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Chemical Equations Review. CH 4 + 2 O 2 CO 2 + 2 H 2 O “ coefficients ”“ subscripts ” coefficients can be changed to achieve mass balance but subscripts are never changed to balance an equation Why? - PowerPoint PPT Presentation
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Chemical Equations ReviewCH4 + 2O2 CO2 + 2H2O
“coefficients” “subscripts”
coefficients can be changed to achieve mass balance but subscripts are never changed to balance an equation Why?
Because changing a subscript changes the compound entirely!!!
So how do we get subscripts?In ionic compounds you simply cross the ions charge
values.
Li + MgCl2 ???????
Single replacement reaction. Why?
Li is a metal, Mg is a metal, Cl is a nonmetal
Li+ replaces Mg2+ and combines with Cl-
The products are Mg + LiCl The balanced equation will be
2 Li + MgCl2 Mg + 2 LiCl
Balancing a Chemical Equation
• write formula for each reactant and product on the correct side of the “reaction arrow”
• count atoms of each element on both sides of arrow
• start with the compound which has the most complex formula
• add coefficients to chemical formulas to balance numbers of each atom
• trial and error begins...
What am I? Mg + HCl MgCl2 + H2
Single replacement
Na2CO3 + HCl NaCl + H2CO3
Double replacement
Cu + S Cu2S Synthesis
NaCl is soluble in water. Solid NaCl dissociates into Na+ and Cl- ions in aqueous solution:NaCl(s) Na+
(aq) + Cl-
(aq)
Pb(NO3)2 + 2NaI PbI2 + 2NaNO3
(aq) (aq) (s) (aq)
See solubility rules
Solubility Rules:
Net Ionic Equations
Balanced Chemical Equation:Pb(NO3)2(aq) + 2NaI(aq) PbI2(s) + 2NaNO3(aq)
“Complete Ionic” Equation:Pb2+
(aq) + 2NO3-(aq) + 2Na+
(aq)+ 2I-(aq) PbI2(s) + 2Na+
(aq) + 2NO3- (aq)
Cancel the “spectator ions” that appear on both sides of the arrow
Pb2+(aq) + 2NO3
-(aq) + 2Na+
(aq)+ 2I-(aq) PbI2(s) + 2Na+
(aq) + 2NO3- (aq)
“Net Ionic” Equation:
Pb2+(aq) + 2I-
(aq) PbI2(s)
For the exam: know how to use solubility rules to predict whether an ionic compound is insoluble or not
Net Ionic Equations Revisited:1) Write the (balanced!) molecular equation first
- Reaction products: swap cations and anions- Predict solubility (using Solubility rules)
2) Write the complete ionic equation next- (s) compounds don’t ionize- (aq) compounds do ionizeion subscripts in the molecular equation become
coefficients in the complete ionic equation!
3) Write the net ionic equation next- cancel spectator ions
The net ionic equation is a “simplified” form of the complete ionic equation
Example: Problem
Ba(NO3)2 + NiSO4
Balanced Molecular Equation:
Ba(NO3)2 + NiSO4 Ni(NO3)2 + BaSO4
Balanced Molecular Equation:
Example: Problem
Ba(NO3)2(aq)+ NiSO4(aq) Ni(NO3)2 (aq)+ BaSO4(s)
Balanced Molecular Equation:
Example: Problem
Ba2+(aq) + 2NO3
-(aq) + Ni2+
(aq) + SO42-
(aq)
Ni2+(aq) + 2NO3
-(aq) + BaSO4 (s)
Balanced Molecular Equation:
Complete Ionic Equation:
Example: Problem
Ba(NO3)2(aq)+ NiSO4(aq) Ni(NO3)2 (aq)+ BaSO4(s)
Ba2+(aq) + 2NO3
-(aq) + Ni2+
(aq) + SO42-
(aq)
Ni2+(aq) + 2NO3
-(aq) + BaSO4 (s)
Balanced Molecular Equation:
Complete Ionic Equation:
Example: Problem
Ba(NO3)2(aq)+ NiSO4(aq) Ni(NO3)2 (aq)+ BaSO4(s)
Ba2+(aq) + 2NO3
-(aq) + Ni2+
(aq) + SO42-
(aq)
Ni2+(aq) + 2NO3
-(aq) + BaSO4 (s)
Balanced Molecular Equation:
Complete Ionic Equation:
Example: Problem
Ba(NO3)2(aq)+ NiSO4(aq) Ni(NO3)2 (aq)+ BaSO4(s)
Net Ionic Equation:Ba2+
(aq) + SO42-
(aq) BaSO4 (s)
What is the Net Ionic Equation for the reaction: HCl(aq) + NaOH(aq) ?
HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq)
H+(aq) + -OH(aq) H2O(l)