Among the second period elements the actual ionization enthalpies are in the order
Li < B < Be < C < O < N < F < N
Explain why
Be has higher `Delta_iH` than B

Among the second period elements the actual ionization enthalpies are in the order Li Explain why O has lower Delta_iH than N and F ?

Why the second ionization enthalpy is greater than the first ionization enthalpy?

How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?

Which elements from the following pairs has highest ionization enthalpy. B and Al, N and Bi.

Which element from the following pair has highest ionization enthalpy B and TI.

The following table shows the position of six elements A,B,C,D,E and F in the periodic table Using the above table , answer the following questions: Out of D and E, which one has a bigger atomic radius and why?

Answer the following questions: The elements in the second period :Li, Be, B,C,N,O,F and Ne have electrons in the two shells K and L . Write down the electronic configuration of these elements.

Why are the first ionization energies of the higher elements of group 16 lower than those of group 15 elements?

Study the below given periodic table in which four elements are indicated by alphabets A,B,C and D Among 'A' and 'C' which element has larger atomic radius?why?

Elements of Group 16 generally show lower values of first ionization enthalpy compared to the elements of corresponding period of group15. why?