Ncert Solutions Chemistry Class 12th
Get insights from 2.6k questions on Ncert Solutions Chemistry Class 12th, answered by students, alumni, and experts. You may also ask and answer any question you like about Ncert Solutions Chemistry Class 12th
Follow Ask QuestionQuestions
Discussions
Active Users
Followers
New answer posted
10 months agoContributor-Level 10
7.70
As Bond dissociation energy generally decreases on moving down the group as the atomic size of the element increases. However, among halogens, the bond dissociation energy of F2 is lower than that of Cl2 and F2 due to the small atomic size of
Thus increasing order for bond dissociation energy among halogens is as follows:I22
As Bond dissociation energy of H-X molecules where X is the halogen decreases with increase in the atomic HI is the strongest acid as it loses H atom easily due to weak bonding between H and I.
So Increasing acid strength is as follows: HF
Basic strength decreases as we move from Nitrogen to Bismuth down the group
New answer posted
10 months agoContributor-Level 10
7.69
(i) XeO3 can be produced by hydrolysis of XeF4 and XeF6 under controlled pH of the medium in which reaction is taking place as shown below:
6XeF4 + 12H2O → 4Xe + 2XeO3 + 24HF + 3O2
XeF6 + 3H2O → XeO3 + 6HF
(ii) XeOF4 can be obtained on partial hydrolysis of XeF6 as shown below:
XeF6 + H2O → XeOF4 + 2HF
New answer posted
10 months agoContributor-Level 10
7.68
ClO- isisoelectronic to ClF as both the compounds contain 26 electrons in all. ClO- : 17+8+1 = 26
ClF : 17+9 = 26
Yes, ClF Molecule is a Lewis base as it accepts electrons from F to form ClF3.
New answer posted
10 months agoContributor-Level 10
7.33
Xe and F2 combine under different conditions to produce XeF2, XeF4, XeF6 as follows:
Ratio | Temperature & Pressure Condition | Reaction |
Excess | at {673K,1bar} | Xe (g) + F2 (g) → XeF2 (s) |
1:5 ratio | at {873K,7bar} | Xe (g) + 2F2 (g) → XeF4 (s) |
1:20 ratio | at {573K,60-70bar} | Xe (g) + 3F2 (g) → XeF6 (s) |
New answer posted
10 months agoContributor-Level 10
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.
New answer posted
10 months agoContributor-Level 10
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]-.
New answer posted
10 months agoContributor-Level 10
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
New answer posted
10 months agoContributor-Level 10
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
New answer posted
10 months agoContributor-Level 10
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.
Taking an Exam? Selecting a College?
Get authentic answers from experts, students and alumni that you won't find anywhere else
Sign Up on ShikshaOn Shiksha, get access to
- 66k Colleges
- 1.2k Exams
- 687k Reviews
- 1800k Answers