The successive ionization energies (in kJ/mol) for an element are shown below.
`{:(E_(1),E_(2),E_(3),E_(4),E_(5)),(577,1820,2740,11600,14800):}`
What is the electron configuration of this element?

Write electronic configuration of element E.

Write the electronic configuration of the elements B and E.

Ionization potential is the minimum amount of energy needed to remove the outermost electron from the gaseous isolated atom. Its unit is eV/atom or kJ/mol. Successive ionization energy is the amount of energy needed to remove electron successively from a gaseous ion, it may be termed as I.E._2, I.E._3 , .... The difference in the values of I.E._1, I.E._2 , . helps to determine electronic configuration of the elements. Which of the element can make MX type compound (X is the halogen)?

Ionization potential is the minimum amount of energy needed to remove the outermost electron from the gaseous isolated atom. Its unit is eV/atom or kJ/mol. Successive ionization energy is the amount of energy needed to remove electron successively from a gaseous ion, it may be termed as I.E._2, I.E._3 , .... The difference in the values of I.E._1, I.E._2 , . helps to determine electronic configuration of the elements. The order of ionic mobility in aqueous solution of the following ions will be (If R, S belong to same group):

The element with the electronic configuration [ X e] 4f^(7) 5d^(1) 6s^(2) lies in the :

The electronic configuration of an element with atomic number 7 i.e. nitrogen atom is.

The first, second and third ionization energies (E_(1),E_(2)&E_(3)) for an element are 7eV, 12.5 eV and 42.5 eV respectively. The most stable oxidation state of the element will be: