What is the difference between 1st 2nd 3rd ionization energies?

Answer 1

The second ionization energy is always greater than the first because once you have pulled off the first electron, you are now trying to remove the second electron from a positively charge ion. Because of the electrostatic attraction between + and -, it is more difficult to pull an electron away from a positively charge ion than a neutral atom.

Answer 2

The second ionization energy is greater than the first. This is because once one electron has been removed, the nucleus has more positive charge per electron left- the atom becomes an ion, positively charged, right? So it is now harder to remove the second electron as it is held more strongly by the nucleus.. the third ionization energy is even larger, and so on...

ionization energies decrease down the Group

or there is increased shielding down Group

Answer 3

the 1st ionization energy is the energy needed to remove an electron from a neutral atom.

the 2nd IE is the energy needed to remove an electron from a +ve ion that carry one +ve charge.

the 3rd IE is the energy needed to remove an electron from a +ve ion that carry two +ve charges.

note : the nth ionization energy is less than the nth+1 ionization energy.

Answer 4

First ionization energy is the energy required to remove one electron from an atom. Second ionization energy is the energy required to remove a second one, and third, well, you get the picture. An ionization energy chart can help you determine what group an element is in. If an element has a relatively low first ionization energy, but then there's a huge jump in ionization energy to second, then it's probably a group 1 element, since group 1 elements (like sodium or potassium) only need to lose 1 electron.

Answer 5

The first ionization energy is the energy it takes to remove an electron from a neutral atom.

The second ionization energy is the energy it takes to remove an electron from a 1+ ion. (That means that the atom has already lost one electron, you are now removing the second.)

The third ionization energy is the energy it takes to remove an electron from a 2+ ion. (That means that the atom has already lost two electrons, you are now removing the third.)

And 2nd ionization energy is higher than 1st ionization energy, 3rd is higher than 2nd, and so forth.

(I just wanted to clarify from an above answer: 2nd i.e. is not the energy it takes to remove 2 electrons together; it's the energy it takes to remove 1 electron from an atom that has already lost 1 electron before.)

Answer 6

the second ionization energy level is always higher then the first ionization energy because at the second level there are more protons (+) then electrons (-) holding (attracting) the electrons down therefore more energy is required to pull out the second electron then the first.( the ionization energy increases as you pull the electrons out and go down an elements electron shells).

Answer 7

The first ionization energy is the energy required to remove the first electron from an atom, the second ionization energy is the energy required to remove the second electron, and the third ionization energy is the energy required to remove the third electron. Typically, each successive ionization energy is higher than the previous one due to the increased electrical attraction between the positively charged nucleus and the remaining electrons.

Answer 8

difference depends on atoms, Each succeeding ionization energy is larger than the preceding energy. I 1 <I 2 <I 3 <...<I n