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
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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Fewer electrons in the highest occupied energy level
Distance of outermost shell from the nucleus.
Because the distance between the positive nucleus and electron shells become larger and the attraction lower.
An important factor is the number of electrons.
increase in atomic size
If you go down a group,the ionization energy decreases,while as you go up a group,the ionization energy increases.
As one proceeds down the group 7A elements, the first ionization energy decreases. this means that the outermost electron is more readily removed as we go down a group.
As you go down the group (any group), ionization energy decreases. So in terms of ionization energy, for the alkali metals, Lithium > Sodium > Potassium > Rubidium > Caesium > Francium
Atomic size decreases from left to right in a period hence ioniztion energy increases from left to right.But atomic size increases from top to bottom in a group hence ionization energy decreases from top to bottom.
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
From left to right on the periodic table, ionization energy increases. From top to bottom in a column (group) the ionization energy decreases.
If you go down a group,the ionization energy decreases,while as you go up a group,the ionization energy increases.
Ionization energy decreases with the rise of atomic number in a group of periodic table.
In fact it increases down the group because ionization energy decreases down the group
The number of energy levels increases from top to bottom of a group. So the electrons are easy to remove. So the ionization energy decreases.
As one proceeds down the group 7A elements, the first ionization energy decreases. this means that the outermost electron is more readily removed as we go down a group.
As you go down the group (any group), ionization energy decreases. So in terms of ionization energy, for the alkali metals, Lithium > Sodium > Potassium > Rubidium > Caesium > Francium
Beryllium is the group 3A element with the highest ionization energy.
Atomic size decreases from left to right in a period hence ioniztion energy increases from left to right.But atomic size increases from top to bottom in a group hence ionization energy decreases from top to bottom.
Beryllium will have the highest. Down a group ionization energy decreases.
Ionization energy increases as you go across a period, but as you go down a group it decreases.
Ionization energy increases as we go across a period. Its value decreases as we go down a group.