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Solutions for Chapter 14: Acids and Bases

Chemistry | 7th Edition | ISBN: 9780618528448 | Authors: Steven S. Zumdahl

Full solutions for Chemistry | 7th Edition

ISBN: 9780618528448

Chemistry | 7th Edition | ISBN: 9780618528448 | Authors: Steven S. Zumdahl

Solutions for Chapter 14: Acids and Bases

Solutions for Chapter 14
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Textbook: Chemistry
Edition: 7
Author: Steven S. Zumdahl
ISBN: 9780618528448

Since 165 problems in chapter 14: Acids and Bases have been answered, more than 51376 students have viewed full step-by-step solutions from this chapter. Chemistry was written by and is associated to the ISBN: 9780618528448. This expansive textbook survival guide covers the following chapters and their solutions. Chapter 14: Acids and Bases includes 165 full step-by-step solutions. This textbook survival guide was created for the textbook: Chemistry, edition: 7.

Key Chemistry Terms and definitions covered in this textbook
  • Carbene

    A neutral molecule that contains a carbon atom surrounded by only six valence electrons (R2C:).

  • Carbocation

    A species in which a carbon atom has only six electrons in its valence shell and bears a positive charge

  • d-Monosaccharide

    A monosaccharide that, when written as a Fischer projection, has the !OH on its penultimate carbon to the right.

  • Dalton’s law of partial pressures.

    The total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone. (5.6)

  • Diastereomers

    Stereoisomers that are not mirror images of each other; refers to relationships among two or more objects

  • electron affinity

    The energy change that occurs when an electron is added to a gaseous atom or ion. (Section 7.5)

  • enantiotopic

    Protons that are not interchangeable by rotational symmetry but are interchangeable by reflectional symmetry.

  • fracking

    The practice in which water laden with sand and other materials is pumped at high pressure into rock formations to release natural gas and other petroleum materials. (Section 18.4)

  • Haber process

    The catalyst system and conditions of temperature and pressure developed by Fritz Haber and coworkers for the formation of NH3 from H2 and N2. (Section 15.2)

  • 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)

  • Ionization potential (IP)

    The minimum energy required to remove an electron from an atom or molecule to a distance where there is no electrostatic interaction between the resulting ion and electron.

  • Lewis acid

    Any molecule or ion that can form a new covalent bond by accepting a pair of electrons.

  • metric system

    A system of measurement used in science and in most countries. The meter and the gram are examples of metric units. (Section 1.4)

  • Optically active

    Refers to a compound that rotates the plane of plane-polarized light

  • photodissociation

    The breaking of a molecule into two or more neutral fragments as a result of absorption of light. (Section 18.2)

  • photosynthesis

    The process that occurs in plant leaves by which light energy is used to convert carbon dioxide and water to carbohydrates and oxygen. (Section 23.3)

  • polysaccharides

    Polymers made up of repeating monosaccharide units linked together by glycoside bonds.

  • Sigma (s) molecular orbital

    A molecular orbital in which electron density is concentrated between two nuclei, along the axis joining them, and is cylindrically symmetrical

  • Tesla (T)

    The SI unit for magnetic fi eld strength.

  • Valence Bond Theory

    A model of bonding that places electron pairs between adjacent atoms to create bonds.

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