Question

elements like barium located toward thr bottom of a group have a lower Attraction for their valence electrons because they have a

Answer 1

Answer:

Barium has a lower attraction for their valence electrons because there are a large number of electrons between the valence electrons and nucleus. And these electron cause great repulsion.

Explanation:

• Barium is present in group number 2. It is present in the last place.  Its atomic number is 56.
• It has 2 electrons in the valence shell. There are 54 electrons between the nucleus and the valance electrons.
• These electrons cause repulsion to each other and the attraction of nucleus lowers for valance electrons due to long distance.

Answer 2

Explanation:

Barium is an alkaline earth metal and it's atomic number is 56 with electronic configuration [tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}4d^{10}5s^{2}5p^{6}6s^{2}.

This results in more number of shells in a barium atom. Hence, valence shell moves far away from the nucleus due to this there is very less attraction between the valence electrons and nucleus of Ba atom.

Thus, we can conclude that elements like barium located toward the bottom of a group have a lower attraction for their valence electrons because they have greater atomic mass.