1) Explain whether Ch 3 OH is going to be soluble in water in terms of intermole

Question

1) Explain whether Ch3OH is going to be soluble in water in terms of intermolecular forces.

2) Interpret the difference in light intensity between the probe in acetic acid solution and in hydrochloric acid solution in terms of [ions].

3) Explain the difference in acidity of MgO dissolved in water and of P4O10 in water in terms of position of the element in the periodic table and bonding.

4)Interpret the difference in physical states of the 3 halogens Chlorine (gas), Bromine (liquid), and Iodine (solid) in terms of position in the periodic table, and London dispersion forces

Explanation / Answer

1. Yes CH3OH is soluble in water due to hydrogen bonding between methanol and water.

2.there is a light intensity difference between acetic acid solution HCl solution because acetate ion absorbs energy because of presence of conjugation and no scope of conjugation in HCL.

3. P4O10 forms acidic solution in water because P is a nonmetal and has higher electronegativity. Where as Mg is a metal and gives basic solution in water.

Chlorine is a gas because it is present in 3rd row and least vander waal attraction exist due to less no of electron than iodine and bromine. Where as bromine exist as liquid due to existance of vanderwaal interaction. Iodine exist as solid due to strong vanderwaal interactio among the three as it has large no of electrons being present in the 5th row.

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