Chemistry

The valence bond theory explains the covalent bond formation for two half-filled orbitals. The bond strength depends on several factors, including the extent of overlap of the two atomic orbitals. The bond strength is directly proportional to the extent of overlap.

In simple words, the greater the amount of overlap between two orbitals, the stronger the covalent bond will be.

JEE asks many questions based on the comparison of bond strength for two different pairs of atomic orbitals forming a covalent bond. For example, why H–F bond stronger than the F–F bond?

Pollution due to oxides of sulphur gets enhanced due to hydrocarbons and oxidizing agents like O? & H? O?

The IUPAC name giving the lowest number to the functional group obeying the lowest set of locants is 1-bromo-5-chloro-4-methylhexan-3-ol.

More the number of strong field ligands in a complex greater the energy absorbed by a complex.

105.8 * (2/4) = 52.9 pm ⇒ r_Li+ + r_X- = 52.9 * (3²/3) = 158.7 pm

M = (a³ * d * N_A) / Z = (3.608 * 10? )³ * 8.92 * 6.022 * 10²³) / 4
M = (46.96 * 10? ²? * 8.92 * 6.022 * 10²³) / 4 = 63 g/mole
the closest answer is choice (1)

P = (nRT) / V = (2 * 0.0831 * 300) / 10 = 4.986 bar

Oxidation state in neutral medium changes from +7 to +4 for MnO? to MnO?

Formaldehyde 2-methyl propanal

E_cell = 1.05 - (0.059 / 2) log ( [Ni²? ] / [Ag? ]²)
= 1.05 - (0.059 / 2) log ( [10? ³] / [10? ³]²)
= 1.05 - (0.059 * 3) / 2 = 1.05 - 0.0885 = 0.9615 volt
There is a misprint in the question. The E? _cell is incorrectly given as 10.5 V. This should have been 1.05 volt.

Statement I is true but statement II is incorrect as 3°-alcohols are the most reactive and give immediate turbidity with Luca's reagent.