shapes of many compounds due hybridisation

shapes of many compounds due hyberdisation

1.shape of BF3 (boron trifluoride)

Ground state
B
(5) 1s^2 2s^2 2px^1 2py^0 2pz^0

excited state

1s^2 2s^1 2px^1 2py^1 2pz^0
{ sp2 hybridisation}
since sp2 hybridisation takes place. so BF3 molecule triangular with bond angle 120°

triangular or trigonal planer

2.shape of CH4 (Methane)

Ground state
C
(5) 1s^2 2s^2 2px^1 2py^1 2pz^0

excited state

1s^2 2s^1 2px^1 2py^1 2pz^1
{ sp3 hybridisation}
since sp3 hybridisation takes place. so CH4 molecule tetrahedral with bond angle 109°.28'

3. shape of PF5 (phosphorus pentafluorine)

Ground state
P
(15) 3s^2 3px^1 3py^1 3pz^1 3d^0

excited state

3s^2 3px^1 3py^1 3pz^1 3d^1
{ sp3d hybridisation}
since sp3d hybridisation takes place. so PF5 molecule is tringonal bipyramidal.

equitorial 120°
axial 90°
axial bond are slightly larger than equatorial bond because axial bond forces greater repulsion than equitorial. so PF5 is quite reactive.

6.shape of SF6 (sulphur hexafluoride)

Ground state
S
(16) 3s^2 3px^2 3py^1 3pz^1 3d^0

excited state

3s^2 3px^1 3py^1 3pz^1 3d^2
{ sp3d2 hybridisation}
since sp3d hybridisation takes place. so SF6 molecule is Octahedral with all bond angle 90°.

so SF6 is no reactive

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Radial probability distribution for p and d orbital, radial wave functions

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Radial probability distribution curves

Radial probhjjhajajbability distribution curves: The probability of finding the electron is given by the quantity sie^2.By radial probability us probability of finding the electron within small Radial space around the nucleus. volume of spherical shell between radius r and r+dr =4πr^2 and probability of finding the electron will be 4πr^2dr sie^2. radial probability distribution curves are obtained by plotting radial probability at various distance from the nucleus . 1.Radial probability distribution curves for S orbital n=1, l= 0. distance from nucleus here A° is called angstrom. the probability of finding of electron in a shell is maximum at distance r=r° (r not) which is 0.529 A° for H atom. diagram shows that probability plot for 2s has(two region of high probability) or (two peaks) separated by node. we conclude that no. of high probability region in S orbital = n no. of node = ( n-1)

Linear combination of atomic orbital, Molecular orbital theory, Difference between bonding & anti bonding moleculer orbital.

Linea combination of atomic orbital molecular orbital are formed by combination of atomic orbital if ꌏ(A) andꌏ(B) are the wave function of atomic orbital of two combining atomic A and B then according to Linea combination of atomic orbital, these two wave function can be added or can be substracted .that means there are two modes of interaction (symmetric and antisymmetric) We know ꌏ(s) = ꌏ(A) +ꌏ(B) ꌏ(a) = ꌏ(A)- ꌏ(B) ꌏ(s) and ꌏ(a) represent wave function of bonding and antibonding moleculer orbital. the formation of moleculer orbital ꌏ(s) and ꌏ(a) from two atomic orbital ꌏ(A) and ꌏ(B) is represented as Molecular orbital theory (MO) theory: main points of mo theory are: 1.whwn atomic orbital combine they formed molecular orbital. 2.Number of molecular orbital formed is equal to number of atomic orbital combine. 3.atomic orbital are uninuclear while molecular orbital a...

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