They both come up with two different compounds/elements then the original compound/element.
decomposition
I believe there are 6... (I'm a chemistry major) Combustion, synthesis, decomposition, single displacement, double displacement, and acid-base.
Neutralization, Double decomposition, Alkylation, Counterion Exchange, Precipitation are all different types of double displacement reactions.
The three basic types of reaction mechanisms are substitution, elimination, and addition. In a substitution reaction, one functional group is replaced by another. In an elimination reaction, two groups are removed from a molecule to form a new double bond or ring. In an addition reaction, two or more reactants combine to form a single product.
Synthesis: 2H2 + O2 -> 2H2O Decomposition: 2H2O -> 2H2 + O2 Single-displacement: Zn + 2HCl -> ZnCl2 + H2 Double displacement: AgNO3 + NaCl -> AgCl + NaNO3
Reactions occur when reactant molecules collide with sufficient energy and proper orientation to break existing bonds and form new ones. This leads to the creation of products with different properties from the original reactants. The speed and likelihood of a reaction happening depend on factors like temperature, concentration, and presence of a catalyst.
Thermal decomposition. MgCO3(s) ==heat==> MgO + CO2
Single displacement reaction and a double displacement reaction are redox reactions. apex- false
If you mean Zn + H2SO4 --> ZnSO4 + H2, then no, it is not a decomposition reaction. In decomposition reactions one reactant is broken down into two or more simpler substances. For example, the electrolysis of water, 2H2O --> 2H2 + O2 is a decomposition reaction. The reaction referred to in your question is a double replacement (displacement) reaction. I apologize that the subscripts are not working at this time.
A single displacement reaction is always a redox reaction, buta double displacement reaction is not a redox reaction.
Synthesis, Decomposition, Single Displacement, Double Displacement
The double displacement reaction is not related to hydrogen bonding.