Why does an atom does not react if it has with 8 electrons in 3rd energy level like Argon gas?
Noble gases are stable.Atoms having 8 electrons at last orbital are called noble gases.
Actually since you are in 8th standard it may be difficult to understand.But Ill explain it to u below
Actually it is not necessary to dig deep into quantum mechanics. There are several reasons why noble gasses are stable (as gasses at room temperature).
First of all, there is the obvious full valence shell. Trend in the periodic table make clear that the charge of the nucleus grows from left to right in every period. The attractive force towards the electrons therefore increases. (This holds also from top to bottom.) Electrons in lower orbitals (n<periodn<period) now shield the charge of the nucleus. This will be somewhat the same throughout the period. (The orbitals also shrink due to higher charge of the nucleus.) In noble gasses the valence shell is completely filled, providing quite a good shield for the next shell. Also the increase in the main quantum number means a significant increase in the energy level of the next orbital. This makes it unlikely, that a noble gas will accept another electron.
Due to the high charge of the nucleus it is also not easy to remove an electron from an orbital. However, this is possible from (at least) Argon on downwards. For example: HArFHArF is stable in a matrix at room temperature. It has a strong covalent σσ bond (H−Ar+H−ArX+) and a not quite as strong ionic bond ([HAr]+⋯F−[HAr]X+⋯FX−). Krypton already does some fancy chemistry, that is stable at room temperature. As Uncle Al has pointed out Xenon is well known for its reactivity.
But why the sudden change? It is fairly intuitive, that the maximum electron density for each orbital with increasing main quantum number is also further away from the nucleus. That makes the valence shell very well polarizeable. Also the electrons are better shielded by the previous shells. However, the natural occurrence of these elements are as (homonuclear) gasses.
However, if you bring these elements in close contact with each other it was found out, that they have a very small dissociation energy (De<1 meVDe<1 meV). This is due to dispersion, and van-der-Waals Forces, which is the main interaction between these elements. However, in He2HeX2no binding mode was observed (instant dissociation).
But that still does not answer, why those elements are stable as gasses, as pointed out that there are in fact attractive forces. The reason is as simple as obvious: Entropy. If two noble gasses would form a molecule/adduct, the bond/association energy of this molecule would have to compensate for the loss of entropy (Two volume elements would become one, hence the gas would have to expand to cover the room previously occupied, which requires work energy).
The explanation by tschoppi also covers, why from a MO point of view there could not be a bond in He2HeX2. Go ahead and ask yourself the question if this would be true for He3HeX3. We also know that orbital overlap is only one component to the truth. There are many other more. If it was not for such a nice thing like dispersion and other weak chemical interactions we would not exist.
Actually since you are in 8th standard it may be difficult to understand.But Ill explain it to u below
Actually it is not necessary to dig deep into quantum mechanics. There are several reasons why noble gasses are stable (as gasses at room temperature).
First of all, there is the obvious full valence shell. Trend in the periodic table make clear that the charge of the nucleus grows from left to right in every period. The attractive force towards the electrons therefore increases. (This holds also from top to bottom.) Electrons in lower orbitals (n<periodn<period) now shield the charge of the nucleus. This will be somewhat the same throughout the period. (The orbitals also shrink due to higher charge of the nucleus.) In noble gasses the valence shell is completely filled, providing quite a good shield for the next shell. Also the increase in the main quantum number means a significant increase in the energy level of the next orbital. This makes it unlikely, that a noble gas will accept another electron.
Due to the high charge of the nucleus it is also not easy to remove an electron from an orbital. However, this is possible from (at least) Argon on downwards. For example: HArFHArF is stable in a matrix at room temperature. It has a strong covalent σσ bond (H−Ar+H−ArX+) and a not quite as strong ionic bond ([HAr]+⋯F−[HAr]X+⋯FX−). Krypton already does some fancy chemistry, that is stable at room temperature. As Uncle Al has pointed out Xenon is well known for its reactivity.
But why the sudden change? It is fairly intuitive, that the maximum electron density for each orbital with increasing main quantum number is also further away from the nucleus. That makes the valence shell very well polarizeable. Also the electrons are better shielded by the previous shells. However, the natural occurrence of these elements are as (homonuclear) gasses.
However, if you bring these elements in close contact with each other it was found out, that they have a very small dissociation energy (De<1 meVDe<1 meV). This is due to dispersion, and van-der-Waals Forces, which is the main interaction between these elements. However, in He2HeX2no binding mode was observed (instant dissociation).
But that still does not answer, why those elements are stable as gasses, as pointed out that there are in fact attractive forces. The reason is as simple as obvious: Entropy. If two noble gasses would form a molecule/adduct, the bond/association energy of this molecule would have to compensate for the loss of entropy (Two volume elements would become one, hence the gas would have to expand to cover the room previously occupied, which requires work energy).
The explanation by tschoppi also covers, why from a MO point of view there could not be a bond in He2HeX2. Go ahead and ask yourself the question if this would be true for He3HeX3. We also know that orbital overlap is only one component to the truth. There are many other more. If it was not for such a nice thing like dispersion and other weak chemical interactions we would not exist.
