Home work - 4
1. Write Lewis dot symbols for atoms of the following elements : Mg, Na, B, O, N, Br.
2. Draw the Lewis structures for the following molecules and ions : H 2 S, SiCl 4 , BeF 2 ,
CO 3 2− , HCOOH
3. Discuss the shape of the following molecules using the VSEPR model: BeCl 2 , BCl 3 ,
SiCl 4 , AsF 5 , H 2 S, PH 3
4. Although geometries of NH 3 and H 2 O molecules are distorted tetrahedral, bond
angle in water is less than that of ammonia. Discuss.
5. Write the resonance structures for SO 3 , NO 2 and NO 3
6. Although both CO 2 and H 2 O are triatomic molecules, the shape of H 2 O molecule is
bent while that of CO 2 is linear. Explain this on the basis of dipole moment.
7. Use molecular orbital theory to explain why the Be 2 molecule does not exist.
8. Calculate the bond order and Compare the relative stability of the following species
and indicate their magnetic properties;
O 2 , O 2 + , O 2 − (superoxide), O 2 2− (peroxide)
9. Describe the hybridisation in case of PCl5. Why are the axial bonds longer as
compared to equatorial bonds?
10. Which hybrid orbitals are used by carbon atoms in the following molecules? CH3
–CH3 ; (b) CH3 –CH=CH2 ; (c) CH3 -CH2 -OH; (d) CH3 -CHO (e) CH3COOH
Answers
Answer:
Home work - 4
1. Write Lewis dot symbols for atoms of the following elements : Mg, Na, B, O, N, Br.
2. Draw the Lewis structures for the following molecules and ions : H 2 S, SiCl 4 , BeF 2 ,
CO 3 2− , HCOOH
3. Discuss the shape of the following molecules using the VSEPR model: BeCl 2 , BCl 3 ,
SiCl 4 , AsF 5 , H 2 S, PH 3
4. Although geometries of NH 3 and H 2 O molecules are distorted tetrahedral, bond
angle in water is less than that of ammonia. Discuss.
5. Write the resonance structures for SO 3 , NO 2 and NO 3
6. Although both CO 2 and H 2 O are triatomic molecules, the shape of H 2 O molecule is
bent while that of CO 2 is linear. Explain this on the basis of dipole moment.
7. Use molecular orbital theory to explain why the Be 2 molecule does not exist.
8. Calculate the bond order and Compare the relative stability of the following species
and indicate their magnetic properties;
O 2 , O 2 + , O 2 − (superoxide), O 2 2− (peroxide)
9. Describe the hybridisation in case of PCl5. Why are the axial bonds longer as
compared to equatorial bonds?
10. Which hybrid orbitals are used by carbon atoms in the following molecules? CH3
–CH3 ; (b) CH3 –CH=CH2 ; (c) CH3 -CH2 -OH; (d) CH3 -CHO (e) CH3COOH