Types of Chemical Reactions

1. Synthesis Reactions A synthesis reaction occurs when two or more simple substances combine to produce a more complex substance. AKA: Combination reaction. The general equation for a synthesis is: A + B  AB HINT: If there is only one product – it is likely a synthesis. Examples of Synthesis Reactions CO 2 + H 2 O  H 2 CO 3 4Fe + 3O 2  2Fe 2 O 3 Li 2 O + H 2 O  2LiOH

2. Decomposition Reactions A decomposition reaction occurs when a complex substance is broken down into two or more simpler substances. Heat is often used to aid in decomposition reactions – these reactions that employ heat are called thermal decompositions. Decompositions and synthesis reactions are opposites. The general equation for a decomposition reaction is: AB  A + B HINT: If there is only one reactant – it is likely a decomposition reaction. Examples of Decomposition Reactions: NH 4 NO 3  N 2 O + 2H 2 O Ca(OH) 2  CaO + H 2 O 2H 2 O 2  2H 2 O + O 2

3. Single Displacements A single displacement reaction occurs when a single element takes the place of one of the elements in a compound. AKA: Single Replacement The general equation for a single displacement reaction is: AB + Z  ZB + A Metals displace metals while nonmetals displace nonmetals. HINT: The single mysterious loner moves into town and breaks up the happy couple! Examples of Single Displacement Reactions Fe + CuSO 4  FeSO 4 + Cu 2K + MgO  K 2 O + Mg 2CuF + Ba  BaF 2 + 2Cu

Not So Fast There… The lone element doesn’t always break up the couple! We can use a tool called the activity series to predict if the compound will stay together or break up. The activity series is a list of metals and hydrogen that are arranged in order of reactivity. Li K Ba Ca Na Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au The rule is that you can only be displaced by an element that is to the left of you. This makes Lithium the strongest and Gold the weakest. There is also a halogen activity series – it is used to predict reactions with halides. F Cl Br I

Using the Activity Series You can use the activity series in three ways: 1)Straight forward Single Displacements 2)Reactions with Acids 3)Reactions with Water Straight Forward Single Displacements –Use the rule of “whoever is more to the left wins” to see if there is a reaction or not. Reactions with Acids –Acids contain hydrogen (positive like the metals). If you are to the left of hydrogen – you react and take its place – if you are to the right – there is no reaction. Reactions with Water –Only the first five elements (Li K Ba Ca Na) will react with water. It will form a hydroxide and hydrogen gas.

4. Double Displacements A double displacement reaction always involves two ionic compounds that switch partners with each other. Again, positive ions switch with positive ions (and/or vice-versa). The general equation for a double displacement reaction is: AB + XY  AY + XB HINT: Two couples switch partners at the dance. Examples of Double Displacement Reactions: Pb(NO 3 ) 2 + 2KI  PbI 2 + 2KNO 3 Na 2 SO 3 + 2HCl  2NaCl + H 2 SO 3 2NaOH + H 2 SO 4  2H 2 O + Na 2 SO 4

Not So Fast There…Again! There are three outcomes for a double displacement reaction: 1)Precipitate – solid formed from two liquids. Use the solubility rules. 2)Gas – some compounds form products that break down further into gases. 3)Water – results from a neutralization between an acid and a base.

5. Combustion Reaction A combustion reaction occurs when a substance (the “fuel”) reacts very rapidly with oxygen to form carbon dioxide and water. Combustion reactions release a good deal of energy in a very short period of time. The general equation for a combustion reaction is: Fuel + O 2  CO 2 + H 2 O HINT: Something combines with oxygen to produce carbon dioxide and water.

Incomplete Combustion If a combustion occurs at a lower temperature, it may result in an incomplete combustion. The products of an incomplete combustion are water, carbon dioxide, carbon monoxide and carbon (a solid residue). The general equation is: Fuel + O 2  H 2 O + CO 2 + CO + C

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