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In a water molecule (H₂O), hydrogen and oxygen atoms are held together by covalent bonds. A covalent bond is formed when atoms share electrons to achieve stability. Oxygen has six valence electrons and needs two more electrons to complete its outer shell (octet rule). Each hydrogen atom has one valence electron and needs one more to complete its duet configuration (like helium).
By sharing electrons, oxygen forms two single covalent bonds with two hydrogen atoms. This creates a stable water molecule in which oxygen attains eight electrons in its valence shell, while each hydrogen atom attains two electrons.
It is important to note that while covalent bonds hold hydrogen and oxygen together within a single water molecule, water molecules are also connected to each other through hydrogen bonds. Hydrogen bonding occurs between the slightly positive hydrogen atom of one water molecule and the slightly negative oxygen atom of another. These intermolecular hydrogen bonds are weaker than covalent bonds but are crucial for the unique physical properties of water, such as its high boiling point, surface tension, and ability to dissolve many substances.
Why not the other options?
Ionic bond: Found in compounds like NaCl, but water is not an ionic compound.
Hydrogen bond: Exists between separate water molecules, not within the same molecule.
Dating bond: This is not a scientific type of bond and is added as a distractor.
Key facts about bonding in water:
Bond type: Polar covalent because oxygen is more electronegative than hydrogen, creating a partial negative charge (δ⁻) on oxygen and partial positive charges (δ⁺) on hydrogens.
Bond angle: 104.5°, giving water a bent or V-shape geometry.
Polarity: The polar nature of water makes it an excellent solvent.
Thus, hydrogen and oxygen in water are held together by covalent bonds.
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