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Organic Chemistry Questions and Short Answers

Why is Bi(V) a stronger oxidant/oxidizing agent than Sb (V)?

Bi (V) represents the +5-oxidation state of Bismuth (Bi). It means Bi has lost 5 electrons from its valence shell. Bi, therefore, wants to gain the lost electrons and is called an oxidizing agent. The process of electron uptake is a reduction reaction.

Bi (V) is a stronger oxidizing agent than Sb (V) and, therefore, will pick up the electrons faster than Sb (V). Due to the electron uptake, it will then go from a +5-oxidation state to a +3-oxidation state. Bi is now less by only three electrons due to the two-electron gain.

How to identify a functional group from an IUPAC nomenclature- with three examples

The longest carbon chain is the parent chain containing the principal functional group. 

The principle functional group is always given the highest priority, lowest number (1 before 2, 3, 4...), and assigned as a suffix while writing the nomenclature. Therefore, the numbering of the parent chain always starts from the principal functional group.

Identify the Functional Isomers of C3H6O- Aldehydes, Ketones and Carboxylic Acids

Question- A and B are two functional isomers of compound C3H6O. On heating with NaOH and I2, Isomer B forms a yellow precipitate of Iodoform whereas Isomer A does not form any precipitate. Write the formulae for A and B.

 

1) Functional Isomers are compounds that have same molecular formula but different functional groups. 

How do polar molecules interact?

A molecule is said to be polar if the bond electrons between the atoms in a covalent bond are unequally distributed, creating two ends. The electron redistribution is marked by showing the separation of charges as a partial charge above the atom's symbol. Therefore, a polar molecule always has a positive and a negative end resulting in a dipole. The pulling of bond electrons by an atom is attributed to its electronegativity.

Why Hydrogen bonds are stronger than dipole-dipole interactions?

Dipole-dipole interactions occur in polar molecules where the difference in electronegativity between the combining atoms creates positive and negative dipoles. These opposite poles align and result in electrostatic attraction throughout the polar medium. So, naturally, the strength of the interaction would depend on the magnitude of the charges and their distance, explained by the Coulombic law. So, the higher the magnitude of the charges and the lesser the distance between them, the stronger the dipole-dipole attractive interaction.