Chemical Reactions and Balancing Equations

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					                             Reactions-- Chapter 8
                                                                       Due       Stamp

1.   Chemical Reactions Notes/WS (in class)                             1/31


2. Balancing Equations WS (in class)                                    1/31


3. Rockets Lab                                                          2/1


4. In the Balance WS (HW)                                               2/6

5. Quiz: Balancing Equations                                           2/7

6. Reaction Types WS (HW)                                               2/9


7. Predicting Products WS (start in class, finish for HW)              2/10

8. Reaction Types Power Point Project—Make a power point showing the   2/13
   4 reaction types in pictures. Groups of 1-3 from any Chem class.
   Email your teacher by due date.

9. Reactions Hot Potato Activity                                       2/14

10. Reaction Types Lab                                                 2/15

11. More Reactions WS-- 2 Pages (start in class, finish for HW)        2/21


12. Practice Practical Quiz                                            2/17

13. Reactions Test and Packet Due                                      2/21,22


Name:
                                Chemical Reactions
I. Define the following on a separate piece of paper:
1. Reactant                                                5. Skeleton equation
2. Product                                                 6. Coefficient
3. Word equation                                           7. Aqueous
4. Chemical equation                                       8. Balanced equation
II. Fill in the chart with the correct symbols and examples
   Symbol                      Description                                  Example of use

                 Used to separate multiple reactants or
                 products

                 Yields

                 Reactant or product in the solid state

                 Reactant or product in the liquid state

                 Reactant or product in gaseous state

                 Substance that is dissolved in water,
                 aqueous solution

                 Heat is supplied to the reaction

                 A catalyst is supplied to the reaction

III. Write the chemical equation for each of the following. Are they balanced?
1. The production of HCl gas from hydrogen and chlorine gases



2. Silver metal reacts with solid sulfur to form silver(I) sulfide



3. Aqueous silver(I) nitrate reacts with copper metal to produce silver metal and aqueous copper(II)
   nitrate



IV. For each of the following, write the total number of atoms present.
1. __________ 4SO2                                         4. __________ 2Fe2(CO3)3

2. __________ 8O2                                          5. __________ 3Ca3(PO4)2

3. __________ 5HNO3                                        6. __________ 18HNO3
                                  Balancing Equations
   A complete chemical reaction has the same number of each type of atom on both sides of the arrow. The number of
    atoms on the left of the arrow must equal the number of atoms on the right side of the arrow because atoms
    are conserved, not lost or created in a reaction.
   You can only add numbers to the front of atoms/compounds.
   Never change the numbers at the bottom because you’ll completely change the compound!


1. ____ Al + ____ CuF  ____ AlF3 + ____ Cu



2. ____ Cr2S + ____ AlF3  ____ Al2S3 + ____ CrF



3. ____ Ag(s) + ____ CuSO4(aq)  ____ Cu(s) + ____ Ag2SO4(aq)



4. ____ Fe2O3 + ____ Al  _____ Al2O3 + ____ Fe


                                                                           Use HOH for Water and you can treat the OH
5. ____ NaOH(aq) + ____ H2S(g)  ____ Na2S(aq) + ____ H2O(l)               as 1 thing. This is useful if you have OH on
                                                                           one side and water on the other.



6. ____C6H12O6 + ____ O2  ____CO2 + ____H2O



7. ____ C3H4(l) + ____ O2(g)  ____ CO2(g) + ____ H2O(g)



8. ____ S2(g) + ____ Ag(s)  ____ Ag2S(s)



9. ____ H2O2(l)  ____ H2O(l) + ____ O2(g)



10. ____ NaHCO3(s)  ____ Na2CO3(s) + ____ H2O(g) + ____CO2(g)



11. ____ K2CO3 + ____ Fe3(PO4)2  ____ FeCO3 + ____ K3PO4
Reaction Types
1. Balance each of the following equations (some are already balanced)
2. To the left of each equation, indicate the reaction type that it represents: C = Combination; D =
Decomposition; SR = Single-replacement; DR = Double-replacement; CN = Combustion

