London dispersion forces are weak intermolecular forces found in all atoms and molecules. However, it is an exclusive force binding the nonpolar molecules due to their lack of functional groups, avoiding competing interactions.
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.
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.
Carbon's nondiscriminatory nature to form bonds with itself and other elements has led to a wide variety of small and large organic compounds. Carbon-hydrogen compounds called hydrocarbons are mostly inert; however, carbon with other elements (N, O, S, halogen) form functional groups, the reactive part of the molecule. The functional group part of the molecule is where chemical transformations occur. Some organic compounds can have more than one functional group.
A chemical bond strength is a force holding the atoms in a bond, and separating such atoms requires energy input. The bonds are of two types- Intermolecular and Intramolecular bonds.
Intramolecular bonds join the atoms in a molecule, whereas Intermolecular bonds are only responsible for closely associating the molecules. Therefore, Intramolecular bonds require higher energy to break than intermolecular bonds.
The dipole moment, a product of charge difference (q) and the distance (d) between the centres of positive and negative charges (µ = q x d), is also directional. The direction is indicated by an arrowhead, which points towards the most electronegative atom, representing the direction of the dipole moment.
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 100oC. The high temperature breaks the Hydrogen bond links to free individual H2O molecules.
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.
A covalent bond holding two atoms is made of two electrons. The bond can cleave or break in two ways - equally (homolytic fission) or unequally (heterolytic fission).
A heterolytic bond cleavage results in unequal bond-breaking where one atom in the bond retains both the bond electrons.