Quesiton concerning Hybridization?
I know how to get the hybridization of the entire compound, but I am confused as far as to just get the hybridization for one element.For example, I can find the hybridization for CH3OH, but I don't know how to find it for just O..Could someone please explain how to do this..
Answer:
If you can't do the atoms you can't do the molecule.
Linear
Combination of
Atomic
Orbitals
Hydrogen electron density is obviously a sphere, 1s2 when bonded. All the early p-block elements are orbitally identical, only difffering in the electron filling. The first bond between any two atoms must be a sigma bond using hybrid orbitals. All others must be pi-bonds using p-orbitals.
You start with an s-orbital and three p-orbitals for each p-block atom. What goes in must come out because angular momentum is conserved. Hold aside any needed p-orbitals for double or triple bonds then hybridize the remainder with the s-orbital. For each atom all hybrid orbitals must be as far way from each other as possible. All p-orbitals must be orthogonal to all hybrid orbitals and to each other. Then, pour in the electrons.
Have you got any multiple bonds in methanol? No. One s-orbital + 3 p-orbitals --> four sp3 orbitals. Maximum avoidance is atom at the centroid and orbitals pointing toward the corners of a tetrahedron. Angle is arccos(-1/3).
Carbon has four valence electrons, one in each hybrid orbital. No charges. Carbon is tetrahedral.
Oxygen has six valence electrons, one in each hybrid orbital then two lone pairs when the other two electrons fill in. Oxygen is (distorted) tetrahedral but with only two bonds. Electron pairs are big so the remaining bonding angle... work it out
If there were an olefin or a carbonyl you'd need a p-orbital/atom for the pi-bond. One s-orbital + 2 p-orbitals --> three sp2 orbitals. Maximum avoidance is atom at the centroid and orbitals pointing toward the corners of a equilateral triangle. Angle is 360/3 = 120 degrees. The p-orbital is orthogonal to the plane of the triangle.
Now show why the central atom in allene, H2C=C=CH2, is sp-hybridized and allene's skeleton is linear.
OK, its been a while since my academic days, but I am not sure how to get the hybridization of "an entire compound".
To me hybridization occurs only with atomic orbitals.
The simplest way to determine hybridization is to determine how many lone pairs, and how many and what kind of bonded pairs are present around an atom.
If the atom contains a total of four lone pairs + single bonded pairs then the atom is sp3 hybridized. (eg in CH4, the C is sp3, in H2O, the O is sp3 since the O has two lone pairs + 2 single bonds to an H atom)
If the atom has a double bond then it is sp2 hybridized. (e.g. Formaldehyde H2C=O the carbon is sp2 hybridized, so is the oxygen)
If the atom has a triple bond it is sp hybridized (e.g. in cyanide, HCN the C is sp hybridized as is the N)
Hope this helps.
Hybridization is never done for the entire molecule, it is always done atom by atom. Hybridization is sp3, sp2, sp, sp3d, or sp3d2.
Since the O in CH3OH has two bonds (one to the H and one to the C, as well as 2 lone pairs of electrons, there are 4 total electron domains. 4 electrons domains mean that you need 4 letters to represent hybridization (this is obviously VERY simplistic
Here are your letters and the order in which you use them:
s p p p d d
I need for letters so I need s, p, p ,p
This means sp3 hybridized. Sp3 hybridized means that the shape around the O in the molecule is tetrahedral (VSEPR shape) or bent (molecular shape).
Because hybridization has to do with what atomic orbitals come together to explain how atoms bond to one another, it is impossible to do this for the molecule as a whole.
The C in this structure is bonded to 3H's and an O, that also means 4 electron domains (lone pair = 1 domain, single bond = 1 domain, double bond = 1 domain, triple bond = 1 domain) 4 domains means you need 4 letters, so again,
s, p, p,p
so the C is sp3 hybridized which means tetrahedral VSEPR shape and since all the domains are actual bonds, tetrahedral molecular shape as well
In the above example, H2C=CH2
Look at the C on the left, it is bonded to 2 H's and a double bond to another C. Since there are 3 electron domains, you need 3 letters, s,p,p which means sp2
Look at the carbon on the right. The C is bonded to 2 H's and double bonded to a C, therefore there are 3 electron domains, which means you need 3 letters, s,p,p which means sp2 again
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Answer:
If you can't do the atoms you can't do the molecule.
