Highest ionization energy to lowest I be ci f
To determine the order of ionization energy from highest to lowest for the elements I (Iodine), Cl (Chlorine), and F (Fluorine), you need to consider their positions in the periodic table.
Ionization energy refers to the amount of energy required to remove an electron from an atom or ion. In general, ionization energy increases from left to right across a period and decreases from top to bottom within a group in the periodic table.
With this information in mind, let's analyze the order of the elements you mentioned:
1. Fluorine (F): Fluorine is located in Group 17 (also known as Group 7A or the halogens) of the periodic table. Within this group, ionization energy generally increases from top to bottom. Therefore, fluorine has the highest ionization energy among the three elements listed.
2. Chlorine (Cl): Chlorine is also in Group 17, directly below fluorine. Since ionization energy generally decreases from top to bottom within a group, chlorine has a lower ionization energy than fluorine.
3. Iodine (I): Iodine resides in the same group as fluorine and chlorine but is located further down the periodic table. As previously mentioned, ionization energy decreases from top to bottom within a group. Therefore, iodine has the lowest ionization energy among the elements you mentioned.
So, the order of ionization energy from highest to lowest is: F > Cl > I.