Answer:
A. lower than
Step-by-step explanation:
Carbondioxide has a lower boiling point compared to that of water.
The interatomic bond in CO₂ is a non-polar covalent bond in which both carbon and oxygen atoms shares the donated electrons equally. CO₂ is a linear compound with the bond angle being 180°. This makes the bonds symmetrically arranged and the dipoles in one direction cancelling out the one in the opposite direction and results in a net dipole that is zero. This also results in the London Dispersion Forces between the molecules of CO₂. London dispersion forces are weak forces of attraction in which the constant motion of electrons in non-polar compounds induces an instant charge seperation.
In water molecules, the interatomic bond is polar covalent bond and the bond angle is bent or v-shaped. The atoms are assymetrical to one another and there is a net positive charge on the hydrogen atom and a negative charge on the more electronegative oxygen. The intermolecular bond between water molecules are hydrogen bonds. Hydrogen bonds are special dipole-dipole attraction in which a hydrogen atom is directly joined to a highly electronegative atom. This hydrogen bonding results in more effective binding of water molecules and it reflects in their physical properties such as a high boiling point.