Anomalous Behaviour of Boron
Like Li and Be, Boron – the first member of group 13 also shows anomalous behaviour due to extremely low size and high nuclear charge/size ratio, high electronegativity and non-availability of d electrons. The main point of differences are,
(1) Boron is a typical non- metal whereas other members are metals.
(2) Boron is a bad conductor of electricity whereas other metals are good conductors.
(3) Boron shows allotropy and exists in two forms – crystalline and amorphous. Aluminium is a soft metal and does not exist in different forms.
(4) Like other non-metals, the melting point and boiling point of boron are much higher than those of other elements of group 13.
(5) Boron forms only covalent compounds whereas aluminium and other elements of group 13 form even some ionic compounds.
(6) The hydroxides and oxides of boron are acidic in nature whereas those of others are amphoteric and basic.
(7) The trihalides of boron (BX3) exist as monomers On the other hand, aluminium halides exist as dimers (Al2X6).
(8) The hydrides of boron i.e. boranes are quite stable while those of aluminium are unstable.
(9) Dilute acids have no action on boron others liberate H2 from them.
(10) Borates are more stable than aluminates.
(11) Boron exhibit maximum covalency of four e.g., BH–4 ion while other members exhibit a maximum covalency of six e.g., [Al(OH)6]3-.
(12) Boron does not decompose steam while other members do so.
(13) Boron combines with metals to give borides e.g. Mg3B2. Other members form simply alloys.
(14) Concentrated nitric acid oxidises boron to boric acid but no such action is noticed other group members.
B + 3HNO3 → H3BO3 + 3NO2
Diagonal relationship between Boron and Silicon
Due to its small size and similar charge/mass ratio, boron differs from other group 13 members, but it resembles closely with silicon, the second element of group 14 to exhibit diagonal relationship. Some important similarities between boron and silicon are given below,
(1) Both boron and silicon are typical non-metals, having high m.pt. b.pt nearly same densities (B=2.35g ml–1 S=2.34 g//ml). low atomic volumes and bad conductor of current. However both are used as semiconductors.
(2) Both of them do not form cation and form only covalent compounds.
(3) Both exists in amorphous and crystalline state and exhibit allotropy.
(4) Both possess closer electronegativity values (B=2.0; Si=1.8).
(5) Both form numerous volatile hydrides which spontaneously catch fire on exposure to air and are easily hydrolysed.
(6) The chlorides of both are liquid, fume in most air and readily hydrolysed by water.
BCl3 + 3H2O → B(OH)3 + 3HCl ; SiCl4 + H2O → Si(OH)4 + 4HCl
(7) Both form weak acids like H3BO3 and H2SiO3.
(8) Both form binary compounds with several metals to give borides and silicide. These borides and silicide react with H3PO4 to give mixture of boranes and silanes.
3Mg + 2B → Mg3B2 ; Mg3B2 + H3PO4 → Mixture of boranes
(Magnesium boride)
2Mg + Si → Mg2Si ; Mg2Si + H3PO4 → Mixture of silanes
(Magnesium silicide)
(9) The carbides of both Boron and silicon (B4 C and SiC) are very hard and used as abrasive.
(10) Oxides of both are acidic and can be reduced by limited amount of Mg In excess of Mg boride and silicide are formed.
B2O3 + 3Mg → 3MgO + 2B; SiO2 + 2Mg → 2MgO + Si
(11) Both the metals and their oxides are readily soluble in alkalies.
2B + 6NaOH → 2Na3BO3 + 3H2↑; Si + 2NaOH + H2O → Na2SiO3 + 2H2↑
(borate) (Silicate)
B2O3 + 6NaOH → 2Na3BO3 + 3H2O ; SiO2 + 2NaOH → Na2SiO3 + H2O
Both borates and silicates have tetrahedral structural units BO42–and SiO4n– respectively. Boron silicates are known in which boron replaces silicon in the three dimensional lattice. Boron can however form planar BO3 units.
(12) Acids of both these elements form volatile esters on heating with alcohol in presence of conc. H2SO4.
B(OH)3 + 3ROH → B(OR)3 + 3H2O ; Si(OH)4 + 4ROH → Si(OR)4 + 4H2O
