1. Electron Configuration: Each hydrogen atom has one proton and one electron. This single electron occupies its 1s orbital.
2. Sharing Electrons: When two hydrogen atoms come close together, their 1s orbitals overlap. This overlap allows the two electrons to be shared between both atoms.
3. Covalent Bond Formation: This sharing of electrons creates a covalent bond, a strong attractive force that holds the two hydrogen atoms together as a molecule. The shared pair of electrons is now attracted to both nuclei, effectively filling the 1s orbitals of both atoms and achieving a stable, lower-energy state.
Key Points:
* Stability: The hydrogen molecule (H₂) is more stable than two separate hydrogen atoms because the shared electrons fill the 1s orbitals of both atoms.
* Electronegativity: Both hydrogen atoms have the same electronegativity, meaning they pull on the shared electrons equally. This leads to a nonpolar covalent bond, where the electron density is evenly distributed.
* Bond Length: The distance between the two hydrogen nuclei in a hydrogen molecule is about 74 picometers (0.74 angstroms).
In summary, a hydrogen molecule is formed by two hydrogen atoms sharing their single electrons through a covalent bond, creating a stable, lower-energy state.
