Element with the largest third ionization energy?
It is Be see http://en.wikipedia.org/wiki/Ionization_... I guess it would be Li as the remaining is in a 1s AO that is very close to the +3 nucleus. But in Be the nuclear charge has increased to+4 and the two remaining e⁻s in the 1s do a poor job of screening each other from that increased nuclear charge (the Slater coeff for a 1s e⁻ is 0.3) so Zeff(Be^2+) > Zeff(Li^2+).
What is the difference between the first, second, and third ionization energies of an element?
They are removing the first, second and third electrons. They get greater as you go along. This is because the electrons get closer to nucleus, which the causes a greater positive pull And also there is less shielding from the other electrons
Which element has the largest difference between the second and third ionization energies?
Mg as you break into a new inner shell for the 3rd IE
How do first, second and third ionization energies compare and contrast?
The first ionization energy is defined as the amount of energy needed to remove the outermost, or highest energy, electron from a neutral atom in the gas phase. This means that it requires the least amount of energy to remove it. The second ionization energy is the amount of energy needed to remove the second outermost electron, etc. As you remove electrons from the shell of an atom, the farthest most electron gets closer and closer to the nucleus, making it harder and harder to remove the electron.You can think of this process is something similar to how our solar system functions; with each planet being an electron and the sun as the nucleus. The pull of the sun on Mercury (the innermost electron) is much greater than the pull on Neptune (the outermost electron).Therefore , the first ionization energy is less than the second, which is less than the third, etc.The differences in magnitude of these energies depends on the element. This can be explained by orbitals and electron shielding.
Which element below has the largest difference between the second and third ionization energies?
My guess it would be Mg because it is group 2 metal with 2 valence electrons.
Why is the second ionization energy of an element higher than the first ionization energy?
The second ionization energy of any element will be higher than its first ionization energy in the way that the first electron is being removed from a neutral atom and the 2nd electron is being removed from a positively charged ion that is already electron deficient, as already 1 electron is being removed so the effective nuclear charge will definitely going to increase , which causes a strong attraction between the nucleus and the outermost electron. So the second ionization energy is higher than that of first ionization energy of an element.Hope You got your ans. :)
Which element has greatest difference between first and second ionization energies?
Na think about it. every one of these atoms would have a higher second ionization energy because the loss of an electron causes the atom to shrink in size. when a group one element loses an electron, it becomes most like the noble gases. therefore, the second ionization energy will be extremely high.