Question

An element has an atomic number of $15$ with which of the following elements will it show similar chemical properties?
(A) $Be\left(4\right)$
(B) $Ne\left(10\right)$
(C) $N\left(7\right)$
(D) $O\left(8\right)$

Answer 1

Hint: Chemical elements that belong to the same group have the same valence electrons and have similar properties. Nitrogen, phosphorus, arsenic, antimony, and bismuth were the elements that belong to the group $15$ . The element with atomic number $15$ is phosphorus.

Complete Step By Step Answer:
The modern periodic table was introduced by Mendeleev, in which the chemical elements are represented in a table in the increasing order of atomic numbers. These chemical elements in the periodic table were arranged in vertical columns and horizontal rows. The vertical columns were known as groups and the horizontal rows were known as periods. There are a total of $7$ periods and $18$ groups in the periodic table.
The group $15$ consists of the elements of nitrogen, phosphorus, arsenic, antimony, and bismuth. The element with atomic number $15$ is phosphorus. Thus, phosphorus has similar properties to nitrogen, arsenic, antimony, and bismuth.
In the given options, nitrogen is present. The atomic number of nitrogen is $7$ and the chemical symbol of nitrogen is $N$ .
Thus, an element that has an atomic number of $15$ will show similar chemical properties with the element of $N\left(7\right)$ .
Option C is the correct one.

Note:
The elements that belong to the same group have similar properties; it is due to the presence of the same valence electrons. The oxidation state, valency of the chemical elements that belong to the same group will be similar.