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Ionic and covalent chemical bonding are both stronger than hydrogen bonding. It’s a polar covalent connection involving oxygen and hydrogen where the hydrogen gains a partial positive charge. This indicates that electrons are being attracted to the more highly electronegative atom. As a result, the hydrogen is drawn to the negative charges of any nearby atom. The hydrogen bond is a sort of chemical bond that is accountable for many of water’s features.
Hydrogen Bonding
A hydrogen atom is sandwiched between two other atoms with a high affinity for electrons, forming a hydrogen bond that is weaker than an ionic or covalent link but stronger than van der Waals forces. Hydrogen bonds can form between atoms in distinct molecules or inside a single molecule. One of the atoms in the pair (the donor), usually a fluorine, nitrogen, or oxygen atom, is covalently bound to a hydrogen atom (FH, NH, or OH), with which it shares electrons unequally; the hydrogen takes on a little positive charge due to its strong electron affinity. The other atom in the pair, which is usually F, N, or O, has an unshared electron pair and is slightly negative in charge. The donor atom efficiently shares its hydrogen with the receiver atom, creating a bond, mostly by electrostatic attraction. Water (H2O) is liquid across a much wider temperature range than would be expected for a molecule of its size due to its strong hydrogen bonding. Because it quickly forms hydrogen bonds with the solute, water is an excellent solvent for ionic compounds and many other compounds. The way a linear protein molecule folds up into its functional form is determined by hydrogen bonding between amino acids. The double-helix structure, which is essential for the transfer of genetic information, is formed by hydrogen bonds among nitrogenous bases in nucleotides on the two strands of DNA (guanine couples with cytosine, adenine partners with thymine).
Hydrogen Bonding properties
Because of the hydrogen bonding that may occur between water and the alcohol molecule, lower alcohols are soluble in water.
Volatility: Because substances with hydrogen bonds between molecules have a greater boiling point, they are less volatile.
Viscosity and surface tension: Hydrogen-bonding-containing compounds have an associated molecule. As a result, their flow becomes more difficult. They have a high surface tension and viscosity.
The decreased density of ice compared to water: In solid ice, hydrogen bonding causes water molecules to form a cage-like structure. In fact, each water molecule is tetrahedral to four other water molecules. In the solid state, the molecules are not as tightly packed as they are in the liquid form. This case-like structure collapses when ice melts, bringing the molecules closer together. As a result, the volume of water reduces but the density increases for the same mass. As a result, at 273 K, ice has a lower density than water. Ice floats because of this.
Conclusion
When hydrogen is covalently bound to an electronegative atom in polar covalent compounds, hydrogen bonds develop. The development of a dipole is caused by the shared pair of electrons leaning towards the electronegative element. Over the electronegative atom, this dipole creates a partial negative charge, whereas the hydrogen atom develops a partial positive charge.
