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[1] [2] In simple terms, formal charge is the difference between the number of valence electrons of an atom in a neutral free state and the number assigned to that atom in a Lewis structure. When determining the best Lewis structure (or predominant resonance structure ) for a molecule, the structure is chosen such that the formal charge on each ...
In terms of Lewis structures, formal charge is used in the description, comparison, and assessment of likely topological and resonance structures [7] by determining the apparent electronic charge of each atom within, based upon its electron dot structure, assuming exclusive covalency or non-polar bonding.
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If the atom is missing a pair of electrons or has a proton, it will have a positive charge. If the atom has electrons that are not bonded to another atom, there will be a negative charge. In structural formulas, the positive charge is indicated by ⊕ , and the negative charge is indicated by ⊖ . [4]
As an example, summing bond orders in the ammonium cation yields −4 at the nitrogen of formal charge +1, with the two numbers adding to the oxidation state of −3: The sum of oxidation states in the ion equals its charge (as it equals zero for a neutral molecule). Also in anions, the formal (ionic) charges have to be considered when nonzero.
Formal charge is determined by using a particular method (homolytic bond cleavage) of assigning "ownership" of each of the molecule's electrons to a particular atomic center within the molecule. This process doesn't change the total number of electrons (or protons) in the molecule, so, yes, by definition, the formal charges of all the atoms ...
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The only charges inside S are the charge Q on the object C, and the induced charge Q induced on the inside surface of the metal. Since the sum of these two charges is zero, the induced charge on the inside surface of the shell must have an equal but opposite value to the charge on C: Q induced = − Q .