hey guys;-
what do you know about hybridization and shape of any molecule!!?
how can we predict shape of any molecule or compound..
answer must contain quality!!
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Answered by
7
Hybridization:--
when an compound is formed eiether through sharing of electrons or through ions a bond between then is formed and it may be covalent or ionic or mettalic bond ,
but due to certain conditions this inductive flow of electrons occur and the electrons are anti-bonded by transfering to new orbitals like from s to p orbital this shuffling of electrons made the compund hybridised.
Shape of molecule depends upon the axis where the electrons are hybrid like sx axis to px axis is called parrallel and while interchange of these axis results in Antiparallel overlapping so, bonds can't be formed
So determine the shape ww need to specify from where eletrons are transferred like from ground s orbital to any other higher n valed orbital
.
All the theory depends upon the central atom its electronic configuration and energy Statica.
Formula to calculate hybridisation is simple = first count the sigma Bonds between adjacent atoms and substract 1 from it .
like Sp4 hybridesed atom will have 3 sigma bonding/bonds etc so on.
when an compound is formed eiether through sharing of electrons or through ions a bond between then is formed and it may be covalent or ionic or mettalic bond ,
but due to certain conditions this inductive flow of electrons occur and the electrons are anti-bonded by transfering to new orbitals like from s to p orbital this shuffling of electrons made the compund hybridised.
Shape of molecule depends upon the axis where the electrons are hybrid like sx axis to px axis is called parrallel and while interchange of these axis results in Antiparallel overlapping so, bonds can't be formed
So determine the shape ww need to specify from where eletrons are transferred like from ground s orbital to any other higher n valed orbital
.
All the theory depends upon the central atom its electronic configuration and energy Statica.
Formula to calculate hybridisation is simple = first count the sigma Bonds between adjacent atoms and substract 1 from it .
like Sp4 hybridesed atom will have 3 sigma bonding/bonds etc so on.
Answered by
7
Hybridization is a beautiful concept that changed the way we thought of geometry and shape of different chemical compounds.
Hybridization said that rather than projecting the orbitals (s,p or d or even more) individually making bonds with other orbitals of adjacent atoms) will make new orbitals that will have nearly equal energy and same in size , shape and different orientation along different axes in the coordinate plane.
How do we know what hybridization central atom has?
There's a simple method to know the hybridization quickly.
Number to decide hybridization = 1/2*( No.of valence electrons in central atom originally + No.of monovalent atoms + Anionic charge - Cationic charge)
So,
if we get 2= it'll be sp hybridization
if 3 = sp2
if 4 = sp3
if 5 = sp3d
if 6 = sp3d2
if 7 = sp3d3
and so on,
Well the geometry given by each hybridization type will be different
sp will give linear shape and the bond angle will be 180°
sp2 will give trigonal planar shape and the bond angle will be 120°
sp3 will give tetrahedral shape and the bond angle will be 109°28'
sp3d will give trigonal bipyramidal shape and the bond angle for the three bonds lying in the same plane will be 120° which are also known as equatorial bonds and two bonds will be attached vertically one up the central atom and one down the central atom. They're also known as axial bonds.
sp3d2 will have octahedral shape where equatorial bonds will have bond angle of 90°
Mostly sp3d2 and sp3d3 compounds become very unstable due to high repulsion between bonds
sp3d3 will have pentagonal bipyramidal hybridization
Here equatorial bond angles are 72°
Here the compound is always very unstable due to high repulsion and exists in a distorted or capped shape.
However, here by the shape I always meant the geometry of the compound that could be predicted.
But , sometimes due to charges or some other electronegativity reasons the shape of the compound might change into T-shape or bent shape and many more different forms
Let's take some examples
1) CH4
Here by the trick
Hybridization
will be 1/2*(4+4) = 4 => sp3 hybridization
Since , central atom that's carbon has four valence electrons and 4 monovalent atoms that's 4 hydrogen atoms.
So, CH4 will have tetrahedral shape and the bond angle will be 109°28'
2) CO2
Hybridization = 1/2*(4) = 2 => sp
here carbon is central atom so I wrote 4 since carbon has 4 valence electrons and yeah don't count the oxygen atoms this time since they are divalent and not monovalent !
So, the geometry of the compound is linear and the bond angle will be 180°
3) NH4+
Hybridization = 1/2(5+4-1) = 4 => sp3
Central atom is Nitrogen so wrote 5 since it has 5 valence electrons
Wrote 4 since there are 4 monovalent hydrogen atoms.
And -1 since there's one Cationic charge here on nitrogen itself.
So, this is it !!
Hole this helps you !
Hybridization said that rather than projecting the orbitals (s,p or d or even more) individually making bonds with other orbitals of adjacent atoms) will make new orbitals that will have nearly equal energy and same in size , shape and different orientation along different axes in the coordinate plane.
How do we know what hybridization central atom has?
There's a simple method to know the hybridization quickly.
Number to decide hybridization = 1/2*( No.of valence electrons in central atom originally + No.of monovalent atoms + Anionic charge - Cationic charge)
So,
if we get 2= it'll be sp hybridization
if 3 = sp2
if 4 = sp3
if 5 = sp3d
if 6 = sp3d2
if 7 = sp3d3
and so on,
Well the geometry given by each hybridization type will be different
sp will give linear shape and the bond angle will be 180°
sp2 will give trigonal planar shape and the bond angle will be 120°
sp3 will give tetrahedral shape and the bond angle will be 109°28'
sp3d will give trigonal bipyramidal shape and the bond angle for the three bonds lying in the same plane will be 120° which are also known as equatorial bonds and two bonds will be attached vertically one up the central atom and one down the central atom. They're also known as axial bonds.
sp3d2 will have octahedral shape where equatorial bonds will have bond angle of 90°
Mostly sp3d2 and sp3d3 compounds become very unstable due to high repulsion between bonds
sp3d3 will have pentagonal bipyramidal hybridization
Here equatorial bond angles are 72°
Here the compound is always very unstable due to high repulsion and exists in a distorted or capped shape.
However, here by the shape I always meant the geometry of the compound that could be predicted.
But , sometimes due to charges or some other electronegativity reasons the shape of the compound might change into T-shape or bent shape and many more different forms
Let's take some examples
1) CH4
Here by the trick
Hybridization
will be 1/2*(4+4) = 4 => sp3 hybridization
Since , central atom that's carbon has four valence electrons and 4 monovalent atoms that's 4 hydrogen atoms.
So, CH4 will have tetrahedral shape and the bond angle will be 109°28'
2) CO2
Hybridization = 1/2*(4) = 2 => sp
here carbon is central atom so I wrote 4 since carbon has 4 valence electrons and yeah don't count the oxygen atoms this time since they are divalent and not monovalent !
So, the geometry of the compound is linear and the bond angle will be 180°
3) NH4+
Hybridization = 1/2(5+4-1) = 4 => sp3
Central atom is Nitrogen so wrote 5 since it has 5 valence electrons
Wrote 4 since there are 4 monovalent hydrogen atoms.
And -1 since there's one Cationic charge here on nitrogen itself.
So, this is it !!
Hole this helps you !
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