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

6. Mendeleev stated that elements arranged in order of increasing atomic mass show a periodic repetition of properties 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: PropertyObserved for Si Predicted for Eka- Silicon Observed for Sn Found for Ge Atomic Mass Melting Point ( o C) Density (g/cm 3 ) Boiling point of chloride ( o C) 28 1410 2.33 57.6 72 High 5.5 100 118 232 7.28 114 73 947 5.35 84

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 n o –Negative electrons, mass of 0, symbol e -

11. x atomic symbol A mass number (atomic mass) z atomic number

12. Atomic mass = number of protons + neutrons Atomic number = number of protons So what's the number of electrons?

13. 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

14. 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 Periodic Law - chemical and physical properties of element vary in a periodic way with their atomic number Hands-On: elemental samples (Helen)

15. 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

16. elements are arranged in increasing order of atomic number, as you go from left to right across the table. –The vertical columns are called "groups“ or “families”. –The horizontal rows are called "periods".

17. representative elements transition elements inner transition elements

19. alkali metalsalkaline earth metals lanthanoids actinoids transition metalshalogensnoble gases

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