Solutions for Chapter 3.4SE: Chemistry: The Central Science 13th Edition

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown

Full solutions for Chemistry: The Central Science | 13th Edition

ISBN: 9780321910417

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown

Solutions for Chapter 3.4SE

Solutions for Chapter 3.4SE
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This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 13. Since 2 problems in chapter 3.4SE have been answered, more than 146154 students have viewed full step-by-step solutions from this chapter. Chemistry: The Central Science was written by and is associated to the ISBN: 9780321910417. Chapter 3.4SE includes 2 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
  • Absolute confi guration

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

  • addition reaction.

    A reaction in which one molecule adds to another. (24.2)

  • changes of state

    Transformations of matter from one state to a different one, for example, from a gas to a liquid. (Section 1.3)

  • chemical kinetics.

    The area of chemistry concerned with the speeds, or rates, at which chemical reactions occur. (13.1)

  • delocalized molecular orbitals.

    Molecular orbitals that are not confined between two adjacent bonding atoms but actually extend over three or more atoms. (10.8)

  • divalent

    An element that forms two bonds, such as oxygen.

  • first order

    A reaction that has a rate equation in which the sum of all exponents is one.

  • galvanic cell

    See voltaic cell. (Section 20.3)

  • Gibbs free energy (G)

    The ultimate arbiter of the spontaneity of a reaction, where DG = DH - T DS.

  • Hund’s rule

    When orbitals of equal energy are available but there are not enough electrons to fi ll all of them completely, one electron is put in each before a second electron is added to any

  • Hydrogen bonding

    The attractive interaction between a hydrogen atom bonded to an atom of high electronegativity (most commonly O or N) and a lone pair of electrons on another atom of high electronegativity (again, most commonly O or N).

  • ionic bond

    A bond between oppositely charged ions. The ions are formed from atoms by transfer of one or more electrons. (Section 8.1)

  • lactone

    A cyclic ester.

  • metallic hydrides

    Compounds formed when hydrogen reacts with transition metals; these compounds contain the hydride ion, H-. (Section 22.2)

  • Order of precedence of functions

    A ranking of functional groups in order of priority for the purposes of IUPAC nomenclature.

  • particle accelerator

    A device that uses strong magnetic and electrostatic fields to accelerate charged particles. (Section 21.3)

  • polar molecule

    A molecule that possesses a nonzero dipole moment. (Section 8.4)

  • polynucleotide

    A polymer constructed from nucleotides linked together.

  • rate constant

    A constant of proportionality between the reaction rate and the concentrations of reactants that appear in the rate law. (Section 14.3)

  • silica

    Common name for silicon dioxide. (Section 22.4)

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