Questions tagged [hybridization]

Hybridisation is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties.

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Hybridization and bonding in ethenone H2C=C=O?

My book says ethenone is a planar molecule, so I was trying to understand its hybridization,I feel that like allenes ethenone too will not be planar. Supposing oxygen and the carbon near it to be in ...
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763 views

Hybridization in Light of Resonance

According to this video: http://www.youtube.com/watch?v=ns4Py96Bkn8&NR=1 1) Is this true? (You might recall I asked a similar question about $\ce{sp^2}$ hybridization implying $\ce{sp^2}$ ...
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How do I find the hybridisation of the orbitals of carbon in a molecule? [duplicate]

What are hybridisation states of each carbon atom in the following compounds? $\ce{CH2=C=O}$ $\ce{CH3CH=CH2}$ $\ce{(CH3)2CO}$ $\ce{CH2=CHCN}$ $\ce{C6H6}$ How do I find the hybridisation of the ...
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Nitric acid vs. chloric acid strength

Here the central chlorine atom is best described as $\ce{sp^3}$ hybridized. This makes sense; the molecule is pyramidal. Also, due to the molecule's pyramidal geometry, this rules out the possibility ...
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Identifying a Positive or Neutral Ligand Inside Coordination Sphere?

There are some coordination compounds like $\ce{Na2[Fe(CN)5NO]}$, where ligands like $\ce{NO}$ are used which exist as both $\ce{NO+}$ (nitrosonium ion) and $\ce{NO^.}$ (neutral nitrosyl). How to ...
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Hybridization - Mixing one atomic s orbital with 2p orbitals

Explain why three ${sp^2}$ hybrid orbitals result when one s atomic orbital is blended with two p atomic orbitals.
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Electronic strucure of cyclopropene radical cation

Suppose I have a cyclopropene molecule with a + charge on the singly bonded carbon.I think the singly bonded carbon is $\mathrm{sp^2}$ hybridised, isn't it? To obtain this species from cyclopropene, ...
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How to calculate the hybridization of ethane with H=½[V+M-C+A]?

I wanted to calculate the hybridization of this molecule $\ce{CH3-CH3}$. I noticed a shortcut formula given in my class notes for calculating the hybridization. It was $$H=\frac{1}{2}×[V+M-C+A].$$ ...
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What is the hybridisation of the carbons in the allyl radical?

The example I am talking about is $\ce{CH2CHCH2^.}$. To find the steric number and hence the hybridization, we use steric number = No. of lone pairs + number of sigma bonds. In this example, the ...
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Does hybridization take place in other atoms apart from central atom in a molecule?

I have seen my textbooks always give formula and description of hybridization of central atom of a molecule. But I wonder will other atoms present (not Hydrogen) go in hybridization or only the ...
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How is hybridisation of a carbon atom determined by looking at the molecule's structure and observing the lone pair and/or sigma bond present? [duplicate]

How can I judge the hybridization of a carbon atom of any carbon containing compound just by looking at its structure? How can I say this by the help of lone pairs and sigma bonds present?
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Is Br sp³-hybridised in HBr?

$\ce{HBr}$ formation can be explained by simple orbital overlap as well as by $\mathrm{sp^3}$ hybridisation of $\ce{Br}.$ Can't we use dipole moment to find if the lone pairs on $\ce{Br}$ are mutually ...
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Why is a alkyne anion more stable than a benzene anion?

I would think the benzene anion (A) is more stable b/c the compound aromatic. Yes I understand that sp hybridized carbons are more stable than sp2 for negative charges, however I thought that ...
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Organic chemistry, hybridization concept [closed]

Hybridization of phenyl cation and venyl[sic] vinyl cation and acetylene cation ,I am totally confused , I think that the hybridization of both phenyl and the venyl cation is SP , I think that in both ...
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Do atoms exist in hybrid form in nature, or do they form hybrid orbitals during molecule formation? [duplicate]

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 ...
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Bonding in PCl3 [duplicate]

Why is there a need to produce 4 equivalent sp3 hybrids? Wouldn't the 3s2 orbital be just fine on its own since it's spherical? Wouldn't it be easier to just be closer to the nucleus and not get ...
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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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How does the phosphate ion look like? [duplicate]

I am trying to understand how a phosphate ion looks like using the VSEPR theory. The phosphorus element has an atomic number of 15, and therefore it has a electron configuration as follow by the ...
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Why is the nitrile nitrogen sp hybridized?

