Concept explainers
(a)
Interpretation:
Whether the given structure is a legitimate Lewis structure is to be determined.
Concept introduction:
For a valid Lewis structure of a molecule, the atoms must not exceed their normal valency. In general, this means atoms from the 2nd row onward of the periodic table must follow the octet rule. The exceptions to this rule are elements from the third row like S, P, etc., which are capable of expanding their octets to a maximum of twelve valence electrons. A hydrogen atom cannot have more than two valence electrons.
(b)
Interpretation:
Whether the given structure is a legitimate Lewis structure is to be determined.
Concept introduction:
For a valid Lewis structure of a molecule, the atoms must not exceed their normal valency. In general, this means atoms from the 2nd row onward of the periodic table must follow the octet rule. The exceptions to this rule are elements from the third row like S, P, etc., which are capable of expanding their octets to a maximum of twelve valence electrons. A hydrogen atom cannot have more than two valence electrons.
(c)
Interpretation:
Whether the given structure is a legitimate Lewis structure is to be determined.
Concept introduction:
For a valid Lewis structure of a molecule, the atoms must not exceed their normal valency. In general, this means atoms from the 2nd row onward of the periodic table must follow the octet rule. The exceptions to this rule are elements from the third row like S, P, etc., which are capable of expanding their octets to a maximum of twelve valence electrons. A hydrogen atom cannot have more than two valence electrons.
(d)
Interpretation:
Whether the given structure is a legitimate Lewis structure is to be determined.
Concept introduction:
For a valid Lewis structure of a molecule, the atoms must not exceed their normal valency. In general, this means atoms from the 2nd row onward of the periodic table must follow the octet rule. The exceptions to this rule are elements from the third row like S, P, etc., which are capable of expanding their octets to a maximum of twelve valence electrons. A hydrogen atom cannot have more than two valence electrons.
(e)
Interpretation:
Whether the given structure is a legitimate Lewis structure is to be determined.
Concept introduction:
For a valid Lewis structure of a molecule the atoms must not exceed their normal valency. In general, this means atoms from the 2nd row onward of the periodic table must follow the octet rule. The exceptions to this rule are elements from the third row like S, P, etc., which are capable of expanding their octets to a maximum of twelve valence electrons. A hydrogen atom cannot have more than two valence electrons.
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Chapter 1 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
- Draw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.) (Assume the central atom does not contain an expanded octet.) (a) bromine dioxide (BrO2) (b) beryllium bromide (BeBr2) (c) phosphorus pentafluoride (PF5)arrow_forwardDraw Lewis structures and any contributing resonance structures for each structure below. Use the proper type of arrow to indicate that they are resonance structures. In which structure is resonance more important? (a) H2SO3 (b) (HSO3)^1- (c) (SO3)^2-arrow_forwardDraw a Lewis Structure for each of the following species and assign formal charge where appropriate. Using electronegative values from the period table that was provided identify polar covalent bonds and label the atoms δ+ and δ−. For each of the molecules indicate whether or not it has a dipole moment. (a)CH5N (b) HCN (c) H2CO (d) CH3NC(e) CH3SOCH3 (f) H6BNarrow_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_forwardA) Consider the indicated molecule. Provide a resonance structure that has a +1 formal charge on both nitrogen atoms. H2N O2Narrow_forwardUsing just a periodic table (not a table of electronegativities), decide which of these is likely to be the most polar bond. Explain your answer! (a) C-F (b) S-F (c) Si-F (d) O-Farrow_forward
- (a) Draw the two resonance structures of the molecule below (ignore structures that violate the octet rule): (b) For the above question, indicate which resonance structure (either the one given, or one that you drew) would be the most significant for this compound. Briefly state the reason for your choice.arrow_forwardThe structure at the right is a skeleton of an anion having the overall formula C6H,NO¯. The hydrogen atoms are not shown. (a) Draw a complete Lewis structure in which the -1 formal charge is on N. Include all H atoms and C. valence electrons. (b) Do the same for a Lewis structure with the -1 formal charge on O. (c) Do the same for a Lewis structure with the -1 formal charge on the C atom that is bonded to three other C atoms.arrow_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
- For the species shown below, identify the structure underneath that is not a valid resonance structure. +) (a) (b) (c) (d) (e) a O e d.arrow_forward(i) Draw a complete Lewis dot structure for each of the following compounds. Clearly (ii) indicate all bonds and lone electrons, as well as the formal charge of each atom in the compound. a) NO3 b) NH4* c) CO2arrow_forwardCompute the formal charge (FC) on each atom in the following structures. (b) The hydronium ion, H3O+arrow_forward
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