![]() ![]() For instance, it is smaller for #"O"# than for #"N"#, since the fourth #2p# electron on #"O"# is paired but the #2p# electrons on #"N"# are not.Įlectron affinity is not particularly patterned or necessarily predictable. ![]() Therefore, the first ionization energy ( #"IE"_1#) for, say, #"B"#, is lower than for #"Be"#, because the #2p# orbitals are higher in energy than the #2s#, and so, #"B"# can be more easily ionized than #"Be"#.įor elements with electrons in a subshell of #l >= 1#, once electron pairing starts occurring, the paired electron is easier to remove than an unpaired electron.Įlectron pairing causes electron repulsion between like-charges which means that the ionization energy required to remove the first electron ( #"IE"_1#) is smaller. The new subshell is higher in energy (less core-like). There are, however, some exceptions to this general rule, as you can see in the diagram below:Įlements on a new row have their final electron start on a new quantum level, so naturally its ionization energy drops a bunch.Įlements in the same row that start to fill a new subshell ( a new #bb(l)#) have a drop in ionization energy downwards. So, in general, ionization energy increases from the bottom-left to the upper-right of the periodic table. The smaller the atomic radius, the more closely the electrons are held by the nucleus, and thus the higher the ionization energy. Note that it means you cannot, say, compare #"N"# and #"S"# fairly, since they have conflicting periodic trends.Īs I said, the ionization energies follow somewhat from atomic radius. This new quantum level is farther out, and therefore, the radius increases as we go downwards on the periodic table. Higher #Z_"eff"# means smaller radius.Ī new quantum level corresponds to the valence shell on a new row (below). ![]() In general, the atomic radius (except for many transition metals) has a pattern where it decreases from the bottom-left to the top-right of the periodic table.Įffective nuclear charge increases from left to right.Īs we go across the periodic table from left to right, protons are more massive than electrons, so adding one proton and one electron to obtain a new atom means that #bb(Z_("eff")uarr)#. Of these, atomic radius is the most predictable, and ionization energy and electron affinity trends follow (at least in part) from such trends. ![]()
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