Organic Chemistry Questions and Short Answers

The bond angle is the angle at which two adjacent bonds converge and meet at the central atom in molecules. 

Polar molecules show Keesom forces. Polar molecules have heteroatoms that differ in electronegativity values such that the electronegativity difference between the two atoms in a polar covalent bond is greater than 0.5 but less than 1.7. For example, HF, HCl, R-OH, etc.

Several characteristic properties of the metals are due to the nature of the metallic bond. Some unique properties include- 

1. High Melting and Boiling points: 

Most probable kinetic energy is the energy possessed by the maximum number of reactant molecules at a temperature T, and it is shown as a peak on the Maxwell-Boltzmann energy distribution graph (fraction of molecules versus Kinetic energy).

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.

Water at room temperature is liquid in nature due to the hydrogen bonds holding the water molecules (H₂O). The close association is hard to break; therefore, water boils at a high temperature of 100^oC. The high temperature breaks the Hydrogen bond links to free individual H₂O molecules.

Debye intermolecular forces of attraction occur between polar and nonpolar atoms or molecules.

When a polar molecule is in the vicinity of a nonpolar molecule, the electronegative end of that polar molecule attracts the electron cloud of the adjacent nonpolar molecule, thereby distorting it and inducing a pole separation. So, the polar molecule is said to have induced polarity in the neighboring nonpolar molecule.

The +I effect is an electron-donating (or an electron-pushing) inductive effect by an atom or group of atoms relative to Hydrogen. It means that a +I group like methyl (-CH₃) will push electrons away from itself more than the hydrogen atom would if it occupied the exact position in the molecule.

The push of electrons is represented with an arrow over the bond, (>) indicating the direction of the electron flow.

A metal atom is large, so the nucleus cannot attract and hold its outermost electrons. The metal loses those electrons and becomes positively charged kernels. The electrons then flow in the solid structure passing between these positive kernels.

Bond lengths are smaller when atoms form multiple bonds. Single overlap between two atoms forms a single covalent bond. So, when they overlap twice and thrice to form double and triple bonds the atoms to come closer to form a tight-knit. Such bonds are even harder to break. So, the bond length of a triple is smaller than a double and single bond.