Demonstration Different Types Of Reactions

Combination Reaction

A combination reaction is where two reactants react together to form one product which is an ionic compound.

The combination between Magnesium (Mg2+) and Oxygen (O2-) will produce Magnesium Oxide
Mg2+ + O2- -------------> MgO 

https://edu.glogster.com/glog/chemical-reaction/1prkmxx63bh?=glogpedia-source

Decomposition Reaction

A decomposition experiment is where a single chemical compound breaks down into two or more single produces or simpler compounds.

https://www.mindmeister.com/457897743/chemical-reaction-types

Metal Carbonate + Heat = Metal Oxide + CO2

Copper Cabonate + Hear = Copper Oxide + CO2

CUCO3 -------> CUO + CO2

Substance: Copper Carbonate = CuCO3

This is called thermal decomposition.

Thermal decomposition is an example of an endothermic reaction, a reaction that gains energy from surroundings.

Displacement Reactions

In a displacement reaction...

a more reactive metal displaces (take over/force out) a less reactive metal.

https://byjus.com/chemistry/displacement-reactions/

Exchange Reaction

Exchange reactions are where the cations and anions that were partners in the reactants they are exchange in the product.

AB+CD > AD + BC

Stability Rules

The following are the solubility rules for common ionic solids. If there two rules appear to contradict each other, the preceding rule takes precedence.

1. Salts containing Group I elements (Li+, Na+, K+, Cs+, Rb+) are soluble . There are few exceptions to this rule. Salts containing the ammonium ion (NH4+) are also soluble. 
2. Salts containing nitrate ion (NO3-) are generally soluble. 
3. Salts containing Cl -, Br -, or I - are generally soluble. Important exceptions to this rule are halide salts of Ag+, Pb2+, and (Hg2)2+. Thus, AgCl, PbBr2, and Hg2Cl2 are insoluble. 
4. Most silver salts are insoluble. AgNO3 and Ag(C2H3O2) are common soluble salts of silver; virtually all others are insoluble. 
5. Most sulfate salts are soluble. Important exceptions to this rule include CaSO4, BaSO4, PbSO4, Ag2SO4 and SrSO4 . 
6. Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al3+ are insoluble. Thus, Fe(OH)3, Al(OH)3, Co(OH)2 are not soluble. 
7. Most sulfides of transition metals are highly insoluble, including CdS, FeS, ZnS, and Ag2S. Arsenic, antimony, bismuth, and lead sulfides are also insoluble. 
8. Carbonates are frequently insoluble. Group II carbonates (CaCO3, SrCO3, and BaCO​3) are insoluble, as are FeCO3 and PbCO3. 
9. Chromates are frequently insoluble. Examples include PbCrO4 and BaCrO4.
10. Phosphates such as Ca3(PO4)2 and Ag3PO4 are frequently insoluble.
11. Fluorides such as BaF2, MgF2, and PbF2 are frequently insoluble.

https://chem.libretexts.org/Textbook_Maps/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Equilibria/Solubilty/Solubility_Rules

Soluble = Dissolves

Insoluble = Doesn't Dissolve (solid in a solution)

Example : 

Sodium Hydroxide was reacted with silver nitrate. An exchange of ions occurred. Sodium nitrate was formed. Rule 1 says that all nitrates are soluble. This means that it won't form a solid. 

Silver Hydroxide was also formed during this exchange reaction. Rule 6 says that all hydroxides are insoluble except sodium and potassium hydroxides. Because silver hydroxide is neither a sodium or potassium hydroxide this means that silver hydroxide is insoluble. That means a solid of AgOH was formed.