Based on the actual electron configurations, explain why the ionization energy of neon is greater than that of fluorine.
2006-09-27 12:24:23 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Ioniation energy is the energy necessary to remove an electron from a neutral atom. Neon has a full outer shell, and is therefore very stable. It is much harder to remove and electron from it that from fluorine, which is extremely electronegative.
2006-09-27 12:28:02 · answer #1 · answered by Anonymous · 0⤊ 0⤋
Neon (Ne) has an atomic number of 10 and is at the 2 Period and the 18 (VIIIA) group of the P.Table.
Fluorine has an atomic number of 9 and it is at the 2 Period and the 17 (VIIA) group of the Table.
So they are in the same period. The ionization energy grows from left to the right for elements of the same period because the number of the protons in the nucleus grows.
So the ionization energy of Ne is greater than that of F. Plus, Neon is a noble gas - 8 electrons in outer shell - that means it has a very stable electron configuration. Very hard to remove an electron.
2006-09-27 12:37:54 · answer #2 · answered by Dimos F 4 · 0⤊ 0⤋