C   D    SR     DR    CN      ____ Pb(NO3)2 + ____ K2CrO4  ____ PbCrO4 + ____ KNO3


C   D    SR     DR    CN      ____ Al + _____ Cl2  ____ AlCl3


C   D    SR     DR    CN      ____ NaOH + ____ NiCl2  ____ NaCl + ____ Ni(OH)2


C   D    SR     DR    CN      ____ Na2SO4 + ____ Al(NO3)3  ____ NaNO3 + ____ Al2(SO4)3


C   D    SR     DR    CN      ____ Sr(OH)2 + ____ NaCl  ____ SrCl2 + ____ NaOH


C   D    SR     DR    CN      ____ HCl + ____ Fe2O3  ____ FeCl3 + ____ H2O


C   D    SR     DR    CN      ____ C6H12O6 + ____ O2  ____ CO2 + ____ H2O


C   D    SR     DR    CN      ____ H2O electricity ____ H2 + ____ O2


C   D    SR     DR    CN      ____ KClO3 heat ____ KCl + ____ O2(g)


C   D    SR     DR    CN      ____ N2 + ____ H2  ____ NH3


C   D    SR     DR    CN      ____ Fe + ____CuSO4  ____FeSO4 + ____Cu


C   D    SR     DR    CN      ____CaCO3  ____CaO + ____CO2


C   D    SR     DR    CN      ____ P + ____ O2  ____ P2O5


C   D    SR     DR    CN      ____ C + ____ H2  ____ CH4


C   D    SR     DR    CN      ____ CH4 + ____ O2  ____ CO2 + ____ H2O


C   D    SR     DR    CN      ____Cl2 + ____ KI ____KCl + ____I2


C   D    SR     DR    CN      ____ MgCO3  ____ MgO + ____ CO2
More Reactions—Page 1= writing equations
1. Write an equation for the reaction that produces iron(II)sulfide from iron and sulfur.




2. Write an equation representing the heating of magnesium carbonate to produce solid magnesium oxide and carbon
    dioxide gas.




3. Write a sentence that completely describes the chemical reaction represented by this balanced equation: 2HCl(aq) +
   CaCO3(s)  CO2(g) + CaCl2(aq) + H2O(l)




4. Write a sentence that completely describes the chemical reaction represented by this balanced equation: 2Ag2O
   4Ag(s) + O2(g)




5. Write a balanced equation representing the reaction of solid magnesium with oxygen gas to produce magnesium
    oxide.




6. Write the balanced equation for the reaction that occurs between aluminum and fluorine gas.




7. Write the balanced equation for the production of oxygen gas and potassium chloride from the decomposition of
    potassium chlorate.




8. Write the balanced equation for the combustion of propane (C3H8) to produce carbon dioxide and water vapor.



9. Write the balanced equation for the reaction between iron(III) chloride and sodium hydroxide. The products are
    iron(III) hydroxide and sodium chloride.
More Reactions—Page 2= reaction types +
predicting products
Identify the reaction type, then fill in the blanks to create a complete and balanced chemical equation.

______________ 1.         Ba(NO3)2 +        Na3PO4  ___________ + ___________


______________ 2.        Al +      O2  ___________


______________ 3.         I2 +    NaBr  ____________ + _____________


______________ 4.         C3H4 +     O2 


______________ 5.         Mg + ___________          Mg(NO3)2 +      Zn


______________ 6.         PbO2 heat ________ +        O2


______________ 7.     ________ +       O2     SO2


______________ 8.         C6H6 +       O2 


______________ 9.         AgNO3 +         NaCl 


______________ 10.        Li +     O2 


______________ 11.       Cl2 + KI 


______________ 12.        MgCl2 


______________ 13.        KCl +     AgNO3 


______________ 14.        Sn + ________             SnBr4


______________ 15.       C8H18 +       O2 


______________ 16.       Al +       KBr 


______________ 17.      __________ + Sr(OH)2          Mn(OH)4 +      SrS

				
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