Respuesta :
Answer : The electron geometry and molecular geometry of the molecule is trigonal planar and bent or angular.
Explanation :
Formula used :
[tex]\text{Number of electron pair}=\frac{1}{2}[V+N-C+A][/tex]
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
Now we have to determine the hybridization of the given molecules.
The given molecule is, [tex]TeO_2[/tex]
[tex]\text{Number of electrons}=\frac{1}{2}\times [6]=3[/tex]
The number of electron pair are 3 that means the hybridization will be [tex]sp^2[/tex] and the electronic geometry of the molecule will be trigonal planar.
But as there are 2 atoms around the central phosphorous atom, the third 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.
Thus, the electron geometry and molecular geometry of the molecule is trigonal planar and bent or angular.
Answer:
The electron geometry and molecular geometry of [tex]\rm TeO_2[/tex] molecule is [tex]\rm sp^3[/tex] hybridization with trigonal planar geometry and bent or angular geometry.
Explanation:
In [tex]\rm TeO_2[/tex], the number of electrons are:
Number of electron pairs = [tex]\rm \frac{1}{2}\;\times\;6[/tex]
Number of electron pairs = 3
The molecule of [tex]\rm TeO_2[/tex] has 3 electron pairs. So it has [tex]\rm sp^3[/tex] hybridization.
The electron geometry of the molecule tends to be trigonal planar. But, the presence of 2 atoms around the central atom and the presence of loan pairs in the structure made the geometry to be bend or angular.
The [tex]\rm TeO_2[/tex] molecule has trigonal planar electron geometry of [tex]\rm sp^3[/tex] hybridization. The molecular geometry tends to be bent or angular.
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