Which of the following statements is/are wrong:a)Van der Waals radius of iodine is more than its covalent radiusb)All isoelectronic ions belong to same period of the periodic tablec)I.E1 of N is higher than that of O while I.E2 of O is higher than that of Nd)The electron affinity N is almost zero while that of P is 74.3 kJ mol–1Correct answer is option 'D'. Can you explain this answer?

Question

Which of the following statements is/are wrong:a)Van der Waals radius of iodine is more than its covalent radiusb)All isoelectronic ions belong to same period of the periodic tablec)I.E1 of N is higher than that of O while I.E2 of O is higher than that of Nd)The electron affinity N is almost zero while that of P is 74.3 kJ mol&#8211;1Correct answer is option 'D'. Can you explain this answer?

Answer

Well, noble gases such as Helium, Neon and Argon have an electron affinity nearly zero because they have octet configuration. Due to this reason , they find it hard to attaract electrons. However higher members of Group 18 in the periodic table such Xenon, krypton and radon, do form compound like XeO2 and XeO4 due to the presence of vacant d- orbitals.

Answer

N has fully half filled p orbital and does not have d orbital so it can not add electron so its E.A. is zero,while p adds electron to its d orbitals(for stabilisation).

Answer

Statement D: The electron affinity of N is almost zero while that of P is 74.3 kJ mol^(-1).

Explanation:
- Electron affinity is defined as the energy change that occurs when an electron is added to a neutral atom in its gaseous state to form a negative ion.
- The electron affinity of nitrogen (N) is indeed almost zero, meaning that it requires very little energy to add an electron to a nitrogen atom and form a nitrogen anion (N^-).
- On the other hand, the electron affinity of phosphorus (P) is 74.3 kJ mol^(-1), which is a relatively high value. This indicates that it requires a significant amount of energy to add an electron to a phosphorus atom and form a phosphorus anion (P^-).
- The higher electron affinity of phosphorus compared to nitrogen is due to the larger size and higher effective nuclear charge of the phosphorus atom, which leads to a greater attraction between the incoming electron and the phosphorus nucleus.
- The relatively low electron affinity of nitrogen can be attributed to its half-filled p orbital and the stable electron configuration it possesses. Adding an electron to nitrogen would require it to enter a higher energy level, making it energetically unfavorable.
- It should be noted that electron affinity values can vary depending on the specific reference values used. The value of 74.3 kJ mol^(-1) for the electron affinity of phosphorus is an approximate value and may differ slightly depending on the source.
- Therefore, statement D is incorrect as the electron affinity of N is almost zero, not the electron affinity of P.

Answer

B

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