Bond Angles

(Polar molecules, Non-polar molecules, etc.)

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Jarrett Peyrefitte 2K
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Bond Angles

Postby Jarrett Peyrefitte 2K » Sun Nov 17, 2019 8:33 pm

How and why do lone pairs affect the bond angles in a molecule, cation, or anion?

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Re: Bond Angles

Postby madawy » Sun Nov 17, 2019 8:36 pm

Lone pair repulsion: Bond angle is affected by the presence of lone pair of electrons at the central atom. A lone pair of electrons at the central atom always tries to repel the shared pair (bonded pair) of electrons. Due to this, the bonds are displaced slightly inside resulting in a decrease of bond angle.

John Arambulo 1I
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Re: Bond Angles

Postby John Arambulo 1I » Sun Nov 17, 2019 8:54 pm

Also, atomic size affects bond angles because a larger atom would have more electrons, thus having more electrons, making the bond angles smaller.

Jacob Villar 2C
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Re: Bond Angles

Postby Jacob Villar 2C » Sun Nov 17, 2019 9:50 pm

The lone pairs located on a central atom will repel the electrons located within covalent bonds, thus decreasing the bond angles.

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Re: Bond Angles

Postby 505306205 » Sun Nov 17, 2019 9:53 pm

Lone pair - lone pair repulsion is stronger than lone-pair bond pair which is stronger than bond pair-bond pair, regardless of whether it involves a cation, anion, or molecule.

Natalie C 1K
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Re: Bond Angles

Postby Natalie C 1K » Sun Nov 17, 2019 10:26 pm

lone pairs repulse electrons of other atoms and decrease bond angles

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Re: Bond Angles

Postby 504939134 » Sun Nov 17, 2019 10:37 pm

Due to lone pair repulsion, the more lone pairs there are the more repulsion there will be.

Grecia Velasco 4D
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Re: Bond Angles

Postby Grecia Velasco 4D » Sun Nov 17, 2019 11:07 pm

Lone pairs increase bond angles because they repulse electrons more than bonded pairs.

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