Chemical Bonding and Molecular Structure
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4 months agoContributor-Level 10
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)
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4 months agoContributor-Level 10
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4 months agoContributor-Level 10
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 extent of overlapping should be large.
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4 months agoContributor-Level 10
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 repel each other. Energy is needed to overcome the force of repulsion. Although the number of new attractive and repulsive forces is the same, but the magnitude of the attractive forces is more. Thus, when two hydrogen atoms approach each other, the overall potential energy of the system decreases. Thus, a stable molecule of hydrogen is formed
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4 months agoContributor-Level 10
4.32.
Sigma bond | Pi bond |
It is formed by axial overlap of the atomic orbitals. | It is formed by the sidewise overlap of the atomic orbitals. |
The bond is quite strong. | It is a comparatively weaker bond. |
Only one lobe of the p-orbitals is involved in the overlap. | Both lobes of the p-orbitals are involved in the overlap. |
Electron cloud of the molecular orbital is symmetrical around the inter-nuclear axis. | The electron cloud is not symmetrical |
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4 months agoContributor-Level 10
4.31. The electron pair involved in sharing between two atoms during covalent bonding is called shared pair or bond pair. At the same time, the electron pair which is not involved in sharing is called lone pair of electrons.
For example: CH4 has 4 bond pairs but H2O has 2 bond pairs and 2 lone pairs.
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