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Tutorial. 1) Using Slater’s rule confirm that the experimentally observed electronic configuration of K (Z = 19), 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 , is energetically more stable than the configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1.
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Tutorial 1) Using Slater’s rule confirm that the experimentally observed electronic configuration of K (Z = 19), 1s2 2s2 2p6 3s2 3p64s1, is energetically more stable than the configuration 1s2 2s2 2p6 3s2 3p63d1. 2) Use Slater’s rules to estimate values of Zeff for (a) a 4s and (b) a 3d electron in a V atom. Using your answer, explain why the valence configuration of the ground state of a V+ ion is likely to be 3d34s1 rather than 3d24s2. 3) Assume three p-block elements A (Z = 6), B (Z = 7) and C (Z = 8) having ground state electronic configuration 1s22s22p2 ,1s22s22p3 and 1s22s22p4 respectively. The increase in Zeff between A and B is 0.69 whereas the increase between B and C is only 0.62. Suggest a reason why the increase in Zeff for a 2p electron is smaller between B and C than between A and B given the configurations of the atoms listed above.
Noble Gas Halogen Transition elements Period Inner transition elements f block elements Alkali Earth Metal Alkali Metal Group
f block elements np6 ns1 np2 np3 np4 np5 np1 ns2 s1 d10 s1 d5 d3 d10 d5 d6 d1 d7 d8 d2
Noble Gases He 1s2 2 Ne 1s22s22p6 10 Ar 1s22s22p63s23p6 18 Kr 1s22s22p63s23p64s23d104p6 36 Xe 1s22s22p63s23p64s23d104p65s24d105p6 54 Rn 1s22s22p63s23p64s23d104p65s24d10 5p66s24f14 5d10 6p6 86
Noble Gas Noble Gases np6
Noble Gases • Neon (Ne) and the elements below it in Group 18 have eight electrons in their outer energy levels. • Their energy levels are stable, so they do not combine easily with other elements.
H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 Alkali Metals 1s1 1s22s1 1s22s22p63s1 1s22s22p63s23p64s1 1s22s22p63s23p64s23d104p65s1 1s22s22p63s23p64s23d104p65s24d10 5p66s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1
Alkali Metal Alkali Metals ns1
Alkali Metals • The alkali metals form compounds that are similar to each other. • Alkali metals each have one outer energy level electron. • It is this electron that is removed when alkali metals react. • The easier it is to remove an electron, the more reactive the atom is. • Unlike halogens, the reactivities of alkali metals increase down the group.
Ionization Energies of Elements np6 ns1 ns2 np4 np5
Ionization Energies of Elements Ionization energy increases across a period and decreases down a group. The variation of first ionization energy (in kilojoules per mole) through the main groups of the periodic table. Why ionization energy of N/P is higher than O/S?
Ionization Energies of Elements The values of the first ionization energies of the elements up to Rn. Ionization energy increases across a period and decreases down a group.
Noble Gas Halogen Halogens np6 np5
Halogens • Fluorine is the most reactive of the halogens because its outer energy level is closest to the nucleus.
ELECTRON AFFINITY Electron affinities are highest for elements near fluorine, particularly the halogens. Electronegativity increases across a period and decreases down a group.
ELECTRON AFFINITY Electron affinities are highest for elements near fluorine, particularly the halogens. Electronegativity increases across a period and decreases down a group.
Books: Books: 1) INORGANIC CHEMISTRY: Duward Shriver and Peter Atkins. 2) Inorganic Chemistry: Principles of Structure and Reactivity by James E. Huheey, Ellen A. Keiter and Richard L. Keiter. 3) Inorganic Chemistry: Catherine Housecroft, Alan G. Sharpe.
