Why ionization energy decreases from top to bottom in a group?

Answer 1

as atomic number is increase the size of the atom goes on increasing as more number of electron is added to the outer most orbit so the nuclear force exerted by the nucleus on electron is less so the affinity to loose electorn is more as the atomic number is increase that is the reason ionization energy decrease with increase in atomic number

Answer 2

The ionization energy (IE) is the amount of energy necessary to remove an electron (usually valence) from a neutral atom. The GENERAL trend is that IE increases across a period and up a group, or the IE decreases as atomic number increases. This is related to the atomic radius of the atom, which has the opposite increasing trend as IE. The bigger an element is, the further away the valence electrons are from the nucleus. Electrons are held in orbit by the attractive force between their own negative charge and the protons in the nucleus' positive charge. So, the attraction becomes weaker as the valence electrons are further from the protons, which would be seen in a larger atom. Since the valence electrons are held loosely in orbit in a large atom, it would require much less energy to overcome the attraction than would the attraction between the valence electrons and the protons of a smaller atom. In other words, it would take less energy to remove an electron from a larger atom (which has a larger atomic number) than a smaller atom because it is easier to overcome the weak force holding the valence electrons in orbit.

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Answer 3

Fewer electrons in the highest occupied energy level

Answer 4

Distance of outermost shell from the nucleus.

Answer 5

Because the distance between the positive nucleus and electron shells become larger and the attraction lower.

Answer 6

An important factor is the number of electrons.

Answer 7

increase in atomic size