CO2 Molecular Geometry and Bond Angles

Carbon dioxide, ie, CO2, is considered one of the best compounds for understanding the concepts of Lewis structure and Molecular Geometry in the beginning. The beginners who want to learn such concepts and their fundamentals or want to know the procedure of drawing the Lewis dot structures for other molecules can also consider this molecule. CO2 is composed of two different types of atoms; oxygen as well as carbon. However, this gaseous molecule is popular for its presence in global warming and the greenhouse effect. Moreover, this gas is very useful in various industries. To know about a given compound’s reactivity, physical and chemical properties, it is important to be aware of its molecular geometry.

Here is the CO2 Lewis Structure for a better understanding:

CO2 Lewis Structure

Understanding the Lewis structure is essential to comprehend the molecular geometry of a given molecule. The given structure tells you the arrangement of electrons inside the molecules and the molecule’s shape. Before knowing the Lewis structure of CO2, it is important to understand the Lewis structure properly.

The Lewis dot structure is a graphical representation in the picture form regarding the arrangement of the valence shell electrons in the molecule. Moreover, these valence electrons are shown by making dots around the individual atoms. The making of lines shows the formation of bonds in the molecule. These structures assist in better understanding the array of atoms, including the electrons involved in forming bonds. Now, after figuring out the process of creating the Lewis structure and its applications, let’s just look at the CO2 Lewis structure. In the case of CO2, the carbon atom is present in the middle position as it is the slightest electronegative atom in the molecule. Moreover, two oxygen atoms are present on the terminals where the sharing of electrons and formation of bonds with the central carbon atom is done by both these atoms.

To know how the bonds are formed and their arrangement, let’s go through the valence electrons of all atoms in the molecule.

Number of valence electrons in Carbon = 4

Number of valence electrons in Oxygen = 6 X 2 = 12

(we will multiply it with 2 because there are 2 atoms of oxygen in this molecule)

Total number of valence electrons present in the molecule =  12 + 4 = 16

Therefore, for now, put carbon in the middle position and create four dots around it. Place two oxygen atoms on both sides of the atom and make six dots around every atom to show their valence electrons.

You must know that to become stable, a molecule needs to complete its octet. Moreover, to become inactive, a molecule requires achieving an electronic configuration similar to inert gases. This is done either by accepting an electron or by donating an electron. The carbon atom will be donating its electrons to both these oxygen atoms because they are more electronegative than the carbon atom.

CO2 Bond Angle

The molecular geometry of the CO2 is linear and arranged like O = C = O, which makes the bond angle of CO2 = 180 degrees. Moreover, the planer-shaped geometry, also called linear geometry, always has molecules with a 180-degree bond angle.

CO2 Molecular Geometry

The concept of CO2 molecular geometry states that the molecular geometry of any compound depends on the arrangement of atoms, bonds, and electron pairs. While discussing CO2, both oxygen atoms make sigma bonds and the central carbon atom, and make their octet complete. Moreover, as an outcome, there are no lone pairs of electrons; however, the bonding pairs of electrons also repel each other. Because of these forces between the electron pairs and valence shells that are repulsive in nature, the CO2 molecule takes a linear shape to maintain the repulsion at the minimum. Hence, the CO2 comprises a linear molecular geometry including the bond angles of 180 degrees and distribution of the electrons, symmetrically.

Conclusion

The CO2 molecular geometry and bond angles notes conclude that the CO2  or carbon dioxide contains a total of 16 valence electrons which show on the outer shell of atoms, ie, four atoms of the carbon as well as 12 of two atoms of oxygen. 

With this, we can effortlessly draw the diagram of the Lewis dot of CO2 by adjusting two double bonds amid carbon and oxygen, ie, O = C = O. CO2’s molecular geometry is linear with a 180-degree bond angle because the charges of the dipole are cancelled with each other when the molecule is arranged symmetrically. 

However, both C = O bonds are polar, but the rest of the molecule is nonpolar in nature. When the carbon dioxide dissolves into the water, it forms H+ ions in the outward appearance of carbonic acid so that it presents acidic behaviour and is considered an acid.