The shape of the carbon(IV) oxide (CO₂) molecule is

Correct answer: Linear

Explanation: In CO₂, the central carbon forms two double bonds (O=C=O) and has no lone pairs. By VSEPR theory, two electron domains around carbon arrange themselves as far apart as possible, giving a linear shape with a bond angle of about 180°.

• Pyramidal — Incorrect. Pyramidal (trigonal pyramidal) needs three bonds and a lone pair on the central atom (e.g., NH₃).
• Linear — Correct. Two bonding regions, no lone pairs on carbon → 180°.
• Angular (bent) — Incorrect. Bent shapes arise when lone pairs are on the central atom (e.g., H₂O, SO₂).
• Tetrahedral — Incorrect. Tetrahedral requires four bonding pairs around the central atom (e.g., CH₄).