Chapter 11 Note guide to go with powerpoint

1. Chapter 11 Chemical Reactions and Equations
Word Equations
Recall that ___________________________ can describe chemical reactions.
•
Reactants are written to the ___________________ of the arrow and products are
written to the _____________ of the arrow.
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Recall how to name and write formulas from your _________________.
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A _________________________ is the formulas of the reactants and products
without the amounts included.
Balancing Chemical Equations
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________________________________ do not require amounts but in order to
use actual equations in chemistry, a ________________________ with amounts must be
written.
Law of Conservation of Mass
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Chemical reactions must obey the _________________________________.
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Reactants must ____________________l the products in amount and mass.
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A __________________________________ compares the amounts of reactants
to products.
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An Example….
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We need two wheels to make a toy car.
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They are sold only in twos.

2. •
Each toy car has one car body (Cb) and 4 wheels are necessary. (W4)
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What would be our balanced chemical equation for the toy car?
Building a Tricycle….
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Again, we need one trike body (Tb) but a tricycle has 3 wheels (W3) and the
wheels only come in packages of two. (W2)
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How many orders of each tricycle should be make so there are no leftover parts?
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Write a balanced “chemical” equation.
Tips and Tricks…
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If there is a ____________________________ on both sides of the equation, keep
it together and balance it as one atom.
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Balance the more ________________________ compounds first.
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The elements that are by themselves should be balanced last.
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Sometimes it is helpful to create a _________________ below the equation to
keep track of the numbers.
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If you have a word equation, write the ____________________________ first,
then balance.
LET’S PRACTICE!
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Balance the equations.

3. •
AgNO3 + H2S Ag2S + HNO3
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Zn(OH)2 + H3PO4 Zn3(PO4)2 + H2O
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Iron(III) chloride + calcium hydroxide iron(III) hydroxide + calcium chloride
Types of Chemical Reactions
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There are ________ general types of reactions.
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Occasionally, a reaction may fit equally into __________ categories.
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____________________ is useful to help determine and predict the products.
Combination Reactions
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It is also called a ______________ reaction.
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________________________ substances combine to create a _______________
new substance.
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Mg + O2  MgO
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K + Cl2  KCl
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Balance these equations!

4. Draw a picture example of a combination reaction.
Decomposition Reactions
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A ______________ compound breaks down into ___________________ simpler
products.
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HgO  Hg + O2
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H2O H2 + O2
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Balance these equations!
Draw a picture example of a decomposition reaction.
Single-Replacement Reaction
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One element ________________ a second element in a compound.

5. •
Requires the ________________________ to determine if the reaction will occur.
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The element that is ___________________ on the series will replace any lower
elements.
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A ___________________ (group 7) can replace any other halogen providing that
it is higher up on the periodic table.
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If a reaction doesn’t occur, write _____________ for no reaction.
Single-Replacement Reactions

6. •
K + H2O  KOH + H2
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Zn + Cu(NO3)2  Cu + Zn(NO3)2
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Br2 + NaI  NaBr + I2
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Br2 + NaCl  NR
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Balance these equations!
Draw a picture example of a single-replacement reaction.
Double-Replacement Reactions
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Sometimes when two solutions are mixed, ____________________________.
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Other times, the _____________ in the two solutions react.
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In these types of reactions, the two ______________ (positive) cations
_______________ places with each other.
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Occasionally, a ________________ will form or a gas will be generated.
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Sometimes, both products are _________________ so you won’t see anything
different
Double-Replacement Reactions
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Na2S + Cd(NO3)2  CdS + NaNO3

7. •
NaCN + H2SO4  HCN + Na2SO4
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Ca(OH)2 + HCl  CaCl2 + H2O
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Balance these equations!
Draw a picture representing a double-replacement Reaction.
Combustion Reactions
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This is a chemical change that takes place when a compound (usually a
hydrocarbon) reacts with ________________ and produces _________________,
_______________ and usually ____________________ in the form of heat and/or light.
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C8H18 + O2  CO2 + H2O
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When balancing, these numbers are usually high.
Draw a picture showing a combustion reaction.
Reaction in Aqueous Solution

8. •
Your world is water-based.
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Most reactions take place in _______________.
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Most equations can show the reactions between compounds but do not show how
the compounds _________________ when dissolved in water.
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They actually separate into the __________________________ when in aqueous
solution.
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You can use these ions to write a _________________________.
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If the ion remains ________________ on both sides of the equation, it is called a
_____________________.
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The ____________________ doesn’t participate in the reaction directly and can
be _______________________.
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The resulting equation is called the ________________________.
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Remember, the resulting equation must be ________________________.
Net Ionic Equations
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A net ionic equation shows only those ___________________ involved in the
reaction and is balanced with respect to both ______________ and _______________.
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Pb (s) + 2Ag+ (aq)  2Ag (s) + Pb +2 (aq)
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There are 2 Ag on both sides and +2 on both sides.
Solubility
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_______________ means it can dissolve in water or be _________________.
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There are rules to determine if something is soluble or not.
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Page. 344 table 11.3 has the rules.

9. •
If something is soluble write _____________
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If it isn’t soluble or is insoluble, it is solid or _____________
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Check the table for the rules.
LET’S PRACTICE!
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Balance this equation.
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Ca+2 + OH- + H+ + PO4-3  Ca+2 + PO4-3 + H2O
LET’S PRACTICE!
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Write the complete and net ionic equations for:

10. •
Sodium hydroxide (aq) and phosphoric acid (aq) makes calcium phosphate and
water.
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Don’t forget to use your solubility rules.