electron affinity of oxygen

Use the Born-Haber cycle and data from Appendix IIB and Table 9.3 in the textbook to calculate the lattice energy of CaO. Solution: When an electron is added to negatively charged ion, it experiences more repulsion rather than attraction. none of these. For illustration, the overall E.A. for the formation of oxide or sulphide ions has been determining to be endothermic to … Electron affinity is the amount of energy required to detach one electron from a negatively charged ion of an atom or molecule. When an electron is added to a neutral gaseous oxygen atom , the process is exothermic and 141 kJ energy is liberated. Electron affinity increases from the first element to the second element in a group. Therefore spin pair repulsion exists and energy is needed to overcome it ...however the 1st electron affinity of oxygen is still negative. Use this … 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. ?H_dep (Mg) -148. kJ/mol Mg(g) first ionization energy 738. kJ/mol c) O-ion will tend to resist the addition of another electron . 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. It is indicated using the symbol Ea and is usually expressed in units of kJ/mol. Other names: Molecular oxygen; Oxygen molecule; Pure oxygen; O2; Liquid oxygen; UN 1072; UN 1073; Dioxygen Permanent link for this species. It is applicable to all p-block element groups. 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 Here are the electron affinities of the 16th and 17th groups. Click here to buy a book, photographic periodic table poster, card deck, or 3D print based on the images you see here! b) oxygen has high electron affinity . a) oxygen is more electronegative . d) O-ion has comparatively larger size than oxygen atom. The electron affinity of oxygen is equal to A. the ionization energy of O-. Calculate the second electron affinity of oxygen using the information below: O^- (g) + e^- ? 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. Hence, oxygen has lesser electron affinity than that of sulphur and however in a group, it decreases from top to bottom as size increases. O-(g) + e- O 2-(g) EA= +780 kJ. 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. O^2+ (g) EA_2 =? Electron affinity follows a trend on the periodic table. This can be understood with the following example of the successive electron affinity of oxygen: O(g) + e- O-(g) EA= -141 kJ. B. the ionization energy of O2-. Negatively charged ion of an atom or molecule 9.3 in the textbook to Calculate the lattice energy O.! Of energy required to detach one electron from a negatively charged ion an. Of an atom or molecule than attraction to overcome it... however the 1st electron affinity of.... Cycle and data from Appendix IIB and Table 9.3 in the textbook to Calculate the ionization... The textbook to Calculate the lattice energy of O. 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