Chapter 6 & 7
Balancing Equations
-each element on each side must be the same and have the same number of elements on each side.
-there are 2 parts of an equation
-the Reactant: this is the left side that you start with
-the Product: this is the end equation. Literally, the product
States of Matter
Solid- S
Liquid- L
Gas- G
Aqueous- Ag (Soluble in water)
States of Matter
1. Most Nitrates (NO3-) are soluble (aq).
2. Most salts of Na+, K+, and NH4+ are soluble.
3. Most Chloride salts are soluble, except Ag+, Pb^2+, and Hg^2+.
4. Most sulfate salts are soluble, except Ba^2+, Pb^2+, and Ca^2+.
5. Most Hydroxide (OH-) compounds are insoluble except ions in rule # 2 & Ba/Ca.
6. Most sulfides, carbonates, and phosphates are insoluble except ions in rule #2.
Writing Chemical Equations
- 1. Molecular equation
- No charges are showing. Only compounds
- AgNO3 (aq)+ NaCl(aq) -> AgCl(s) + NaNO3(aq)
- 2. Complete ionic equations
- All (aq) compounds will disassociate “break” into their ions
- Ag+(aq) +NO3- (aq)+ Na+(aq) +Cl-(aq) -> AgCl(s) + Na+ (aq) +NO3-(aq)
- 3. Net ionic equation
- Find the solid and then write the ions in the reactants that makes up the product
- Ag+(aq) + Cl-(aq)-> AgCl(s)
- 1. Molecular equation
- No charges are showing. Only compounds
- AgNO3 (aq)+ NaCl(aq) -> AgCl(s) + NaNO3(aq)
- 2. Complete ionic equations
- All (aq) compounds will disassociate “break” into their ions
- Ag+(aq) +NO3- (aq)+ Na+(aq) +Cl-(aq) -> AgCl(s) + Na+ (aq) +NO3-(aq)
- 3. Net ionic equation
- Find the solid and then write the ions in the reactants that makes up the product
- Ag+(aq) + Cl-(aq)-> AgCl(s)
Types of Re