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Solutions for Chapter 4.11: Enantiomeric Excess

Organic Chemistry | 8th Edition | ISBN: 9780134042282 | Authors: Paula Yurkanis Bruice

Full solutions for Organic Chemistry | 8th Edition

ISBN: 9780134042282

Organic Chemistry | 8th Edition | ISBN: 9780134042282 | Authors: Paula Yurkanis Bruice

Solutions for Chapter 4.11: Enantiomeric Excess

This textbook survival guide was created for the textbook: Organic Chemistry, edition: 8. Since 5 problems in chapter 4.11: Enantiomeric Excess have been answered, more than 31069 students have viewed full step-by-step solutions from this chapter. Organic Chemistry was written by and is associated to the ISBN: 9780134042282. Chapter 4.11: Enantiomeric Excess includes 5 full step-by-step solutions. This expansive textbook survival guide covers the following chapters and their solutions.

Key Chemistry Terms and definitions covered in this textbook
  • alkylation

    A reaction that achieves the installation of an alkyl group. For example, an SN2 reaction in which an alkyl group is connected to an attacking nucleophile.

  • Anomers

    Carbohydrates that differ in confi guration only at their anomeric carbons.

  • Antibonding molecular orbital

    A molecular orbital in which electrons have a higher energy than they would in isolated atomic orbitals

  • Avogadro’s number (NA).

    6.022 3 1023; the number of particles in a mole. (3.2)

  • column chromatography

    A technique by which compounds are separated from each other based on a difference in the way they interact with the medium (the adsorbent) through which they are passed.

  • conjugate acid–base pair

    An acid and a base, such as H2O and OH-, that differ only in the presence or absence of a proton. (Section 16.2)

  • cycloalkane

    An alkane whose structure contains a ring.

  • electron configuration

    The arrangement of electrons in the orbitals of an atom or molecule (Section 6.8)

  • enantiotopic

    Protons that are not interchangeable by rotational symmetry but are interchangeable by reflectional symmetry.

  • equilibrium constant

    The numerical value of the equilibrium-constant expression for a system at equilibrium. The equilibrium constant is most usually denoted by Kp for gas-phase systems or Kc for solution-phase systems. (Section 15.2)

  • Henry’s law

    A law stating that the concentration of a gas in a solution, Sg, is proportional to the pressure of gas over the solution: Sg = kPg. (Section 13.3)

  • Homotopic groups

    Atoms or groups on an atom that give an achiral molecule when one of the groups is replaced by another group. The hydrogens of the CH2 group of propane, for example, are homotopic. Replacing either one of them with deuterium gives 2-deuteropropane, which is achiral. Homotopic groups have identical chemical shifts under all conditions

  • hydroxyl group

    An OH group.

  • imidazole

    A compound containing a five-membered ring that is similar to pyrrole but has one extra nitrogen atom at the 3 position.

  • phosphoglycerides

    Compounds that are very similar in structure to triglycerides, with the main difference being that one of the three fatty acid residues is replaced by a phosphoester group.

  • Pro-S-hydrogen

    Replacing this hydrogen by deuterium gives a chiral center with an S confi guration

  • specific heat 1Cs2

    The heat capacity of 1 g of a substance; the heat required to raise the temperature of 1 g of a substance by 1 °C. (Section 5.5)

  • symmetric stretching

    In IR spectroscopy, when two bonds are stretching in phase with each other.

  • Thermochemistry

    The study of the energy of chemical structures.

  • Vibrational infrared region

    A common type of spin-spin coupling involving the H atoms on two C atoms that are bonded to each other.

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