Respuesta :
Answer:
he configuration with the highest electronic affinity is 2s2 2p5
Explanation:
Electronic affinity is the variation of energy when we add an electron to a neutral atom to form an ion
When an electron is added, it must occupy a space is the sub-level of the atom, giving more stability when it approaches the configuration of a complete shell with eight electrons (noble gas), so the affinity must increase when moving in a period Group VIII noble gases)
Let's examine the given settings
In this case, when adding an electron, 2s2 is very far from a complete level configuration, so its affinity must be small.
2s2 2p2 when adding an electro the one has a little more affinity, but is still a long way from a full shell, it would be missing 3 electrons
2s2 2sp5 this is the atom with the highest electronic affinity, since i = that when adding an electron the ion has the configuration of a noble gas. This is the most stable on the list
2s2 2p6 already has a full shell making it very difficult to insert an electron into this atom.
In summary, the configuration with the highest electronic affinity is 2s2 2p5
Answer:
2s2 2p6.
Explanation:
Electron affinity is a term used to measure of the attraction between the incoming electron and the nucleus - the stronger the attraction, the more energy is released. The factors which affect this attraction are: nuclear charge, distance, electronic configuration and screening.
Comparing the following electronic configuration of their outermost shell:
2s2
2s2 2p2
2s2 2p5
2s2 2p6
Generally, Eae increases across the period(more positive), where the noble gases are the most negative. This is because of their fully filled shells.
Therefore, 2s2 2p6 has fully filled orbitals, therefore it will have the highest negative electron affinity.
