Explain the following : (i) Gallium has higher ionisation enthalpy than aluminium (ii) Boron does not exist as B3+ ion (iii) Aluminium forms [AlF6] 3– ion but boron does not form [BF6] 3– ion (iv) PbX2 is more stable than PbX4. (v) Pb4+ acts as an oxidising agent but Sn2+ acts as a reducing agent.

This is a Short Answers Type Questions as classified in NCERT Exemplar (i) When moving down the periodic table within a group, ionization enthalpy generally decreases due to increased atomic radius. However, in the case of gallium (Ga) and aluminum (Al), gallium experiences a higher effective nuclear charge due to less shielding from its inner electrons, resulting in a higher ionization enthalpy compared to aluminum. (ii) As boron is smaller in size and the sum of its first three ionization enthalpies i.e. ΔH1+ΔH2+ΔH3 is very large so boron does not allow to lose its all three valence electrons and exist as +3 ion rather it shares electrons to make covalent bonds. (iii) As compared to boron, aluminium is larger in size and has vacant d-orbital through which it can expand its coordination number from +4 to +6. Can easily acquire the sp3d2 hybridisation State. On the other hand, boron is smaller in size with no d-orbitals and can expand its coordination number maximum up to +4 so boron can maximum the form BF4− but not BF62−. (iv) Lead is extra stable in its +2 oxidation state than in +4 oxidation state due to inert pair effect. (v) Due to the inert Pair effect, lead is more stable in its +2 oxidation state than in +4. So if it is present in +4 oxidation state in any compound it can readily reduce itself by gaining two electrons. Thus acting as an oxidising agent. Reaction: Pb4++2e−→Pb2+ While for Sn2+, +4 oxidation state is extra stable than +2 oxidation state so in any compound where acid is present in +2 oxidation state it loses two more electron and oxidises itself to +4 oxidation state. Thus acting as a reducing agent. Reaction: Sn2+→Sn4++2e−

Explain the following :

(i) Gallium has higher ionisation enthalpy than aluminium (ii) Boron does not exist as B³⁺ ion (iii) Aluminium forms [AlF₆] ^3– ion but boron does not form [BF₆] ^3– ion (iv) PbX₂ is more stable than PbX_4._(v)_Pb_{⁴⁺ acts as an oxidising agent but Sn²⁺ acts as a reducing agent.}

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Alok Kumar Singh | Contributor-Level 10

10 months ago

This is a Short Answers Type Questions as classified in NCERT Exemplar

(i) When moving down the periodic table within a group, ionization enthalpy generally decreases due to increased atomic radius. However, in the case of gallium (Ga) and aluminum (Al), gallium experiences a higher effective nuclea

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Chemistry NCERT Exemplar Solutions Class 11th Chapter Eleven 2025

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(i) Boron in [B(OH)₄]⁻	(a) sp²
(ii) Aluminium in [Al(H₂O)₆]³⁺	(b) sp³
(iii) Boron in B₂H₆	(c) sp³d²
(iv) Carbon in Buckminsterfullerene
(v) Silicon in SiO₄⁴⁻
(vi) Germanium in [GeCl₆]²⁻

Column I	Column II
(i) Diborane	(a) Used as a flux for soldering metals
(ii) Gallium	(b) Crystalline form of silica
(iii) Borax	(c) Banana bonds
(iv) Aluminosilicate	(d) Low melting, high boiling, useful for measuring high temperatures
(v) Quartz	(e) Used as catalyst in petrochemical industries.

Column I	Column II
(i) BF₄⁻	(a) Oxidation state of central atom is +4
(ii) AlCl₃	(b) Strong oxidising agent
(iii) SnO	(c) Lewis acid
(iv) PbO₂	(d) Can be further oxidised
	(e) Tetrahedral shape

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