Answer:
Carbon dioxide
Explanation:
The Lewis structure of carbon dioxide shows that the carbon in CO2 must make 2 sigma bonds and it has no lone pairs.
The bond angle from O = C = O is 180° because the geometry is a linear geometry.
Considering the definition of molecular geometry, the geometry of the CO₂ molecule is linear, whose angles are 180°.
First of all, you have to know that molecular geometry is the three-dimensional arrangement of the atoms that make up a molecule.
In other words, molecular geometry is the spatial distribution in which atoms are arranged around a central atom. This arrangement has a significant influence on the physical and chemical properties of substances.
The molecular geometry of a substance can be predicted with great accuracy using the VSEPR (Valence Shell Electron Pair Repulsion) model. This model expresses that the geometry around a given central atom of a molecule is that which minimizes the repulsion of the pairs of electrons, which are those pairs of electrons used to form bonds and the unused ones that remain as free pairs around every atom in the molecule.
CO₂ is known as a linear triatomic molecule. This means that CO₂ has three atoms arranged in a line with carbon in the middle and one oxygen atom at each end.
That is, the carbon (central atom) has two atoms attached to the oxygen and no free pair. These links will want to be as far apart as possible, and for this, they will have to oppose each other 180 °.
That is, as the C atom only has two bonding electronic clouds, the molecular geometry with respect to the C atom is linear, because both clouds repel each other until they are as far apart as possible.
Finally, the geometry of the CO₂ molecule is linear, whose angles are 180°. ( See attached image).
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