G.G.N PUBLIC SCHOOL
Assignment- Chemical Bonding
CLASS- XI
1 Use molecular orbital theory to explain why Be2 molecule does not
exist.
2 Explain the formation of and bonds in C2H4 with the help of
Diagram. Mention the hybrid state of two carbon atoms.
3 What is the hybridization of central atom in following-- NH3 ,
C 2 H2
4 What is the dipole moment of CCl4 molecule? Account for
your answer.
5. Describe the hybridization in case of PCl5. Why are axial
bonds longer as compared to the equatorial bonds?
6 Which of the two as higher dipole moment and why? NF3 or
NH3
7 Which of the two is steam volatile and why? o-nitrophenol or
p-nitrophenol .
8 What shapes are associated with sp3d and sp3d2 hybrid
orbitals? Explain with one eg of each.
9 .In the reaction: N2 N2+, O2 ---O2+, Why is there an increase in
bond order in going from O2 ---O2+, while there is a
decreaseon going from N2 N2+ ?
10 All C-O bond lengths in CO3 2-are equal. Account for this
observation.
11 Explain why BeH2 molecule has zero dipole moment
although the Be- H bonds are polar?
12 Draw the resonating structures of carbon dioxide molecule.
13 Why is NF3 trigonal pyramidal while BF3 is trigonal planar,
though both are tetra atomic molecules?
14 Predict the shape of ClF3 and BF3 on the basis of VSEPR theory
15 Draw lewis structure of a) Phospine b) Hydrogen peroxide
c) Nitrogen trifluoride
16 a) Compare dipole moment of Water, Ammonia and Nitrogen
trifluoride b) Why water has bent shape.