Question

describe the electronic configuration of noble gases metals and nonmetals.​

Answer 1

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Answer:

In the chemical characteristics of both metals and non-metals we have studied that these are different because of difference in the electronic configuration of their atoms. In fact, the atoms of both have an urge or desire to acquire the electronic configuration of nearest noble gas atoms which are quite stable. the elements belonging to noble gas family are:

1. Helium (He) -----> (2)

2. Neon (Ne) ----> (2,8)

3. Argon (Ar) ----> (2,8,8)

4. Krypton (Kr)----> (2,8,18,8)

5. Xenon (Xe) ----> (2,8,18,18,8)

6. Radon (Rn) ----> (2,8,18,32,18,8)

The last member is radioactive in nature. It we look at electronic distribution of these elements, we find that the first element Helium has 2 electrons dear outermost shell also called valence shell. We quiet often say that Helium has a complete duplet while the other member have complete octet.

Since, the member of the noble gas family have the maximum number of electrons in their valence shells of the atoms that are premissible according to Bohr - Bury rule, these are quite stable. Their atoms do not have any desire to take part in chemical combination.

Now let us look at the electronic configuration of some metals and nonmetals:

Metals:

1. Sodium (Na) ----> (2,8,1)

2. Magnesium (Mg)----> (2,8,2)

3. Aluminium (Al) ----> (2,8,3)

4. Potassium (K) ----> (2,8,8,1)

5. Calcium (Ca) ----> (2,8,8,2)

Non - metals:

1. Nitrogen (N) ----> (2,5)

2. Oxygen (O) ----> (2,6)

3. Fluorine (F) ----> (2,7)

4. Sulphur (S) ----> (2,8,6)

5. Chlorine (Cl) ----> (2,8,7)

From the electronic configuration, it is quite clear that neither the atoms of metals nor of non-metals have a stable configuration like noble gas elements. This means that dear atoms do not have either 2 or 8 electrons in their valence shells. However, they have strong urge or desire to achieve the same. Metals listed above have the configuration of noble gas elements like Neon or Argon if their are atoms lost electrons present in the valence shell. Similarly, the non-metals listed can achieve the same if their atoms gain certain number of electrons.

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Answer 2

Answer:

In the chemical characteristics of both metals and non-metals we have studied that these are different because of difference in the electronic configuration of their atoms. In fact, the atoms of both have an urge or desire to acquire the electronic configuration of nearest noble gas atoms which are quite stable. the elements belonging to noble gas family are:

1. Helium (He) -----> (2)

2. Neon (Ne) ----> (2,8)

3. Argon (Ar) ----> (2,8,8)

4. Krypton (Kr)----> (2,8,18,8)

5. Xenon (Xe) ----> (2,8,18,18,8)

6. Radon (Rn) ----> (2,8,18,32,18,8)

The last member is radioactive in nature. It we look at electronic distribution of these elements, we find that the first element Helium has 2 electrons dear outermost shell also called valence shell. We quiet often say that Helium has a complete duplet while the other member have complete octet.

Since, the member of the noble gas family have the maximum number of electrons in their valence shells of the atoms that are premissible according to Bohr - Bury rule, these are quite stable. Their atoms do not have any desire to take part in chemical combination.: