| 11. | This can then be used to find the hybridization because there is character around the nuclei of the bonding electrons.
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| 12. | The bond order is equal to the number of bonding electrons minus the number of antibonding electrons, divided by 2.
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| 13. | How was the trigonal bipyramid derived as the shape that allows bonding electrons stay as far from each other as possible?
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| 14. | The ionic cores ( nuclei plus non-bonding electrons ) are assumed to be stable and are treated as a single object.
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| 15. | If the bonding orbital is closer to period 2 than period 3, I guess that would keep the bonding electrons well protected?
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| 16. | All bonds basically consist of positive charged nuclei attracted to a negative charged electron cloud consisting of the " bonding electrons ".
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| 17. | The lewis structure shows you 2 pairs of pi bonding electrons already in the ring and 2 more available pairs on the oxygen.
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| 18. | Like carbon, its four bonding electrons enable it to combine with many other elements or compounds to form a wide range of compounds.
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| 19. | Triplet oxygen is better described by a bond order of one and two halves instead of two to better reflect its unpaired bonding electrons.
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| 20. | Half the difference in the number of antibonding and bonding electrons is the usual way to calculate the bond order of a localised bond.
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