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Solutions for Chapter 4.83: SUMMARY

Elementary Principles of Chemical Processes | 4th Edition | ISBN: 9780470616291 | Authors: Richard M. Felder Ronald W. Rousseau, Lisa G. Bullard

Full solutions for Elementary Principles of Chemical Processes | 4th Edition

ISBN: 9780470616291

Elementary Principles of Chemical Processes | 4th Edition | ISBN: 9780470616291 | Authors: Richard M. Felder Ronald W. Rousseau, Lisa G. Bullard

Solutions for Chapter 4.83: SUMMARY

Solutions for Chapter 4.83
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This expansive textbook survival guide covers the following chapters and their solutions. Chapter 4.83: SUMMARY includes 1 full step-by-step solutions. Elementary Principles of Chemical Processes was written by and is associated to the ISBN: 9780470616291. This textbook survival guide was created for the textbook: Elementary Principles of Chemical Processes, edition: 4. Since 1 problems in chapter 4.83: SUMMARY have been answered, more than 41790 students have viewed full step-by-step solutions from this chapter.

Key Chemistry Terms and definitions covered in this textbook
  • 1,2-addition

    A reaction involving the addition of two groups to a conjugated p system in which one group is installed at the C1 position and the other group is installed at the C2 position.

  • bent

    A type of geometry resulting from an sp3-hybridized atom that has two lone pairs. For example, the oxygen atom in H2O.

  • Born-Haber cycle.

    The cycle that relates lattice energies of ionic compounds to ionization energies, electron affinities, heats of sublimation and formation, and bond enthalpies. (9.3)

  • chemical equilibrium

    A state of dynamic balance in which the rate of formation of the products of a reaction from the reactants equals the rate of formation of the reactants from the products; at equilibrium the concentrations of the reactants and products remain constant. (Section 4.1;Chapter 15: Introduction)

  • Contributing structures

    Representations of a molecule or ion that differ only in the distribution of valence electrons.

  • coordination-sphere isomers

    Structural isomers of coordination compounds in which the ligands within the coordination sphere differ. (Section 23.4)

  • debye (D)

    A unit of measure fordipole moments, where 1 debye = 10-18 esu×cm.

  • decarboxylation

    A reaction involving loss of CO2, characteristic of compounds containing a carbonyl group that is beta to a COOH group.

  • dipole-dipole interactions

    Theresulting net attraction between two dipoles.

  • double helix

    The structure for DNA that involves the winding of two DNA polynucleotide chains together in a helical arrangement. The two strands of the double helix are complementary in that the organic bases on the two strands are paired for optimal hydrogen bond interaction. (Section 24.10)

  • 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)

  • heat of combustion

    The heat given off during a reaction in which an alkane reacts with oxygen to produce CO2 and water.

  • Hydration

    The addition of water.

  • ion–dipole force

    The force that exists between an ion and a neutral polar molecule that possesses a permanent dipole moment. (Section 11.2)

  • Michael acceptor

    The electrophile in a Michael reaction.

  • molecular hydrides

    Compounds formed when hydrogen reacts with nonmetals and metalloids. (Section 22.2)

  • Primary (1°) amine

    An amine in which nitrogen is bonded to one carbon and two hydrogens

  • radical inhibitor

    A compound that prevents a radical chain process from either getting started or continuing.

  • solvolysis

    A substitution reaction in which the solvent functions as the nucleophile.

  • sulfonation

    An electrophilic aromatic substitution reaction in which an SO3H group is installed on an aromatic ring.

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