Solutions for Chapter 6.1: Introduction toChemical Bonding

Modern Chemistry: Student Edition 2012 | 1st Edition | ISBN: 9780547586632 | Authors: Jerry L. Sarquis, Mickey Sarquis

Full solutions for Modern Chemistry: Student Edition 2012 | 1st Edition

ISBN: 9780547586632

Modern Chemistry: Student Edition 2012 | 1st Edition | ISBN: 9780547586632 | Authors: Jerry L. Sarquis, Mickey Sarquis

Solutions for Chapter 6.1: Introduction toChemical Bonding

Since 6 problems in chapter 6.1: Introduction toChemical Bonding have been answered, more than 24572 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: Modern Chemistry: Student Edition 2012, edition: 1. Modern Chemistry: Student Edition 2012 was written by and is associated to the ISBN: 9780547586632. Chapter 6.1: Introduction toChemical Bonding includes 6 full step-by-step solutions.

Key Chemistry Terms and definitions covered in this textbook
  • acid-dissociation constant (Ka)

    An equilibrium constant that expresses the extent to which an acid transfers a proton to solvent water. (Section 16.6)

  • Arrhenius equation

    An equation that relates the rate constant for a reaction to the frequency factor, A, the activation energy, Ea, and the temperature, T: k = Ae-Ea>RT. In its logarithmic form it is written ln k = -Ea>RT + ln A. (Section 14.5)

  • Brønsted-Lowry base

    A proton acceptor

  • cell potential

    The potential difference between the cathode and anode in an electrochemical cell; it is measured in volts: 1 V = 1 J>C. Also called electromotive force. (Section 20.4)

  • Dipeptide

    A molecule containing two amino acid units joined by a peptide bond

  • electrochemistry

    The branch of chemistry that deals with the relationships between electricity and chemical reactions. (Chapter 20: Introduction)

  • endothermic

    Any process with a positive DH (the system receives energy from the surroundings).

  • entropy

    The measure of disorder associated with a system.

  • equilibrium constant

    The numerical value of the equilibrium-constant expression for a system at equilibrium. The equilibrium constant is most usually denoted by Kp for gas-phase systems or Kc for solution-phase systems. (Section 15.2)

  • insulators

    Materials that do not conduct electricity. (Section 12.7)

  • Isoelectric point (pI)

    The pH at which an amino acid, polypeptide, or protein has no net charge

  • mole

    A collection of Avogadro’s number 16.022 * 10232 of objects; for example, a mole of H2O is 6.022 * 1023 H2O molecules. (Section 3.4)

  • nucleosides

    The product formed when either d-ribose or 2-deoxy-d-ribose is coupled with certain nitrogen heterocycles (called bases).

  • parts per billion (ppb)

    The concentration of a solution in grams of solute per 109 (billion) grams of solution; equals micrograms of solute per liter of solution for aqueous solutions. (Section 13.4)

  • Protecting group

    Reversibly creating an unreactive group for the purpose of preventing a functional group from potentially reacting to give an unwanted product or products

  • rate-determining step

    The slowest elementary step in a reaction mechanism. (Section 14.6)

  • tertiary

    A term used to indicate that exactly three alkyl groups are attached directly to a particular position. For example, a tertiary carbocation has three alkyl groups attached directly to the electrophilic carbon atom (C+).

  • Thermolysis

    Cleavage by heating

  • Wohl degradation

    A process that involves the removal of a carbon atom from an aldose. The aldehyde group is first converted to a cyanohydrin, followed by loss of HCN in the presence of a base.

  • Z (Section 5.2C)

    From the German, zusammen, meaning opposite. Specifi es that groups of higher priority on the carbons of a double bond are on the same side

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