The electron dot structure, also known as the Lewis structure, of carbon dioxide (CO₂) can be determined by considering the valence electrons of each atom and arranging them to satisfy the octet rule.

1. Count the Total Valence Electrons:

» Carbon (C) is in Group 4, and oxygen (O) is in Group 6 of the periodic table. Carbon has 4 valence electrons, and each oxygen has 6 valence electrons.

» For CO₂, the total number of valence electrons is: 4(from C)+2 × 6(from O)=16 electrons.

2. Arrange the Atoms:

» Carbon is the central atom in CO₂ since it is less electronegative than oxygen. The oxygen atoms will be bonded to the carbon atom.

3. Connect Atoms with Single Bonds:

» Carbon forms double bonds with each oxygen to share electrons and achieve a stable electron configuration.

4. Distribute Remaining Electrons:

» Place the remaining electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of 8 electrons (except for hydrogen, which follows the duet rule).

5. Check for Octet Rule:

» Ensure that each atom (except hydrogen) has 8 electrons in its outer shell. Carbon and oxygen should have a full octet