The lewis structure for co2 has a central the lewis structure for c o 2 has a central blank atom attached to blank atoms.
1. atom attached to the lewis structure for c o 2 has a central blank atom attached to blank atoms. atoms.
2. these atoms are held together by these atoms are held together by blank bonds. bonds.
3. carbon dioxide has a carbon dioxide has a blank electron geometry. electron geometry.
4. the carbon atom is the carbon atom is blank hybridized. hybridized.
5. carbon dioxide has two carbon dioxide has two blankπ bonds and two blankσ bonds.π bonds and two carbon dioxide has two blankπ bonds and two blankσ bonds.σ bonds.

See the explanation

Explanation:

1) The Lewis structure for   has a central Carbon atom attached to Oxygen atoms.

In the  we will have a structure:  O=C=O the central atom "carbon" we will have 2 sigma bonds and 2 pi bonds, therefore, we have an Sp hybridization. For O we have 1 pi and 1 sigma bond, therefore, we have an Sp2 hybridization.

2) These atoms are held together by double bonds.

Again in the structure of : O=C=O we only have double bonds.

3. Carbon dioxide has a Carbon dioxide has a Linear electron geometry.

Due to the double bonds we have to have a linear structure because in this geometry the atoms will be further apart from each other.

4. The carbon atom is Sp hybridized.

We will have for carbon 2 pi bonds, so we will have an Sp hybridization.

5. Carbon dioxide has two Carbon dioxide has two C(p) - O(p) π bonds and two C(sp) - O(Sp2) σ bonds.

(See figures)

Figure 1: Carbon hybridization

Figure 2: Oxygen hybridization

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

the correct answer would be d. hope this !