Concept explainers
(a)
Interpretation:
The formal charges on each atom of the given structure are to be computed. Also, the charge on the entire structure is to be stated.
Concept introduction:
A charge that is assigned to an atom, on the assumption that all the electrons in the
The formal charge on an atom is calculated by the formula,
(b)
Interpretation:
The formal charges on each atom of the given structure are to be computed. Also, the charge on the entire structure is to be stated.
Concept introduction:
A charge that is assigned to an atom, on the assumption that all the electrons in the chemical bonds are equally shared, is known as the formal charge. The sum of the formal charges on the independent atoms should equal the total charge present on the ion.
The formal charge on an atom is calculated by the formula,
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Organic Chemistry
- The Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.arrow_forwardA stable triatomic molecule can be formed that containsone atom each of nitrogen, sulfur, and fluorine. Threebonding structures are possible, depending on which is thecentral atom: NSF, SNF, and SFN.(a) Write a Lewis diagram for each of these molecules,indicating the formal charge on each atom.(b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom?(c) Does consideration of the electronegativities of N, S,and F from Figure 3.18 help rationalize this observedstructure? Explain.arrow_forwardThe molecular ion S3N, has the cyclic structure 'N All S-N bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is –0.375 and on each S atom is +0.041. Show that this result is consis- tent with the overall +1 charge on the molecular ion. Z-Sarrow_forward
- Draw Lewis structures for the following compounds and ions, showing appropriateformal charges.(a) [CH3OH2 ]+ (b) NH4Cl (c) (CH3)4NCl(d) NaOCH3 (e) +CH3 (f) -CH3(g) NaBH4 (h) NaBH3CN (i) (CH3)2O¬BF3(j) [HONH3]+ (k) KOC(CH3)3 (l) [H2C“OH]arrow_forwardA stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule— namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain. 100. The gasarrow_forwardDraw a Lewis structure for each of the following molecule: (a) chlorodifluoromethane, CHCIF2 (b) propanoic acid C2H5CO2H (basic structure pictured below) (c) acetonitrile, CH3CN ( the framework is H3C-C-N) (d) allene, H2CCCH2arrow_forward
- There is persuasive evidence for the brief existence of the unstable molecule OPCl. (a) Draw a Lewis diagram for this molecule in which the octet rule is satisfied on all atoms and the formal charges on all atoms are zero. (b) The compound OPCl reacts with oxygen to give O2PCl. Draw a Lewis diagram of O2PCl for which all formal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.arrow_forwardAssign formal charges to all atoms in the following Lewis diagrams. (a) ClO, :ö: (b) SO2 ö-s=0 :ö-Cl-ö: :0: (e) BrO5 :0-Br-ö: (d) NOŽ ö=N-ö: :0:arrow_forward(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0arrow_forward
- (d) Explain the following terms, giving an example of where each occurs. (i) Polar covalent bonding (ii) Van der Waals forces (iii) Dipoles (iv) Electronegtivityarrow_forwardChemistry (a) Write three more resonance structures for each of compounds 1 and 2. (b) In each of compounds 1 and 2, determine which resonance structure contributes the most and explain your answer. (c) Are the 3/4 structures resonance structures or different compounds? Same question for 5/6 structures. Explain your answers.arrow_forward(a) Draw three resonance structures for the molecule SCO which is arranged in the order of S-C-O. Indicate formal charges if necessary. Show step-by-step process clearly. (NHSB) (* b) Which of above structures is the most favored one? Explain your answer, nlluoelom :) Which is the least favored structure? Explain your answer.arrow_forward