WRITING & BALANCING CHEMICAL EQUATIONSmsthompsonschemistrysite.weebly.com/uploads/3/3/1/7/... ·...
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WRITING & BALANCING CHEMICAL EQUATIONS
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Law of Conservation of MassDefinition•matter is neither created nor destroyed
Application•each side of a chemical equation must have equal masses (what goes in, must come out)
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Chemical EquationsChemical Equationsobey the law of conservation of mass when properly written
reactants on the left; products on the right
an arrow separates the reactants from the products
symbols used in complete chemical equations:
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Symbol Meaningyields; produces
reversiblereactants are heated
catalyst added to reactants(l) liquid phase(s) solid phase(g) gas phase(aq) aqueous phase: dissolved in H2O
acids and bases are usually in the aqueous (aq) phase
metals are usually in the solid (s) phase
pt
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Balanced Equations
Definition•have equal numbers of each type of atom on each side of the equation
•an unbalanced equation has unequal numbers of atoms on each side of the equation
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Rules:
•you can never change a subscript
•you may only change coefficients
•you cannot place a coefficient in the middle of a formula
•coefficients are only allowed in the front of a formula
•ensure that the final coefficients are reduced
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Example:
Balance this equation: H2 + Cl2 → HCl
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Now try the PRACTICE…
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Chemical
Reactions
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Synthesis
Reactions
Definition• two or more reactants combine to form one
product
• A + B → AB
Example• 2Mg + O2 → 2MgO
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Decomposition
Reactions
Definition• a single reactant breaks down into two or
more products
• AB → A + B
Example• FeS → Fe + S
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Single Replacement
Reactions
Definition• a single element or diatomic molecule reacts with a compound to produce a new compoundand a single element or diatomic molecule
• metals (A) and (B) swap positions:A + BC → B + AC
• nonmetals (A) and (C) swap positions:A + BC → C + BA
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Example• metals swap:
Cu + 2AgNO3 → Ag + Cu(NO3)2
• nonmetals swap:
Cl2 + 2NaBr → Br2 + 2NaCl
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Activity Series
a metal will only replace another metal if it is more reactiveif the metal is not more reactive, then the reaction will not occur.
ACTIVITY SERIESfor single replacement reactions
MOST REACTIVECesium (Cs)
Rubidium (Rb)Potassium (K)Sodium (Na)Lithium (Li)
Strontium (Sr)Calcium (Ca)
Magnesium (Mg)Aluminum (Al)
Zinc (Zn)Chromium (Cr)
Iron (Fe)Cadmium (Cd)
Cobalt (Co)Nickel (Ni)
Tin (Sn)Lead (Pb)
Hydrogen (H)Copper (Cu)Silver (Ag)
Mercury (Hg)Gold (Au)
Platinum (Pt)LEAST REACTIVE
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AB + CD AD + CB
Compound + compound yields compound + compound
DOUBLE
Replacement
Reactions
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LiF + KOH LiOH + KF
Notice that the positive and negative ions switched positions
DOUBLE
Replacement
Reactions
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CxHy + O2 CO2 + H2O
Hydrocarbon + Oxygen yields Carbon Dioxide + Water
COMBUSTION
Reactions
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• C2H4 + O2 ____ + ____
• C3H8 + ____ CO2 + _____
COMBUSTION
Reactions
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HCl + NaOH HOH + NaCl
Strong Acid + Strong Base produces Water + SaltWater can be written as: HOH or H2O
ACID-BASE
Reactions
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Acid-Base Rxn:
• HF + KOH ____ + ____
• HNO3 + Ca(OH)2 ____ + ____
• ____ + ____ HOH + Li3PO4