Hybridisation is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties.
Questions tagged [hybridization]
382 questions
11
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Hybridisation of ClO2
Find the hybridization as well identify the pπ-pπ as well as pπ-dπ bonds in $\ce{ClO2}$.
$\ce{ClO2}$ has 2 $\sigma$ bonds, 1 lone pair, 2π bonds and 1 odd electron.
Hybridisation is equal to number of $\sigma$ bonds + lone pairs. Since we consider…
Abhinav
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Why is this atom sp² hybridised?
I'm doing exercises on hybridisation, and I was given this molecule:
I'm wondering about this (electron deficient) oxygen atom. My intuition says it should be ${sp^2}$ like the answer says, but honestly I only see that it's $sp$ hybridised. Is it…
user1160
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The logic for hybridisation formula
Hybridisation for a molecule is given by:
$$\frac{1}{2}(V + H - C + A)$$
Where,
V = Number of valance electrons in central atom
H = Number of surrounding monovalent atoms
C = Cationic charge
A = Anionic charge
If this expression is 2 then its $sp$…
dark32
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Hybridization sp3 and sp2
When we calculate the electrons and orbital numbers in $\ce{CH4}$ $sp^3$ hybridization we have taken 3 electrons from $2p$ of $\ce{C}$ and 1 electron from $2s$ of $\ce{C}$ but in $\ce{C2H4}$ we have $2sp^2$ (2 electrons from $2p$ and 1 from…
ordinary chemistry student
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Shape of sp³ hybrid orbital
I have a doubt regarding the shape of the $\mathrm{sp^3}$ hybridised orbital. I looked up for it on stackexchange and found a post where the guy said that where ever the orbitals interfere with opposite signs of the wavefunction they cancel out and…
user8167818
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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.
RAUSHAN KUMAR
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Why does sp2 hybridization imply adjacent sp2 hybridization?
EDIT: I misquoted my teacher; he said something more along the lines of: in conjugated systems, if an atom is $\ce{sp^2}$ hybridized, then every atom it is bound to is also $\ce{sp^2}$ hybridized. Would this be accurate?
My teacher said that if…
Dissenter
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Unconventional hybridisation states
I just came across a table with interesting hybridisation schemes I have never seen before. The table is shown below. I was wondering if anyone could give me some examples of atoms in particular molecules which possess one of those weird…
Tan Yong Boon
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Why is the F-F bond in fluorine a p-p sigma bond?
Won't the lone pairs hybridize to $\mathrm{sp^3}$ making it an $\mathrm{sp^3}$-$\mathrm{sp^3}$ $\sigma$ bond? If it still is $\mathrm{p^\sigma}$-$\mathrm{p^\sigma}$ bond what is the spatial location of the lone pairs?
Ankurs
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What is the hybridization of diatomic nitrogen, diatomic anything like oyxgen, bromine; hydrogen and chlorine in HCl?
I'm guessing sp hybridization for nitrogen in diatomic nitrogen based on the lone pair on nitrogen and the triple bond but there is no mixing of s and p orbitals so I want to say that there is no hybridization. Are there any chemicals without…
user35622
4
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1 answer
sp2 hybridization Group V elements
I'm confused about $\mathrm{sp^2}$ hybridization in the formation of $\ce{NO3-}$ ion. Valence electrons of N are $\mathrm{(2s)^2}$ and $\mathrm{(2p)^3}$.
Is one of $\mathrm{2s}$ electrons kicked up to one of the $\mathrm{2p}$ orbitals, and then the…
Michael
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sp, sp2 and sp3 hybrid orbitals are actual solutions of Schrodinger's equation or only a heuristic?
According to Wikipedia's article about orbital hybridisation:
[...] today it is considered an effective heuristic for rationalising the
structures of organic compounds. [...] Hybrid orbitals are assumed to be mixtures of atomic orbitals,…
Sparkler
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Hybridization of Oxygen in Orthoboric Acid
What should be the hybridization of the oxygen atom?
A) It should be $\mathrm{sp^2}$ as 1 lone pair must be in the unhybridized orbital for back bonding with boron which has a vacant p-orbital
B)It should be $\mathrm{sp^3}$ (2bp + 2lp)
(In my…
iBoy
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Do atoms exist in hybrid form in nature, or do they form hybrid orbitals during molecule formation?
Do atoms exist in hybrid form in nature, or do they form hybrid orbitals during molecule formation?
Take methane for example. Does carbon atom exist with $\ce{sp^3}$ hybrid orbitals in nature and then hydrogen forms bond with only $\ce{sp^3}$ carbon…
Pratha
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2
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Why is this PH3 considered to be an unhybridized molecule?
Also, don't hybrid orbitals appear in all molecules?
The answer by "ron" says "the molecule can be viewed as being unhybridized":
How does lone pair of a central atom affect the dipole moment?
Sam S.
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