Linear
Combination of
Atomic
Orbitals
Hydrogen electron density is obviously a sphere, 1s2 when bonded. All the early p-block elements are orbitally identical, only difffering in the electron filling. The first bond between any two atoms must be a sigma bond using hybrid orbitals. All others must be pi-bonds using p-orbitals.
You start with an s-orbital and three p-orbitals for each p-block atom. What goes in must come out because angular momentum is conserved. Hold aside any needed p-orbitals for double or triple bonds then hybridize the remainder with the s-orbital. For each atom all hybrid orbitals must be as far way from each other as possible. All p-orbitals must be orthogonal to all hybrid orbitals and to each other. Then, pour in the electrons.
Have you got any multiple bonds in methanol? No. One s-orbital + 3 p-orbitals --> four sp3 orbitals. Maximum avoidance is atom at the centroid and orbitals pointing toward the corners of a tetrahedron. Angle is arccos(-1/3).
Carbon has four valence electrons, one in each hybrid orbital. No charges. Carbon is tetrahedral.
Oxygen has six valence electrons, one in each hybrid orbital then two lone pairs when the other two electrons fill in. Oxygen is (distorted) tetrahedral but with only two bonds. Electron pairs are big so the remaining bonding angle... work it out
If there were an olefin or a carbonyl you'd need a p-orbital/atom for the pi-bond. One s-orbital + 2 p-orbitals --> three sp2 orbitals. Maximum avoidance is atom at the centroid and orbitals pointing toward the corners of a equilateral triangle. Angle is 360/3 = 120 degrees. The p-orbital is orthogonal to the plane of the triangle.
Now show why the central atom in allene, H2C=C=CH2, is sp-hybridized and allene's skeleton is linear.
OK, its been a while since my academic days, but I am not sure how to get the hybridization of "an entire compound".
To me hybridization occurs only with atomic orbitals.
The simplest way to determine hybridization is to determine how many lone pairs, and how many and what kind of bonded pairs are present around an atom.
If the atom contains a total of four lone pairs + single bonded pairs then the atom is sp3 hybridized. (eg in CH4, the C is sp3, in H2O, the O is sp3 since the O has two lone pairs + 2 single bonds to an H atom)
If the atom has a double bond then it is sp2 hybridized. (e.g. Formaldehyde H2C=O the carbon is sp2 hybridized, so is the oxygen)
If the atom has a triple bond it is sp hybridized (e.g. in cyanide, HCN the C is sp hybridized as is the N)
Hope this helps.
Hybridization is never done for the entire molecule, it is always done atom by atom. Hybridization is sp3, sp2, sp, sp3d, or sp3d2.
Since the O in CH3OH has two bonds (one to the H and one to the C, as well as 2 lone pairs of electrons, there are 4 total electron domains. 4 electrons domains mean that you need 4 letters to represent hybridization (this is obviously VERY simplistic
Here are your letters and the order in which you use them:
s p p p d d
I need for letters so I need s, p, p ,p
This means sp3 hybridized. Sp3 hybridized means that the shape around the O in the molecule is tetrahedral (VSEPR shape) or bent (molecular shape).
Because hybridization has to do with what atomic orbitals come together to explain how atoms bond to one another, it is impossible to do this for the molecule as a whole.
The C in this structure is bonded to 3H's and an O, that also means 4 electron domains (lone pair = 1 domain, single bond = 1 domain, double bond = 1 domain, triple bond = 1 domain) 4 domains means you need 4 letters, so again,
s, p, p,p
so the C is sp3 hybridized which means tetrahedral VSEPR shape and since all the domains are actual bonds, tetrahedral molecular shape as well
In the above example, H2C=CH2
Look at the C on the left, it is bonded to 2 H's and a double bond to another C. Since there are 3 electron domains, you need 3 letters, s,p,p which means sp2
Look at the carbon on the right. The C is bonded to 2 H's and double bonded to a C, therefore there are 3 electron domains, which means you need 3 letters, s,p,p which means sp2 again
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