Respuesta :
Answer:
[tex]BH_3[/tex]
Explanation:
Hybridization in [tex]H_2O[/tex] is sp3. Two bond pair and two lone pairs are present. Bond angle of molecule having sp3 hybridization is 109°5”. Because of lone pair, bond angle reduced to 104.5.
In [tex]NH_3[/tex], hybridization is sp3 and have three bond pairs and one lone pair. Because of lone pair, bond angle in NH3 is 107°.
In [tex]BH_3[/tex], hybridization is sp^2 with three bond pairs.
Bond angle of molecule having sp2 hybridization is 120°. As no lone pair is present. Therefore, bond angle will be 120°.
In [tex]CH_4[/tex] and [tex]SiH_4[/tex], hybridization is sp^3 with 4 bond pairs. As no lone pair is present. Therefore, bond angle in both the molecules will be 109°5”.
Therefore, among given, BH_3 will have highest bond angle.
The specie that has the largest bond angle in the context of the question is BH3.
The bond angle is defined as the angle formed between two atoms that are bonded to the same central atom.
Bond angles can be predicted on the basis of the valence shell electron pair repulsion theory (VSEPR).
According to the theory, tetrahedral species have a bond angle of 109°. The species; H2O, NH3, CH4, SiH4 have four electrons on the outermost shell of the central atom and their molecular geometry is based on a tetrahedron.
However, owing to the presence of lone pairs of electrons on the central atoms of the some molecules; H2O and NH3 deviates from the expected tetrahedron. NH3 is trigonal pyramidal while H2O is bent. Both have bond angles less than the predicted 109°.
BH3 is trigonal planar and has a bond angle of 120°.
Hence, based on the prediction of VSEPR theory, BH3 has the largest bond angle.
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