Question

An element x (atomic number 17) reacts with an element y (atomic number 20) to form a divalent halide. (a) what is the position of element x and y in the periodic table? (b) what will be the nature of oxide of element y? identify the nature of bonding in the compound formed.

Answer 1

a ) Position of X = 17 group , 3rd period

Position of Y = 2nd group ,4 th period

b) metal oxide

c) ionic bonding

Answer 2

Answer:

For a: X belongs to Period 3 and Group 17 of the periodic table whereas element Y belongs to Period 4 and Group 2 of the periodic table.

For b: It will form a basic oxide.

For c: Compound formed will have ionic bond.

Explanation:

• For a:

We are given two elements:

X having atomic number 17. The electronic configuration of this element is $1s^22s^22p^63s^23p^5$

This element belongs to Group 17 and period 3 of the periodic table.

Y having atomic number 20. The electronic configuration of this element is $1s^22s^22p^63s^23p^64s^2$

This element belongs to Group 2 and period 4 of the periodic table.

• For b:

Element Y is a metal and when a metal reacts with oxygen to produce metal oxide, it forms basic oxide.

$Y+O\rightarrow YO$

• For c:

Ionic bond is formed by the complete transfer of electrons from one element to another element. The element which loose electrons is known as electropositive element and the one which gains electron is known as electronegative element.

This bond is formed between a metal and a non-metal.

Element X is Chlorine and element Y is calcium.

So, calcium will loose 2 electrons and two chlorine atoms will gain 1 electron each. Thus, forming an ionic bond.