Substance DITRIBUTION/TRANSPORTATION REGULATION of substances Body PROTECTION.
Describe how substances react with other substances Examples: Combustibility – Will a substance...
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Transcript of Describe how substances react with other substances Examples: Combustibility – Will a substance...
Describe how substances react with other substances
Examples:Combustibility – Will a substance burn?Reactivity – Will a substance react with other
substances and how easily?Metals in Groups 1 and 2 are very reactiveSodium (Na) is very reactive, especially with waterDon't try this at home!Hydrogen (H) is also very reactiveThe Hindenburg Disaster - Oh, the humanity!
Stability – Usually do not react with other substancesNoble gases in Group 18Helium (He) is now used in Blimps
Occurs when 2 or more substances are combined and changed into new substances with new properties
Also called chemical reactionsReactants – the substances that change, or reactProducts – the new substances that are producedDuring a chemical reaction, bonds between
atoms are broke and new bonds are formed.Law of Conservation of Matter (Mass) – Matter
cannot be created, nor destroyed. It can only be transformed. So…..
….the starting masses of the reactants is always equal to the final mass of the products
Example:Photosynthesis
6CO2 + 6H2O C6H12O6 + 6O26 molecules of carbon dioxide and 6 molecules of
water are the reactantsSugar and 6 molecules of water are the productsThere are 6 carbon atoms, 12 hydrogen atoms, and
18 oxygen atoms on each side of the equationThis means the equation is balancedA chemical equation must be balanced to satisfy
the Law of Conservation of Matter (Mass)
Temperature changes Instant hand warmers, instant ice packs
Light and sound are producedFireworks
Color changesAutumn leaves, iron rusting, mixing chemicals to
make paintOdor changes
Food spoiling Bubbles or gas form
Alka-seltzerPrecipitate forms
Cave formations made of calcium carbonateExample of a precipitate
Chemical reactions always involve energy changes2 Types of reactions
Exothermic Reactions – Give off energy (heat)Exo = outsideExamples: fireworks exploding, wood burning, iron oxide
(rust) forming, hand warmersEndothermic Reactions – absorb energy (heat)
Endo = insideExamples: instants cold packs, add salt to ice
Activation energy – the smallest amount of energy needed to start a chemical reactionDepends on reactants and other conditions, like
temperature
How fast a reaction occursAffected by 5 main factors
Concentration of reactant particles More particles = faster reaction
Total surface area of the reactantsMore surface area = faster reactionThink alka-seltzer
TemperatureWarmer = faster & colder = slowerOvens & refrigerators
Nature of the reactantsGroups 1 & 2 are very reactive
Adding certain substances to the reaction Inhibitor – slows reactionCatalyst – speeds reaction
Enzymes – catalysts produced by living things – Think salivaElephant Toothpaste – example of a reaction with a
catalyst
Acids – compounds that release hydrogen ions (H+) in waterLemons, oranges, grapefruits – citric acidVinegar – acetic acidSulfuric acid, hydrochloric acid
Have a sour taste - Warning never taste unknown chemicals
Strong acids are corrosive – they eat away or break down materials
Hydrochloric acid in our stomachs helps us digest food
Bases – compounds that release hydroxide ions (OH-) in water – also called alkalineSoapBaking PowderSodium hydroxide
Have a bitter taste – Warning never taste unknown chemicals
Strong bases are corrosive – they eat away or break down materials
Sodium hydroxide is in drain cleaners
Scale used to describe the strengths of acids and bases
Measure of hydrogen ions in the solutionScale ranges from 0-14
7 is neutral (water)0-7 = acid (the lower the number, the stronger the acid)7-14 = base (the higher the number, the stronger the
base)