1. Covalent Bonds:
* Within the molecule: Each hydrogen atom shares its single electron with the oxygen atom, forming a single covalent bond. This sharing of electrons creates a stable molecule.
* Polarity: Oxygen is more electronegative than hydrogen, meaning it attracts the shared electrons more strongly. This creates a partial negative charge (δ-) on the oxygen atom and a partial positive charge (δ+) on each hydrogen atom. This makes the water molecule polar.
2. Intermolecular Forces:
* Hydrogen Bonds: The strong polarity of the water molecule leads to hydrogen bonding. The partially positive hydrogen atoms on one water molecule are attracted to the partially negative oxygen atom on another water molecule. These hydrogen bonds are relatively strong intermolecular forces, responsible for many of water's unique properties.
* Van der Waals forces: While weaker than hydrogen bonds, these temporary, fluctuating forces also play a role in the interactions between water molecules.
Summary:
* The water molecule is held together by covalent bonds between the oxygen and hydrogen atoms.
* The polar nature of the water molecule results in hydrogen bonding between molecules, making water a highly cohesive and versatile substance.
Consequences of this bonding:
* High boiling point: Hydrogen bonds require a lot of energy to break, leading to water's relatively high boiling point.
* Good solvent: Water's polarity allows it to dissolve many polar substances, earning it the title of "universal solvent".
* Surface tension: The strong hydrogen bonds create surface tension, allowing water to form droplets.
This combination of covalent bonding and strong intermolecular forces makes water a unique and essential molecule for life on Earth.
