Concept explainers
Interpretation:
The Lewis structure for each negative ion is to be written and the formal negative charge is to be assigned to the correct atom.
Concept introduction:
The Lewis structure of a molecule is a representation of the molecule in which valence electrons of an atom are involved and are structurally represented.
The number of valence electrons of the atom is equal to the number of the group to which it belongs. Bonding atoms attain stable electronic configuration and a stable electronic configuration, generally, has eight electrons in the valence shell.
To attain stable configuration, atoms share their electrons with each other.
The formal charge is calculated as follows:
Here, F is the formal charge, Z is the group number of the element or valence electrons, S is the number of shared electrons, and U is the number of unshared electrons.
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ORGANIC CHEM. VOL.1+2-W/WILEYPLUS
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- Compute the formal charge (FC) on each atom in the following structures.(a) Methane (CH4)arrow_forwardWrite Lewis formulas, including unshared pairs, for each of the following. Carbon has four bonds in each compound. (a) Propane (C3H8) (c) Methyl fluoride (CH3F) (b) Methanol (CH4O) (d) Ethyl fluoride (C2H5F)arrow_forwardThe two compounds nitrogen dioxide and dinitrogen tetraoxide are introduced in Section 3.13. (a) NO2 is an odd-electron compound. Draw the best Lewis diagrams possible for it, recognizing that one atom cannot achieve an octet configuration. Use formal charges to decide whether that should be the (central) nitrogen atom or one of the oxygen atoms. (b) Draw resonance forms for N2O4 that obey the octet rule. The two N atoms are bonded in this molecule.arrow_forward
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