Question

What are Hydrogen molecules?
A) Monoatomic and form $X_2^{2 - }$ type ions
B) Diatomic and form $X_2^ -$ type ions
C) Diatomic and form $X_{}^ -$ as well as $X_{}^ +$ type ions
D) Monoatomic and form $X_{}^ -$ type ions

Answer 1

In this question, we know the electronic configuration of a Hydrogen atom is $1{s^1}$. For our solution first we want to write the electronic configuration of each hydrogen molecule with respect to given ionization power and check for the stability of the molecule.

Complete step-by-step answer:
In order to solve this question we are going to write the electronic configuration of the ions in their current state. We know that the molecule which contains only one atom is termed as monatomic and molecule with two atoms is termed as diatomic molecule.

The electronic configuration of a Hydrogen atom is $1{s^1}$. In order to attain stability it will always share an electron from another hydrogen atom and form a stable diatomic molecule. Generally when an atom loses an electron it gains positive charge and while gaining an electron it will become negatively charged.

If we write the Electronic configuration of all the four ions:

(a) The electronic configuration of $X_2^{2 - }$ ions is: Here we have 2- ionization power it means the molecule gain two electron and forms an unstable electronic configuration and doesn’t form monoatomic molecule because now it contain 3 electrons in total.

(b) The electronic configuration of $X_2^ -$ ions is: Here we have 1- ionization power it means the molecule gains one electron and forms a stable electronic configuration and forms a diatomic molecule because now it contains 2 electrons in total.

(c) the electronic configuration of $X_{}^ -$ and $X_{}^ +$ ions is: Here we have 1- ionization power it means the molecule gain one electron and forms hydride ion ($H_{}^ -$) and forms a stable diatomic molecule because now it contain 2 electrons in total. Next we have 1+ ionization power. It means the molecule loses one electron and forms hydronium ion ($H_{}^ +$) and forms a stable diatomic molecule.

(d) the electronic configuration of $X_{}^ -$ ions is: Here we have 1- ionization power it means the molecule gain one electron and forms hydride ion ($H_{}^ -$) and forms a stable diatomic molecule not a monatomic molecule.

This proves that Hydrogen can form diatomic molecules with $H_{}^ -$and $H_{}^ +$type ions and hence option ‘C’ is correct.

Note: Student can make in writing the correct electronic configuration of the elements. Also an important concept here is that the stability of each molecule depends on electrons present in them. Particles consist of a single nucleus with a positive charge encompassed by a haze of negatively charged electrons. At the point when ions approach each other intently, the electron clouds cooperate with one another and with the cores.