A problem was found: does trichlorosilane react more violently with ethanol than tetrachlorosilane?
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In the previous discussion, we used anhydrous ethanol to absorb the distilled tetrachlorosilane vapor, and it was observed that the temperature of the anhydrous ethanol increased slightly during the absorption process. Today, we used anhydrous ethanol to absorb trichlorosilane vapor under the same conditions, and the temperature of the anhydrous ethanol increased significantly this time, with a considerable amount of heat being released. Is it because trichlorosilane reacts more vigorously with ethanol?
I’m wondering if it’s because silicon tetrachloride reacts with ethanol step by step, with the ethoxy group gradually replacing the chlorine atoms on silicon tetrachloride? When replacing the last chlorine atom, the spatial constraints make the reaction slower; whereas in silicon trichloride, the presence of a hydrogen atom allows the ethoxy group to replace the chlorine quite easily, so the reaction proceeds rapidly. SiCl4+CH3CH2OH=Si4
Reply to 2# *lihuagong: I think this is due to the different properties of tetrachlorosilane and trichlorosilane. Under the same conditions, trichlorosilane is more chemically reactive than tetrachlorosilane, as it reacts more vigorously with ethanol.
Reply to 3# Egu Ting: Is this causal relationship incorrect? Is trichloro more reactive than tetrachloro because it reacts more vigorously with ethanol? Hehe, it’s because they’re lively that their reactions are intense, right! So does anyone know why it’s lively?
Oh, I think silicon tetrachloride has a symmetric and stable structure, while silicon trichloride has an asymmetric structure, which is why it reacts easily with other substances.
Reply to 2# *lihuagong: Theoretically, the first chlorine atom can be easily removed; as the reaction proceeds, the steric hindrance caused by the ethoxy group leads to a reduction in the rate of the reaction.
Reply to 6# yuanyao9394: I think it’s the same as well.
Reply to 7# *lihuagong: If the reaction is exothermic, a cold water bath is required. I carried out the hydrolysis of monomethyltrichlorosilane in a cold water bath; the HCl present also plays a role here. However, I kept the flow rate very low, so the reaction remained under control