Linked Questions
40 questions linked to/from Why does F replace the axial bond in PCl5?
4
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Why are the axial bonds of PF5 longer than those of the equatorial bonds? (Hybridization) [duplicate]
The axial bonds of $\ce{PF5}$ are longer than those of the equatorial positions.
One explanation is that because the axial bonds are experiencing more repulsion
than those of the equatorial and ...
- 1,411
0
votes
1
answer
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What is the hybridisation in BrF5 [duplicate]
What is the hybridisation of $\ce{BrF5}$ ? I find different sources giving different answers.
When I approach this problem , I don't find any exceptional case like $\ce{SH6}$ (in which hybridisation ...
3
votes
0
answers
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In PCl2F3, why are two Cl atoms not on axial position? [duplicate]
According to these sites:
Chemistry Help
Molbase
in $\ce{PCl2F3}$, both $\ce{Cl}$ and one $\ce{F}$ atom are on equatorial position, and other 2 $\ce{F}$ atoms are on axial position as follows:
The ...
- 707
3
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0
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Why are d orbitals used in the hybridisation of PCl5 and similar compounds? [duplicate]
Phosphorus uses its $\ce{3s}$, three $\ce{3p}$ and one $\ce{3d}$ orbitals for its hybridization in $\ce{PCl5}$ and similar compounds.
However, shouldn't it use its $\ce{4s}$ rather than $\ce{3d}$ ...
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0
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0
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where will be highly electronegetive atom placed? [duplicate]
consider a molecule PCl3F2 here F is more electronegetive than Cl, which of them should occupy axial position??when i searched on internet i found these two images , they increased my confusion ...
- 1,417
99
votes
2
answers
39k
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What is Bent's rule?
I'm all bent out of shape trying to figure out what Bent's rule means. I have several formulations of it, and the most common formulation is also the hardest to understand.
Atomic s character ...
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10
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3
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Why does nitrogen have a maximum covalency of 4?
As nitrogen has 1 lone pair and 3 electrons, either it should have maximum covalency of 5 or 3. But why does it have a maximum covalency of 4 instead?
Why did it leave 1 electron? Why did it have to ...
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15
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3
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How does chlorine form more than 1 bond?
How are perchlorate or chlorate or chlorite ions and their respective acids or compounds formed. $\ce{Cl}$ can't form more than one bond but still...
$\rightarrow$'Perchlorate ion'
$\rightarrow$'...
- 1,693
34
votes
2
answers
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Hypervalency and the octet rule
I realize that the octet rule is more a suggestion than a rule, and that it applies mainly to non-transition metal compounds. Still, compounds that don't have an octet, like $\ce{BH3}$, tend to ...
- 85.4k
22
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2
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What is the favoured geometry of chlorine trifluoride?
Why is the first structure on the left more stable than the second one on the right?
In the first one the angle between the two pair of nonbonding electrons is about 120° which is a lot less than ...
- 1,926
24
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1
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PBP vs TBP geometry?
Why are the axial bond lengths greater than those of the equatorial bonds in a trigonal bi-pyramid (TBP) geometry molecule; but the opposite is true for pentagonal bi-pyramid (PBP) geometry molecules? ...
- 2,585
11
votes
3
answers
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Why the bond angle of PH3 is lesser that that of PF3?
We can explain why the bond angle of $\ce{NF3}$ (102°29') is lesser than $\ce{NH3}$ (107°48') by the VSEPR theory, since lone pair lone pair repulsion is greater than lone pair bond pair repulsion. ...
- 890
7
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2
answers
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How are the hybrid orbitals of sulfur hexafluoride shaped?
On the fluorine end the fluoride atoms are simply completing a $3p$ orbital.
On the sulfur end one could posit a hybrid of one $3s$ orbital, two $3p$ orbitals and a three inner $2p$ orbitals. However,...
8
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4
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Why does stannous chloride occur despite the octet rule?
Shouldn't reaching an octet be any atom's "goal"?
However, I've recently learned about cases that are either expanding octets, or have lesser than "enough" electrons for an octet abiding. e.g.:
S in ...
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11
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2
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Why an asymmetric geometry with sp3d and sp3d3 hybridization?
A molecule in which the central atom is $sp^3d^2$ hybridized ($\ce{SF_6}$), for example, acquires an octahedral shape, which can be explained by assuming that the hybrid orbitals arrange themselves to ...
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6
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1
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Why are axial bonds are longer than equatorial bond in sp3d hybridized atoms?
