Interactive chemistry - Hybridisation

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HYBRIDISATION AND MOLECULAR GEOMETRY

Explore sp, sp² and sp³ hybridisation through interactive molecular experiments.

🎯 Learning outcomes

1. Understand the concept of hybridisation.
2. Identify s and p atomic orbitals.
3. Understand excitation and orbital mixing.
4. Observe the formation of sp, sp² and sp³ orbitals.
5. Understand sigma bond formation by orbital overlap.
6. Identify lone pairs and bond pairs.
7. Predict molecular geometry using VSEPR theory.

🔬 Experiment 1: Select a molecule

BeCl₂ – Beryllium chloride BF₃ – Boron trifluoride NH₃ – Ammonia H₂O – Water

Hybridisationsp

Bond angle180°

Molecular shapeLinear

🧬 Experiment 2: Observe hybridisation

Follow the five stages. Press Next to observe the changes in atomic orbitals.

Ground-state configuration

s orbital p orbital Hybrid orbital Electron Bond overlap

⚛️ Experiment 3: Final molecule formation

Observe the actual arrangement of atoms after hybridisation and bond formation.

Central atomBe

Sigma bonds2

Lone pairs0

📐 Experiment 4: Compare hybridisation

sp

s + p

2 orbitals

Linear

180°

sp²

s + 2p

3 orbitals

Trigonal planar

120°

sp³

s + 3p

4 orbitals

Tetrahedral electron geometry

109.5° ideal angle

🧠 Experiment 5: VSEPR theory

Valence Shell Electron Pair Repulsion

Electron pairs in the valence shell of a central atom repel each other. They arrange themselves to minimise repulsion.

Order of repulsion:

LP–LP > LP–BP > BP–BP

LP = Lone pair
BP = Bond pair

BeCl₂ – AX₂ BF₃ – AX₃ CH₄ – AX₄ NH₃ – AX₃E H₂O – AX₂E₂

📖 Concept index

1. Meaning of hybridisation

Hybridisation is the intermixing of atomic orbitals of almost equal energy in the valence shell of an atom and their redistribution into the same number of equivalent orbitals with equal energy and shape.

2. Excitation of atoms

An electron may be promoted from a lower-energy orbital to an available higher-energy orbital. This provides the required unpaired electrons for the bonding model.

3. Formation of sp orbitals

One s orbital and one p orbital mix to form two equivalent sp hybrid orbitals. They are directed in opposite directions at 180°.

Example: BeCl₂.

4. Formation of sp² orbitals

One s orbital and two p orbitals mix to form three equivalent sp² hybrid orbitals. They are arranged in one plane at 120°.

Example: BF₃.

5. Formation of sp³ orbitals

One s orbital and three p orbitals mix to form four equivalent sp³ hybrid orbitals. Their ideal electron-domain arrangement is tetrahedral.

Examples: NH₃ and H₂O.

6. Sigma bonds

A sigma bond forms through head-on or axial overlap of orbitals along the internuclear axis.

7. Pi bonds

A pi bond forms through sideways overlap of parallel unhybridised p orbitals. It is not involved in the four molecular examples above.

8. Molecular shape versus electron geometry

Electron geometry considers both bonding pairs and lone pairs. Molecular shape describes the positions of atoms only.

NH₃: tetrahedral electron geometry, trigonal pyramidal molecular shape.

H₂O: tetrahedral electron geometry, bent molecular shape.

📝 Assessment

🌟 Well done!

You have completed the interactive hybridisation laboratory.