Question

which one has lower first ionization enthalpy Be+ or Mg2+ ? plz answer only if u know the answer dont type anything just for points​

Answer 1

Answer:

Mg²

Explanation:

The first ionization enthalpy of magnesium is lower than the first ionization enthalpy of Beryllium Be becuase Be,Mg,Ca belongs to one group ,so down the group ionization energy will decrease so The first ionization enthalpy of magnesium is lower than the first ionization enthalpy of Beryllium Be (Lithium sodium anyhow belongs to first group how ever they are having low ionization potentials than these Be,Mg,Ca)

Answer 2

Answer: Be+ < Mg²+ that is the ionisation enthalpy (I.E) of Be+ is less than Mg 2+ .

Explanation: In any period the noble gas has the highest I.E because of its stability so I.E Be < Ne . But when we talk about Be+ then it has Li like configuration but it should be noted that I.E of Be+ >Li as even though they have same no. of electrons Be+ has an extra proton which pulls the electron with greater force . However, I.E of Be+ will be still less than Ne .So, Li < Be+ <Ne →[1]

Now, Mg is in the 3rd period but Mg 2+ has Ne like configuration. Since, it has two more protons than Ne and the same no. of electrons we can say that I.E of

Ne < Mg 2+ →[2]

From [1] and [2]

Li < Be+ < Ne < Mg 2+

Clearly , Be+ < Mg 2+

Hope it helps