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Answer 1 · 2016-10-09T09:45:03

Do you speak of a redox reaction?

When aluminum chloride is formed, we conceive that aluminum metal is oxidized:

#Al(s) rarr Al^(3+) + 3e^-# #(i)#

And gaseous chlorine is reduced:

#1/2Cl_2(g) + e^(-) rarr Cl^-# #(ii)#

As with any chemical reaction, both MASS and CHARGE are conserved.

TO represent the formation of #"aluminum chloride"#, we simply add, #(i)+3xx(ii)#:

#Al(s) + 3/2Cl_2(g) rarr AlCl_3(s)#

And of course mass and charge have been conserved, as required.