1. Reaction Type # 2 – Single Replacement

2. Single Replacement Reactions

3. Single Replacement Reactions: Characteristics:
Atom (s) of a lone element replace the atom (s) of an element in a compound
Metals replace metals (or cations replace cations)
Non-metals replace non-metals (or anions replace anions)

4. Single Replacement Reactions: Characteristics:
Metal Cation Replacement:
For the reaction:
A + BC  B + AC
A and B are cations
A “replaces” B in the compound

5. Single Replacement Reactions: Characteristics:
Non-metal Anion Replacement:
For the reaction:
D + EF  ED + F
D & F are anions
D “replaces” F in the compound
Non metal replacements usually involve halogens

6. Restrictions on Single Replacement Reactions
Activity Series of Metals:
A characteristic of metals and halogens referring to their reactivity
Determines whether or not a single replacement reaction will occur or not
Activity Series for Non-Metals:
Non-metals (Halogens) : as you move down the group on the periodic table activity decreases
Works the same way as the metals series, its just found on the periodic table, not on a separate table

7. Restrictions on Single Replacement Reactions
A single replacement reaction WILL NOT OCCUR if the reactivity of the pure element reactant is less than that of the compound reactant
If the lone element is BELOW the one in the compound on the activity series = no reaction
i.e.:
Sn (s) + NaNO3 (aq) 
no reaction b/c tin is less reactive than sodium

8. Restrictions on Single Replacement Reactions
A single replacement reaction WILL OCCUR if the reactivity of the pure element reactant is greater than that of the compound reactant
If the lone element is ABOVE the one in the compound on the activity series = reaction
i.e.:
Cu (s) + 2AgNO3 (aq)  Cu(NO3)2 (aq) + 2Ag (s)
Reaction occurs because the reactivity of copper is higher than silver

9. Identifying Single Replacement Reactions
Single replacement reactions ALWAYS have 1 lone element and 1 compound on the reactants side and the products side
Reactants will always be:
1 lone element + 1 compound
Products will always be:

10. States for Single Replacement Reactions
Lone elements:
Look at the periodic table to determine the states of the lone elements
Compounds – Reactant Side:
Ionic compounds MUST be in solution (aqueous) in order to split the ions up for an exchange
Compounds – Product Side:
Check the solubility table to determine if they stay aqueous, or precipitate out as a solid
Remember, if the product is water, it will be a pure liquid

11. Examples 1) Al + H2SO4  ____ + ________ 2) Cl2 + KI  ____ + ________
For each reaction:
Predict the products
Re-write the balanced equation underneath
Provide the states of all of the chemical involved
Provide the names for all of the chemicals involved
1) Al + H2SO4  ____ + ________
2) Cl2 + KI  ____ + ________
3) Li + HOH  ____ + ________
4) Ca + AlPO4  ____ + ________
5) Fe2O3 + Ag  ____ + ________