Question

which among the following has smallest bond angle....a)H2S b)NH3 c)SO2 d)H2O

Answer 1

Answer:

❤️❤️NH3 is smallest bond angle .❤️❤️

Explanation:

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Answer 2

The molecule that has smallest bond angle is, $H_2S$

Explanation :

Formula used  :

$\text{Number of electron pair}=\frac{1}{2}[V+N-C+A]$

where,

V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

(a) The given molecule is, $H_2S$

$\text{Number of electrons}=\frac{1}{2}\times [6+2]=4$

The number of electron pair are 4 that means the hybridization will be $sp^3$ and the electronic geometry of the molecule will be tetrahedral.

But as there are 2 atoms around the central sulfur atom, the third and fourth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be bent or angular and the bond angle will be, $104.5^o$

(b) The given molecule is, $NH_3$

$\text{Number of electrons}=\frac{1}{2}\times [5+3]=4$

The number of electron pair are 4 that means the hybridization will be $sp^3$ and the electronic geometry of the molecule will be tetrahedral.

But as there are 3 atoms around the central nitrogen atom, the fourth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be trigonal pyramidal and the  bond angle will be, $107.5^o$

(c) The given molecule is, $SO_2$

$\text{Number of electrons}=\frac{1}{2}\times [4]=2$

The number of electron pair are 2 that means the hybridization will be $sp$ and the electronic geometry of the molecule will be linear and the bond angle will be, $180^o$

(d) The given molecule is, $H_2O$

$\text{Number of electrons}=\frac{1}{2}\times [6+2]=4$

The number of electron pair are 4 that means the hybridization will be $sp^3$ and the electronic geometry of the molecule will be tetrahedral.

But as there are 2 atoms around the central sulfur atom, the third and fourth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be bent or angular and the bond angle will be, $104.5^o$

As the bond angle of $H_2S$ and $H_2O$ is same but actually bond angle of $H_2O$ is more than $H_2S$ due to high electronegativity of oxygen the bond pair of electrons between hydrogen and oxygen attracted towards the oxygen. Thus, the repulsion between the bond pair decreases and repulsion become more and make a large bond angle.

The increasing order of bond angle is:

$H_2S<H_2O<NH_3<CO_2$

Hence, the molecule that has smallest bond angle is, $H_2S$

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