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Solutions for Chapter 20: Aldehydes and Ketones

Organic Chemistry,  - Standalone Book | 2nd Edition | ISBN: 9781118452288 | Authors: David R. Klein

Full solutions for Organic Chemistry, - Standalone Book | 2nd Edition

ISBN: 9781118452288

Organic Chemistry,  - Standalone Book | 2nd Edition | ISBN: 9781118452288 | Authors: David R. Klein

Solutions for Chapter 20: Aldehydes and Ketones

Solutions for Chapter 20
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Textbook: Organic Chemistry, - Standalone Book
Edition: 2
Author: David R. Klein
ISBN: 9781118452288

Chapter 20: Aldehydes and Ketones includes 95 full step-by-step solutions. Since 95 problems in chapter 20: Aldehydes and Ketones have been answered, more than 72729 students have viewed full step-by-step solutions from this chapter. Organic Chemistry, - Standalone Book was written by and is associated to the ISBN: 9781118452288. This textbook survival guide was created for the textbook: Organic Chemistry, - Standalone Book, edition: 2. This expansive textbook survival guide covers the following chapters and their solutions.

Key Chemistry Terms and definitions covered in this textbook
  • Achiral

    An object that lacks chirality; an object that has no handedness

  • alkynide ion

    The conjugate base of a terminal alkyne.

  • Brønsted–Lowry acid

    A substance (molecule or ion) that acts as a proton donor. (Section 16.2)

  • carbon black

    A microcrystalline form of carbon. (Section 22.9)

  • cholesteric liquid crystalline phase

    A liquid crystal formed from flat, disc-shaped molecules that align through a stacking of the molecular discs. (Section 11.7)

  • copolymer

    A complex polymer resulting from the polymerization of two or more chemically different monomers. (Section 12.8)

  • Dalton’s law of partial pressures

    A law stating that the total pressure of a mixture of gases is the sum of the pressures that each gas would exert if it were present alone. (Section 10.6)

  • doping

    Incorporation of a hetero atom into a solid to change its electrical properties. For example, incorporation of P into Si. (Section 12.7)

  • electron configuration

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

  • electrospray ionization (ESI):

    In mass spectrometry, an ionization technique in which the compound is first dissolved in a solvent and then sprayed via a high-voltage needle into a vacuum chamber. The tiny droplets of solution become charged by the needle, and subsequent evaporation forms gas-phase molecular ions that typically carry one or more charges.

  • energy-level diagram

    A diagram that shows the energies of molecular orbitals relative to the atomic orbitals from which they are derived. Also called a molecular-orbital diagram. (Section 9.7)

  • half-reaction

    An equation for either an oxidation or a reduction that explicitly shows the electrons involved, for example, Zn2 + 1aq2 + 2 e- ¡ Zn1s2. (Section 20.2)

  • hydrogen bonding

    Bonding that results from intermolecular attractions between molecules containing hydrogen bonded to an electronegative element. The most important examples involve OH, NH, and HF. (Section 11.2)

  • Le Châtelier’s principle

    A principle stating that when we disturb a system at chemical equilibrium, the relative concentrations of reactants and

  • Lewis structure

    A representation of covalent bonding in a molecule that is drawn using Lewis symbols. Shared electron pairs are shown as lines, and unshared electron pairs are shown as pairs of dots. Only the valence-shell electrons are shown. (Section 8.3)

  • peptidases

    A variety of enzymes that selectively hydrolyze specific peptide bonds.

  • Phasing

    The sign of the wave function at particular coordinates in space, either plus or minus. Phasing is often represented by colors, such as red or blue

  • thioacetal

    A compound that contains two SR groups, both of which are connected to the same carbon atom.

  • triglyceride

    A triester formed from glycerol and three long-chain carboxylic acids.

  • valence bond theory

    A theory that treats a bond as the sharing of electrons that are associated with individual atoms, rather than being associated with the entire molecule.