Explain why an atom with a high ionization energy value is not likely to form a positive ion?

Answer 1

let's say sodium loses an electron and becomes smaller sodium atom (Na) : [Ne]3s^1 => sodium ion (Na^+) : [Ne]


now lets say a chlorine ion gains an electron and therefore becomes larger
chlorine atom (Cl) : [Ne]3s^1 3p^5 => chlorine ion (Cl-) : [Ne]3s^2 3p^6




see how chlorine becomes negative?


ionization-energy: energy required to remove an electron from a gaseous atom. For example, 8.64 X 10^-19 J is required to remove an electron from a gaseous lithium atom. The energy required to remove the first electron from an atom is called the first ionization energy. Therefore, the first ionization energy of lithium equals 8.64 X 10^-19 J. The loss of the electron results in the formation of a Li^+ion.
In other words, ionization-energy is how strongly an atom's nucleus holds onto its valence electrons. High ionization-energy means it has a strong hold while low ion... means it has a weak hold. Such atoms are likely to form positive ions.


to answer your question directly: Because an atom with a high ionization-energy holds onto its valence electrons, and therefore are less likely to give up its electrons and become positive (because when an atom's nucleus lets go of an electron, it automatically becomes positive).

Answer 2

Ionization energy is an indicator of how easy an electron is removed. It can be seen as a measurement of the effective nuclear charge. When the ionization energy is high, the nuclei holds the electron tightly making the formation of a cation difficult, which is science means less likely.

Answer 3

The lower the ionization energy, the less energy it takes to remove an electron. In other words, it is easier to remove electrons from an atom with a low ionization energy.