PART 1: Introduction to Chemical Reactions 9a In a chemical reaction… atoms are ____________ (fill...
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Transcript of PART 1: Introduction to Chemical Reactions 9a In a chemical reaction… atoms are ____________ (fill...
![Page 1: PART 1: Introduction to Chemical Reactions 9a In a chemical reaction… atoms are ____________ (fill in the blank)](https://reader034.fdocuments.us/reader034/viewer/2022050908/56649e405503460f94b30f9a/html5/thumbnails/1.jpg)
PART 1:
Introduction to Chemical Reactions9a
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In a chemical reaction…
atoms are____________
(fill in the blank)
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What are some common reactions in your everyday life?
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How can you tell when a chemical reaction has
taken place?
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Formation of a ___________________
also known as a ___________________
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HOW DO CHEMISTS REPRESENT CHEMICAL
REACTIONS?
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Chemists use ______________ to represent chemical reactions. The starting substances are
__________________What you
end up with are _____________When do you use chemical equations in your own life?
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REAL LIFE EXAMPLE: You are going to bake cookies. You know that:
____flour + ____sugar + ____baking powder + ___butter + ___chocolate chips makes ___cookies
This is a _______________EQUATION. What are the product(s)? What are the reactant(s)?
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What else do you need to know….
if you already know that you need to bake them at 350 for ½ hour??
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You need to know the _________________
______________________ of the ingredients with respect to each other.
In other words, you need a
___________________ ________________ (Remember – cooking is chemistry!!)
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HOW MIGHT A CHEMIST USE A
CHEMICAL EQUATION?
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You are an EVIRONMENTAL CHEMIST concerned about
GLOBAL WARMING
You are asked to determine how much carbon dioxide will be produced from the amount of methane burned by a factory. The first thing you need is a WORD EQUATION
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methane + oxygen yields
carbon dioxide + water
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Word equations are clunky and they don’t tell you very much… You can make your equation less clunky if you use
_________________________instead of words.
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__ CH4 + __O2
__CO2 + __ H2O
This type of equation is a
____________
equation.
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In addition, to give more information in an equation, symbols are used to
represent the _____________________ of the substances, including:
Solids = _______ Aqueous = ______Gases = _______ Liquids = ______
(Aqueous means __________________
_________________________________
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__ CH4(g) + __ O2(g)
__ CO2 (g) +__ H2O(l)
This equation still doesn’t have enough information…What else do you need?
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What law allows us to balance equations? State this law.
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CH4
O2
CO2
H2O
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A very important rule in balancing equations: never change the
________________________
For example: ______ cannot be changed to _______
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PART 2
BALANCING EQUATIONS
The Skill
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The Law of Conservation of Mass says…
You must have the same number of atoms of a particular element on
both sides of a chemical equation…
i.e., the equation must be BALANCED!
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There are 2 different types of numbers in chemical equations.
COEFFICIENTS
__ CH4 + 2 O2 __CO2 + 2 H2O
SUBSCRIPTS
Subscripts cannot be changed while balancing an equation…remember CO vs CO2?
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However, COEFFICIENTS can be changed in order to balance an equation.
Begin by counting the number of atoms of each element…
___ Na(s) + ___ Cl2 (g) ___ NaCl (s)
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___H2 (g) +___ N2 (g) ___ NH3 (g)
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__ Al2O3(s) ___ Al(s)+ ___O2(g)
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___ Fe(BrO3)3 → ___ FeBr3 + ___ O2
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ANOTHER RULE: If you balance an equation, and
then find that all of the coefficients are divisible by a common number,
you must divide them by that number…
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2CH4 + 4O2 2CO2+4H2O
WRONG!
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CH4 + 2O2 CO2+2H2O
RIGHT!!
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Hint #1If a polyatomic ion appears
unchanged on both sides of the equation, balance it as a UNIT
– not as individual atoms
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__Al(NO3)3 + __LiOH
__LiNO3 + __ Al(OH)3
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[ ]
[ ][ ]
[ ]
Al(NO3)3
[ ]
[ ]
[ ]Al(OH)3
][LiOH LiNO3
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__(NH4)3PO4 +__ BaSO4
__(NH4)2SO4 +__Ba3(PO4)2
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Example of an acid-base reaction.
__ H2SO4 + __KOH ___K2SO4 + __ H2O
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Hint #2 First, balance an element that only appears in one reactant
and one product (leaving oxygen to last and hydrogen to
second last.)
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__C3H8 +__O2 __CO2 + __H2O
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__C5H12 (g)+__O2(g)
__CO2(g) + __H2O(l)
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HINT #3If you balance all of the elements and the polyatomic ions, except for one element, and there’s an odd # of that last element on one side, and an even number on the other side – balance that element with a fractional number (containing ½) and
then double all of the coefficients
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__C5H10 + __O2 __CO2 + __H2O
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__C6H14 + __O2 __CO2 + __H2O