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Identify what atomic hybrid orbitals overlap to from the bonds present F4ClO?
Wiki User
∙ 13y ago
Never heard about it but it is easy to find out the kind of hibridization if the ion exists.
valence electrons 42
central atom Cl (Extended octet)
four single bonds to F
one single coordinate bond or double bond to O
One non bonding pair
Total : need six equivalent orbitals to draw an octhaedric electronic geometry so hibridizate 1s 3p and 2d into 6 sp3d2 equivalent orbitals
Molecular geometry should be square pyramid
Wiki User
∙ 13y ago
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How is a molecular orbital formed?
In molecular orbital theory, MO theory, molecular orbitals are "built" from atomic orbitals. A common approach is to take a linear combination of atomic orbitals (LCAO), specifically symmetry adapted linear combinations (SALC) using group theory. The formation of a bond is essentially down to the overlap of the orbitals, the orbitals being of similar energy and the atomic orbital wave functions having the correct symmetry.
Is it true that with hybridization several atomic orbitals overlap to form the same total number of equivalent hybrid orbitals?
True.
Why sigma bond is formed?
By the overlap of atomic orbitals. In valence bond theory these atomic orbitals may be s, p or d orbitals or "hybrids" such as sp3. This is a complex area and the above is a very simple explanation.
The quantum mechanical model of bonding assumes that atomic orbitals overlap and produce?
molecular orbital
What two orbitals overlap in a single bond?
overlapping that occurs along the orbital axis of 2 atomic orbitals is known as linear overlapping and these orbitals are called sigma atomic orbitals therefore these bonds are known as sigma bonds
What two atomic orbitals or hybrid atomic orbitals overlap to form the c equals c bond in ethene?
sp2 hybrid orbitals overlap.
How is a molecular orbital formed?
In molecular orbital theory, MO theory, molecular orbitals are "built" from atomic orbitals. A common approach is to take a linear combination of atomic orbitals (LCAO), specifically symmetry adapted linear combinations (SALC) using group theory. The formation of a bond is essentially down to the overlap of the orbitals, the orbitals being of similar energy and the atomic orbital wave functions having the correct symmetry.
Is it true that with hybridization several atomic orbitals overlap to form the same total number of equivalent hybrid orbitals?
True.
A bond forms when two atomic or hybrid orbitals overlap to form a single bond A bond forms when two p orbitals overlap in a double or triple bond?
sigma, pi
Why sigma bond is formed?
By the overlap of atomic orbitals. In valence bond theory these atomic orbitals may be s, p or d orbitals or "hybrids" such as sp3. This is a complex area and the above is a very simple explanation.
The quantum mechanical model of bonding assumes that atomic orbitals overlap and produce?
molecular orbital
What two orbitals overlap in a single bond?
overlapping that occurs along the orbital axis of 2 atomic orbitals is known as linear overlapping and these orbitals are called sigma atomic orbitals therefore these bonds are known as sigma bonds
In C2H4 what are the atomic orbitals that participate in forming the sigma bond between the C and H atoms?
sp3 sp3 orbitals overlap Could you please explain why? :) Thank you!!
How would you expect the extent of overlap of atomic orbitals to vary in the series FICl IBr I2 and?
I2 then FICl IBr
Which has greatest bond strength br-s s-h or s-cl?
Compare their atomic sizes; the bond strength is determined by the amount of "overlap" between their orbitals. What shapes give you the most overlap?
Why do metals participate in covalent bonds?
Covalent bonding does not necessarily require that the two atoms be of the there is good overlap between the atomic orbitals of participating atoms.
What bond restricts rotation about the axis of double or triple bonds?
Double and triple bonds each have another type of bond different from the initial single bond present between the two bonded atoms. The sigma bond, the initial single bond, is formed through a head-on overlap of two atomic orbitals. Rotation about this bond does not change the overlap, and so rotation is allowed.But double and triple bonds have pi bonds, formed by side-on overlap between the atomic orbitals (typically either p or d orbitals). These bonds surround the sigma bond and were rotation to occur, the orbitals involved with the pi bonds would cease to overlap and these bonds would be broken.Therefore, the specific bond that restricts rotation about the axis of a double or triple bond would be the pi bond(s) involved.
