Final answer:
A) Hydrogen bond
Hydrogen bonds are the intermolecular forces that connect two water molecules, due to water being a polar molecule with slight charges on the oxygen and hydrogen atoms. These bonds are indicated by a dotted line and are not as strong as covalent bonds, but are crucial for the unique properties of water.
Step-by-step explanation:
Intermolecular Forces in Water Molecules
The connection between two water molecules is due to an intermolecular force (IMF) known as hydrogen bonding. This is different from a covalent bond, which occurs within a water molecule between the oxygen and hydrogen atoms, and ionic or metallic bonds which are not present between water molecules.
Hydrogen bonding occurs because water is a polar molecule, with a slight positive charge on the hydrogen atoms and a slight negative charge on the oxygen atom. In a hydrogen bond, the positively charged side of one water molecule will attract and form a bond with the negatively charged side of another water molecule.
It is important to note:
- A covalent bond is a strong bond within a molecule where two atoms share electrons.
- An ionic bond is the attraction between oppositely charged ions, which forms crystals rather than discrete molecules.
- Hydrogen bonds are indicated with a dotted line since they are weaker than covalent bonds.
- The asymmetric shape and the molecular dipole of water molecules facilitate the formation of hydrogen bonds, which result in high surface tension and a variety of other unique properties of water.