Periodic Table

1. Periodic Table

3. In 1669 German merchant and amateur alchemist Hennig Brand attempted to created a Philosopher’s Stone; an object that supposedly could turn metals into pure gold. He heated residues from boiled urine, and a liquid dropped out and burst into flames. This was the first discovery of phosphorus.

4. In 1680 Robert Boyle also discovered phosphorus, and it became public.In 1809 at least 47 elements were discovered, and scientists began to see patterns in the characteristics.In 1863 English chemist John Newlands divided the than discovered 56 elements into 11 groups, based on characteristics.

5. In 1869 Russian chemist Dimitri Mendeleev started the development of the periodic table, arranging chemical elements by atomic mass. He predicted the discovery of other elements, and left spaces open in his periodic table for them.

6. In 1886 French physicist Antoine Bequerel first discovered radioactivity. Thomson student from New Zealand Ernest Rutherford named three types of radiation; alpha, beta and gamma rays. Marie and Pierre Curie started working on the radiation of uranium and thorium, and subsequently discovered radium and polonium. They discovered that beta particles were negatively charged.

7. In 1894 Sir William Ramsay and Lord Rayleigh discovered the noble gases, which were added to the periodic table as group 0. • In 1897 English physicist J. J. Thomson first discovered electrons; small negatively charged particles in an atom. John Townsend and Robert Millikan determined their exact charge and mass.In 1900 Bequerel discovered that electrons and beta particles as identified by the Curies are the same thing.

8. In 1903Rutherford announced that radioactivity is caused by the breakdown of atoms.In 1911 Rutherford and German physicist Hans Geiger discovered that electrons orbit the nucleus of an atom.

9. In 1913 Bohr discovered that electrons move around a nucleus in discrete energy called orbitals. Radiation is emitted during movement from one orbital to another.

10. In 1914 Rutherford first identified protons in the atomic nucleus. He also transmutated a nitrogen atom into an oxygen atom for the first time. English physicist Henry Moseley provided atomic numbers, based on the number of electrons in an atom, rather than based on atomic mass.

11. In 1932 James Chadwick first discovered neutrons, and isotopes were identified. This was the complete basis for the periodic table. In that same year Englishman Cockroft and the Irishman Walton first split an atom by bombarding lithium in a particle accelerator, changing it to two helium nuclei.

12. In 1945Glenn Seaborg identified lanthanides and actinides (atomic number >92), which are usually placed below the periodic table

13. Copper is one of the transition metals. Transition Metals

14. Transition metals • The transition elements are located in groups IB to VIIIB of the periodic table. • Because they possess the properties of metals, the transition elements are also known as the transition metals. These elements are very hard, with high melting points and boiling points.

15. Transition Metals • Low ionization energies • Positive oxidation states • Very hard • High melting points • High boiling points • High electrical conductivity • Malleable • Five d orbitals become more filled, from left to right on periodic table

16. Nonmetals • The nonmetals are located on the upper right side of the periodic table. Nonmetals are separated from metals by a line that cuts diagonally through the region of the periodic table containing elements with partially filled p orbitals.

17. Nonmetals • High ionization energies • High electronegativities • Poor thermal conductors • Poor electrical conductors • Brittle solids • Little or no metallic luster • Gain electrons easily

18. Properties Nonmetals • Nonmetals have high ionization energies and electronegativities. They are generally poor conductors of heat and electricity. Solid nonmetals are generally brittle, with little or no metallic luster. Most nonmetals have the ability to gain electrons easily. Nonmetals display a wide range of chemical properties and reactivities.

19. Metals • Metals are located on the left side and the middle of the periodic table. Group IA and Group IIA (the alkali metals) are the most active metals. The transition elements, groups IB to VIIIB, are also considered metals.

20. Metals • Metals are shiny solids are room temperature (except mercury), with characteristic high melting points and densities. Many of the properties of metals, including large atomic radius, low ionization energy, and low electronegativity, are due to the fact that the electrons in the valence shell of a metal atoms can be removed easily. One characteristic of metals is their ability to be deformed without breaking. Metals are good heat conductors and electrical conductors.

21. Metals • Shiny 'metallic' appearance • Solids at room temperature (except mercury) • Bismuth Is an ex. Of a metal.

22. Noble gases • The noble gases, also known as the inert gases, are located in Group VIII of the periodic table. Group VIII is sometimes called Group O.

23. Noble Gases • The noble gases are relatively nonreactive. This is because they have a complete valence shell. They have little tendency to gain or lose electrons. The noble gases have high ionization energies and negligible electronegativities. The noble gases have low boiling points and are all gases at room temperature.

24. Noble gases • Fairly nonreactive • Complete valence shell • High ionization energies • Very low electronegativities • Low boiling points (all gases at room temperature)

25. Rare Earth Metals • When you look at the Periodic Table, there is a block of two rows of elements located below the main body of the chart. These elements, plus lanthanum (element 57) and actinium (element 89), are known collectively as the rare earth elements or rare earth metals.

26. Rare Earth • The rare earths are silver, silvery-white, or gray metals. • The metals have a high luster, but tarnish readily in air. • The metals have high electrical conductivity. • The rare earths share many common properties. This makes them difficult to separate or even distinguish from each other. • There are very small differences in solubility and complex formation between the rare earths. • The rare earth metals naturally occur together in minerals (e.g., monazite is a mixed rare earth phosphate). • Rare earths are found with non-metals, usually in the 3+ oxidation state. There is little tendency to vary the valence. (Europium also has a valence of 2+ and cerium also a valence of 4+.)

27. Rare earth • Plutonium Is a rare earth metal.

28. Alkali Metals • The alkali metals are the elements located in Group IA of the periodic table.

29. Alkali Metals • Lower densities than other metals • One loosely bound valence electron • Largest atomic radii in their periods • Low ionization energies • Low electronegativities

30. Alkali Metals • Sodium

31. Alkaline Earth Metals • The alkaline earths are the elements located in Group IIA of the periodic table. • The alkaline earths possess many of the characteristic properties of metals. Alkaline earths have low electron affinities and low electronegativities

32. Alkaline Earth Metals • Two electrons in the outer shell • Low electron affinities • Low electronegativities • Readily form divalent cations. • Magnesium