The atomic radius of carbon is larger than that of oxygen. This can be explained by considering a few key factors related to atomic structure.
Atomic radius generally refers to the distance from the nucleus of an atom to the outermost shell of electrons. As you move across a period in the periodic table, the atomic radius tends to decrease. This is because, as you move from left to right, protons are added to the nucleus, which increases the positive charge. This increased nuclear charge pulls the electron cloud closer to the nucleus, resulting in a smaller atomic radius.
Carbon is located in Group 14 and Period 2 of the periodic table, while oxygen is in Group 16 of the same period. Since carbon has fewer protons (6) than oxygen (8), the nuclear charge of oxygen is greater. Therefore, oxygen’s electrons are drawn in more tightly than those of carbon, leading to a smaller atomic radius for oxygen.
In conclusion, carbon has a larger atomic radius than oxygen due to the difference in their atomic structure and the effect of nuclear charge on the electron cloud.