Lewis Structures in Action: CO₂ and NO₂ Examples

The video tutorial explains how to draw Lewis structures for carbon dioxide (CO2) and nitrite ion (NO2-). It details the placement of atoms based on electronegativity, counting valence electrons, and forming bonds to satisfy the octet rule. For CO2, carbon is central, and double bonds are formed with oxygen. For NO2-, nitrogen is central, and a double bond is formed to complete the octet, considering the ion's charge.

Why is carbon placed in the central position in a carbon dioxide molecule?

• Because it has more valence electrons than oxygen

• Because it is more electronegative than oxygen

• Because it has fewer valence electrons than oxygen

• Because it is less electronegative than oxygen

How many valence electrons are used to form single bonds in a carbon dioxide molecule?

• 8 electrons

• 6 electrons

• 4 electrons

• 2 electrons

What is done to satisfy the octet rule for carbon in carbon dioxide?

• Add more single bonds

• Remove electrons from oxygen

• Form double bonds with oxygen

• Transfer lone pairs from carbon to oxygen

How many total valence electrons are present in the nitrite ion?

• 18 electrons

• 19 electrons

• 17 electrons

• 16 electrons

What is the role of the additional electron in the nitrite ion?

• It forms a triple bond

• It is placed on the central atom

• It balances the charge

• It is shared between nitrogen and oxygen