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If I have seen further it is by standing on the shoulders of giants.                             Sir Isaac Newton

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18th Century:  Gas Chemistry 19th Century:  Organic Chemistry 20th Century:  Nuclear Chemistry 21st Century:  Quantum Chemistry

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"Of course the elements are earth, water, fire
and air. But what about chromium? Surely you
can •t ignore chromium. "

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Democritus:  470-380  BC Coined the term “atom” Aristotle:  384-322 BC Four Element Concept

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In 1665 in Oxford, along with his assistant  Robert Hooke devised the vacuum chamber. First prominent scientist to perform controlled experiments and publish his work. Boyles Law:  P1V1  = P2V2.

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First person to make good use of the balance changing chemistry from qualitative to quantitative Disproved Phlogiston Theory/instead proposed Combustion Theory Law of Conservation of Mass Beheaded by guillotine in 1794 Antoine Lavoisier YouTubeVideo.com

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Law of Constant Proportions 1799 the proportions of the components of a chemical compound are always the same no matter how it is prepared. B ecame more clear to scientists in 1803 with the help of John Dalton. FYI:  First to identify the sugar that comes from grapes as glucose.

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Avogadro’s Hypothesis:  1811. At the same temperature and pressure, equal volumes of gases contain the same number of molecules. Extremely radical for the time period, was not accepted for another 50 years (Karlsruhe Conference 1860).

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Daltons Atomic Theory: (1803). Elements are made of tiny particles called atoms. All atoms of the same element are identical (later to be revised). The atoms of a given element are different from those of any other element. Elements combine to form compounds. M ass is neither created or destroyed in a chemical reaction, but can be rearranged.

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Law of Octaves. Any given element will exhibit analogous behaviour to the 8th element following it in the periodic table.

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Late 1860’s, arranged the 63 known elements (known by atomic weights) into groups based on chemical and physical properties. Where a gap existed, he predicted a new element would be found and its properties, Ga (1875), Sc (1879), Ge (1886) were found during his lifetime.

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Meyer’s 1864 textbook included an abbreviated version of the periodic table consisting of appx. ½ of the elements listed in order by atomic weight and demonstrated periodic valence changes as a function of atomic weight. In 1868 he constructed an extended table and gave it to a colleague to evaluate

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Starting with his discovery of plutonium in 1940, he discovered all the trans uranium elements (94-102). He reconfigured the periodic table by placing the actinide series below the lanthanide series. 1951 received Nobel Prize in chemistry for his work.

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Nobel Prize in physics 1906. 1871 became a professor at the Cavendish Laboratories in Cambridge England. Experimented with electrical currents inside empty glass tubes (cathode rays). Bold proposal that these mysterious rays are streams of particles  much smaller than atoms.

Proposed the first model of the atom with subatomic particles. Credited with the discovery of the electron based from his work with cathode ray tubes. Plum Pudding Model:  the atom is made up of a positively charged pudding with negative electrons distributed throughout to neutralize the atom.

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Performed in 1909 determined the size of the charge of an electron. Oil Drop Experiment.

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New Zealand, 1871-1937, physicist. Awarded a scholarship to Cambridge University (1894) where he was influenced by JJ Thomson to study the recently discovered x-rays. Coined the terms:  alpha, beta and gamma rays, half-life, proton. Given credit for the proton, and nucleus.

1907 went to Univ. of Manchester to work with Hans Geiger 1908 received Nobel Prize in chemistry for his work with radiation and the atomic nucleus Appx1909 discovered the atomic nucleus and proposed a model of the atom Gold Foil Experiment (1909)-the atom is mainly empty space through which electrons move and there is a tiny dense region “nucleus” centrally located that contained all of an atom’s positive charge

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Died at the age of 27, shot through the head by a Turkish bullet at Gallipoli in 1915. “ein schwerer Verlust für die Naturwissenschaften”. Studied the frequency of x-rays given off by cathode ray tubes when electrons strike the anode.

Found that there was a relationship between the frequencies (v) of the x-rays given off by the cathode ray tube and the atomic number of the metal used to form the anode. Conclusion:  The atomic number was equal to the positive charge (charge on the nucleus) of an atom.  (1914). This then caused the periodic table to be reorganized based on atomic number of the element, not atomic weight.

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1911 spent two years working with Ernest Rutherford. Main studies were with radioactivity. Along with Rutherford and others noticed that the proton did not account for all the mass of an atom, that the atomic mass was always more than the atomic number.

Hypothesis of the time was that there was a proton-electron pairing in the nucleus making up for the difference of the mass. Influenced by the work of Frederick and Marie –Joliot Curie and their work with radiation. 1932 neutron discovered to be the “neutral” particle that weighed 0.1% more than the proton accounting for the mass. 1935 Nobel Prize for his work.

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1922 Nobel Prize in physics for his work on the atomic structure. Studied under Rutherford in Manchester. Expanded Rutherford's theory that electrons could travel in certain orbits and that the outer orbits determined the chemical properties of the atom.

Also described the way atoms emit radiation by suggesting that if an electron gains energy it can jump from ground state to a higher energy level “excited” state.  And when the electron loses energy and falls back to a lower energy level, it gives off a photon of light. 1939 visited the USA and re-laid news that German scientists were working on splitting the atom, which spurred the creation of the Manhattan Project.

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Werner Heisenberg (1901-1976, German Physicist)

Influenced by the work of James Chadwick. 1927 Uncertainty Principle:  It is impossible to know both the exact location & velocity of an electron at any given time. Nobel Prize in Physics in 1932 for the creation of quantum mechanics, the application which has led among other things to the discovery of the allotropic forms of hydrogen.

History of Chemistry