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Solutions for Chapter 19: Carbon and Organic Compounds

Modern Chemistry: Student Edition 2006 | 1st Edition | ISBN: 9780030391071 | Authors: R. Thomas Myers, Keith B. Oldham, Salvatore Tocci

Full solutions for Modern Chemistry: Student Edition 2006 | 1st Edition

ISBN: 9780030391071

Modern Chemistry: Student Edition 2006 | 1st Edition | ISBN: 9780030391071 | Authors: R. Thomas Myers, Keith B. Oldham, Salvatore Tocci

Solutions for Chapter 19: Carbon and Organic Compounds

Solutions for Chapter 19
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Textbook: Modern Chemistry: Student Edition 2006
Edition: 1
Author: R. Thomas Myers, Keith B. Oldham, Salvatore Tocci
ISBN: 9780030391071

This textbook survival guide was created for the textbook: Modern Chemistry: Student Edition 2006, edition: 1. Modern Chemistry: Student Edition 2006 was written by and is associated to the ISBN: 9780030391071. This expansive textbook survival guide covers the following chapters and their solutions. Chapter 19: Carbon and Organic Compounds includes 57 full step-by-step solutions. Since 57 problems in chapter 19: Carbon and Organic Compounds have been answered, more than 43833 students have viewed full step-by-step solutions from this chapter.

Key Chemistry Terms and definitions covered in this textbook
  • Absolute confi guration

    Which of the two possible isomers an enantiomer is (i.e., whether it is the right- or left-handed isomer).

  • alkyl group

    A substituent lacking p bonds and comprised of only carbon and hydrogen atoms.

  • allotropes.

    Two or more forms of the same element that differ significantly in chemical and physical properties. (2.6)

  • angle strain

    The increase in energy associated with a bond angle that has deviated from the preferred angle of 109.5°.

  • carbides.

    Ionic compounds containing the C2 22 or C42 ion. (22.3)

  • chair conformation

    The lowest energy conformation for cyclohexane, in which all bond angles are fairly close to 109.5° and all hydrogen atoms are staggered.

  • chiral

    A term describing a molecule or an ion that cannot be superimposed on its mirror image. (Sections 23.4 and 24.5)

  • E2

    A bimolecular b-elimination reaction.

  • effusion

    The escape of a gas through an orifice or hole. (Section 10.8)

  • electrophilic aromatic substitution

    A substitution reaction in which an aromatic proton is replaced by an electrophile and the aromatic moiety is preserved.

  • elemental semiconductor

    A semiconducting material composed of just one element. (Section 12.7)

  • enantiomeric excess

    For a mixture containing two enantiomers, the difference between the percent concentration of the major enantiomer and the percent concentration of its mirror image.

  • Graham’s law

    A law stating that the rate of effusion of a gas is inversely proportional to the square root of its molecular weight. (Section 10.8)

  • Ground state

    The lowest energy state of a system.

  • homogeneous equilibrium

    The equilibrium established between reactant and product substances that are all in the same phase. (Section 15.4)

  • Hund’s rule

    A rule stating that electrons occupy degenerate orbitals in such a way as to maximize the number of electrons with the same spin. In other words, each orbital has one electron placed in it before pairing of electrons in orbitals occurs. (Section 6.8)

  • hydride ion

    An ion formed by the addition of an electron to a hydrogen atom: H-. (Section 7.7)

  • Isomers

    Different compounds with the same molecular formula.

  • nomenclature

    A system for naming organic compounds.

  • salt

    An ionic compound formed by replacing one or more hydrogens of an acid by other cations. (Section 4.3)

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