True or false?
Hydrogen bonds between water molecules are comparable in strength to hydrogen-carbon covalent bonds?
No. Hydrogen bonds (those between molecules as opposed to those withing the same molecule) are about 1/20 as strong as the covalent bonds.
False.
Hydrogen bonds between water molecules are not comparable in strength to hydrogen-carbon covalent bonds. To understand why, we need to look at the nature of these two types of bonds.
Hydrogen bonds occur when a hydrogen atom is attracted to an electronegative atom, such as oxygen or nitrogen. In the case of water, the hydrogen bonds form between the hydrogen atoms of one water molecule and the oxygen atom of another water molecule. These bonds are relatively weak compared to covalent bonds and are classified as intermolecular forces.
On the other hand, hydrogen-carbon covalent bonds are formed when a hydrogen atom is directly bonded to a carbon atom, as in hydrocarbons. Covalent bonds involve the sharing of electrons between atoms, resulting in stronger bonds.
The strength of a hydrogen bond is usually around 5-10% of the strength of a typical covalent bond. Despite being weaker, hydrogen bonds still play a crucial role in many biological and chemical processes, including the unique properties of water, DNA structure, and protein folding.
In summary, hydrogen bonds between water molecules are not comparable in strength to hydrogen-carbon covalent bonds. Hydrogen bonds are weaker and are intermolecular forces, while hydrogen-carbon covalent bonds are stronger and involve the sharing of electrons between atoms.