Ncert Solutions Chemistry Class 11th
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4.39. Define hydrogen bonds. Is it weaker or stronger than the van der Waals forces?
4.39. Define hydrogen bonds. Is it weaker or stronger than the van der Waals forces?
4.39. When hydrogen is attached with highly electronegative element in a covalent bonding the electrons of the covalent bond are shifted towards the more electronegative atom. Thus, a partially positively charged hydrogen atom forms a bond with the other more electronegative atom. This bond is
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4.38. Describe the hybridisation in case of PCl5. Why are the axial bonds longer as compared to equatorial bonds?
4.38. Describe the hybridisation in case of PCl5. Why are the axial bonds longer as compared to equatorial bonds?
4.38. P has ground state valence shell electronic configuration 3s23p3 and the first excited state valence shell electronic configuration is 3s13p33d1. P undergoes sp3d hybridization and has trigonal bipyrami geometry. Because axial bond pairs suffer more repulsive interaction from the equatori
Upvote 4.37. Write the significance of plus and minus sign in representing the orbitals.
4.37. Write the significance of plus and minus sign in representing the orbitals.
4.37. Molecular orbitals are represented by wavefunctions. A positive sign in an orbital indicates a positive wavefunction while a negative sign in an orbital shows a negative wavefunction.
Upvote 4.36. Compare the relative stability of the following species and indicate their magnetic properties: O2, O2, O2– (Superoxide), O22- (peroxide)
4.36. Compare the relative stability of the following species and indicate their magnetic properties: O2, O2, O2– (Superoxide), O22- (peroxide)
4.36. O2: Bond order = 2, paramagnetic
O2+: Bond order = 2.5, paramagnetic
O2–: Bond order = 1.5, paramagnetic
O22-: Bond order = 1, diamagnetic
Order of relative stability is
O2+ > O2 > O2– > O22-
(2.5) (2.0) (1.5) (1.0)
Upvote 4.35. Use molecular orbital theory to explain why the Be2 molecule does not exist.
4.35. Use molecular orbital theory to explain why the Be2 molecule does not exist.
Upvote <p><strong>4.37. Write the significance of plus and minus sign in representing the orbitals.</strong></p>
<p><strong>4.35. Use molecular orbital theory to explain why the Be<sub>2</sub> molecule does not exist.</strong></p>
4.34. Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.
4.34. Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.
4.34. The combining atomic orbitals should have comparable energies like, 1s orbital of one atom can combine with 1s atomic orbital of another atom, 2s can combine with 2s.
The combining atomic orbitals must have proper orientations so that they are able to overlap to a considerable extent.
The
Upvote 4.33. Explain the formation of H2 molecule on the basis of valence bond theory.
4.33. Explain the formation of H2 molecule on the basis of valence bond theory.
4.33. Let us consider the combination between atoms of hydrogen HA and HB and eA and eB be their respective electrons.
As they tend to come closer, two different forces operate between the nucleus and the electron of the other and vice versa. The nuclei of the atoms as well as their electrons re
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