Ncert Solutions Chemistry Class 11th
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12.2. Indicate the σ and π-bonds in the following molecules:
C6H6, C6H12, CH2Cl2, CH=C=CH2, CH3NO2, HCONHCH3
12.2. Indicate the σ and π-bonds in the following molecules:
C6H6, C6H12, CH2Cl2, CH=C=CH2, CH3NO2, HCONHCH3
Single bond contains only one sigma bond and double bond contains one sigma and one pi bond.
- In this structure, nine single bonds and three double bonds are present. So, there are 12σ and 3π bonds present.
- In this structure, eighteen single bonds are present. So, there are only 18σ bonds present.
- In th
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4.26. Is there any change in the hybridisation of B and N atoms as a result of the following reaction?
BF3 + NH3 ——-> F3B.NH3
4.26. Is there any change in the hybridisation of B and N atoms as a result of the following reaction?
BF3 + NH3 ——-> F3B.NH3
4.26. In BF3, B atom is sp2 hybridised. In NH3, N is sp3 hybridised.
After the reaction, hybridisation of B changes from sp2 to sp3, while the hybridisation of N remains the same.
Upvote 4.25. Describe the change in hybridisation (if any) of the Al atom in the following reaction.
AlCl3 + Cl– ——> AlCl4-
4.25. Describe the change in hybridisation (if any) of the Al atom in the following reaction.
AlCl3 + Cl– ——> AlCl4-
4.25. Electronic configuration of 13Al in ground state= 1s2 2s2 2p6 3s2 3p1
Electronic configuration of 13Al in excited state = 1s2 2s2 2p6 3s1 3px13py1
Hence, hybridisation will be sp2 and this makes the geometry to be Trigonal planar (in case of
Upvote 4.24. What is meant by hybridisation of atomic orbitals? Describe the shapes of sp, sp2, sp3 hybrid orbitals.
4.24. What is meant by hybridisation of atomic orbitals? Describe the shapes of sp, sp2, sp3 hybrid orbitals.
4.24. Hybridisation: It is defined as the process of intermixing of atomic orbitals of slightly different energies to give rise to new hybridized orbitals having equivalent energy and identical shapes.
Shapes of Orbitals:
sp hybridisation: When one s-and one p-orbital intermix then it i
Upvote 4.23. Which out of NH3 and NF3 has higher dipole moment and why?
4.23. Which out of NH3 and NF3 has higher dipole moment and why?
4.23. The dipole moment of NH3 (1.47D) is higher than the dipole moment of NF3 (0.24D), even though the molecular geometry is pyramidal for both the molecules. In each molecule, N atom has one lone pair. F is more electronegative than H and N? F bond is more polar than N? H bond. Hence, NF3? is
Upvote 4.22. Explain why BeH2 molecule has a zero dipole moment although the Be—H bonds are polar.
4.22. Explain why BeH2 molecule has a zero dipole moment although the Be—H bonds are polar.
4.22. BeH2is a linear molecular (H—Be—H), the bond angle = 180°. Be—H bonds are polar due to difference in their electronegativity but the bond polarities cancel each other. Thus, molecule has resultant dipole moment of zero
Upvote 4.21. Apart from tetrahedral geometry, another possible geometry for CH4 is square planar with the four H atoms at the comers of the square and the C atom at its centre. Explain why CH4 is not square planar?
4.21. Apart from tetrahedral geometry, another possible geometry for CH4 is square planar with the four H atoms at the comers of the square and the C atom at its centre. Explain why CH4 is not square planar?
4.21. According to VSEPR theory, if CH4 were square planar, the bond angle would be 90°. For tetrahedral structure, the bond angle is 109°28? Therefore, in square planar structure, repulsion between bond pairs would be more and thus the stability will be less.
Moreover, the orbitals of carbon in
Upvote <p><strong>4.20. The skeletal structure of CH<sub>3</sub>COOH as shown below is correct, but some of the bonds are shown incorrectly. Write the correct Lewis structure for acetic acid.</strong></p>
<p><strong><picture><img src="https://images.shiksha.com/mediadata/images/articles/1741770757phpivoQPu.jpeg" alt="" width="234" height="134"></picture></strong></p>
4.19. Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3.
4.19. Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3.
4.19. N2 < SO2 < ClF3 < K2O
The ionic character in a molecule is dependent upon the electronegativity difference between the constituting atoms. The greater the difference, the greater will be the ionic character of the molecule.
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