Class 11th
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New answer posted
2 months agoContributor-Level 9
[SiCl?]?² is not known because six larger chloride ions can't be accomodated around Si? due to its small size.
New answer posted
2 months agoContributor-Level 9
C? H? → possible structure of C? H? are; CH? -C (CH? )=CH? and CH? -CH=CH-CH?
(Unsaturation factor = 1)
Ozonolysis of CH? -C (CH? )=CH? gives acetone (B) and formaldehyde.
Oxidation of CH? -C (CH? )=CH? with KMnO? /H? gives acetone (B) and CO?
The question states it gives C? H? O (B). Hence the alkene is 2-Methylpropene (A).
[Reaction scheme showing ozonolysis and permanganate oxidation of 2-methylpropene]
New answer posted
2 months agoContributor-Level 10
CrO? ²? (Cr? ) → Cr? ³, Total oxidation number change = 3
MnO? (Mn? ) → Mn? ², Total oxidation number change = 5
Cr? O? ²? (Cr? ) → 2Cr? ³, Total oxidation number change = 6
C? O? ²? (C? ³) → 2CO? (C? ), Total oxidation number change = 2
New answer posted
2 months agoContributor-Level 9
B.D.E H-H < B.D.E D-D
B.D.E H-H = 435.9 kJ / mole
B.D.E D-D = 443.4 kJ / mole
E H ≈ E D - 7.5
New answer posted
2 months agoContributor-Level 10
Rotamers or conformers arises due to free rotation along σ - bond.
New answer posted
2 months agoContributor-Level 10
Rutherford atomic model can not explain hydrogen spectrum it is explained by Bohr's atomic model and from Bohr's atomic model, uncertainity principle can't be explained.
New answer posted
2 months ago
Contributor-Level 10
Density ∝ molar mass, as size of given molecules is nearly same
New answer posted
2 months ago
Contributor-Level 9
(a) Phenol with Br? / H? O gives 2,4,6-tribromophenol. (High ionisation due to polar solvent and high activation of ring)
(b) Phenol with Br? in CS? /CHCl? /FeBr? gives a mixture of o- and p-bromophenol, with p-bromophenol as the major product. (less ionisation due to non- polar solvent)
[Chemical reactions showing bromination of phenol under different conditions]
New answer posted
3 months agoContributor-Level 10
Bohr's model played an important role in the development of quantum theory. It introduced the idea of quantised electron orbits. It disproved claims of classical mechanics, which predicted that electrons would spiral into the nucleus. Bohr proposed that electrons can exist only in specific, stable energy levels called stationary states. There would be transitions between these levels that would help Bohr explain the line spectra of hydrogen. That together linked the atomic structure with the concept of energy quantisation. Even though the model could not explain multi-electron atoms, it laid the foundation for modern quantum mechanics.
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