the study of matter, itsproperties and its changes ortransformations.Matter is anything that has mass and takesup space.

ents(HomogeneousMixtures)HeterogeneousMixtures

A mixture is a substance made by combiningtwo or more different materials in such a waythat no chemical reaction occurs. Mixtures can be separated by physical means. Ex. Party Mix, boiling Kool Aid

Mixture where the two different substancesthat are combined together are mixed verywell.Any portion of the sample has the sameproperties and composition.Example: Salt WaterMilk

Mixture where the different parts or eachsubstance can be separated physically.Different parts are visible.Example: Toppings on a PizzaChocolate chip cookieSalad

How do we know that a sample of matter is apure substance? A pure substance is made up of all the sameparticles.A pure substance also has constantproperties. Example: pure water, aluminumfoil.Pure substances can be either elements orcompounds.

Compounds are pure substances that containtwo or more different elements in a fixedproportion. Example: Water H2O 2 parts hydrogen to1 part oxygen.Salt NaCl 1 sodium to 1 clorine

Elements are pure substances that cannot bebroken down into simpler substances. Elements contain only one kind of atom. Example: Oxygen, hydrogen, iron, etc.( anything on the periodic table )

Homogeneous MixtureHeterogeneous MixtureElementCompoundPure SubstanceMixture

SaltSugarWoodRockWaterMilkPlasticGlassMercury Apple JuiceSyrupGoldAirOxygenSilverCookiesCakeSand

There are 3 states of matter: Solid,Liquid and Gas. http://www.harcourtschool.com/activity/states of matter/index.html

A Physical Property is a characteristic of asubstance. Usually these are properties that wecan detect with our senses. Changing the size or amount of the substancedoes not change the physical properties.

Color – red, green, white, etc. Texture – smooth, fine, coarse. Taste – sour, sweet, salty. Odour – what smell does the substance have? States of matter at room temperature:- solid, liquid, gas.

Malleable is the ability of a solid to behammered or bent into different shapes.Aluminum foil is malleable. Gold is malleablesince it can be hammered into thin sheets. Hardness – the measure of the resistance ofa solid to being scratched or dented

Ductility – The ability to stretch a substanceinto a wire. Viscosity – the ability of a substance to flowor pour. Luster – How shiny is the substance?

Boiling Point – the temperature at which aliquid changes state and becomes a gas. Melting Point – the temperature at which asolid changes state and becomes liquid.

Baking soda is: solid at roomtemperature white in color crystal form dissolves easily inwater.

A chemical property is a behaviour thatoccurs when a substance changes to a newsubstance. For example:Is the substance combustible?Does the substance have a reaction with acid?Does the substance react with water?

1.In a physical change, the substance involvedremains the same substance, even though itmay change state or form.2.Can be undone quite easily.Key: No new substance is created. Examples: melting ice, freezing water,dissolving salt into water, breaking a stick.

1.In a chemical change, the original substance ischanged into one or more different substancesthat have different properties.2.Not easily undone – almost impossibleKey: New substance almost always formed. Examples: burning wood, baking a cake,digesting food

A new color appears. Heat or light is given off. Bubbles of gas are formed. The change is difficult to reverse.

Here are some examples of physical changes:

Here are some other examples of chemicalchanges:

Chemical orPhysical Changes

Cutting a piece of wood.

Chewing of food

Rusting Nail

Ice Melting

Burning a Match

Stretching a Rubber Band

Breaking a Stick

Tarnishing Silver

Ripening Tomatoes

Water Boiling

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Negatively charged ( - ) Almost have no mass Located around the outside of the nucleus

Same mass as neutrons Positively charged ( ) Located in center of atom (nucleus) Number of protons in an atom is equal to theelements atomic number.

Same mass as proton No charge Located in nucleus Number per atom is based on the followingformula: #Neutrons Atomic Mass – Atomic Number

Bohr suggested that: Electrons move around the nucleus in circular pathscalled orbits, like planets around the sun. The order of filling of electrons in the first four orbitsis 2, 8, 8, 2.

1.2.3.Find the # of protons, neutrons, and electronsDraw protons (p ), (n0) in circle (i.e. “nucleus”)Draw electrons around in shells - 2, 8, 8, 2 arethe numbers of electrons allowed in the ringsfor the first 20 elements.LiHe2 p 2 n03 p 4 n0

A molecule is formed when 2 or more atomsjoin together chemically. Ex. H2, O2, N2 A compound is a molecule that contains atleast 2 different elements. Ex. H2O, CO2 All compounds are molecules, but not allmolecules are compounds.

Elements are arranged to help us to explainand predict physical and chemical properties.

Period – elements in the same row; rows arenumbered from top to bottom Family – elements in the same column; theseelements have similar properties

Tend to have similar physical and chemical properties.Found in same vertical column.1.Alkali Metals – shiny, silvery metals, compounds solublein water2.Alkaline Earth Metals – shiny, silvery metal, compoundsinsoluble in water3.Transition Metals – center columns4.Halogens – nonmetals, react readily with alkali metals5.Noble Gases - nonreactive

The elements that occupy the far left columnof the periodic table are called Alkali Metals. Called Group 1 elements These elements are extremely reactive.

Found in group 2. Form compounds that are often insoluble inwater.

Halogens occupy the 17th column of theperiodic table. ( F, Cl, Br, I, At)These elements are the most reactive nonmetals.All halogens are poisonous elements thatreact readily with sodium and other alkalimetals.

Metalloids are elements that possess bothmetallic and nonmetallic properties.They are found in different groups on the farright side of the periodic table.Examples: Silicon, boron, germanium,arsenic, selenium, antimony, tellurium,polonium, and astatine are all metalloids.

Noble Gases are the elements that occupythe far right column of the periodic table.( He, Ne, Ar, Kr, Xe, Rn )Also Called inert gases because Noble gasesgenerally do not form compounds.All gases at room temperature.

METALS ShinyMalleableConductorsMost of them react withacidMostly solidsNON METALS DullBrittleMostly insulatorsDo not react with acidSolids, liquids and gases atroom temperature.

Metals and non-metals combine to form ioniccompounds by transferring electrons. Metal atoms lose electrons to form positiveions. Non-metal atoms gain electrons to formnegative ions.

How do we know that a sample of matter is a pure substance? A pure substance is made up of all the same particles. A pure substance also has constant properties. Example: pure water, aluminum f