Chemical Bonding and Molecular Structure

Chemical Bonding and Molecular StructureNEET Chemistry · Class 11 · NCERT Chapter 4

Overview Notes NEET Questions Interactive Learning

3 interactive concept widgets for Chemical Bonding and Molecular Structure. Drag any slider, change any number, and watch the formula and the answer update live. Built so you understand how each NEET problem actually works, not just the final number.

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VSEPR shape predictor (bond pairs + lone pairs)

Bond polarity calculator (EN difference → bond type)

Hybridization and geometry lookup (sigma, pi, lone pairs)

VSEPR and molecular geometry

Select bonding pairs and lone pairs to predict the 3D shape of any molecule. Covers linear, bent, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral geometries.

VSEPR theory

VSEPR shape predictor

Select bonding pairs and lone pairs to predict molecular geometry, hybridization, and bond angles. Click any preset molecule for instant results.

Select the number of bonding pairs and lone pairs on the central atom to predict the molecular geometry.

H₂O

NH₃

BF₃

CH₄

PCl₅

SF₆

CO₂

XeF₄

SO₂

ClF₃

Bonding pairs: 4

Lone pairs: 0

Molecular geometry

Tetrahedral

Hybridization

sp³

Bond angle

109.5°

Description

Four bonding pairs pointing to the corners of a tetrahedron.

Steric number: 4 (4 bonding + 0 lone)

Examples: CH₄, NH₄⁺, CCl₄

Try this

H₂O: 4 electron pairs (sp³) but only 2 are bonding, giving bent geometry with 104.5° bond angle (not 109.5°).
Key rule: lone pairs occupy more space than bonding pairs and compress bond angles.
PCl₅ (sp³d) and SF₆ (sp³d²) involve d-orbital participation. Period 3+ elements can exceed the octet.

Bond polarity and hybridization

Enter any two elements to compute electronegativity difference and bond type (nonpolar/polar covalent/ionic). Also look up hybridization, geometry, and sigma/pi counts for common molecules.

Chemical bonding

Bond polarity classifier

Select two elements to find their electronegativity difference and classify the bond as nonpolar covalent, polar covalent, or ionic.

Select two elements to calculate their electronegativity difference and classify the bond.

H-F

H-Cl

H-O

H-N

C-H

C-O

Na-Cl

K-Br

C-C

N-H

Element A

EN = 2.20

—

Element B

EN = 3.98

Bond type

Ionic

The electronegativity difference is large. One atom effectively transfers its electron(s) to the other, forming ions. The bond is predominantly electrostatic.

|EN(H) − EN(F)| = |2.20 − 3.98| = 1.78

F is more electronegative (EN = 3.98). It pulls bonding electrons toward itself.

H +

▶

F −

Arrow points toward the more electronegative atom

Classification thresholds

EN diff < 0.5: Nonpolar covalent

0.5 ≤ EN diff ≤ 1.7: Polar covalent

EN diff > 1.7: Ionic

Try this

C-H bond (diff = 0.35) is nonpolar covalent, which is why hydrocarbons are nonpolar.
H-F has the largest diff (1.78) among common covalent bonds, putting it on the ionic border.
Na-Cl (diff = 2.23) is clearly ionic. In NaCl crystal, Na transfers its 3s electron to Cl.

Hybridization

Hybridization explorer

Select a compound to see hybridization type, sigma and pi bond count, lone pairs on the central atom, and geometry.

Select a compound to see hybridization, sigma/pi bond count, lone pairs, and geometry of the central atom.

BeCl₂

BF₃

C₂H₄ (each C)

C₂H₂ (each C)

CH₄

NH₃

H₂O

PCl₅

SF₆

XeF₄

Central atom: Be in BeCl₂

Hybridization

Geometry

Linear

Bond angle

180°

Sigma (σ) bonds

Pi (π) bonds

Lone pairs (central)

Key point

Be uses one s and one p orbital. Electron-deficient (only 4 electrons around Be).

Quick reference: steric number rule

Steric number = bonding pairs + lone pairs on central atom.
SN=2 → sp (linear) | SN=3 → sp² (planar) | SN=4 → sp³ (tetrahedral)
SN=5 → sp³d | SN=6 → sp³d²

All single bonds are sigma (σ). Double bond = 1σ + 1π. Triple bond = 1σ + 2π.

Try this

Every single bond is a sigma bond. Pi bonds only exist in double or triple bonds — they use unhybridized p orbitals.
The hybridization of the central atom is determined by its steric number, not the molecular formula directly.
XeF₄ has 2 lone pairs that sit opposite each other (trans) in the octahedral arrangement, giving a square planar molecule.

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