Respuesta :
as I think my friend
option a and c can it's answer
a can it's answer
BECAUSE OF STRONG ATTRACTIVE FORCE BETWEEN ELECTRON AND PROTON, THERE IS MUCH ENERGY REQUIRED TO REMOVE OR ACCEPT AN ELECTRON.
and c can it's answer beacuse
When we go down the group, the size of atom increases due to which the shield effect of d and f orbital decreases. Hence, required less ionization enthalpy.
hope it will helpful for you Mark my answer as brainly
option a and c can it's answer
a can it's answer
BECAUSE OF STRONG ATTRACTIVE FORCE BETWEEN ELECTRON AND PROTON, THERE IS MUCH ENERGY REQUIRED TO REMOVE OR ACCEPT AN ELECTRON.
and c can it's answer beacuse
When we go down the group, the size of atom increases due to which the shield effect of d and f orbital decreases. Hence, required less ionization enthalpy.
hope it will helpful for you Mark my answer as brainly
Explanation:
When an electron is removed from a gaseous atom or ion then the energy required to do so is known as ionization energy.
When we move down a group then there is increase in mass of elements. This is due to increase in the number of electrons in an atom which increase the number of shells also.
Hence, these layers of electron shells will shield the nucleus of the atom. As a result, it would be easy to remove an electron from the outermost shell. Because of this less energy is needed to remove an electron hence, larger is the atomic radius of an atom lower will be its ionization energy.
Thus, we can conclude that of elements in the same group those at the bottom of the periodic table have low ionization energies because of following.
- Layers of electron shells shield the protons attractive force.
- Their atomic radius is larger.
