Respuesta :
The element with low ionization value is "Lithium (Li), because it has a low effective nuclear charge and a large radius." Ionization energy is defined as energy that an isolated gaseous atom needs to absorb to free an electron. The elements, Lithium (Li), Fluorine (F), Nitrogen (N), and Neon (Ne) are in period 3 of the periodic table. When you move across a period from left to right the number of protons increase which in turn leads to an increase in effective nuclear charge. In addition, the atomic radius decreases because of the increase in nuclear charge.This leads to electrons being held more tightly by the nucleus, hence more ionization energy is required to remove the valence electrons.
Li has the lowest ionization energy because it has a low effective nuclear charge and large radius.
The elements F, Li, Ne and N belongs to period 3 of the periodic table.
Ionization energy is the energy required to remove an electron from the elemental gaseous state.
In the period on moving from left to right, the effective nuclear charge decreases and this will lead to the reduced force on the atom. The radius decreases on moving across the period. Thus, the Li molecule will have the lowest ionization energy value.
The F is a halogen and usually forms a negative ion, but due to its larger size and effective nuclear charge, it has higher ionization energy.
The Ne being a noble gas has a complete octet, and thus the removal of electrons from the gaseous state requires high ionization energy.
The nitrogen has not a complete energy level, but the energy to remove electron is larger as compared to Li due to its size, and thus have higher ionization energy.
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