Organic Chemistry (9th Edition) by John E. McMurry

By John E. McMurry

Grasp natural chemistry with assistance from this confirmed best-seller! John McMurry's natural CHEMISTRY is continually praised because the so much truly written booklet to be had for the path. In John McMurry's phrases: "I wrote this publication simply because i admire writing. i am getting nice excitement and delight from taking a sophisticated topic, turning it round until eventually I see it sincerely from a brand new perspective, after which explaining it in basic words." via his lucid writing and talent to teach the wonder and common sense of natural chemistry, McMurry makes studying stress-free. the top praise that may be given to a chemistry publication applies to McMurry: it really works!

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Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it. 18 chapter 1 Structure and Bonding Table 1-2 Comparison of C ] C and C ] H Bonds in Methane, Ethane, Ethylene, and Acetylene Bond strength (kJ/mol) (kcal/mol) Bond length (pm) (sp3) C O H 439 105 109 Ethane, CH3CH3 (sp3) C O C (sp3) (sp3) C O H 377 421 90 101 154 109 Ethylene, H2C P CH2 (sp2) C P C (sp2) (sp2) C O H 728 464 174 111 134 109 Acetylene, HC q CH (sp) C q C (sp) (sp) C O H 965 558 231 133 120 106 Molecule Bond Methane, CH4 120 pm, and its strength is about 965 kJ/mol (231 kcal/mol), making it the shortest and strongest of any carbon–carbon bond.

We’ll return to this topic in Chapters 14, 15, and 30 for a more in-depth discussion. Molecular orbital (MO) theory describes covalent bond formation as arising from a mathematical combination of atomic orbitals (wave functions) on different atoms to form molecular orbitals, so called because they belong to the entire molecule rather than to an individual atom. Just as an atomic orbital, whether unhybridized or hybridized, describes a region of space around an atom where an electron is likely to be found, so a molecular orbital describes a region of space in a molecule where electrons are most likely to be found.

Mechanism-type problems are now grouped together under this topic title. Copyright 2016 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it.

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