In 

molecule, the hybridization of carbon 1, 2, 3 and 4 respectively, are:

The molecule is $$CH_2 = C = CH - CH_3$$, which is 1,2-butadiene (an allene derivative). We number the carbons from left to right as C1, C2, C3, and C4.

Carbon 1 ($$CH_2=$$): This carbon is double-bonded to C2 and has two hydrogen atoms. It has three regions of electron density (two C-H bonds and one C=C bond), so it is $$sp^2$$ hybridized.

Carbon 2 ($$=C=$$): This carbon is involved in two double bonds (one with C1 and one with C3). It has only two regions of electron density, so it is $$sp$$ hybridized. This is characteristic of the central carbon in an allene system.

Carbon 3 ($$=CH-$$): This carbon is double-bonded to C2 and single-bonded to C4 and one hydrogen. It has three regions of electron density, so it is $$sp^2$$ hybridized.

Carbon 4 ($$-CH_3$$): This carbon is single-bonded to C3 and three hydrogen atoms. It has four regions of electron density, so it is $$sp^3$$ hybridized.

The hybridizations are $$sp^2, sp, sp^2, sp^3$$ respectively, which matches Option (2).