Question

Page 4 ofs 5) Give the hybridization each around the nitrogen is actually planar does this imply about the nitrogen atom's h or each non-hydrogen atom in this molecule. Note that the geometry y tigonal planar and not tetrahedral as you may expect. What hybridization? (10 pts) N CH3 CH2 ?-?.

Answer 1

What is Hybridization?

The valence band theory was introduced by Heitler and London which is based on the concept of formation of covalent bonds, but later on, this theory was improved by Linus Pauling who introduced this concept. Hybridization is defined as the concept of mixing two atomic orbitals with the same energy levels to give a degenerated new type of orbitals. This intermixing is based on quantum mechanics.

The atomic orbitals of the same energy level can only take part in hybridization and both full filled and half-filled orbitals can also take part in this process provided they have equal energy. During the process, the atomic orbitals of similar energy are mixed together such as the mixing of two ‘s’ orbitals or two ‘p’ orbital’s or mixing of an ‘s’ orbital with a ‘p’ orbital or ‘s’ orbital with a ‘d’ orbital.

sp Hybridization

• This type involves mixing of one ‘s’ orbital and one ‘p’ orbital of equal energy to give a new hybrid orbital known as an sp hybridized orbital.
• The mixture of s and p orbital and the formed sp orbital is maintained at 1800.
• Example of sp-hybridized is: BeCl2

sp2 Hybridization

• This kind involves mixing of one ‘s’ orbital and two ‘p’ orbital’s of equal energy to give a new hybrid orbital known as sp2.
• A mixture of s and p orbital formed in trigonal symmetry and is maintained at 1200.
• Example of sp2 hybridized is: Ethylene (C2H4)

  sp3 Hybridization

• This type involves mixing of one ‘s’ orbital and three ‘p’ orbital’s of equal energy to give a new hybrid orbital known as sp3.
• A mixture of s and p orbitals formed is in tetrahedral symmetry and is maintained at 109.28
• Example of sp3 hybridization: Ethane (C2H6)   

  sp3d Hybridization

• It involves mixing of one ‘s’ orbital, three ‘p’ orbital’s and one ‘d’ orbital of equal energy to give a new hybrid orbital known as sp3d hybridized.
• The mixture of s, p and d orbital’s forms trigonal bipyramidal symmetry. Example: Phosphorus pentachloride(PCl5)
• shortcut formula for finding hybridisation is -

  0.5(V+M-C+A)

  V= No. Of valence electrons of central atom

  M- No. Of monovalent atom

  C- Total Cation charge

  A- Total Anion charge

  For eg:-

• CH4

• So CH4 has central atom carbon which has four valence electrons and it has 4 monovalent hydrogen atom. As there is no plus or minus charge on compound so

  0.5(4+4)= 4

  2) SO4^2-

  The central atom is sulphur with 6 valence electrons. It has no monovalent atom. The total Anion charge is 2

  So 0.5(6+2)- 4

  Now match the number you get with:-

  Sp- 2

  Sp2-3

  Sp3-4

  Sp3d-5

  Sp3d2- 6 and so on

  The above two species hence have sp3 hybridisation.

  Points to be noted:-

• Monovalent atoms means hydrogen, alkali metals and group 17 elements
• If charge on compound is -2 you have to take 2 and never take the sign. Only the number. Remember the number of positive charge is to be subtracted in formula and vice versa
• Rarely in 2–3 compound the formula won't work but for the rest, bam!!   I hope it is ok.Thank You.