Drawing the Lewis structure (Electron Dot Structure) of Carbon Dioxide (CO₂) is a fundamental exercise in high school chemistry. It perfectly demonstrates how atoms share electrons via covalent bonding to achieve a stable noble gas configuration (the octet rule).
Even though carbon dioxide is non-polar, it is highly soluble in water because it chemically reacts with water to form weak Carbonic Acid (H₂CO₃). This is how fizzy cold drinks are made!
Before drawing, we must know how many outer-shell (valence) electrons we have to work with.
The least electronegative atom is placed in the center. Carbon is less electronegative than Oxygen, so Carbon sits in the middle: O — C — O
Carbon needs 4 more electrons to complete its octet (8), and each Oxygen needs 2 more.
To make everyone happy with 8 electrons, Carbon forms a Double Covalent Bond with each Oxygen atom.
Structure so far: O = C = O
We have 16 total electrons. We used 8 electrons in the two double bonds (4 per double bond). Remaining electrons = 16 - 8 = 8 electrons.
We place these 8 electrons as non-bonding pairs (Lone Pairs) on the Oxygen atoms to complete their octets.
Because there are no lone pairs pushing down from the central carbon atom, the two double bonds push as far away from each other as possible (180°).
This makes the CO₂ molecule perfectly Linear in shape. Furthermore, because the two highly electronegative oxygen atoms are pulling equally in exact opposite directions, the individual dipole moments cancel out, making CO₂ a Non-Polar molecule.
There are two double bonds. Since a double bond counts as two covalent bonds, there are a total of **four covalent bonds** in a single CO₂ molecule.
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