Question

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Answer 1

Answer:

the elements 1

$568this \: formua$

Explanation:

ans

$20 \: eleement \: isli$

Answer 2

Explanation:

1. The atomic size of alkali metal atom is big. So, the outermost electron is far away from the positively chraged nucleus. The valence shell electron can be easily removed as the attractive force experienced by the valence electron is very low. Hence, alkali metals have low ionisation enthalpy.

2. noble gases

So technically, the noble gases have the largest ionization energies, but since they're special and it's not often that electrons would even be removed from the atom (it rarely occurs), we would usually say that the halogens is the group with the largest ionization energies.

3.The first ionization of Beryllium is greater than that of Boron because Beryllium has a stable complete electronic configuration (1s22s2) so it, require more energy to remove the first electron from it, where as Boron has electronic configuration (1s22s23s1) which need lesser energy than that of Beryllium.

4.Oxygen also has an unexpectedly low ionisation energy, less than that of nitrogen. This is due to an electron being added to an already half full orbital in oxygen, which results in electron electron repulsion, which will lower the ionisation energy.