Question | Answer |
Combination (Synthesis) reactions | 2 simpler substances make a more complex compound |
Chemical Reactions | 1. Combination
2. Decomposition
3. Single replacement
4. Double replacement
5. Neutralization
6. Combustion
7. Reduction- oxidation |
Metal oxide Reaction | Metal heated w oxygen gas. Ex. magnesium oxide |
Non metal + O Reaction | nonmetal + O = nonmetal oxide
S + O = Sulfur dioxide (Binary Molecular Comp) |
Metal + nonmetal Reaction | Make ionic compounds.Ex. sodium chloride
Fixed charge (predictable)
Transition (not predictable) |
Decomposition | single compound breaks into simpler substances.
Need heat or light.
Ionic with O = metal & O |
Carbonate decompositions | Metal hydrogen carbonates = metal carbonate + water + carbon dioxide
Metal carbonates = metal oxide + carbon dioxide |
Activity Series | Sequence of metals arranged accorging to their ability to undergo a reaction.
(First the most reactive)
A metal that displaces another metal because it is more active. (Better opponent).
Ex metal that displaces another metal in a replacement reaction |
Activity Series list | Li, K, Ba, Sr, Ca, Na, Mg, ,Al, Mn, Zn, Fe, Cd, Co, Ni, Sn, Pb, (H), Cu, Ag, Hg, Au |
Single replacement reaction | More active metal takes the place of a less active metal in a compound.
If metal is before another metal in the activity series= displacement will occur |
Aqueous Acid Displacement | Precede H = metal will react with acid
Follow H= NR |
Active Metals | Metals that are active enough to react directly with water to make metal hydoxide + hydrogen gas
Li, Na, K, Rb, Cs, Ca, Sr, Ba
Li, |
Solubility Rules (Only solubles in water) | Compounds that have:
1. alkali metal ions (Li, Na, K, ammonium ion)
2. acetate ion
3. nitrate ion
4. halide ions (Cl, Br, I); no helide compounds (Ag,mercury I, Pb II)
5. Sulfate ion; no sulfate compounds with (Sr, Ba, Pb II) |
Double replacement reaction | 2 ionic compounds aq that switch anions and make 2 new compounds
If 1 of the products is is insoluble a predictable ppt will form (In this case NR) |
Precipitation reaction | This happens in double displacement reactions
if 1 of the products is insoluble in water |
Total Ionic Equation | Expresses strong acids,bases, and soluble ionic compounds as ions.
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) + Na+(aq) + NO3-(aq) |
Ionization | lets us see ionic solutions more accurately by showing strong electrolytes in their ionized form |
Net Ionic Equation | Shows only the components involved with the reaction |
Spectator Ions | They appear in both sides of the equation
They don't participate in the overall reaction |
Writing Net Ionic equation | 1. Complete and balance the nonionized equation
2. Convert the nonionized equation into the total ionic equation (electrolytes in ionized form and weak electrolytes, water and gases in nonionized form)
3. Cancell all spectators (NR if all gone) |
Neutralization Reaction | Reaction of an acid and a base
Hx + BOH = Bx (salt)+ water
[Products salt and water] |
Acid | substance that makes H+ ions in water (protons)Ex. Hydrochloric acid, nitric acid, sulfuric acid |
Base | substance that makes OH- ions in water
Ex. sodium hydroxide, potassium hydroxide |
Salt | ionic compound produced by an acid-base reaction |
Combustion reactions | involve oxygen and make energy (heat) so that a flame results |
Oxidation Reduction (Redox reaction) | Transfer of e- from one substance to another.
Ex. reactions of metal + nonmetal (synthesis)
Combustion and single replacement reactions
Total e- lost = total e- gained |
How Oxidation-Reduction reactions work | 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)
Iron loses electrons and is oxidized.
Fe → Fe3+ + 3 e-
Oxygen gains electrons and is reduced.
O2 + 4 e- → 2 O2- |
Oxidation Number | how many e- have been lost or gained |
7 Rules for oxidation numbers | 1. mt or nonmt in free state= 0
2. monoat I= its charge
3. Hydrogen I= +1
4. Oxygen I= -2
5. Molecular= more electronegative element has a negative charge equal to its charge as anion
6. Ionic comp: sum of ox #s = 0
7. Poly I =sum of ox #s = poly ch |
Oxidized | Losing electrons |
Reduced | Gaining electrons |
oxidation agent | substance that causes oxidation by accepting e-. The oxidizing agent is reduced |
Reducing agent | substance that causes reduciton by donating e-. The reducing agent is oxidized |
Classification Summary | Chemical Reactions
~Reduction-oxidation Reactions
Synthesis (Combination)
Decomposition
Single Replacement
Combustion
~Double Replacement
Precipitation Reactions
Acid-Base (Neutralization) |
Molecular equation | shows the complete formulas of all reactants and products. |