Question

discuss bond angles of molecules with the help of electronegativity​

Answer 1

For molecules with more than 3 atoms, the energetics of bond angle are more complex, and you see a number of interesting empirical results such as "scissoring" (if you look at the external bond angles in small-ring compounds, the tighter the ring bond angle, the larger the external bond angles). Again, this can be modeled by VSEPR or by Walsh diagrams.

How many atoms can easily fit around the central atom. For example, one reason that the bond angle in NH3 is larger than that in OH2 is because the third hydrogen in ammonia "gets in the way" of the other two, and pushes the bond angle open. By contrast, PH3 and SH2 both have bond angles near 90 degrees.


There does appear to be an electronegativity effect in that NH3 has a larger bond angle than NF3, but there's some geometry going on there: N-H bonds are about half as long as N-F bonds. That means that you can have smaller bond angles if the ligand atoms (F) are touching each other, even though F has about 1.75 times the radius of hydrogen.

Answer 2

Answer:

• The electronegativity of an atom exists influenced by both its atomic number and the distance that its valence electrons reside from the charged nuclei.

Explanation:

• Electronegativity exists as a chemical property that represents the tendency of an atom or a functional group to attract electrons toward itself.
• The electronegativity of an atom exists influenced by both its atomic number and the distance that its valence electrons reside from the charged nuclei.

The electronegativity of pendant groups declines, the bond polarity of the bonds declines, and bond angles rise going from left to right and from F to Br. As more electron density stays on the central atom, electron repulsion between the bonded pairs increases, and bond angles increase.

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