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Solutions for Chapter 4.60: 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 4.60: SUMMARY

Solutions for Chapter 4.60
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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. This expansive textbook survival guide covers the following chapters and their solutions. Since 1 problems in chapter 4.60: SUMMARY have been answered, more than 41697 students have viewed full step-by-step solutions from this chapter. Chapter 4.60: SUMMARY includes 1 full step-by-step solutions.

Key Chemistry Terms and definitions covered in this textbook
  • Alkene metathesis

    A reaction in which two alkenes interchange the carbons attached to their double bonds.

  • coordination number

    The number of adjacent atoms to which an atom is directly bonded. In a complex the coordination number of the metal ion is the number of donor atoms to which it is bonded. (Sections 12.37 and 24.2)

  • critical mass.

    The minimum mass of fissionable material required to generate a self-sustaining nuclear chain reaction. (19.5)

  • deoxyribonucleic acids (DNA).

    A type of nucleic acid. (25.4)

  • Dextrorotatory

    Refers to a substance that rotates the plane of polarized light to the right

  • diastereotopic

    Nonequivalent protons for which the replacement test produces diastereomers.

  • displacement reaction

    A reaction in which an element reacts with a compound, displacing an element from it. (Section 4.4)

  • Electrophile

    From the Greek meaning electron loving. Any species that can accept a pair of electrons to form a new covalent bond; alternatively, a Lewis acid.

  • ether

    A compound in which two hydrocarbon groups are bonded to one oxygen. (Section 24.4)

  • Ka

    A measure of the strength of an acid: Ka = Keq 3H2O4 = 3H3O+ 4 3A- 4 3HA4

  • Molecular orbital (MO) theory

    A theory of chemical bonding in which electrons in molecules occupy molecular orbitals that extend over the entire molecule and are formed by the combination of the atomic orbitals that make up the molecule

  • Oxonium ion

    An ion in which oxygen bears a positive charge.

  • polyprotic acid

    A substance capable of dissociating more than one proton in water; H2SO4 is an example. (Section 16.6)

  • precipitation reaction

    A reaction that occurs between substances in solution in which one of the products is insoluble. (Section 4.2)

  • protium

    The most common isotope of hydrogen. (Section 22.2)

  • solubility

    The amount of a substance that dissolves in a given quantity of solvent at a given temperature to form a saturated solution. (Sections 4.2 and 13.2)

  • spectroscopy

    The study of the interaction between matter and electromagnetic radiation.

  • systematic name

    A name that is assigned using the rules of IUPAC nomenclature.

  • Twist-boat conformation

    A nonplanar conformation of a cyclohexane ring that is twisted from and slightly more stable than a boat conformation.

  • Valence electrons

    Electrons in the valence (outermost) shell of an atom.

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