Question

Lab: Classifying Reactions

Answer 1

1.Synthesis reactions
< Two or more reactants combine to make 1 new product.
2.Decomposition reactions
A single reactant breaks down to form 2 or more products.
3.Single-replacement reactions
A single element replaces a similar element of an adjacent reactant compound.
4.Double-replacement reactions
Two ionic compounds exchange ions, producing 2 new ionic compounds.
5.Combustion reactions
A single element or compound combines with oxygen gas releasing energy. This rapid oxidation is called burning.
6. Double Replacement or (Metathesis) Reactions
When you see two binary ionic compounds (including acids), the compounds switch partners to form two new compounds. The driving force and product is either a gas, a precipitate, or a weak electrolyte.
7. redOx (Oxidation - Reduction) Reactions
Memorize the common strong oxidizers, generally ions with lots of oxygen, MnO4-, Cr2O72-, IO3-, etc
8. complex Ion Formation
These are usually formed from a transition metal surrounded by ligands (polar molecules or negative ions). As a "rule of thumb" you place twice the number of ligands around an ion as the charge on the ion... example: the dark blue Cu(NH3)42+ (ammonia is used as a test for Cu2+ ions), and Ag(NH3)2
Etc.

Answer 2

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