# Hybridization

Hybridization mixes atomic orbitals on one atom to make new, equal orbitals that match the observed shape. One s plus three p gives four sp³; one s plus two p gives three sp²; one s plus one p gives two sp.

Chemistry (university) · Part 02: Chemical bonding and molecular shape · Card 8 of 9 · Last updated 2026-10-19

## Analogy

Mixing paint colours: blend a few pure colours to get new identical shades.

## Example

**Carbon examples**

CH₄: 4 groups, sp³, 109.5°
C₂H₄: 3 groups, sp², 120°
C₂H₂: 2 groups, sp, 180°

## In practice

Carbon in methane is sp³, in ethene sp² and in ethyne sp, which explains why their shapes are tetrahedral, planar and linear.

## Practice

### Flashcards

- **What hybridization has a 120° bond angle?** sp² (trigonal planar).
- **What is a sigma bond?** A bond formed by head-on overlap of orbitals along the line between the nuclei.

## Questions people ask

### How do I find the hybridization of an atom?

Count its electron groups: bonded atoms plus lone pairs. Two groups means sp, three means sp², four means sp³. Double and triple bonds count as one group each. This count also matches the VSEPR geometry, so the two ideas support each other.

### What is the difference between a sigma and a pi bond?

A sigma bond forms by head-on overlap of orbitals along the line between the nuclei. A pi bond forms by sideways overlap of p orbitals above and below that line. A double bond is one sigma plus one pi, and a triple bond is one sigma plus two pi.

## Related concepts

- [Bond polarity and dipole moment](https://studyvisually.com/learn/science/chemistry-university/chemistry-university-part-2/chemistry-university-part-2-concept-6)
- [VSEPR theory](https://studyvisually.com/learn/science/chemistry-university/chemistry-university-part-2/chemistry-university-part-2-concept-7)

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