iii) Why Beryllium has more Ionization Potential value than Boron?
iv) Why Nitrogen has more Ionization Potential value than oxygen?
a) CH
2 = C = C - CH - CH
2
- CH
2
- CH - CH
2
| | | | Cl Cl OH OH
Depending on the above structure of the compound give answers for the following questions.
i) What are the substituents in the above compound?
ii) What is the functional group in the above compound.
iii) What is the IUPAC name of the compound.
iv) What type of Hybridisation present on 6th and 7th carbon atoms of the above compound.
Answers
(iii) Following are the electronic configurations of two elements:
Boron: 1s2 2s2 2p1
Beryllium: 1s2 2s2
According to periodic trends, boron should have a higher ionization energy but because its valence electron (2p1) is shielded by the 2s electrons, less energy is required to remove the 2p electron(s) from a boron atom than is requried to remove the 2s electron from a beryllium atom.
(iv) Following are the electronic configurations of two elements:
N: 1s2, 2s2, 2p3
O: 1s2, 2s2, 2p4
As we can see that Nitrogen has half filled p orbitals which is relatively stable configuration as compared to 2p4 configuration of Oxygen atom so it is difficult to remove one electron from this stable configuration. Further, removal of one electron from Oxygen atom is relatively easy because it results in half filled stable p orbital configuration. That's why ionisation energy of Nitrogen is more than Oxygen.
(a) It would be easy to answer this question if the compound's structure is more clear. It is difficult to understand.
Hope this helps... : )