Why is methane non-polar even though C-H bonds have some polarity?

Each C-H bond is very slightly polar, but the four bond dipoles point toward the four corners of a tetrahedron. Because the geometry is perfectly symmetric, the dipoles cancel out exactly, leaving methane with zero net dipole moment.

What is the C-H bond length in methane?

The C-H bond length in methane is 109 pm (1.09 Å). This is the equilibrium distance between the carbon and hydrogen nuclei where the attractive and repulsive forces balance. It is one of the shortest single bonds carbon forms.

How is methane different from ethylene and acetylene in shape?

Methane (CH₄) is sp³ hybridized with a tetrahedral shape and 109.5° bond angles. Ethylene (C₂H₄) is sp² with a planar shape and 120° angles. Acetylene (C₂H₂) is sp with a linear shape and 180° angles. Hybridization controls geometry directly.

Is methane geometry tested in NEET?

Yes. Methane's tetrahedral geometry, 109.5° bond angle, and sp³ hybridization are recurring NEET topics from the Chemical Bonding chapter. The concepts also apply to every saturated alkane and to the sp³ carbons in alcohols, amines, and haloalkanes.

PhysicalEasyNEET: 3-4 Q3D

Methane (CH₄) — Tetrahedral Geometry

Chemical Bonding & Molecular Structure

Explore the perfect 109.5° tetrahedral geometry of methane. Drag to rotate and see why sp³ hybridization gives this shape — the foundation of all alkane chemistry.

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How to use this lab

1Molecule ko drag karke har angle se ghumao.
24 C–H bonds dekho — sab 109.5° pe, perfect tetrahedral.
3Niche card mein sp³ · Tetrahedral · 109.5° confirm karo.

What you're seeing

Methane (CH₄) has one carbon atom bonded to four hydrogens. The four bonds spread out as far apart as possible, forming a tetrahedron. This is the geometry of every sp³-hybridized carbon you'll meet in NEET.

Key NEET facts

▸Bond angle: 109.5° — the only geometry that puts 4 bonds farthest apart
▸Hybridization: sp³ — one s + three p orbitals mix
▸C-H bond length: 109 pm
▸Geometry name: tetrahedral

Memory trick

4 hydrogens, 4 corners of a tetrahedron, 109.5° apart — maximum distance, minimum repulsion.

Common questions

What is the hybridization of carbon in methane?›

Carbon in methane is sp³ hybridized. One 2s orbital mixes with three 2p orbitals to form four equivalent sp³ hybrid orbitals, each containing one electron. These four hybrid orbitals overlap with hydrogen 1s orbitals to form four identical C-H sigma bonds.

What is the bond angle in CH₄ and why?›

The H-C-H bond angle in methane is exactly 109.5°. This is the angle that puts four bonded pairs as far apart as possible in 3D space, minimizing electron pair repulsion. The resulting shape is a perfect tetrahedron with carbon at the centre.

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Atomic Orbitals — s, p, d Shapes in 3D

Atomic Structure

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