This site, from which the above image was taken, indicates that the hybridization of the orbitals on the C and N atoms in hydrogen cyanide is sp. I can certainly see how that would be the case for ...
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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 ...
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length of bond, bond angle and p character in bond

My reference data: http://www.rsc.org/suppdata/ra/c4/c4ra06781a/c4ra06781a1.pdf Consider these five chemicals: A: $\ce{CH4}$ (methane) B: $\ce{CH3Cl}$ (chloromethane) C: $\ce{CH2Cl2}$ (...
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Why is an alkyne more acidic than an alkene? Or, why is acetylene more acidic than ethylene?

pKa acetylene ~ 25 pKA ethylene ~ 44 I'm not looking for the "because alkyenes are sp hybridized and more s character means their electrons are held tighter" answer because I'm not the biggest fan ...
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Why does AsH5 not exist?

Why does $\ce{AsH5}$ not exist? Is it because the s-orbital of H doesn't and can't overlap with the d-orbital of As after As makes $\rm sp^{3}d$ hybridization?Theoretically the bond can occur because ...
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Hybridization of oxygen in phenol [duplicate]

What is the hybridization of oxygen in phenol molecule? I assume it is $sp^3$ hybridized because it forms 2 bonds - 1 with benzene, another with hydrogen, as in how oxygen is hybridized in a water ...
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How does an hybridised orbital become unhybridised after bond cleavage?

In $\ce{CH4}$, $1 s$ and $3 p$ orbitals are hybridised into four $sp^3$ orbitals. But on homolytic bond cleavage an unpaired electron remains in an unhybridised $p$ orbital? Similarly in heterolytic ...
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Type of hybridisation

State the hybridisation of asterisked carbon in $\ce{CH3-CH=C^{✪}=CH2}$ I am not sure between $sp^2$ and $sp$ hybridization. Because of double bond I think it should be $sp^2$ but because of 2 $\pi$ ...
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Effects of orbital overlap and electronegativity on polarity of binary halogen acids

I have discerned these factors affecting orbital overlap: Symmetry Type of orbital Nodes along the internuclear axis $n$ quantum number of the atomic orbitals - the number of shells of electrons Size ...
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Why does sp hybridised orbital have more directional character than p orbital?

It states so in my textbook. But since s orbital is non directional, shouldn't sp hybridized orbital be less directional in character than p orbital?
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Hybridization of carbon in CO2

I know that if there exists a carbon atom with single bonds only (with other atoms),then it is $\mathrm{sp^3}$ hybridized. And if at least one of the bond is double bond then its $\mathrm{sp^2}$ ...
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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 ...
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sp² hybridized orbital

I do not understand why and how an atom with $\ce{sp^2}$ hybridization has only one p orbital?? For example in pyridine why is the lone pair of nitrogen not counted as a pi electron.
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Bond energy and s-character [closed]

While studying the basics of chemical bonding, I've often come across the following statements: 1. The bond energy increases with the increase in the s-character in a hybrid orbital, i.e sp3 sp2-sp2, ...
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Determining central atom in NCl3

Less electronegative atom is the central atom. $\ce{N}$ is more electronegative than $\ce{Cl}$ as $\ce{Cl}$ has larger atomic radius. So why in $\ce{NCl3}$, $\ce{N}$ is the central atom?
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Is fluorine sp3 hybridized in BF3

Since BF3 has the shape of tetrahedral, and in the provided solution, Boron is sp2, why is Fluorine sp3 hybridized?
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How to compare energy levels in hybridized sp orbitals?

