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19 Nov 2019
He Consider the electron affinities for the p-block elements in Figure 6.18 Note that the magnitude of electron affinity tends to increase from left to right, meaning that more energy is released when an electron is added to the atom. However, the elements in Group SA (15) do not follow this trend. They have electron affinities that are smaller in magnitude than the preceding element. In fact, nitrogen does not have a measurable electron affinity at all. How do you account for this observation? 10 Ne BCNO Al Si P S CAr Ga Ge As Se In Sn Sb Te Xe TI Pb Bi Po At Rn Kr 51 81 b Why do the elements in Group SA (15) that are heavier than nitrogen have a measurable electron affinity, but nitrogen does not? RE 6.18 Electron affinities (in ev) for the p-block elements c Another general trend in electron affinity is that its magnitude decreases (less energy is released when arn electron is added) from top to bottom down a group. However, Periods 2 and 3 do not follow this trend. The electron affinities for the Period 3 atoms in the p-block all have a greater magnitude then their groupmates in Period 2. How do you account for the fact that it is more energetically favorable to add an electron toa Period 3 atom than it is to add an electron to the analogous Period 2 atom?
He Consider the electron affinities for the p-block elements in Figure 6.18 Note that the magnitude of electron affinity tends to increase from left to right, meaning that more energy is released when an electron is added to the atom. However, the elements in Group SA (15) do not follow this trend. They have electron affinities that are smaller in magnitude than the preceding element. In fact, nitrogen does not have a measurable electron affinity at all. How do you account for this observation? 10 Ne BCNO Al Si P S CAr Ga Ge As Se In Sn Sb Te Xe TI Pb Bi Po At Rn Kr 51 81 b Why do the elements in Group SA (15) that are heavier than nitrogen have a measurable electron affinity, but nitrogen does not? RE 6.18 Electron affinities (in ev) for the p-block elements c Another general trend in electron affinity is that its magnitude decreases (less energy is released when arn electron is added) from top to bottom down a group. However, Periods 2 and 3 do not follow this trend. The electron affinities for the Period 3 atoms in the p-block all have a greater magnitude then their groupmates in Period 2. How do you account for the fact that it is more energetically favorable to add an electron toa Period 3 atom than it is to add an electron to the analogous Period 2 atom?
Casey DurganLv2
12 Jul 2019