Account for the following: (a) Sulphurous acid is a reducing agent (b)Fluorine forms only one oxoacid (c) Boiling point of noble gases increases from He to Rn.

boiling points of noble gases increase from helium to Neon (T/F)

Give reasons for the following: (i) Binary compounds of oxygen and fluorine are called fluorides. (ii) Fluorine forms only one oxoacid HOF. (iii) Noble gases have very low melting and boiling points.

Which factor is most responsible for the increase in boiling points of noble gases from He to Xe?

Which factor is most responsible for the increase in boiling points of noble gases from He to Xe?

(a) Account for the following : (i) Ozone is thermodynamically unstable. (ii) Solid PCl_(5) is ionic in nature. (iii) Fluorine forms only one oxoacid HOF.

Account for the follwing : (i) Bi(v) is a stronger oxidizing agent then Sb(v). (ii) N-N single bond is weaker then P - P Single bond. (iii) Noble gases have very low boiling points.

Answer the following with relevant reason. (i)Xenon has closed shell configuration but is known to give compounds with fluorine. (ii)The boiling points of noble gases increase with increase in atomic number. (iii)Why helium and neon do not form clathrate compounds with quinol ?

Account for the following observations (a) AlCl_(3) is a Lewis acid (b) Though fluorine is more electronegative than chlorine yet BF_(3) is a weaker Lewis acid than BCI_(3) (c) PbO_(2) is a stronger oxidising agent than SnO_(2) (d) The +1 oxidation state of thallium is more stable than its +3 state.

(a) Account for the following : (i) Acidic character increases from HF to HI. (ii) There is a large difference between the melting and boiling points of oxygen and sulphur. (iii) Nitrogen does not form pentahalide. (b) Draw the structures of the following : (i) CIF_(3) (ii) XeF_(4)

Give at least one example to explain the following properties. (a) Sulphuric acid is a dibasic acid. (b) Sulphuric acid is a dehydrating agent. (c) Sulphuric acid is an oxidising agent.