The H–H bond is classified as a sigma bond because it forms from the direct, head-on overlap of two hydrogen atomic orbitals, creating a single bonding region along the line between the two nuclei.
Think of each hydrogen atom as having one tiny cloud where its electron likes to hang out, called an orbital, and when two hydrogens get close those clouds bump straight into each other end to end, which makes a strong connection right between the two nuclei; that straight, centered overlap is what chemists call a sigma bond, and it is symmetrical around the line joining the atoms so the electron density is highest directly between them, holding the atoms together; because the overlap is head on the bond has no nodal plane through the bond axis, making it the simplest and strongest kind of single covalent bond for two s orbitals.
A common mistake is thinking any bond formed between atoms is a sigma bond, but some bonds are formed by sideways overlap and are called pi bonds, so remember sigma is end to end while pi is side to side; another error is picturing orbitals as solid balls instead of fuzzy clouds, which can make it hard to see why overlap matters, so imagine the clouds merging where they touch to make the bond; a final confusion is assuming only s orbitals can make sigma bonds, but p orbitals can also overlap head on to form sigma bonds when they point toward each other, so check how the orbitals are oriented.
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Why H2 Is a Sigma Bond
- Each hydrogen has one orbital
- Orbitals overlap end to end
- Overlap occurs along bond axis
- Electron density highest between nuclei
- No nodal plane through bond axis
- Sigma bond is strongest single bond
Why H2 Is a Sigma Bond
- Assuming every bond is a sigma bond
- Thinking orbitals are solid balls
- Believing only s orbitals form sigma bonds
H2, sigmaBond, chemicalBonding, atomicOrbitals, molecularOrbital, covalentBond, orbitalOverlap, sOrbitals, piBond, chemistryBasics
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