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प्रश्न
Describe the general trends in the following properties of the elements in Groups 13 and 14.
Ionisation enthalpy
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उत्तर
In group 13, the standardised trend of decrease of Ionisation enthalpy is not monitored.
As we move from Boron to Aluminium the atomic size increases and ionisation enthalpy decreases but when we move ahead from Aluminium to Gallium, the screening effect of 3d electrons comes into play. The poor shielding effect of the electrons lead to the increase in nuclear charge on the valence electrons and results in increase of ionisation enthalpy.
Moving from gallium to Indium, due to The shielding effect of 4d electrons the ionisation enthalpy decreases.
From Indium to thallium, 4f electrons come into action their poor shielding effect increases the effective nuclear charge on valence electrons hence the ionisation of Thallium energy further increases.
The decreasing order of ionization enthalpy for group-13 elements will be: B > Ti > Ga > Al > In
As we move down in group 14 the ionisation enthalpy decreases in the order: C > Si > Ge > Pb > Sn
On moving down the group the size of the atom increases which results in the large decrease in ionisation energy from carbon to silicon but as we move from silicon to heavier metals small decrease in the ionisation energy is observed. This is mainly due to the less screening effect of d-electrons in germanium and tin, and due to fully filled d and f electrons in lead.
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संबंधित प्रश्न
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| Column I | Column II |
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| (ii) Galluim | (b) Crystalline form of silica |
| (iii) Borax | (c) Banana bonds |
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| (v) Quartz | (e) Used as catalyst in petrochemical industries |
Describe the general trends in the following properties of the elements in Groups 13 and 14.
Atomic size
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Though fluorine is more electronegative than chlorine yet BF3 is a weaker Lewis acid than BCl3
BCl3 exists as monomer whereas AlCl3 is dimerised through halogen bridging. Give reason. Explain the structure of the dimer of AlCl3 also.
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