Download Pb(NO 3 ) - MorgansChemistry

Warm-up April 5th
Write the balanced chemical equation
for:
Balance each chemical equation

Ba(ClO3)2  BaCl2 + O2

Mg(NO3)2 + KCl  MgCl2 + KNO3
Types of
Reactions
A. Combustion

Hydrocarbon + oxygen  carbon dioxide
and water

CH4 + 2O2  CO2 + 2H2O

2C8H18 + 25O2  16CO2 + 18H2O
B. Synthesis


the combination of 2 or more substances
to form a compound
only one product
A + B  AB
B. Synthesis
H2 + Cl2  2 HCl
C. Decomposition


a compound breaks down into 2 or more
simpler substances
only one reactant
AB  A + B
C. Decomposition
2 H 2O  2 H 2 + O 2
D. Single Replacement

one element replaces another in a
compound


metal replaces metal (+)
nonmetal replaces nonmetal (-)
A + BC  B + AC
D. Single Replacement
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
E. Double Replacement


ions in two compounds “change partners”
cation of one compound combines with
anion of the other
AB + CD  AD + CB
E. Double Replacement
Pb(NO3)2 + K2CrO4  PbCrO4 + 2KNO3
Warm-up November 16th

Balance each chemical equation

Ba(ClO3)2  BaCl2 + O2

Mg(NO3)2 + KCl  MgCl2 + KNO3
Reactions in aqueous solutions



Many reactions happen in solution
Makes it so the ions separate so they can
interact.
Solids, liquids, and gases are not
separated, only aqueous
Complete ionic equations:
Every aqueous compound is written as separate
ions
 Solids, liquids and gases as whole compounds
MgCl2(aq) + PbSO4(aq) → MgSO4(aq) + PbCl2(s)
Complete net ionic equation:
Mg2+(aq) + Cl-(aq) + Pb2+(aq) + SO4(aq) →
Mg2+(aq) + SO4(aq) + PbCl2(s)

FeBr3(aq) + 3KOH(aq)  3KBr(aq) + Fe(OH)3(s)
Fe3+(aq)+ Br-(aq) + 3K+(aq) +3OH-(aq) →3K+(aq) +3Br-(aq) +
Fe(OH)3(s)
K+ and Br- do not change, they are spectator
ions
Fe3+(aq) +3OH-(aq) →Fe(OH)3(s)
This is what really happens in the reaction!
Net Ionic Equations




Shows only those particles that change
before and after.
Eliminate spectator ions
Needs to be balanced in terms of both
mass and charge
Fe3+(aq) +3 OH-(aq) →Fe(OH)3(s)
Write the Net Ionic Equation
for:
HCl (aq) + Ba(OH)2 (aq) → BaCl2(s) + HOH (l)
Al(s) + FeSO4(aq) → Al2(SO4)3(aq) + Fe(s)
K2CO3(aq) + MgI2(aq) →MgCO3(s) + KI(aq)
Predicting precipitates



Precipitate-Solid formed from aqueous
solution.
You can predict them if you know some
general rules for solubility.
Look at your Reference Tables!
Is it soluble?







LiBr
Ba(NO3)2
CaSO4
PbCl2
CaCO3
K2CO3
Cd(ClO3)2
Is there a reaction?




For double replacement- has to make gas,
solid or water.
Water from an acid- H+ and a
hydroxide- OH- makes HOH
Solids- from solubility rules
Exchange ions and see if something is
insoluble
Predict the products and write
the net ionic equations for each:

MgSO4 + NaOH →

H2SO4 + KOH →

K3PO4 + FeF3→