Question

Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization energy required ionization energy required Fr — Fr te ? Sn Sn +e ? Pb Pb + e Cs → Cs +ė ? He He té ? Ne → Net te 1 (least) 3 (most)

Answer 1

Jonisation energy is the energy required to remove the most loosely bound electron from a gaseous atom in its ground state to form a cation. As the size of the atom un creases effective nuclear change experienced. on the valence electron decreases, electron valence electron can easily be removed and conisation energy decreases Hence we can say along a period ionisation energy increases from left to right AM Down the group ionisation energy decreases ie knisation energy is least for 1st group metals and maximum for 18th group (noble gases) I fy → httē ; Fo belongs to ist group. Hence least le 12 Pb Pbitte Pb: 14th group. B He Het te He: 18th group. (Noble gas). It has completely filled k shell. Difficult to remove one a @ICS -> cst +ē ; Cs. It group 12 Sn Sut t ê ; Sn 14th group 13 Ne Wet tê; Ne: 18th group.