Question

Based on position in the periodic table and electron configuration, arrange these elements in order of decreasing Ei1.

Rank the elements from highest to lowest ionization energy. To rank items as equivalent, overlap them.

Hints

Help Reset Na F Li N B O Lowest ionization energy Highest ionization energy Part B Examine the following set of ionization energy values for a certain element. How many valence electrons does an atom of the neutral element possess? Ionization step Ionization energy (kJ/mol) Ei1 1012 Ei2 1903 Ei3 2912 Ei4 4956 Ei5 6273 Ei6 22233 Ei7 25997 Enter your answer numerically as an integer.

Answer 1

The electronic configurations of the atoms are as follows: Na(11)-1s 2s 2p6 3s F(9) 1s 2s 2p Li(3) 1s 2s N(7) 1s 2s 2p B(5)-1s 2s 2p' O(8) 1s 2s 2p In the periodic table, when we move from left to right direction in a period, atomic size of the elements decreases due to increase in nuclear charge. Therefore, ionization energy also increases while going from left to right in a period. Also, since the size of sodium atom is the largest amongst all, it will have the lowest onization energy Hence, the order should be: But, according to the electronic configuration, nitrogen have half-filled electronic configuration. Hence, it is more stable and requires more energy to remove an electron from its outermost shell. Therefore, ionization energy of nitrogen is larger than that of oxygen. Therefore, the final order of ionization energy from highest to lowest is as follows F>N>O> B> Li> Na According to the given ionization energies of a certain element, there is large jump from Ei5 (6273) to Ei6(22233). This implies, that there are 5 valence electrons in that element Hence, the electronic configuration wil be ns np and it belongs to 5th group

Answer 2

F>N>O>B>Li>Na