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Solutions for Chapter 13: Introductory Chemistry 5th Edition

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Full solutions for Introductory Chemistry | 5th Edition

ISBN: 9780321910295

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Solutions for Chapter 13

Solutions for Chapter 13
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Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. Since 132 problems in chapter 13 have been answered, more than 437958 students have viewed full step-by-step solutions from this chapter. This expansive textbook survival guide covers the following chapters and their solutions. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Chapter 13 includes 132 full step-by-step solutions.

Key Chemistry Terms and definitions covered in this textbook
  • Beer’s law

    In UV-Vis spectroscopy, an equation describing the relationship between molar absorptivity (e), absorbance (A), concentration (C), and path length (l): e = A (C Ž l)

  • Brønsted–Lowry acid

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

  • chemical bond

    A strong attractive force that exists between atoms in a molecule. (Section 8.1)

  • conformation

    A three-dimensional shape that can be adopted by a compound as a result of rotation about single bonds.

  • cycloalkanes.

    Alkanes whose carbon atoms are joined in rings. (24.2)

  • diastereomers

    Stereoisomers that are not mirror images of one another.

  • extensive property

    A property that depends on the amount of material considered; for example, mass or volume. (Section 1.3)

  • frequency

    The number of times per second that one complete wavelength passes a given point. (Section 6.1)

  • geometric isomerism

    A form of isomerism in which compounds with the same type and number of atoms and the same chemical bonds have different spatial arrangements of these atoms and bonds. (Sections 23.4 and 24.4)

  • Glycol

    A compound with hydroxyl (!OH) groups on adjacent carbons.

  • Hund’s rule

    A rule stating that electrons occupy degenerate orbitals in such a way as to maximize the number of electrons with the same spin. In other words, each orbital has one electron placed in it before pairing of electrons in orbitals occurs. (Section 6.8)

  • Living polymer

    A polymer chain that continues to grow without chain-termination steps until either all of the monomer is consumed or some external agent is added to terminate the chain. The polymer chains will continue to grow if more monomer is added.

  • malonic ester synthesis

    Asynthetic technique that enables the transformationof a halide into a carboxylic acid with theintroduction of two new carbon atoms.

  • Mass spectrometry

    An analytical technique for measuring the mass-to-charge ratio (m/z) of ions.

  • Mercaptan

    A common name for a thiol; that is, any compound that contains an -SH (sulfhydryl) group

  • N-Terminal amino acid

    The amino acid at the end of a polypeptide chain having the free !NH2 group

  • Peptide bond

    The special name given to the amide bond formed between the a-amino group of one amino acid and the a-carboxyl group of another amino acid

  • sigma 1S2 bond

    A covalent bond in which electron density is concentrated along the internuclear axis. (Section 9.6)

  • sp2-hybridized orbitals

    Atomic orbitals that are achieved by mathematically averaging one s orbital with two p orbitals to form three hybridized atomic orbitals.

  • tetrahedral

    The geometry of an atom with four bonds separated from each other by 109.5°.

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