How to compare energy levels in $\ce{sp, sp^2, sp^3}$ orbitals? Since a higher energy level implies lower stability, an $\ce{sp-sp}$ bond must have the lowest energy level, since it is formed by the ...
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What is the oxidation state of carbon atoms in Ethanoic acid?

The oxidation states of $sp^2$ and $sp^3$ carbon in ethanoic acid are $-3$ if we do not consider the electronegativity difference of these two carbons due to their different hybridisation but this ...
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Hybridization molecule

Why is SO32- sp3 hybridized even though it forms a double bond with the oxygen (in resonance)? I thought double bonds needed a p orbital so I would think it would be sp2d so it can still have an ...
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Hybridisation of terminal nitrogen in diazomethane

I have a few questions about the terminal nitrogen (highlighted in red) in diazomethane, $\ce{CH2N2}$. Is that nitrogen $\mathrm{sp}$ or $\mathrm{sp^2}$ hybridised? What type of orbitals do the lone ...
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Determining the orbitals that overlap to form a sigma bond

In the chapter on molecular orbitals, my chemistry book mentions three types of sigma bonds: those formed by s-s ($\ce{H2}$), s-p ($\ce{HCl}$), p-p ($\ce{Cl2}$) hybrid-s ($\ce{CH4}$) and hybrid-hybrid ...
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Hybridization of nitrogen in a ring [closed]

Is there a well defined way to discern the hybridization of a nitrogen atom in ring, like pyrrole? How can you know whether the nitrogen's lone pair are in the conjugated system or not?
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Relation between various bond angles of Nitrogen compounds

I was thinking what could be order of bond angles of NH3, NF3, N(CH3)3 and N(C2H5)3. Considering NF3 and NH3: Since there is backbonding between 2p-2p orbitals of N and F, there will be a partial ...
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Why does hybridization produce a more stable configuration?

My text, and the other sources I've checked, include information on the effects, and kinds, of hybridized orbitals; however, they do not explain what properties of hybridized bonds conduce greater ...
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Doesn't the fact that the lone pair on the nitrogen in amides occupy a p orbital contradict Hund's rules?

Since the $\ce{sp^2}$ hybridized orbitals are lower in energy than the p orbital shouldn't the $\ce{sp^2}$ orbitals fill first? Why is this not the case - two electrons fill the p orbitals while all ...
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Do all sigma bonds are stronger than pi bonds? [closed]

Many textbooks refer that sigma bonds are stronger than pi bonds . But each individual bond ( between different atoms) have different bond energy. So how we know for sure that every possible sigma ...
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How does hybridisation affect an otherwise chiral centre? [closed]

In basic theory, a carbon atom with four nonidentical substituents attached, makes a chiral centre. Thus any molecule is chiral as long as it has a chiral centre (except meso compounds). I thought ...
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Polarity of xenon fluoride

The structure of xenon fluoride is a capped octahedron. The lone pair is stereochemically active, i.e. it will rotate about. The dipole moments of the axial fluorides will get cancelled, and so will ...
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Can Carbon Form bonds without Hybridization?

Carbon has two electrons in its p orbital which should be able to form bonds, are there any examples in which this occurs instead of carbon hybridizing before bonding?
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Structure of OSF4

Recently I had given a test where I was asked to specify the hybridisation of $\ce{OSF4}$ and its structure. I guessed that the structure would be trigonal bipyramidal, but I was unsure since I hadn't ...
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Why does basicity go down along the group 15 hydrides? [duplicate]

As we go down Group 15, the sizes of atoms increase and these are the central atoms in their corresponding hydrides. Shouldn't the large size of central atom (in case of $\ce{Bi}$) actually help the ...
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What is the hybridisation of hydrogen in methane? [duplicate]

I am trying to understand hybridisation. In methane carbon has $\mathrm{sp^3}$ hybridisation, but what is the hybridisation of hydrogen? Is it $\mathrm{sp^3}$? If yes then why?