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.
Did you know that, back in the 1900s, it was believed that a hook and a loop type of closure was the covalent bond responsible for holding atoms in a molecule? Interesting, right?
The molecule H2N-NH2, also known as hydrazine, each Nitrogen atom has 3 bond pairs (two N-H and one N-N bonds) and one lone pair. So, the steric number of each Nitrogen atom is,
steric number=number of bond pairs + number of lone pairs
steric number=3 + 1 = 4
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.
A metallic bond is a chemical bond seen in metals consisting of tightly bound metal atoms of the same type.
Metals are large atoms that do not firmly hold their outermost valence electrons and easily lose them. Once the electrons are lost, the metal atoms become positively charged, called kernels. The position of these kernels is fixed to avoid repulsions and is part of the solid structure.
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.
Hydrogen bonding is a type of electrostatic interaction occurring in molecules in which the H atom is sandwiched between highly electronegative atoms like F, O, and N, one to which it is covalently bonded. For example, HF, H2O, NH3, etc.
The atoms or group of atoms are classified based on the Inductive effect as electron-withdrawing (-I) or electron-donating (+I) relative to Hydrogen.
The common functional groups showing +I and -I effect are:
+I group | -I group |
|---|---|
O- |
All atoms and molecules show London Dispersion Force, a primary way atoms and molecules interact. Most of the time, molecules have additional stronger forces than the London Dispersion Force, which is the weakest. Therefore, London Dispersion forces are exclusively seen in the nonpolar molecules since they don't have other competing functional groups leading to other interfering intermolecular interactions.
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.