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The correct order of second I. E. of C, N, O and F are in the order:
- a)F > O > N > C
- b)C > N > O > F
- c)O > N > F > C
- d)O > F > N > C
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
The correct order of second I. E. of C, N, O and F are in the order:a)...
The electronic configuration of oxygen is 1s2 2s2 2p4 on removing one electron we get a half filled configuration which is stable. So among these it will b the hardest to remove the second electron of oxygen. The size of fluorine is less than nitrogen. On removing one electron, its size will decrease again and so, its second I.E will be greater than nitrogen. carbon has the least second I.E because on removing the second electron, it will complete octet and attain stability
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Community Answer
The correct order of second I. E. of C, N, O and F are in the order:a)...
The correct order of second ionization energy of elements C, N, O, and F is:
Explanation:
First, let us understand what second ionization energy is. It is the energy required to remove a second electron from a positively charged ion of an element. The second ionization energy is always higher than the first ionization energy because it is more difficult to remove an electron from a positively charged ion than from a neutral atom.
Now, let us compare the second ionization energies of the given elements:
- Carbon (C): The first ionization energy of carbon is relatively low (1086.5 kJ/mol), but the second ionization energy is considerably higher (2352.6 kJ/mol). This is because after losing one electron, a positively charged carbon ion (C+) becomes more stable by having a noble gas electron configuration (similar to helium). Removing a second electron requires more energy because it disrupts this stable configuration.
- Nitrogen (N): The first ionization energy of nitrogen is higher than carbon (1402.3 kJ/mol), and the second ionization energy is even higher (2856 kJ/mol). This is because after losing one electron, the resulting nitrogen ion (N+) still has a half-filled p-subshell, which is a relatively stable configuration. Removing a second electron requires more energy to disrupt this stability.
- Oxygen (O): The first ionization energy of oxygen is higher than nitrogen (1313.9 kJ/mol), and the second ionization energy is even higher (3952.3 kJ/mol). This is because after losing one electron, the resulting oxygen ion (O+) has a stable noble gas configuration (like neon). Removing a second electron requires even more energy to disrupt this stability.
- Fluorine (F): The first ionization energy of fluorine is the highest among the given elements (1681 kJ/mol), and the second ionization energy is even higher (3374.2 kJ/mol). This is because after losing one electron, the resulting fluorine ion (F+) has a stable noble gas configuration (like neon). Removing a second electron requires even more energy to disrupt this stability.
Therefore, the correct order of second ionization energy is:
O > F > N > C
which is given in option (D).
Explanation:
First, let us understand what second ionization energy is. It is the energy required to remove a second electron from a positively charged ion of an element. The second ionization energy is always higher than the first ionization energy because it is more difficult to remove an electron from a positively charged ion than from a neutral atom.
Now, let us compare the second ionization energies of the given elements:
- Carbon (C): The first ionization energy of carbon is relatively low (1086.5 kJ/mol), but the second ionization energy is considerably higher (2352.6 kJ/mol). This is because after losing one electron, a positively charged carbon ion (C+) becomes more stable by having a noble gas electron configuration (similar to helium). Removing a second electron requires more energy because it disrupts this stable configuration.
- Nitrogen (N): The first ionization energy of nitrogen is higher than carbon (1402.3 kJ/mol), and the second ionization energy is even higher (2856 kJ/mol). This is because after losing one electron, the resulting nitrogen ion (N+) still has a half-filled p-subshell, which is a relatively stable configuration. Removing a second electron requires more energy to disrupt this stability.
- Oxygen (O): The first ionization energy of oxygen is higher than nitrogen (1313.9 kJ/mol), and the second ionization energy is even higher (3952.3 kJ/mol). This is because after losing one electron, the resulting oxygen ion (O+) has a stable noble gas configuration (like neon). Removing a second electron requires even more energy to disrupt this stability.
- Fluorine (F): The first ionization energy of fluorine is the highest among the given elements (1681 kJ/mol), and the second ionization energy is even higher (3374.2 kJ/mol). This is because after losing one electron, the resulting fluorine ion (F+) has a stable noble gas configuration (like neon). Removing a second electron requires even more energy to disrupt this stability.
Therefore, the correct order of second ionization energy is:
O > F > N > C
which is given in option (D).
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