Octahedral

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

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MaryBanh_2K
Posts: 87
Joined: Wed Sep 18, 2019 12:21 am

Octahedral

Postby MaryBanh_2K » Fri Nov 15, 2019 12:16 am

What is the difference between octahedral, square pyramidal, and square planar?

005321227
Posts: 90
Joined: Sat Sep 07, 2019 12:15 am

Re: Octahedral

Postby 005321227 » Fri Nov 15, 2019 12:23 am

The shape of the orbitals is octahedral. One orbital contains a lone pair of electrons so the remaining five atoms connected to the central atom gives the molecule a square pyramidal shape

William Chan 1D
Posts: 68
Joined: Sat Sep 14, 2019 12:15 am

Re: Octahedral

Postby William Chan 1D » Fri Nov 15, 2019 12:51 am

All of the mentioned shapes have 6 pairs of electrons around the central atom. What differs is how many lone pairs and bonding pairs each has.

Octahedral structures have 6 bonding pairs and 0 lone pairs.

Square pyramidal structures have 5 bonding pairs and 1 lone pair. This one, as the name suggests, looks like a square pyramid.

Square planar structures have 4 bonding pairs and 2 lone pairs. This one looks like a square, but unlike the tetrahedral structure, the bonding pairs are spread out in one plane, giving it a cross or square shape.

Shail Avasthi 3C
Posts: 86
Joined: Fri Aug 30, 2019 12:17 am

Re: Octahedral

Postby Shail Avasthi 3C » Fri Nov 15, 2019 12:54 am

All three have the 6 regions of electron density arranged as an octahedral. The difference is in the number of lone pairs and the number of bonding regions. If the molecular shape is an octahedral, then it has 6 bonding regions (i.e. 6 atoms bound to the central atom). If the molecular shape is square pyramidal, then it has 5 bonding regions and 1 lone pair. If the molecular shape is square planar, then it has 4 bonding regions and 2 lone pairs.

Jedrick Zablan 3L
Posts: 68
Joined: Sat Aug 17, 2019 12:17 am

Re: Octahedral

Postby Jedrick Zablan 3L » Fri Nov 15, 2019 12:55 am

The presence of lone pairs and number of bonded atoms is the difference in the shapes. Octahedral has no lone pairs with 6 bonded atoms. Square Pyramidal has one lone pair with 5 bonded atoms. Square planar has two lone pairs with 4 bonded atoms. The single lone pair of Square Pyramidal creates a repulsion that results in the pyramid shape. The double lone pair of Square Planar balances out to create the planar shape.

Megan Jung 3A
Posts: 50
Joined: Thu Jul 11, 2019 12:17 am

Re: Octahedral

Postby Megan Jung 3A » Fri Nov 15, 2019 9:32 am

All three have 6 regions of electrons either bonded or lone pairs. Octahedral has 6 bonding regions and 0 lone pairs. Square pyramid has 5 bonds and 1 lone pair. Square planar has 4 bonds and 2 lone pairs.


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