THE PERIODIC TABLE

1. THE PERIODIC TABLE

2. Dmitri Mendeleev • A Russian scientist who began to classify the 60 known elements of his time • Worked with the indivisible model of an atom • Atomic masses were known in comparison to hydrogen, which was set as "1"

3. “I began to look about and write down the elements with their atomic weights and typical properties, analogous elements and like atomic weights on separate cards, and this soon convinced me that the properties of elements are in periodic dependence upon their atomic weights.”--Mendeleev, Principles of Chemistry, 1905, Vol. II

4. Mendeleev discovered that the properties of the elements repeated at regular intervals when the elements are arranged in order of increasing atomic mass periodicity: the occurrence of similar physical and chemical properties of elements at regular intervals

5. He left blank spaces for where he predicted (based on properties) an element should be • He predicted (accurately!) the properties of yet-undiscovered elements!!!

7. Observed properties of Eka-Silicon and observed properties of Germanium:

8. In the meantime… • Thomson and Rutherford discovered the proton and the electron

9. Chadwick, in Rutherford’s lab made another discovery: the neutron!

10. SO… an atom is made of • Positive protons, mass of 1, symbol p+ • Uncharged neutrons, mass of 1, symbol no • Negative electrons, mass of 0, symbol e-

11. Atomic mass = number of protons + neutrons Atomic number = number of protons Number of protons = number of electrons (in a neutral atom)

12. Moseley working together with Rutherford discovered that the element's properties could be even better predicted using the number of charges the atom had: atomic number

13. elements were re-arranged by atomic number (as in the modern Periodic Table) • elements arranged in order of increasing atomic number show a periodic repetition of properties • each column of the periodic table (called a group) has similar properties (periodic trends) • The vertical columns are called "groups“ or “families”. • The horizontal rows are called "periods". The Periodic Law - chemical and physical properties of element vary in a periodic way with their atomic number

14. The modern Periodic Table • Scientists divide elements into 3 categories 1. Metals • Alkali metals • Alkaline earth metals • Transition elements • Inner transition elements 2. Non-metals • Halogens • Noble gases 3. Metalloids

18. representative elements transition elements inner transition elements

19. alkali metals noble gases alkaline earth metals halogens transition metals lanthanoids actinoids

20. Metals • left side and centre of periodic table • Solid at room T (except mercury, Hg) • Silver (except Cu and Au) • Shiny, conduct electricity and heat, malleable and ductile

21. malleable: capable of being shaped, the degree to which it can be shaped by pounding with a hammer ductile: physical property of being capable of sustaining large deformations without breaking (for example being drawn into a wire)

22. Non-metals • Right side of periodic table • Found in all three states • Variety of colours • Poor conductors of heat/electricity • Usually brittle (having little elasticity: easily cracked or fractured or snapped )

23. Metalloids • Along zig-zag line dividing metals and non-metals • Metalloids are: Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium • Have some metallic and non-metallic properties • Ex. Si - silicon: shiny, nonmalleable, a semi-conductor