Chemical Bonding: Ionic, Covalent, VSEPR, MOT & Hybridization
Study ionic and covalent bonds, VSEPR theory, molecular orbital theory, hybridization, hydrogen bonding and bond parameters for JEE Main Chemistry.
The central idea of this chapter
Atoms combine to achieve stable electronic configuration. This chapter connects atomic structure with molecular properties through different bonding types.
What should you understand first?
Chemical Bonding is an important chapter in inorganic chemistry. Focus on ionic and covalent bonding, VSEPR shapes, molecular orbital theory, hybridization and hydrogen bonding. These concepts also support the understanding of molecular structure and properties.
Core concepts
- Ionic bond e transfer
- Covalent bond e sharing
- VSEPR theory lp-bp repulsion
- MOT BMO, ABMO
- Hybridization sp, sp2, sp3
Useful building blocks
- Bond order BO = (Nb−Na)/2
- Dipole moment μ = q × d
- Formal charge V−L−S/2
- H-bond H with F,O,N
- Fajan's rule polarization
Chemical Bonding formula sheet
Understand bonding concepts with molecular geometry. Apply VSEPR and MOT for predicting shapes and properties.
| Topic | Formula / Relation | Meaning or use |
|---|---|---|
| Ionic bond | Metal + Non-metal | Electron transfer, electrostatic |
| Covalent bond | Non-metal + Non-metal | Electron sharing |
| Bond order (MOT) | BO = (Nb − Na)/2 | Nb = bonding, Na = antibonding |
| Bond length | Generally decreases as bond order increases | Higher bond order generally means shorter bond length |
| Bond energy | Generally increases with bond order | Higher bond order generally means a stronger bond |
| Dipole moment | μ = q × d | Charge × distance |
| Formal charge | FC = V − L − S/2 | V = valence, L = lone, S = shared |
| VSEPR order | lp-lp > lp-bp > bp-bp | Repulsion strength |
| Hybridization | sp, sp2, sp3, sp3d, sp3d2 | Mixing of orbitals |
| sp hybrid | Linear, 180° | Examples: BeCl2, C2H2 |
| sp2 hybrid | Trigonal planar, 120° | Examples: BF3, C2H4 |
| sp3 hybrid | Tetrahedral electron geometry, 109.5° | Examples: CH4 (tetrahedral), NH3 (trigonal pyramidal), H2O (bent) |
| Hydrogen bond | H−F/O/N...H | Intermolecular attraction |
| Fajan's rule | Small cation, large anion | More covalent character |
How to approach Chemical Bonding problems
First identify bond type (ionic/covalent), then apply VSEPR for shape or MOT for bond order. Use hybridization for geometry prediction.
Ionic & covalent bonds
- Ionic character? EN difference
- Lattice energy? ∝ q1q2/r
- Covalent character? Fajan's rule
- Dipole moment? μ = q × d
- Formal charge? V−L−S/2
VSEPR, MOT & hybridization
- Molecular shape? VSEPR theory
- Bond order? BO = (Nb−Na)/2
- Hybridization? Count σ + lp
- H-bonding? H with F,O,N
- Magnetic nature? Unpaired e
How to prepare Chemical Bonding
Start with ionic and covalent bonding, then master VSEPR theory and molecular shapes. Finish with MOT, hybridization and hydrogen bonding.
What to do
- Learn ionic bond formation and lattice energy
- Master covalent bond characteristics and formal charge
- Practise VSEPR theory for all molecular shapes
- Understand MOT and bond order calculations
- Revise hybridization and hydrogen bonding
Common mistakes
- Confusing molecular shape with electron geometry
- Wrong bond order calculation in MOT
- Forgetting lone pairs in hybridization
- Mixing up H-bond strength order
- Wrong formal charge calculation
Ready to test Chemical Bonding?
Revise the formula sheet, then solve mixed JEE Main problems on ionic/covalent bonds, VSEPR, MOT and hybridization.
Chemical Bonding FAQ
Short answers to frequently tested ideas in this chapter.
An ionic bond is the electrostatic attraction between oppositely charged ions, commonly formed when electrons are transferred from one atom to another.
VSEPR theory predicts molecular geometry based on electron pair repulsion. Lone pairs repel more than bond pairs, determining molecular shape.
Hybridization is mixing of atomic orbitals to form new hybrid orbitals. Common types are sp, sp2, sp3, sp3d and sp3d2.