Why are axial bonds are longer than equatorial bond in case of $\mathrm{sp^3d}$ hybridization? I have done some research but I can't seem to find the answer.
4
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1
answer
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Comparing SN2 reaction rate for phenacyl chloride and methyl chloride
KI in acetone undergoes $\mathrm{S_N2}$ reaction with (1) and (2). Compare the rates of the reactions.
Like many kinds of these questions there are many factors involved. One is the steric effect, ...
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1
vote
2
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11k
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Are there square planar complexes with sp2d hybridization?
We were taught (Under the section 'Valence Bond Theory') seven types of geometries a transition metal complex may assume and its corresponding hybridization states,
Linear - $\ce{sp}$
Trigonal planar ...
- 18.8k
3
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1
answer
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Bond Lengths: Equatorial vs Axial in Trigonal Bipyramidal
Why is it that the axial bond length is less than equatorial bond length in $\ce{PF2Cl3}$ and $\ce{SF2Cl2}$ even though both have trigonal bi-pyramidal geometry?
I know that in general axial bond ...
- 39
9
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2
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755
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Bonding in hypervalent molecules
I don't know where they go the electrons of the extended-valence in molecules like $\ce{SF6}$ or $\ce{PCl5}$ for instance because my teacher said that the d orbitals can't interact with s and p (or ...
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14
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1
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Bonding in Square Antiprismatic Compounds
Both $\ce{IF_8^-}$ and $\ce{XeF_8^{2-}}$ have (distorted) square antiprismatic geometries.
I've been wondering how to explain the bonding in such compounds. Hypercoordinate bonding (as used to ...
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2
votes
1
answer
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Which species occupy the equatorial positions in VSEPR's trigonal bipyramidal and octahedral geometry
Which species (electronegative, double and triple bonded atoms, ions, lone pair etc.) occupy the equitorial position in the trigonal bipyramidal and octahedral geometry when we find the shape using ...
- 309
8
votes
1
answer
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What is θ in Bent's rule equation (%s - character)?
I was learning about Bent's Rule. I came across a formula
$$\cos\theta = \frac{s}{s-1}$$
I am quite confused about $\theta$. I know that it represents bond angle. But for a compound like $\ce{PCl5}$, ...
- 125
2
votes
2
answers
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Structure of AsF3Cl2
Since the molecule has 5 bonding pairs and zero lone pairs, the shape should be trigonal bipyramidal. But one thing i am confused about is which atom(s) will occupy the axial and the planar positions, ...
- 427
4
votes
2
answers
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Is ClH7 possible? [duplicate]
Chlorine can be $sp^3d^3$ hybridized.
If so, it can form $\ce{ClH_7}$ and then chlorine, being more electronegative, will have (-7) as its oxidation number. But we know that the oxidation number of $\...
- 102
3
votes
2
answers
1k
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Structure of phosphorus pentachloride
Why is the shape of $\ce{PCl5}$ trigonal bipyramidal? All the $\ce{Cl}$ atoms must be at equal distances forming a star like shape. However, in the actual shape, the distance between the $\ce{Cl}$ ...
- 545
6
votes
2
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Geometry of AsF5 molecule
Which of the following is the best description of the arrangement of fluorine atoms around the arsenic atom in a molecule of $\ce{AsF5}$?
(a) trigonal bipyramid
(b) octahedron
(c) tetrahedron
(d) ...
- 1,143
8
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1
answer
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Geometries of SCl2(OCH3)2 and SF2(OCH3)2
I am not able to understand the difference between structure of $\ce{SCl_{2}(OCH_{3})_{2}}$ and $\ce{SF_{2}(OCH_{3})_{2}}$.
I am already well versed with Molecular Orbital and VSEPR theories. I found ...
2
votes
1
answer
2k
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Suggest possible structures for the compound PF3(Ph)(NMe2) using the NMR data
use these data to suggest the possible structure for the compound PF3(Ph)(NMe2):
19F Spectrum, two signals:
a doublet of doublets, J=56 and 819Hz, -39.5ppm, relative intensity 2
a doublet of ...
- 1,053
2
votes
1
answer
989
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Would the lone pair be in the equatorial plane or the axial plane for bromine pentafluoride? [duplicate]
I've been learning chemical bonding and I'm confused about the structure of $\ce{BrF5}$.
It has a square bipyramidal geometry but a square pyramidal shape - I got that.
I don't get why the lone pair ...
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