Concept explainers
(a)
Interpretation:
All resonance contributors for the given molecule are to be drawn. The curved arrows that indicate which pairs of electrons are shifted in going from one resonance structure to the next are to be included.
Concept introduction:
Resonance exists in molecules or ions for which there are two or more valid Lewis structures. For such molecules or ions, each valid Lewis structure is called a resonance contributor. Resonance contributors differ only in the position of their valence electrons, not their atoms.
(b)
Interpretation:
All resonance contributors for the given ion are to be drawn. The curved arrows that indicate which pairs of electrons are shifted in going from one resonance structure to the next are to be included.
Concept introduction:
Resonance exists in molecules or ions for which there are two or more valid Lewis structures. For such molecules or ions, each valid Lewis structure is called a resonance contributor. Resonance contributors differ only in the position of their valence electrons, not their atoms.
(c)
Interpretation:
All resonance contributors for the given ion are to be drawn. The curved arrows that indicate which pairs of electrons are shifted in going from one resonance structure to the next are to be included.
Concept introduction:
Resonance exists in molecules or ions for which there are two or more valid Lewis structures. For such molecules or ions, each valid Lewis structure is called a resonance contributor. Resonance contributors differ only in the position of their valence electrons, not their atoms.
(d)
Interpretation:
All resonance contributors for the given molecule are to be drawn. The curved arrows that indicate which pairs of electrons are shifted in going from one resonance structure to the next are to be included.
Concept introduction:
Resonance exists in molecules or ions for which there are two or more valid Lewis structures. For such molecules or ions, each valid Lewis structure is called a resonance contributor. Resonance contributors differ only in the position of their valence electrons, not their atoms.
(e)
Interpretation:
All resonance contributors for the given molecule are to be drawn. The curved arrows that indicate which pairs of electrons are shifted in going from one resonance structure to the next are to be included.
Concept introduction:
Resonance exists in molecules or ions for which there are two or more valid Lewis structures. For such molecules or ions, each valid Lewis structure is called a resonance contributor. Resonance contributors differ only in the position of their valence electrons, not their atoms.
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Chapter 1 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
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- Calculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forwardFor each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-Narrow_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_forward
- Using the symbols 8- and &+, indicate the direction of polarity, if any, in each covalent bond. (а) С—СІ (b) S-H (c) C-S (d) Р—Нarrow_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_forwardWhich of the following are not related as resonance structures? OH (A) `NH. NH (B) ОН (C) CH2 (D)arrow_forward
- State whether each of these statements is true or false. (a)A carbon–carbon triple bond is shorter than a carbon–carbonsingle bond. (b) There are exactly six bonding electrons inthe O2 molecule. (c) The C—O bond in carbon monoxide islonger than the C—O bond in carbon dioxide. (d) The O—Obond in ozone is shorter than the O—O bond in O2. (e) Themore electronegative the atom, the more bonds it makes toother atoms.arrow_forwardHelp me pleasearrow_forwardDraw Lewis structures for the following compounds.(a) ammonia, NH3 (b) water, H2O(c) hydronium ion, H3O+ (d) propane, C3H8(e) dimethylamine, CH3NHCH3 (f) diethyl ether, CH3CH2OCH2CH3(g) 1-chloropropane, CH3CH2CH2Cl (h) propane-2-ol, CH3CH(OH)CH3(i) borane, BH3 (j) boron trifluoride, BF3Explain what is unusual about the bonding in the compounds in parts (i) and (j)arrow_forward
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