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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?

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