Essential Question

1. Essential Question How can you predict an element’s properties by its placement on the periodic table?

2. Atom • The atom has electrons orbiting the nucleus in fixed paths called orbitals. *This is an outdated model, but very useful for teaching chemistry*

3. Nails Bohr’s Planet model of Atoms • These orbits are referred to as energy levels 1 2 3

4. Table Development • 1869 Russian scientist Dmitri Mendeleev organized known elements by atomic mass • He noticed that at regular intervals the chemical properties of elements repeated. So, He placed elements with similar properties in the same column.

5. Table Development • Henry Moseley developed the modern periodic table arranging the elements by Atomic Number • Elements with similar chemical properties are in the same column

6. Modern Table • Elements are arranged by atomic number

7. Modern Table • Horizontal rows are PERIODS 1 2 3 4 5 6

8. Modern Table • Vertical Columns are GROUPS 17 18 1 2 13 14 15 16 3 4 5 6 7 8 9 10 11 12

9. Table Properties • Elements Found in the Same Group Have Very Similar Chemical Properties All Very Reactive Metals

10. Electron Configuration • Outermost electrons are called valence electrons. The # of valence electrons determines chemical properties • Elements in a group have the same number of valence e- Be 2-2 Mg 2-8-2 Ca 2-8-8-2 Sr 2-8-18-8-2 Ba 2-8-18-18-8-2 Ra 2-8-18-32-18-8-2

11. Practice • Draw the electron configuration for carbon, iron, and potassium

12. Table Properties • Elements in the Same Period do not have similar chemical properties. Extremely Un-Reactive Metal Liquid Metal Extremely reactive Metal Very Un-Reactive Gas

13. Periodic Table Topic 2: Metals & Non-Metals

14. Metals and Non-Metals • Most of the 114 known elements are Metals. • Less than 20 of all the elements are considered Non-Metals. • About 7 elements are considered SemiMetals or Metalloids.

16. Metal Properties • Good Conductors of Electricity • Metals Have Luster • Solid at room Temp (except for Hg) • Are Malleable (shapeable) • Are Ductile (made into wire)

17. Non-Metal Properties • Non-Metals do not conduct Electricity • Non-Metals are Brittle • Can be a Gas at Room Temp • Have No Luster

18. Semimetals • Semimetals may have luster. • Semimetals may conduct electricity. • Semimetals may be shaped.

19. Practice • Label Metals, Nonmetals, and Metalloids

21. Activity: How metallic or non-metallic is an element? Most ACTIVE Non-Metal Most ACTIVE Metal

22. Stable electron configuration • For stability, atoms need 8 (or 0) valence electrons • This is why atoms become ions

23. # of electrons • Metals are electron losers • Non-metals are electron gainers

24. Periodic Table Topic 3: Special Groups

25. Alkali & Alkaline Earth Metals • Never found in nature due to their high reactivity, only as compounds. • Francium is the most reactive metal there is. Alkali Metals

26. The Halogens Halogens Group 17

27. The Nobel Gases • Will not react with any other elements due to Stable valence electron configuration. • Eight valence electrons is called a STABLE OCTET, all elements try to achieve this electron configuration.

28. The Transition Metals Transition Metals

29. Transition Metals • All metals in the middle of the table. • Not reactive under most conditions. • Are reactive at high temperatures (oxidize)