Question

Why does Fluorine have a higher ionization energy than Iodine?

Answer 1

Hint: In order to answer this question, we will give the accurate reason of why Fluorine has a higher ionization energy than Iodine and then we will explain the properties of both the given elements.

Complete answer:
Fluorine has higher ionization energy than iodine because the size of fluorine is smaller than the iodine. This suggests that fluorine has a lower shielding effect. As a result, the nucleus of fluorine attracts more valence electrons than that of iodine.
Fluorine is at a lower energy level than Iodine and does not receive the same level of protection. As a result, fluorine has a higher nuclear effect on the electrons around it, requiring more energy to remove them.
As a result, the new electron will be more repelled. As a result, additional energy is required to defeat this force. Fluorine is in the upper group, which means the nucleus is closer to the valence electrons and is held tighter; iodine is in the lower group, which means Coulomb's Law says there is less attraction.
Fluorine is the lightest halogen and exists as a very poisonous, pale yellow diatomic gas under normal conditions. It is particularly reactive being the most electronegative element, reacting with all other elements except argon, neon, and helium.
Fluorine is found in coal, clay, and rocks and is found naturally in the earth's crust. Industries release hydrogen fluorides into the air as a result of combustion operations. Fluorine is present in the atmosphere in 0.6 parts per billion (ppb) as organic chloride compounds and salt spray. In city contexts, the element has been measured at roughly 50 parts per billion.
Iodine is the heaviest of the stable halogens; it is a glossy, purple-black non-metallic solid that melts to a deep violet liquid at 114 degrees Celsius and boils to a violet gas at 184 degrees Celsius under ordinary conditions.

Note:
Because the distance between the nucleus and the outer electrons is large and the relative charge experienced by the outer electrons is tiny, the nucleus' attractive force on the outermost electrons is tiny, therefore removing one of those outer electrons requires little energy. As a result, of the four elements \[F,{\text{ }}Cl,Br,{\text{ }}and{\text{ }}I\] , iodine has the lowest initial ionisation energy.