Concept explainers
Interpretation:
The two reasonable Lewis structures corresponding to the formula
Concept introduction:
The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.
The rules to draw Lewis structure are given as,
• Determine the electronegativity and the number of valence electrons contributed by each atom.
• Generally, the lowest electronegativity atom is the central atom.
• Write the skeleton structure of the molecule.
• Two valence electrons are used to form a bond in skeleton structure between the central and outer atoms.
• Satisfy the octets of each atom by distributing the valence electrons as nonbonding electrons. It is better to start with the outermost atoms.
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Organic Chemistry
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- Write 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_forwardWrite all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardA complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.arrow_forward
- Carbon, nitrogen, and oxygen form two different polyatomic ions: cyanate ion (NCO) and fulminate ion (CNO). Write Lewis structures for each anion, including near-equivalent resonance structures (do not add any arrows between structures) and indicating formal charges. The isocyanate ion also has two near-equivalent structures, but the formal charge on the nitrogen attom cannot be reduced to zero: Cyanate ion (NCO)arrow_forwardThe carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]arrow_forwardWrite the Lewis structure for each ion. Include resonance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge. HSO4-arrow_forward
- What are the formal charges present in in the ion CH3NH3*? Assume all atoms other an hydrogen hau an octet and that there are two central atoms. O N is 0 and C is +1 O N is +1 and C is -1 O N is +1 and C is 0 O N is 0 and C is 0 O N is +2 and C is -1arrow_forwardWrite Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Bicarbonate ion, HCO3 -arrow_forwardPlease note that "geometry" refers to the molecular or ionic geometry. A. The Lewis diagram for NF3 :F—N—F BF: On .. is: The electron-pair geometry around the N atom in NF3 is There are atom, so the geometry of NF3 is lone pair(s) around the centralarrow_forward
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