What type of bond forms between water molecules?

What type of bond forms between water molecules?

• A. Covalent bonds
• B. Ionic bonds
• C. Hydrogen bonds
• D. Van der Waals forces

Answer: (C)

Water molecules exhibit hydrogen bonding due to the polarity of the water molecule. Each water molecule consists of one oxygen atom covalently bonded to two hydrogen atoms. The oxygen atom is more electronegative than the hydrogen atoms, resulting in a partial negative charge on the oxygen side and partial positive charges on the hydrogen sides. This creates a polar molecule. When water molecules are close to each other, the partial positive charge of the hydrogen atoms in one water molecule is attracted to the partial negative charge of the oxygen atom in another water molecule. This interaction forms a hydrogen bond, which is a relatively weak bond compared to covalent and ionic bonds but is significant in determining many of the physical properties of water, such as its high boiling point, surface tension, and solvent capabilities. Covalent bonds, while present within each water molecule, are not responsible for the attraction between separate water molecules. Ionic bonds involve the transfer of electrons between atoms, which does not occur in water-water interactions. Van der Waals forces are weak intermolecular attractions that can occur between all types of molecules but are not the primary interactions in water. Therefore, the formation of hydrogen bonds between water molecules is a defining feature of their interactions and is crucial to the unique properties of water.

Water molecules exhibit hydrogen bonding due to the polarity of the water molecule. Each water molecule consists of one oxygen atom covalently bonded to two hydrogen atoms. The oxygen atom is more electronegative than the hydrogen atoms, resulting in a partial negative charge on the oxygen side and partial positive charges on the hydrogen sides. This creates a polar molecule.

When water molecules are close to each other, the partial positive charge of the hydrogen atoms in one water molecule is attracted to the partial negative charge of the oxygen atom in another water molecule. This interaction forms a hydrogen bond, which is a relatively weak bond compared to covalent and ionic bonds but is significant in determining many of the physical properties of water, such as its high boiling point, surface tension, and solvent capabilities.

Covalent bonds, while present within each water molecule, are not responsible for the attraction between separate water molecules. Ionic bonds involve the transfer of electrons between atoms, which does not occur in water-water interactions. Van der Waals forces are weak intermolecular attractions that can occur between all types of molecules but are not the primary interactions in water. Therefore, the formation of hydrogen bonds between water molecules is a defining feature of their interactions and is crucial to the unique properties of water.