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P-block elements

P-block elements. General electronic configuration of the groups are : ns 2 np 3 ,ns 2 np 4 , ns 2 np 5 , ns 2 np 6 . . Radii increase down the group, however down the group the increse is small due to filling of electrons in d and f shells.

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P-block elements

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  1. P-block elements

  2. General electronic configuration of the groups are: ns2np3,ns2np4, ns2np5, ns2np6.

  3. Radii increase down the group, however down the group the increse is small due to filling of electrons in d and f shells. The value of ionisation enthalpy decreases down the group due to increase in size. Electron gain enthalpy is the tendency of an element to accept electron. Study of this property in group 17 is more important. These elements Have the strong tendency to accept one electron and complete their octet. However the values of F are more –ve than that for Cl. This is due to the smaller size and strong repulsive force existing in F as compared to Cl.

  4. The property of the element to form bonds with itself, hence exiting as a chain is called catenation. The first element of the groups having smaller size however have the tendency to form multiple bonds with itself and thus exist as discrete molecule. Catenation tendency increases down the group. Eg. N2vs P4

  5. Stability - NH3>PH3>AsH3>SbH3>BiH3. Bond dissociation enthalpy - NH3>PH3>AsH3>SbH3>BiH3 Reducing character - NH3<PH3<AsH3<SbH3<BiH3 Basic character - NH3>PH3>AsH3>SbH3>BiH3. Acidic character - N2O3> P2O3> As2O3> Sb2O3> Bi2O3

  6. Acidic character - H2O < H2S < H2Se < H2Te Thermal stability - H2O > H2S > H2Se >H2Te Reducing character - H2S < H2Se < H2Te Boiling point - H2S < H2Se < H2Te < H2O Reducing property of dioxides – SO2 > SeO2 > TeO2

  7. Stability of halides - F-> Cl-> Br- > I – • Oxidising property – F2> Cl2>Br2> I2 • Acidic strength – HF< HCl< HBr< HI • Stability & bond dissociation enthalpy - HF> HCl> HBr> HI • Stability of oxides of halogens – I > Cl > Br • Ionic character of halides – MF > MCl> MBr> MI

  8. Important structures

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