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UNIT VIChemical Reactions
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VI.1 INTRODUCTION TO CHEMICAL EQUATIONS
A chemical reaction (or chemical change) involves the formation of a __________________________.
reactants (starting materials) form a chemically different product.
Changes that accompany chemical reactions include:
____________________________________ ____________________________________ ____________________________________
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VI.1 INTRODUCTION TO CHEMICAL EQUATIONS
A chemical reaction equation is ____________________________________________________________________________________________________________________________________________________________________________________
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VI.1 INTRODUCTION TO CHEMICAL EQUATIONS
Ex: 2H2 + O2 → 2H2 O
The word equation is: “Hydrogen gas reacts with oxygen gas to form water”.
Coefficient is __________________________________________________________________________________________
refers to the
_____________________________________________
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VI.2 THE CONSERVATION LAWS
In a CLOSED system, the total mass of products is EQUAL to the total mass of reactants involved in a chemical reaction.
mass (reactants) = mass (products)
A system (part of the universe being studied) is CLOSED when nothing can enter or leave the system.
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VI.2 THE CONSERVATION LAWS
Law of Conservation of Mass: states that the total ___________ of ALL REACTANTS before a chemical reaction equals the total __________ of ALL PRODUCTS after the chemical reaction.
For this to be true: the total number of ___________ must be
constant bonds between atoms are broken and new
bonds form...but same atoms are there
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VI.2 THE CONSERVATION LAWS
More laws of conservation on page 106 in Hebden!
Law of conservation of atoms Law of conservation of electrical charge Law of conservation of energy
Questions: p. 106-107: #1-6
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VI.3 BALANCING CHEMICAL EQUATIONS
To write and balance an equation:
write what you believe is happening (include the formulae of reactants and products)
balance each side so the two sides are EQUAL balance by placing a ________________ in
front of a formulaNEVER change ________________ on atoms
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VI.3 BALANCING CHEMICAL EQUATIONS
Steps to balancing an equation (guidelines) Start with atoms which occur once on each
side Then balance the metals (or any other non-
hydrogen, non-oxygen atoms) Balance polyatomic ions as a whole Leave H and O until very last
*if a fraction (ex: 3/2) occurs during balancing, multiply the equation by the whole number (ex:2) to eliminate the fraction.
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VI.3 BALANCING CHEMICAL EQUATIONS
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VI.3 BALANCING CHEMICAL EQUATIONS
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VI.3 BALANCING CHEMICAL EQUATIONS
Example #1:___ Na + ___ H2O → ___ NaOH + ___ H2
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VI.3 BALANCING CHEMICAL EQUATIONS
Example #2: __(NH4)2SO4 + __NaOH → __NH3 + __H2O +
__Na2SO4
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VI.3 BALANCING CHEMICAL EQUATIONS
Example #3: ___ AgNO3 + ___ CuCl2 → ___ AgCl + ___Cu(NO3)2
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VI.3 BALANCING CHEMICAL EQUATIONS
Example #4: ___ CuSO4 + ____ Fe → ____Cu + ___Fe2(SO4)3
http://phet.colorado.edu/en/simulation/balancing-chemical-equations
Questions: p. 110-111 #7-52 (every third question) – PRACTICE
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VI.4 WRITING PHASES IN REACTION EQUATIONS & USING CHEMICAL WORD EQUATIONS
Phases are also shown in chemical reaction equations
s = solid phasel = liquid phaseg = gaseous phaseaq = aqueous phase (dissolved in water)
ex: 2H2(g) + O2(g) → 2H2 O(g)
The word SOLID can also be stated as crystal, powder, and precipitate (precipitate is formed when two liquid or aqueous solutions react)
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VI.4 WRITING PHASES IN REACTION EQUATIONS & USING CHEMICAL WORD EQUATIONS
Diatomic molecules - seven of the elements form diatomic molecules:
N, O, F, Cl, Br, I and H (p. 113) * on the periodic table, they form the shape
of a 7 plus one (H)
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VI.4 WRITING PHASES IN REACTION EQUATIONS & USING CHEMICAL WORD EQUATIONS
Writing chemical equations from the word equation:
Ex #1: Aqueous bromine is replaced by chlorine in potassium bromide to form potassium chloride.
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VI.4 WRITING PHASES IN REACTION EQUATIONS & USING CHEMICAL WORD EQUATIONS
Ex #2: Solid aluminum oxide and aqueous sulphuric acid produce water and aqueous aluminum sulphate
Questions: p.113 # 57, 58-64 (even)