The shape of CH4 is

Step 1: Analyze the question You're asked for the molecular shape of methane, CH₄.

Step 2: The concept (VSEPR theory) Electron pairs around a central atom repel each other and arrange themselves as far apart as possible. The shape depends on the number of bonding pairs and lone pairs on the central atom.

Step 3: Solution

• Carbon (atomic number 6) has the configuration 1s² 2s² 2p², so it has 4 valence electrons.
• Each of the 4 electrons pairs with an electron from a hydrogen atom, forming 4 C-H covalent bonds.
• There are 4 bonding pairs and 0 lone pairs around carbon.
• Four electron pairs are farthest apart when they point to the corners of a tetrahedron.
• The H-C-H bond angle is 109.5°.

Comparison with other shapes:

• Linear (e.g., BeCl₂, CO₂): 2 electron pairs, 180°
• Planar/trigonal planar (e.g., BF₃): 3 pairs, 120°
• Pyramidal (e.g., NH₃): 3 bonding pairs + 1 lone pair, about 107°
• Tetrahedral (e.g., CH₄): 4 bonding pairs, 109.5°

Step 4: Answer The shape of CH₄ is tetrahedral, which is option D.

Tip: Count the electron pairs on the central atom.

• 4 bonding pairs and no lone pairs gives tetrahedral (CH₄).
• 3 bonding pairs and 1 lone pair gives pyramidal (NH₃).
• 2 bonding pairs and 2 lone pairs gives bent/V-shaped (H₂O).

Remember: lone pairs change the shape, so with no lone pairs the shape follows directly from the number of bonds.