Chapter 7 Flashcards
Physical state
(l) (g) (s)
Melcular style equation
Compounds are writing by their neutral chemical formula.
All reactants are specified in the physical state they appear in.
Arrow is used
The products are added after the arrow (including physical state)
Good place to start balancing
Metals
Double displacement
(AB+CD->AD+CB
Synthesis
A+B -> AB
Decomposition
AB->A+B
Single displacement
A+BC->AC+B
Molecular equation
Complete, neutral, and smallest form
Ionic equations
Metal and non metal
Shown
Kl(aq) -> K+(aq)+I-aq)
Shows charges
Complete ionic equation
Shows all ions explicitly
Combination of other two
2K+(aq) + 2I-(aq) + Pb2+(aq) + 2NO3-(aq) -> 2K+(aq) + 2NO3-(aq) + PbI2(s)
The net ionic
Complete ionic without spectator ions
Spectator ions
Ions that do not undergo chemical change
Precipitation reactions
Reactions that form a solid, called precipitate, made upon mixing two aqueous solutions.
Acid-base reactions (neutralization)
Acid + base =
Water + Salt
Gas evolution
Aqueous factions that form a gas and aqueous product
Intermediate product
In gas evolution reactions sometimes create an intermediate product that then decomposes into a gas because it is unstable.
If bubbles are involved, the reaction is
A gas evolution
Gas revolution intermediate reactions
Sulfides
Gas evolved
Intermediate: None
Gas evolved: H2S
2HCl(aq)+K2S(aq)-> H2S(g) + 2KCl(aq)
Gas revolution intermediate reactions
Carbonates and bicarbonates
Gas evolved
Intermediate product: H2CO3
Gas evolved: CO2
Example: 2HCl(aq)+K2CO3(aq)->H2O(l) +CO2(g) + 2KCl(aq)
Gas revolution intermediate reactions
Sulfites and bisulfites
Gas evolved
Intermediate product: H2SO3
Gas evolved: SO2
Example: 2HCl(aq) + K2SO3(aq)-> H2O(l) + SO2(g)+ KCl(aq)
Gas revolution intermediate reactions
Ammonium
Gas evolved
NH4OH
NH3
Example: NH4Cl(aq)+KOH(aq)-> H2O(l)+NH3(g) +KCl(aq)
O i l R i g
Oxidation is losing electrons
Redox is gaining electrons
What is needed to trigger a decomposition reaction?
1
2
3
Light
Heat
Electrical current
