1) how might the radius affect the electron affinity? 2) how might the Z* affect
ID: 551407 • Letter: 1
Question
1) how might the radius affect the electron affinity? 2) how might the Z* affect the electron affinity? 3) explain the reason for the general trend in electron affinity across a period? 4) explain the reason for the general trend in electron affinity down a group? Figure 4: Table and Graph of Electron Affinities (k.J/mol) (http://colossus.chem.umass.edu/chandler/ch111/Electronaffinity.gif) Kilojoules per mole Electron Affinities He -73 Atomic Number 10 F Ne -27 1-122| >0 |-141 |-328| >0 S CI Ar -60 :0 , | AI |-134| -72 |-200| -349 E150 200 ·250 “300 350 Ga Ge As Se Br Kr -30 |-119 -78 | -195 | -325 -48-4 In Sn Sb TeI 30-107-103 Rb Sr -190-295 0 1A 2A 3A 4A 5A 6A 7A 8AExplanation / Answer
1) electron affinity is defined as the amount of energy released when an electron is accepted by atom. as the atomic radii decreases electron affinity increases. An atom is said to have high EA if it is ready to accept the electron and form anions and is said to have lo EA if it is not willing to accept electron.
2) As the atomic number (Z) is increasing down the group the EA decreases but when Z increases along the period EA increases.
3) Electron affinities across the period increases because the electrons which are added to the shells of atoms are more closer to the nucleus hence stronger attraction and thus the electron gives lots of energy.
4) Electron affinity down the group is decreasing because the electrons added to the shells are placed at a higher energy level far away from the nucleus which has less nuclear charge affect and sheilding affect increases. if the distance between electrons and nucleus is greater the attraction is less and releases low energy and viceversa.
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