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In which of the following pairs of molecules/ ions, the central atoms have sp^{2} hybridization?

  • Option 1)

    NO^{-}_{2} and NH_{3}

  • Option 2)

    BF_{3} and NO^{-}_{2}

  • Option 3)

    NH^{-}_{2} and H_{2}O

  • Option 4)

    BF_{3} and NH^{-}_{2}

 

Answers (1)

best_answer

As we learnt in

Dettermination of shape of molecules using VSEPR Theory -

calculate \:X

\\X=(No.\;of\:valence\:electrons\:of\:central\:atom\:)+(No.\:of\:other\:atom\:)+(Negative\:charge\:on\:the\:molecule)-(Positive\:charge\:on\:the\:molecule)

-

 

 H=\frac{1}{2} \left [ V+M-C+A \right ]

V = Valence electrons 

M = No. of surrounding monovalent atoms 

C = Atomic charge 

A = amionic charge

For BF_{3},\ H=\frac{1}{2} \left [3+3-0+0 \right ]=3\:or\:sp^{2}\:hybridization

For , for\ NO_{2}^{-},\ H=\frac{1}{2}\left [ 5+0+1 \right ]=3\:or\:sp^{2}\:hybridization


Option 1)

NO^{-}_{2} and NH_{3}

This solution is incorrect 

Option 2)

BF_{3} and NO^{-}_{2}

This solution is correct 

Option 3)

NH^{-}_{2} and H_{2}O

This solution is incorrect 

Option 4)

BF_{3} and NH^{-}_{2}

This solution is incorrect 

Posted by

prateek

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