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434 3s_6_ 17 [154, , , , , , , , , d-block, , V8) 29210) iT 2, , , , , , , , , , , , , , , , , 3d 4p >, 4d 5p 4, 5d 6p >, , , , 6d, , , , , , , , , , , , °, , P block is present at extreme right of, periodic table., , o It has general electronic configuration, ns?np!®., o It includes solids, liquids and gases., , o The elements of this group are metal,, non- metal and metalloids., , o If we move along period in periodic, table, non-metallic character increases, and if we move down the group, the, non-metallic character decreases., , o In this group: As we move down, the, , Docent GG ek ea coer: Lear Sek

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Stable due to’ Inert pair effect.”, , Inert pair effect : |t is “reluctance in the, participation of s electrons in bond, formation due to poor shielding effect by, d and f orbital .As a result, s electrons are, , tightly bounded ., , 15! member is different from its, congeners due to:, , o Small size, , Highest ionization energy., , ©, , O°, , High electro-negativity., , No vacant d orbital., , O°, , They show maximum co-valence of 4, because of no vacant d orbital., , o First member also has tendency to, form multiple bonds because in them p, can takes place (because of its small, , size) ., , oO

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Physical properties of group 13:, Atomic size and Ionic radii:, , o If we compare group 11 with group 13,, then group 13 is smaller due to, increased nuclear charge., , Example: Out of Be and B ,Boron is, smaller ., , o Down the group, size increases, because nuclear charge decreases, (due to addition of new shell)., , o Expected order : B <Al<Ga<in<T|, o But actual the order is :BGa<In<T|, , o The reason behind it: Is due to filling of, d-orbital in Gallium, the effective, nuclear charge on valence electron, increases (because of poor shielding, effect by d and f orbital)., , o Therefore, nucleus pull electron more, effectively and size decreases., , Thug tt Ud m™® a nt

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LIETCALT FAIMALT TPIT (MEL auow MGIIIUET! t1Go, d-electrons and Aluminum doesn't, have) ., , lonization energies, , o If we compare ionization energy of, group 13 and group 2, we can say that, the ionization of group 13 is more,, because of their small size and, increased nuclear charge., , o But actually group 2 has high, ionization energy, than group 13 due to, completely filled s orbital in group 2, elements., , o In case of Be and B, the electronic, configuration of Be is 1s22s* and in, boron it is 1s22s22p'. So, due to this, reason the ionization energy of Boron, is less than Beryllium., , Down the group ionization energy, decreases, as the size increase and, nuclear charge decrease., , So , the expected order is : B>Al>Ga>In>T|