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    Quantum Numbers
    Quantum Numbers
    Quantum Numbers
    Ebook33 pages21 minutes

    Quantum Numbers

    By IntroBooks Team

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    About this ebook

    Modern Chemistry Lavoisier's results and Atomic Theory
    provided chemists their first in depth understanding related to
    the nature of chemical reactions. Another cornerstone which
    dealt with the inherent property of all matter came a few years
    later in the form of atomic theory advanced in 1805 by an
    English schoolteacher, John Dalton. This theory puts forward
    the theory that matter constitutes of small particles which are
    named atoms and that chemical changes take place between
    atoms or groups of atoms. Finally, being equipped with in
    depth views about the nature of matter and of chemical
    reactions, chemistry began making rapid strides.
     
    Very soon one after the other the gas laws of Joseph Louis
    Gay-Lussac and that of Joseph Louis Proust's law of definite
    proportions came into being. In this period too came the
    hypothesis of Amedeo Avogadro, an Italian chemist, about the
    number of molecules in a volume of gas. To Dalton's theory
    that the atoms of a single element have the same weight,
    Avogadro, in 1811, added the idea that one quart (or other
    volume) of a gas has the number of molecules which are
    exactly same as that of any other gas with an equal volume if
    both are allowed to rest at the same temperature and pressure.
     
    His calculations also showed that if the gas is an element, such
    as hydrogen or oxygen, the atoms usually unite in pairs to
    form molecules (written H2, O2, and so on). The scientists
    knew, however, that equal volumes of different gases have
    unequal weights. Avogadro's hypothesis implied that this showed
    relative weights of single atoms. This has been proved to be
    correct, and today Avogadro's law may be stated thus: equal
    volumes of all gases under the same conditions of temperature
    and pressure contain the same number of molecules. Humphry
    Davy, about 1806, isolated a number of elements to add to the
    growing list.
     
    Jons Jakob Berzelius, in 1826, analyzed hundred of compounds
    and published accurate tables of atomic weights. Friedrich
    Wohler's synthesis of urea in 1828 proved that organic
    compounds could be made in the laboratory and opened a
    vast new field of chemistry. This began the development of the
    concept that organic compounds have geometric structure.
    Friedrich Kekule proposed cyclic (ring) structure of benzene
    about this time. Michael Faraday, formulated the laws of
    electrochemistry in 1834.

    LanguageEnglish
    PublisherIntroBooks
    Release dateNov 26, 2019
    ISBN9781393193258

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      Book preview

      Quantum Numbers - IntroBooks Team

      Quantum

      Numbers

      IntroBooks #354

      readintrobooks.com

      Copyright © 2017 IntroBooks

      All rights reserved.

      Preface

      Modern Chemistry Lavoisier’s results and Atomic Theory provided chemists their first in depth understanding related to the nature of chemical reactions. Another cornerstone which dealt with the inherent property of all matter came a few years later in the form of atomic theory advanced in 1805 by an English schoolteacher, John Dalton. This theory puts forward the theory that matter constitutes of small particles which are named atoms and that chemical changes take place between atoms or groups of atoms. Finally, being equipped with in depth views about the nature of matter and of chemical reactions, chemistry began making rapid strides.

      Very soon one after the other the gas laws of Joseph Louis Gay-Lussac and that of Joseph Louis Proust's law of definite proportions came into being. In this period too came the hypothesis of Amedeo Avogadro, an Italian chemist, about the number of molecules in a volume of gas. To Dalton's theory that the atoms of a single element have the same weight, Avogadro, in 1811, added the idea that one quart (or other volume) of a gas has the number of molecules which are exactly same as that of any other gas with an equal volume if both are allowed to rest at the same temperature and pressure.

      His calculations also showed that if the gas is an element, such as hydrogen or oxygen, the atoms usually unite in pairs to form molecules (written H2, O2, and so on). The scientists knew, however, that equal volumes of different gases have unequal weights. Avogadro's hypothesis implied that this showed relative weights of single atoms. This has been proved to be correct, and today Avogadro's law may be stated thus: equal volumes of all gases under the same conditions of temperature and pressure contain the same number of molecules. Humphry Davy, about 1806, isolated a number of elements to add to

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