Water has hydrogen bonding because it contains hydrogen atoms bonded to highly electronegative oxygen atoms. In a water molecule (H2O), each oxygen atom forms two covalent bonds with two hydrogen atoms. However, the oxygen atom is more electronegative than hydrogen, causing it to pull the shared electrons closer to itself. This results in a partial negative charge on the oxygen atom and partial positive charges on the hydrogen atoms.
The partially positive hydrogen atoms in one water molecule can form weak electrostatic attractions with the partially negative oxygen atoms in neighboring water molecules. These attractions are known as hydrogen bonds. The hydrogen bonds in water are responsible for many of its unique properties, such as high boiling and melting points, high surface tension, and its ability to dissolve a wide range of substances.
On the other hand, carbon dioxide (CO2) does not have hydrogen bonding. While carbon dioxide molecules contain carbon and oxygen atoms, there is no direct covalent bond between hydrogen and oxygen. Instead, carbon dioxide molecules are held together by strong covalent bonds between carbon and oxygen. As a result, carbon dioxide does not exhibit hydrogen bonding.