You may need the following data: electron affinity of oxygen EA_1=-141 kJ/mol, EA_2=744 kJ/mol; ionization energy of calcium IE_1=590 kJ/mol, IE_2=1145 kJ/mol for the formation of oxide or sulphide ions has been determining to be endothermic to … The general trend for electron affinity down the group is that it decreases because of the increase in atomic radius.The exception of \$\ce{Cl}>\ce{F}\$, I can understand is because fluorine has a high electron density and it is unfavourable to add more electrons as it would only increase the electron -electron repulsion. Use this … Calculate the second electron affinity of oxygen using the information below: O^- (g) + e^- ? Click here to buy a book, photographic periodic table poster, card deck, or 3D print based on the images you see here! Electron affinity increases from the first element to the second element in a group. Solution: When an electron is added to negatively charged ion, it experiences more repulsion rather than attraction. When an electron is added to a neutral gaseous oxygen atom , the process is exothermic and 141 kJ energy is liberated. Therefore spin pair repulsion exists and energy is needed to overcome it ...however the 1st electron affinity of oxygen is still negative. none of these. O^2+ (g) EA_2 =? Hence, oxygen has lesser electron affinity than that of sulphur and however in a group, it decreases from top to bottom as size increases. The second electron affinity (EA 2) is always larger than the first electron affinity (EA 1) as it is hard to add an electron into a negative ion than a neutral atom. O-(g) + e- O 2-(g) EA= +780 kJ. This can be understood with the following example of the successive electron affinity of oxygen: O(g) + e- O-(g) EA= -141 kJ. Electron affinity is the amount of energy required to detach one electron from a negatively charged ion of an atom or molecule. For illustration, the overall E.A. b) oxygen has high electron affinity . B. the ionization energy of O2-. Use the Born-Haber cycle and data from Appendix IIB and Table 9.3 in the textbook to calculate the lattice energy of CaO. d) O-ion has comparatively larger size than oxygen atom. It is indicated using the symbol Ea and is usually expressed in units of kJ/mol. The electron affinity of oxygen is equal to A. the ionization energy of O-. It is applicable to all p-block element groups. C. the second ionization energy of O. D. twice the electron affinity of O+.E. But in the case of oxygen, the first electron is added to a 2p subshell where one electron is already present. c) O-ion will tend to resist the addition of another electron . a) oxygen is more electronegative . 1st Electron Affinity is usually exothermic as the energy released when the nucleus attracts the the additional electron is larger than the energy absorbed to overcome inter-electronic repulsion. 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