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Shape and Geometry Using VSEPR

Repulsions be...

Question

Repulsions between the different types of electron pairs are assumed to be equal, what would have been the shapes of $H_{2} O$ and $N H_{3}$ molecules?

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Solution

If Repulsions between the different types of electrons pairs are assumed to be equal then $H_{2} O$ will be linear and ${N H}_{3}$ will be in $T -$ shape.

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Similar questions

How many molecules have the same type of shape from the following molecules?
$H_{3} O^{+}, N H_{3}, C l O_{3}^{-}, P H_{3}, H_{2} O, ¯ C H_{3}$ ___

Q. According to VSEPR model, what makes the shapes of

{C H}_{4}, {N H}_{3}

H_{2} O

Q. How many lone pair of electrons are present on the central atom of

C H_{4}, H_{2} O, N H_{3}, P C l_{3}

P C l_{5}

Q. Given below is the table showing shapes of some molecules having lone pairs of electrons. Fill up the blanks left in it.

Molecule type	$bp$	$lp$	Shape	Example
$A B_{2} E_{2}$	2	P	Bent	$H_{2} O$
$A B_{3} E_{2}$	3	2	Q	$C l F_{3}$
$A B_{5} E$	5	R	S	$B r F_{5}$
$A B_{4} E_{2}$	4	2	T	U

Q. The molecules having the same hybridization, shape and number of lone pairs of electrons are :

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