Concept explainers
(a)
Interpretation:
For the given skeleton of an anion having the overall formula
Concept introduction:
Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired
(b)
Interpretation:
For the given skeleton of an anion having the overall formula
Concept introduction:
In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.
(c)
Interpretation:
For the given skeleton of an anion having the overall formula
Concept introduction:
In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.
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Organic Chemistry: Principles and Mechanisms (Second Edition)
- The following is a skeleton of a molecular anion having the overall formula C7H6NO–. The H atoms are not shown. Starting with the structure drawn below, complete the Lewis structure by adding all H atoms, valence electrons, and π bonds. This structure will have a –1 formal charge on the oxygen.arrow_forwardDraw resonance structures for the bicarbonate ion, HCO3-. (a) Does HCO3- have the same number of resonance structures as the CO32- ion? Are any less likely than others? (b) What are the formal charges on the O and C atoms in HCO3- ? What is the average formal charge on the O atoms? Compare this with the O atoms in CO32- . (c) Protonation of HCO3- gives H2CO3. How do formal charges predict where the H+ ion will be attached?arrow_forwardDraw Lewis structures for each of the following ions. One atom in each ion has a formal charge that is not zero.Determine which atom it is, and what the formal charge is. (a) the C2H5 anion; (b) the CH3O cation; (c) the CH6N cation;(d) the CH5O cation; (e) the C3H3 anion (all three H atoms are on the same carbon)arrow_forward
- Methyl isocyanate, CH3NCO, was made infamous in 1984when an accidental leakage of this compound from a storagetank in Bhopal, India, resulted in the deaths of about3800 people and severe and lasting injury to many thousandsmore. (a) Draw a Lewis structure for methyl isocyanate.(b) Draw a ball-and-stick model of the structure,including estimates of all the bond angles in the compound.(c) Predict all the bond distances in the molecule.(d) Do you predict that the molecule will have a dipolemoment? Explain.arrow_forward1.) What is the Lewis structure for the methylthiolate anion, CH3S-. Carbon is the central atom. Show any nonzero formal charges. 2.) Proteins are large molecules that affect almost every function of the human body. Proteins are composed of smaller building blocks called amino acids. The simplest amino acid is glycine. When dissolved in water, two atoms in a glycine molecule have a formal charge. In the lewis structure of glycine C2H5NO2 all bonds are drawn (image is provided), but the unbonded valence electrons (lone pairs) are missing. Copy the structure and draw the missing valence electrons (lone pairs). Locate the 2 atoms that have a nonzero formal charge. Calculate the charge at these sites.arrow_forwardThe hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main componentof rocket propellants. Draw Lewis structures for both ions. (a) What is the formal charge of Cl in the hypochlorite ion?(b) What is the formal charge of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (c) What is theoxidation number of Cl in the hypochlorite ion? (d) Whatis the oxidation number of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (e) In a redox reaction,which ion would you expect to be more easily reduced?arrow_forward
- The structural formulas for ethanol, CH3CH2OH, and propene, CH;CH=CH,2, are нн H Н—С—С—0—н H-C-C=C-H нн H H H Ethanol Propene (a) Complete the Lewis structure for each molecule showing all valence electrons. (b) Using the VSEPR model, predict all bond angles in each molecule.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_forwardGiven two possible resonance forms of NCS and the associated formal charges. Predict whether a or b is more stable. (a) (b) :N=C=S: c=N=s: -1 0 0 -2 +1 0arrow_forward
- Write Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Bicarbonate ion, HCO3 -arrow_forward2. Below are drawn four possible isomers (partial Lewis structures with different atomic connectivity) for an anion with the molecular formula C₂H4NO. 10 A B D "TOTT" raptor H H -0- (a) First, add enough electrons as either lone pairs or r bonds to give an overall negative charge. Show all lone pairs in each completed Lewis structure, and show any atomic formal charges that result. (b) Then, for each isomer, consider if other resonance structures can contribute. Since this is an anion, look for a strong electron donor with an adjacent electron acceptor. For each additional resonance structure you draw (some isomers may have more than one additional RS, some may have none), circle the electron pairs in the original Lewis structure which have moved, and draw a curved arrow depicting the motion required to create the new RS. If you have colored pens, color coding your electrons pairs is nice (but not required).arrow_forwardWrite Lewis structures for these ions. Show all valence electrons and all formal charges. (Q) Acetate ion, CH3COO-arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning