1. Chapter 8 test

3. Terms you must know Decomposition reaction Activity series
Spectator ions
Balanced equation
Double-replacement
Catalyst
Combustion reaction
Net ionic reaction
Single replacement
Combination reaction

4. Be familiar with the parts of a chemical equation
Reactants
Products
Yield symbol
Catalyst
Heat (energy)

5. Know the rules for balancing equations
Determine the correct formulas for all reactants and products
Write the reactants on the left side of the yield sign and the products on the right
Count the number of atoms of each element on each side of the yield sign
Balance the elements (or polyatomic ions) one at a time using coefficients (never change formulas)
Make sure coefficients are in lowest ratios

6. Balancing strategy CaCl2(aq) + H3PO4(aq) Ca3(PO4)2(s) + HCl(aq)
Here’s an unbalanced equation
Let’s start by listing all the atoms and polyatomic ions in a center column

7. Balancing strategy CaCl2(aq) + H3PO4(aq) Ca3(PO4)2(s) + HCl(aq) PO4 Ca
Now, let’s count up all the atoms of each element on each side of the yield sign

8. Balancing strategy CaCl2(aq) + H3PO4(aq) Ca3(PO4)2(s) + HCl(aq)
Now, let’s start changing the amounts of each element by changing the coefficients

9. Balancing strategy 3CaCl2(aq) + 2H3PO4(aq) Ca3(PO4)2(s) + 6HCl(aq)
red, blue, green … in that order!

10. Let’s try these… ___ V2O5 + ___ CaS  ___ CaO + ___ V2S5
___ Mn(NO2)2 + ___ BeCl2  ___ Be(NO2)2 + ___ MnCl2
___ AgBr + ___ GaPO4  ___ Ag3PO4 + ___ GaBr3
___ H2SO4 + ___ B(OH)3  __ B2(SO4)3 + ___ H2O
___ S8 + ___ O2  ___ SO2
10) ___ Fe + ___ AgNO3  ___ Fe(NO3)2 + ___ Ag

11. ___ AgBr + ___ GaPO4  ___ Ag3PO4 + ___ GaBr3

12. ___ H2SO4 + ___ B(OH)3  __ B2(SO4)3 + ___ H2O

13. ___ Fe + ___ AgNO3  ___ Fe(NO3)2 + ___ Ag

14. Balancing equations
We do it because of the law of conservation of mass
Atoms are not created in chemical reactions but new compounds are

15. Be familiar with the reactivity series of metals – will some single replacement reactions proceed?

16. Will these reactions proceed?
____ Ca + ____ Na2SO4 
____ Pb + ____ Fe(NO3)3 

17. Will these reactions proceed?
____ Ca + ____ Na2SO4 
____ Pb + ____ Fe(NO3)3 
These reactions will only occur if the pure element on the reactant side of the equation is higher on the activity series than the element it replaces.
These reactions will not proceed!

18. Be familiar with the characteristics of all types of reactions:
Combination
Decomposition
Single replacement
may or may not proceed
Double replacement
Either an aqueous solution OR a chemical reaction will occur
Combustion
Hydrocarbons + O2 yields CO2 + H2O

19. ____ NaBr + ____ H3PO4  ____ Na3PO4 + ____ HBr
Type of reaction: ____________________
____ Ca(OH)2 + ____ Al2(SO4)3  ____ CaSO4 + ____ Al(OH)3
____ Mg + ____ Fe2O3  ____ Fe + ____ MgO
____ C2H4 + ____ O2  ____ CO2 + ____ H2O
____ PbSO4  ____ PbSO3 + ____ O2

20. ____ NaBr + ____ H3PO4  ____ Na3PO4 + ____ HBr
Type of reaction: ____________________
____ Ca(OH)2 + ____ Al2(SO4)3  ____ CaSO4 + ____ Al(OH)3
____ Mg + ____ Fe2O3  ____ Fe + ____ MgO

21. ____ Ca(OH)2 + ____ Al2(SO4)3  ____ CaSO4 + ____ Al(OH)3

22. Be familiar with diatomic atoms
H2, O2, Cl2, N2, etc.
These are not ionic; they are molecular
There is no charge
They can be reactants or products
They can be the products in net ionic reactions

24. Understand the solubility rules
These will tell you whether you have a precipitate or not
This is essential in writing net ionic reactions

25. Understand net ionic equations
There is no net ionic reaction unless you have a solid, liquid or gas formed
Otherwise, all you have is a bunch of ions in an aqueous solution
These are characteristic of single and double replacement reactions

26. Understand combustion reactions
O2 is a reactant
CO2 and H2O are products
Know how to balance these…sometimes the coefficients are quite large