Group the following electronic configurations of neutral elements in sets according to those you would expect to show similar chemical properties.
a. 1s^22s^22p^63s^23p^3
b. 1s^22s^22p^63s^23p^63d^104s^24p^5 c. 1s^22s^22p^63s^23p^6
d. 1s^22s^22p^3

The pair of elements that tend to show the same chemical properties are a and d.

The elements belonging to the same group tend to show the same chemical properties. Based on the electronic configuration, the element having the same number of valence electrons belongs to the same group.

The valence electrons in the given configurations are:

a. = 5

b. = 7

c. = 8

d. = 5

The element a and d tend to show the same number of valence electrons. Thus both the elements will show the same chemical properties.

The pair of elements that tend to show the same chemical properties are a and d.

For more information about electronic configuration, refer to the link:

link

Option A and D

Explanation:

The element with electronic configuration 1s^22s^22p^63s^23p^3 and the element with electronic configuration 1s^22s^22p^3 will show similar chemical properties as they both have the same valence electrons of 5 each. The valence electron of the two elements shows that they both belong to the same group. Elements in the same group naturally have the same chemical properties because they have the same combining power i.e valence electron.

they are all solids.