Reaction Type # 2 – Single Replacement

Single Replacement Reactions

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)

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

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

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

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

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

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:

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

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  ____ + ________