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Solutions for Chapter 6: ELECTRONIC STRUCTURE OF ATOMS

Chemistry: The Central Science | 11th Edition | ISBN: 9780136006176 | Authors: Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward

Full solutions for Chemistry: The Central Science | 11th Edition

ISBN: 9780136006176

Chemistry: The Central Science | 11th Edition | ISBN: 9780136006176 | Authors: Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward

Solutions for Chapter 6: ELECTRONIC STRUCTURE OF ATOMS

Solutions for Chapter 6
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Textbook: Chemistry: The Central Science
Edition: 11
Author: Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward
ISBN: 9780136006176

This expansive textbook survival guide covers the following chapters and their solutions. Chapter 6: ELECTRONIC STRUCTURE OF ATOMS includes 95 full step-by-step solutions. Chemistry: The Central Science was written by and is associated to the ISBN: 9780136006176. Since 95 problems in chapter 6: ELECTRONIC STRUCTURE OF ATOMS have been answered, more than 100404 students have viewed full step-by-step solutions from this chapter. This textbook survival guide was created for the textbook: Chemistry: The Central Science , edition: 11.

Key Chemistry Terms and definitions covered in this textbook
  • beta particles

    Energetic electrons emitted from the nucleus, symbol 0-1e or b-. (Section 21.1)

  • calorimetry.

    The measurement of heat changes. (6.5)

  • chain reaction

    A reaction (generally involving radicals) in which one chemical entity can ultimately cause a chemical transformation for thousands of molecules.

  • chemical nomenclature

    The rules used in naming substances. (Section 2.8)

  • chromatogram

    In gas chromatography, a plot that identifies the retention time of each compound in the mixture.

  • cycloalkanes

    Saturated hydrocarbons of general formula CnH2n in which the carbon atoms form a closed ring. (Section 24.2)

  • diamagnetism

    The circulation of electron density in the presence of an external magnetic field, which produces a local (induced) magnetic field that opposes the external magnetic field.

  • exothermic

    Any process with a negative DH (the system gives energy to the surroundings).

  • geminal

    Two groups connected to the same carbon atom. For example, a geminal dihalide is a compound with two halogens connected to the same carbon atom.

  • Haworth projection

    A way to view furanose and pyranose forms of monosaccharides. The ring is drawn fl at and most commonly viewed through its edge with the anomeric carbon on the right and the oxygen atom of the ring to the rear

  • Hydrophilic

    From the Greek, meaning water-loving.

  • Ketose

    A monosaccharide containing a ketone group.

  • nucleotide

    Compounds formed from a molecule of phosphoric acid, a sugar molecule, and an organic nitrogen base. Nucleotides form linear polymers called DNA and RNA, which are involved in protein synthesis and cell reproduction. (Section 24.10)

  • primitive lattice

    A crystal lattice in which the lattice points are located only at the corners of each unit cell. (Section 12.2)

  • Prochiral hydrogens

    Refers to two hydrogens bonded to a carbon atom. When a different atom replaces one or the other, the carbon becomes a chiral center. The hydrogens of the CH2 group of ethanol, for example, are prochiral. Replacing one of them by deuterium gives (R)-1-deuteroethanol; replacing the other gives (S)-1-deuteroethanol

  • Reductive elimination

    Elimination of two substituents at a metal center, causing the oxidation state of the metal to decrease by two.

  • solubility-product constant (solubility product)1Ksp2

    An equilibrium constant related to the equilibrium between a solid salt and its ions in solution. It provides a quantitative measure of the solubility of a slightly soluble salt. (Section 17.4)

  • solute

    A substance dissolved in a solvent to form a solution; it is normally the component of a solution present in the smaller amount. (Section 4.1)

  • sp3 Hybrid orbital

    A hybrid atomic orbital formed by the combination of one s atomic orbital and three 2p atomic orbitals.

  • Valence Bond Theory

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