Both CO2 and N2O are linear but dipole moment of CO2 is zero but for N2O it is non-zero, why?

The answer lies in the structure of these molecules, CO₂ is symmetrical molecule while N₂O is unsymmetrical, thus for N₂O, dipoles do not cancel each other, leaving the molecule with a resultant dipole, while the bond moment of CO₂ cancel each other, so CO₂ has no net dipole moment.

Related Questions:

Question(1): Why aqueous solution of AlCl₃ is acidic in nature ?

Question(2): What happen when aq AlCl₃ react with Acid or Base?

Question(3): Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Question(4): Arrange in increasing order of extent of hydrolysis [ CCI₄, MgCI₂, AICI₃, PCl₅, SiCI₄].

Question(5): Although Sulphur contain vacant d-orbital but SF6 does not undergo hydrolysis. Why ?

Question(6): CCl₄ can not be hydrolysed but SiCl4 can be. Why?

Question(7): What are the hydrolysis products of urea ?

Question(8): Why SF₆ is inert where as SF₄ is highly reactive towards H₂0 ?.

Question(9): Why SF₆ behave inert towards hydrolysis?

Question(10): Why PCl₃ hydrolysed while NCl₃ can not be hydrolysed?

Question(11): Why hydrolysis of NCl3 gives NH4OH and HOCl, while PCl3 on hydrolysis gives H3PO3 and HCl?

Question(12): NCl3 and PCl3 on hydrolysis give different kinds of products. These is because of

NCl3 and PCl3 on hydrolysis give different kinds of products. These is because of

(A) Attack of lone pair of water takes place to N and P respectively.

(B) Attack of lone pair of water takes place to Cl and Cl respectively.

(C) Attack of lone pair of water takes place to Cl and P respectively.

(D) None of these

Solution: (C) Their is no vacant d- orbitals hence attack of lone pair of water takes place to Cl and P respectively.

Related Questions:

Question(1): Why aqueous solution of AlCl₃ is acidic in nature ?

Question(2): What happen when aq AlCl₃ react with Acid or Base?

Question(3): Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Question(4): Arrange in increasing order of extent of hydrolysis [ CCI₄, MgCI₂, AICI₃, PCl₅, SiCI₄].

Question(5): Although Sulphur contain vacant d-orbital but SF6 does not undergo hydrolysis. Why ?

Question(6): CCl₄ can not be hydrolysed but SiCl4 can be. Why?

Question(7): What are the hydrolysis products of urea ?

Question(8): Why SF₆ is inert where as SF₄ is highly reactive towards H₂0 ?.

Question(9): Why SF₆ behave inert towards hydrolysis?

Question(10): Why PCl₃ hydrolysed while NCl₃ can not be hydrolysed?

Question(11): Why hydrolysis of NCl3 gives NH4OH and HOCl, while PCl3 on hydrolysis gives H3PO3 and HCl?

Why hydrolysis of NCl3 gives NH4OH and HOCl, while PCl3 on hydrolysis gives H3PO3 and HCl?

 The hydrolysis of PCl₃ may be contrasted with that of NCl₃ this difference is due to the change in polarity of P-Cl bond in PCl₃ in contrast to N-Cl bond in NCl₃.

PF₃ is not sensetive to H₂O due to strong P-F bond F being more electronegative  than oxygen forms a strong covalent bond with p in coparison with P-O bond.

Related Questions:

Question(1): Why aqueous solution of AlCl₃ is acidic in nature ?

Question(2): What happen when aq AlCl₃ react with Acid or Base?

Question(3): Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Question(4): Arrange in increasing order of extent of hydrolysis [ CCI₄, MgCI₂, AICI₃, PCl₅, SiCI₄].

Question(5): Although Sulphur contain vacant d-orbital but SF6 does not undergo hydrolysis. Why ?

Question(6): CCl₄ can not be hydrolysed but SiCl4 can be. Why?

Question(7): What are the hydrolysis products of urea ?

Question(8): Why SF₆ is inert where as SF₄ is highly reactive towards H₂0 ?.

Question(9): Why SF₆ behave inert towards hydrolysis?

Question(10): Why PCl₃ hydrolysed while NCl₃ can not be hydrolysed?