Class 12th

7.33

Xe and F₂ combine under different conditions to produce XeF₂, XeF₄, XeF₆ as follows:

7.66

4NaCl + MnO₂ + 4H₂SO₄ MnCl₂ + 4NaHSO₄ + 2H₂O + Cl₂

Manganese (IV) oxide reacts with sodium chloride and sulfuric acid to produce manganese (II) chloride, chlorine, sodium bisulfate and water.

This reaction takes place at a temperature near 100°C.

Cl₂ + NaI  2NaCl + I₂

Chlorine reacts with sodium iodide to produce sodium chloride and iodine. Chlorine - diluted solution.

Sodium iodide - cold solution.

7.65 

Let the oxidation state of P be x:

7.64 

Neil Bartlett first performed an experiment in which reaction between oxygen and PtF₆ was carried out which lead to the formation of a red coloured compound O₂ ⁺ [PtF₆ ]^-.

He observed that the first ionization energy of Oxygen and Xenon is almost same (~1170 kJ/mol). So, he tried to react Xe and PtF₆ in which he was successful to obtain a red coloured compound Xe⁺ [PtF₆]^-.

7.63

By Deacon's process Cl₂ can be prepared from HCl in presence of CuCl₂

4HCl + O₂? 2Cl₂ + 2H₂O

Cl₂ on treating with water gives HCl

Cl₂ + H₂O? HCl + HOCl

7.62 

Chlorine gas reacts with water to give Hydrochloric acid and Hypochlorous acid

Cl₂ + H₂O HCl (Hydrochloric Acid) + HOCl (Hypochlorous acid)

Fluorine gas reacts with water to give Hydrogen ions, Fluorine ions, Oxygen gas and Hydrofluoric acid. 2F₂ + 2H₂O  4H⁺ + 4F^- + O₂ + 4HF

7.61

Most of the halogens are coloured because they absorb radiations which are in the visible region which in turn excite the valence electrons to higher energy levels. As the amount of energy which is required to excite the electrons to a higher level is different for different halogens, each halogen has a different colour.

7.60

ClO₂ which is called as Chlorine Dioxide has following uses:

It is used as a bleaching agent in paper pulp and textile

It is used as disinfectant in sewage and for purification of drinking

Chlorine dioxide is used to control tastes and odours associated with algae and decaying

7.59

Both chlorine and nitrogen have almost the same electronegativity values, but chlorine rarely forms hydrogen bonding. This is because in comparison to chlorine, nitrogen has a smaller size and as a result, a higher electron density per unit volume. Hence nitrogen forms hydrogen bonding more readily.

Chlorine has larger atomic size as compared to nitrogen and so has lower electron density per unit volume. Hence chlorine does not readily form hydrogen bonding.