The Sn compounds with oxidation state of +4 are more stable than those of +2. The principal reactions of Sn exhibit the group valency of 4 & thus the O.N. of Sn & Pb in SnCl4 & PbCl2 are +4 & +2 respectively.

The dioxide may also be prepared by heating stannic acid or by heating tin metal in air at high temperatures. In the presence of air, stannous oxide burns to form the dioxide, or stannic oxide, SnO2, a white insoluble solid. Stannous oxide, SnO, a black insoluble powder, is obtained by heating stannous oxalate in the absence of air. The two hydroxides of tin, Sn(OH)2 and Sn(OH)4, are produced by adding a soluble hydroxide to solutions of stannous and stannic salts. Stannic sulphide, SnS2, is produced by passing hydrogen sulphide through a solution of stannic salt. Stannous sulphide, SnS, is yielded as a dark brown precipitate by the action of hydrogen sulphide on a solution of stannous chloride. In cold and very dilute nitric acid, tin dissolves to form stannous nitrate and ammonium nitrate in concentrated nitric acid, it produces metastannic acid, H2SnO3. It dissolves in hydrochloric acid to form stannous chloride, SnCl2, and in aqua regia to form stannic chloride, SnCl4, and it reacts with sodium hydroxide solution to form sodium stannite and hydrogen gas. Tin forms stannic acid, H2SnO4, when heated in air or oxygen at high temperatures. Tin, symbol Sn, metallic element that has been used by people since ancient times. pop corn tin cans dissolves in hydrochloric acid to form stannous chloride, sncl2, and in aqua regia to form stannic chloride, sncl4, and it reacts with sodium hydroxide solution to form sodium stannite and hydrogen gas

Dry HCl might work too, I think, instead of chlorine.

SnCl4 needs hot tin and dry chlorine, and you condense and collect the SnCl4 vapours. Sn + HCl = SnCl2 SnCl2 + HCl = SnCl4 (not balanced) For to get SnCl4 it is necessary to react the SnCl2 with chlorine. My inorganic textbooks tell me that Sn reacts with HCl to form SnCl2.

Sno2 core shell sncl4.5h2o