Video Transcript
Group 15 elements have similarities
in the electronic configurations of their atoms. How do the electronic
configurations of the group 15 elements terminate? (A) d10, (B) d3, (C) p5, (D) p3, or
(E) s2.
In order to solve this problem, let
us first remember that the electronic configuration is based on repeating patterns
within the groups in the periodic table. With respect to the electronic
configuration, the periodic table can be split into four blocks: s, p, d, and f.
When looking at the elements in
group one and two of the periodic table, they have an electronic configuration
ending in s. The same is true for helium. Elements in group 13 through 18 of
the periodic table have an electronic configuration ending in p. The electronic configurations of
the atoms in groups three through 12 terminate in d. And the electronic configurations
for the inner transition metals terminate in f.
Let us find group 15 on the
periodic table. Since group 15 is in the p block
for the electronic configuration, we can conclude that options (A) d10, (B) d3, and
(E) s2 are incorrect.
In order to determine how many
electrons are in the p sublevel of the group 15 elements, let us compare the valence
electrons at the start of the p block, which is group 13. The p-block elements begin with
group 13 and end in the electronic configuration of p1, since there is only one
valence electron in that sublevel. Group 14 elements end in p2, since
there are two valence electrons in that sublevel. And group 15 elements have three
valence electrons and will therefore end in the electronic configuration of p3.
Therefore, the electronic
configurations of the group 15 elements terminate in p3, option (D).
