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The correct order of second ionization potential among the following elements : Be, B, C, N and O is
- a)N > O > B > C > Be
- b)Be > C > B > O > N
- c)O > N > B > C > Be
- d)O > N > C > B > Be
Correct answer is option 'C'. Can you explain this answer?
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Understanding Second Ionization Potential
The second ionization potential (IP2) refers to the energy required to remove the second electron from a gaseous atom. The order of IP2 among the elements Be, B, C, N, and O can be explained through their electronic configurations and stability.
Factors Influencing Ionization Potential
- Electron Configuration:
- Be (1s² 2s²) has a stable electron configuration, and removing one electron results in a filled 1s subshell.
- B (1s² 2s² 2p¹) has a less stable configuration after the removal of one electron.
- C (1s² 2s² 2p²) and N (1s² 2s² 2p³) have half-filled and stable configurations which influence IP2.
- O (1s² 2s² 2p⁴) has a configuration that is less favorable after losing the first electron.
- Nuclear Charge and Shielding:
- As you move from Be to O, the nuclear charge increases, which increases the attraction between the nucleus and the electrons, thereby increasing the second ionization potential.
Order of Second Ionization Potential
1. Oxygen (O): Highest IP2 due to stable electron configuration after removal of one electron.
2. Nitrogen (N): Next highest, as it has a half-filled p orbital, providing stability.
3. Carbon (C): Lower than N, due to its less stable configuration after one electron is removed.
4. Boron (B): Lower than C as it has a single p electron, making it easier to remove.
5. Beryllium (Be): Lowest IP2 because after removing one electron, it reaches a stable noble gas configuration.
Conclusion
Thus, the correct order of second ionization potential is O > N > C > B > Be, confirming that option 'C' is correct.
The second ionization potential (IP2) refers to the energy required to remove the second electron from a gaseous atom. The order of IP2 among the elements Be, B, C, N, and O can be explained through their electronic configurations and stability.
Factors Influencing Ionization Potential
- Electron Configuration:
- Be (1s² 2s²) has a stable electron configuration, and removing one electron results in a filled 1s subshell.
- B (1s² 2s² 2p¹) has a less stable configuration after the removal of one electron.
- C (1s² 2s² 2p²) and N (1s² 2s² 2p³) have half-filled and stable configurations which influence IP2.
- O (1s² 2s² 2p⁴) has a configuration that is less favorable after losing the first electron.
- Nuclear Charge and Shielding:
- As you move from Be to O, the nuclear charge increases, which increases the attraction between the nucleus and the electrons, thereby increasing the second ionization potential.
Order of Second Ionization Potential
1. Oxygen (O): Highest IP2 due to stable electron configuration after removal of one electron.
2. Nitrogen (N): Next highest, as it has a half-filled p orbital, providing stability.
3. Carbon (C): Lower than N, due to its less stable configuration after one electron is removed.
4. Boron (B): Lower than C as it has a single p electron, making it easier to remove.
5. Beryllium (Be): Lowest IP2 because after removing one electron, it reaches a stable noble gas configuration.
Conclusion
Thus, the correct order of second ionization potential is O > N > C > B > Be, confirming that option 'C' is correct.
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