List three oxoacids of halogens in their different oxidation state.

The oxoacids of halogens exist in four different forms. They are hypohalous acid, halous acid, halic acid and perhalic acid. These are not stable to same extent. Most of these exists only in aqueous solution or in the for of their salts. The three oxoacids of halogens in their different oxidation state are as follows. 1. Hypochlorous acid HOCl with oxidation state of chlorine + 1 . 2. Chlorous acid HOClO with oxidation state of chlorine + 3 . 3. Chloric acid HOClO 2 with oxidation state of chlorine + 5 .

Explain the thermal stability of hydrides of gr - 15 elements.

The thermal stability of group - 15 hydrides decreases sharply in going from NH 3 to BiH 3 . SbH 3 and BiH 3 are thermally unstable. As we go down the group, the M - H bond length increases. Therefore, the M - H bond enthalpy decreases down the group. As a result, the thermal stability of MH 3 type of hydrides decreases in going from top to bottom in the group.

Draw the structure of XeF 2 , XeF 4 and XeOF 4 .

XeF 2 has trigonal bipyramidal structure. Xenon involves sp 3 d hybridisation. In XeF 2 three-lone-pairs are at three equatorial positions and two unpaired electrons from two σ -bond with F -atom. Trigonal bipyramidal geometry of XeF 2 XeF 4 has the square planar geometry. Xenon involves sp 3 d 2 hybridisation of xenon which adopts octahedral geometry where two positions are occupied by lone pairs. Square planar geometry of XeF 4 XeOF 4 has square pyramidal structure which involves sp 3 d 2 hybridisation of xenon. In xenon oxytetrafluoride, one position is occupied by a lone pair. Square pyramidal geometry of XeOF 4

How are XeF 6 and XeO 3 prepared?

XeF 6 can be prepared by heating a mixture of xenon and fluorine in the ratio 1 : 20 in a nickel vessel at 600 K under 60 - 70 bar pressure. Xe g Xenon + 3 F 2 g Fluorine → 60 - 70 bar 600 K XeF 6 s Xenon hexafluoride XeO 3 can be prepared by the hydrolysis of XeF 4 and XeF 6 under controlled pH of the medium in which reaction is taking place. The reactions are : 6 XeF 4 Xenon tetrafluoride + 12 H 2 O Water → 4 Xe Xenon + 2 XeO 3 Xenon trioxide + 24 HF Hydrogen fluoride + 3 O 2 Oxygen XeF 6 Xenon hexafluoride + 3 H 2 O Water → XeO 3 Xenon trioxide + 6 HF Hydrogen fluoride

How is nitric acid prepared by Ostwald’s process? Give the reaction involved.

On industrial scale, nitric acid can be prepared by the catalytic oxidation of ammonia. This process of manufacturing nitric acid is called Ostwald's process. In this process, conversion of ammonia to nitric acid is done through the following steps: Step 1: Oxidation of ammonia to nitric acid- Ammonia is oxidised by air in the presence of platinum catalyst at 800 ° C to give nitric oxide. 4 NH 3 g + 5 O 2 g ⇌ 800 ° C , 6 - 7 atm Pt + Rh ( 9 : 1 ) 4 NO g + 6 H 2 O Step 2: Oxidation of nitric oxide to nitrogen dioxide- The nitric oxide is oxidised to nitrogen dioxide by air at temperature below 100 ° C . 2 NO + O 2 → < 100 ° C 2 NO 2 Step 3: Formation of nitric acid- Nitrogen dioxide is then converted to nitric acid by absorbing nitrogen dioxide in water in the presence of air. 4 NO 2 + 2 H 2 O + O 2 → 4 HNO 3

H 2 O is liquid where as H 2 S is gas at room temperature. Give reason.

H 2 O and H 2 S are hydrides of group 16 elements. Due to the polar character of the O - H bond, water molecules form intermolecular hydrogen bond. Hence, water exist in the liquid state. But H 2 S do not form intermolecular hydrogen bond. The only force acting between the molecules of H 2 S is van der Waals' forces. Hence, it exists in the gaseous state.

List three oxoacids of sulphur in different oxidation states and draw their structures.

The three oxoacids of sulphur are sulphurous acid, sulphuric acid and dithionic acid. In sulphurous acid H 2 SO 3 , sulphur exist in + 4 oxidation state. Its structure is as follows In sulphuric acid H 2 SO 4 , sulphur exist in + 6 oxidation state. Its structure is as follows In dithionic acid H 2 S 2 O 6 , sulphur exist + 5 oxidation state. Its structure is as follows

Draw the structure of IF 7 , BrF 5 and ClF 5 and mention the type of hybridisation and geometry in each case.

The interhalogen compounds are covalent in nature. IF 7 is sp 3 d 3 hybridised and its structure is pentagonal bipyramidal. The BrF 5 and ClF 5 both are sp 3 d 2 hybridised. They show square pyramidal structure. Structure of BrF 5 Structure of ClF 5

E M B I B E

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter -1 - The p-Block Elements>Nagaland Board-2018>Q 6

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12th Nagaland Board

IMPORTANT

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Give reason: Electron gain enthalpy of chlorine is higher than fluorine.

Chapter-Wise 3D Chemistry Videos from Embibe Experts EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY

04 min 46 sec

Oxoacids of Halogens

Halogens generally form four kinds of oxoacids, namely, hypohalous acids, halous acids, halic acids and perhalic acids. Let’s delve into the world of oxoacids.

05 min 55 sec

Chemical Properties of Halogens

The halogens are known as reactive elements due to their high electronegativity, which is due to their highly effective nuclear charge. Learn about the react...

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Properties of Group 17 Elements

The Group 17 elements are known to be highly reactive elements. They form halides with most of the metals and non-metals. Let’s explore a few of these proper...

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