3-3 The Periodic Table

1. GO 3 Describe ideas used in interpreting the chemical nature of matter, both in the past and present, and identify example evidence that has contributed to the development of these ideas 3-3 The Periodic Table

2. Guided Question What is the periodic table of elements? And how is it organized?

3. Mendeleev A picture of Mendeleev’s Original Periodic table and the scientist himself!

4. 1869 – Dmitri Mendeleev • Organized the 63 known elements into a series of rows and columns based on physical and chemical properties • He left gaps in the table explaining there were elements that had not been discovered yet • He then hypothesized about the physical and chemical properties of the atoms that would fill the voids • After his table was published, gallium was discovered and with properties almost exactly the same as Mendeleev predicted, it fit in an open space!

5. Breaking Down the Element

6. Breaking Down the Element Indicates number of Protons in the nucleus & number ofelectrons orbiting

7. Understanding the Periodic Table Need to know: • Metals are Yellow • Non-metals are green • Metalliods are purple

8. Metals vs. Non-metals ___

9. OR vs

10. Metals • Grouped on the Right side of the periodic table (88 of the elements are metals) • Physical Properties: • Shiny solids at room temperature • High conductors of heat and electricity • Ductile (can be formed into wires) • Malleable (rolled and can be beaten into thin sheets)

11. Non-metals • Grouped on the right side of the periodic table • Physical Properties: • May be solid, liquid or gas at RT • Poor conductors of heat and electricity (called Insulators) • Solid forms are dull and brittle

12. Metalloids • have both metallic and non-metallic properties Tellurium Silicon

13. Understanding the Periodic Table • Each horizontal version is called a PERIOD (1 to 7) • Each Vertical column forms a group (or FAMILY) (1-18)

14. Understanding the Periodic Table Need to know: • Group 1 • Group 2 • Group 17 • Group 18

15. ____ Metals – Group 1

16. Alkali Metals – Group 1 Sodium Lithium Cesium The most reactive of the metals They react when exposed to air or water As you move down the group, reactivity increases.

17. Alkaline Earth Metals – Group 2

18. Alkaline Earth Metals – Group 2 • They react when exposed to air or water but not as strong as that of the alkali metals

19. Halogens– Group 17

20. Halogens– Group 17 • The most reactive non-metals (Fluorine can etch glass) • Can combine with other elements to form new substances; Ex: Na +F = sodium fluoride found in Toothpaste • Various colors and physical states • F and Cl = yellowish green gas; • Br = dark red liquid; • I = purple-black solid with a metallic crystalline sheen

21. Inert Gases – Group 18

22. Inert Gases – Group 18 • Also known as the NOBEL GASES • The most Stable and unreactive elements; long thought that they could not combine with other elements • 1962 – Canadian Chemistry Neil Bartlett (B.C.) was the first to prepare a compound containing a noble gas (XeF4)

23. What is the deal with

24. Hydrogen • Considered to be a Non metal element (Sometimes has a special or separate spot on some versions of the Periodic Table) • Here are basic facts about the Hydrogen element in the periodic table: • Is the most abundant element in the universe (75% of everything is H) • Hydrogen gas is extremely flammable (The Hindenburg) • Is a colourless and odourless gas at room temp • Can take on a negative charge (H-) or a positive charge (H+) • Hydrogen is the lightest of all elements - atomic mass 1.00794