Concept explainers
Interpretation:
The two resonance structures of
Concept introduction:
For many molecules, it is impossible to explain all their properties by a single Lewis structure. In such a case, more than one Lewis structure is drawn to explain the properties. Such structures of a compound are called resonating structures, and this phenomenon is called resonance.
Resonating structure are represented by double headed arrow.
Resonance structure differs only in the position of their electrons, not in the positions of their atoms.
Resonance structures are hypothetical and cannot be isolated.
The rules for drawing the resonance structures are as follows:
Only lone pair of electrons and pi electrons can participate in conjugation in the formation of various resonating structures.
The single bonds present in the molecule do not break or form in the resonance structures.
The placement of atoms present in the molecule remains fixed.
The octet of all atoms is completely filled.
Due to the attraction toward electrons, the ions and molecules get some charge on them, which is called formal charge.
The formal charge is given by:
Formal charge = Total number of valence electrons in a free atom –total number of associated electrons.
The octet rule states that every element in the main group should have eight electrons in its valence shell in order for it to attain the noble gas configuration.
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Chemistry
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- Write all possible resonance structures for the following species. Assign a formal charge to each atom. In each case, which resonance structure is the most important? (a) NO2 (nitrogen is central) (b) ClCNarrow_forwardWrite the correct Lewis structure and assign a formal charge to each atom in fulminate ion, CNO.arrow_forwardFor each of the following, use formal charges to choose the Lewis formula that gives the best description of the electron distribution: a ClO2F b SO2 c ClO3arrow_forward
- In which of the following molecules does the sulfur have an expanded octet? For those that do, write the Lewis structure. (a) SO2 (b) SF4 (c) SO2Cl2 (d) SF6arrow_forwardWrite Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Amide ion, NH2 (b) Bicarbonate ion, HCO3 (c) Carbonate ion, CO32 (d) Nitrate ion, NO3 (e) Formate ion, HCOO (f) Acetate ion, CH3COOarrow_forwardA complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.arrow_forward
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