Activity Series

We are going to ignore the second half for today And we will ignore the halogens for now Leaving a list of metals

This list has the most reactive metals on the top and the least reactive metals on the bottom. Meaning the elements in the top would rather be in a compound more then the elements on the bottom.

A single replacement reaction will only happen if the element by itself is higher on the list then the element in the compound. For example: Ni + KOH  Find Ni Find K Ni is lower then K so this will not react. We would write “No rxn” No rxn

Here is another example: Al + CuCl 2  Find Al Find Cu Al is higher then Cu so this can react. We can then write the products. What element will be by itself now? What will the compound look like? Balance Cu + AlCl 3

Here is another example: Mn + AgNO 3  Find Mn Find Ag Mn is higher then Ag so this can react. We can then write the products. What element will be by itself now? What will the compound look like? Mn will have a +2 charge In other problems it will be Mn(II) Balance Ag + Mn(NO 3 ) 2

Here is another example: Sn(IV) + NaCN  Find Sn Find Na Sn is lower then Na so this is no reaction No rxn

Practice Na + ZnSO 4  Cr(II) + Fe 2 O 3  Pb(II) + CaCO 3  Fe(III) + PbI 2  K + LiOH 

The halogen This works the same way with the halogens Example: Br 2 + NaCl  Bromine is below chlorine so its no reaction.

The halogen Example: F 2 + KI  Fluorine is above Iodine so this will react. What element will be by itself now? What will the compound look like? Balance

Practice F 2 + AlCl 3  I 2 + ZnCl 2  Cl 2 + FeBr 2 