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  Reaction Classification Homework Help - K-12 Grade Level, College Level Chemistry

Introduction of Reaction Classification

There are five common types of reactions and two that are special cases of the following

1.      Decomposition

2.      Synthesis

3.      Double displacement

4.      Single displacement

5.      Combustion

Decomposition

  • Decomposition = one compound → two (or more pieces).

AB → A + B

  • Pieces can be the elements or simpler compounds

              i.      Element examples:

1.      HgO → Hg + O2

2.      H2O → H2 + O2

3.      MgCl2 → Mg + Cl2

4.      FeS → Fe + S

              ii.      Simpler compound examples

1.      CaCO3 → CaO + CO2

2.      Na2CO3 → Na2O + CO2

3.      KClO3 → KCl + O2

4.      Ba(ClO3)2 → BaCl2 + O2

              iii.      Acids and bases

1.      (Base) Ca(OH)2 → CaO + H2O

2.      (Base) NaOH → Na2O + H2O

3.      (Acid) HNO3 → N2O5 + H2O

4.      (Acid) H3PO4 → P2O5 + H2O

  • Note that how, in each example we consider so far, there is only one substance on left-hand (reactant) side. This is always case in a decomposition reaction.

Single Displacement

  • One element replaces another element in a compound in Single displacement,.
  • In single displacement one reactant is always an element. It does not matter if element is written first or second on the reactant side. And Other than that reactant all the reactant will be a compound.
  • Two possibilities:

1.      Cations switch.

AX + Y ---> YX + A

§ Element Y replaced A (in the compound AX) to form a new compound YX and the free element A. Remember that the A and Y are both cations (positively-charged ions) in this example.

§ Examples

1.      Cu + AgNO3 → Ag + Cu(NO3)2

2.      Fe + Cu(NO3)2 → Fe(NO3)2 + Cu

3.      Ca + H2O → Ca(OH)2 + H2

4.      Zn + HCl → ZnCl2 + H2

2. Anions switch places:

A + XY → XA + Y

§ Element A has replaced Y (in the compound XY) to form a new compound XA and the free element Y. Remember that the A and Y are both anions (negatively-charged ions) in this example.

§ Examples

1.      Cl2 + NaBr → NaCl + Br2

2.      Br2 + KI → KBr + I2

Double Displacement

§ Double displacement, the cations and anions of two different compounds switch places.

§ Both reactants are compounds, each with a cation part and an anion part.

§ Diatomic elements do not count; they are included in the single displacement category.

AB + XY → AY + XB

§ A and X are the cations (positively-charged ions) in this instance, with B and Y being the anions (negatively-charged ions).

§ Examples:

1.      KOH + H2SO4 → K2SO4 + H2O

2.      FeS + HCl → FeCl2 + H2S

3.      NaCl + H2SO4 → Na2SO4 + HCl

4.      AgNO3 + NaCl → AgCl + NaNO3

If you look at any organic chemistry book you will come to know that what appears to be a very large frequently intimidating, number of reactions. These are "tools" of a chemist and to use these tools effectively and efficiently, we should arrange them in a sensible manner and look for patterns of reactivity that permit us make plausible predictions. Generally these reactions occur at special sites of reactivity that are known as the functional groups and these constitute one organizational scheme that helps us catalog and remember reactions. 

Finally, the best way to get proficiency in organic chemistry is to understand how reactions take place and to recognize the several factors that affect their course.

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