Periodic Table and Electron Configurations

1. Periodic Tableand Electron Configurations Honors Chemistry Unit 3

2. Modern Periodic Table • Elements are arranged by increasing atomic number. • Recall that atomic number gives the number of protons in the nucleus of an atom.

3. The Periodic Law says: • When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. • Horizontal rows = periods • There are 7 periods • Each row (or period) is the energy level • Vertical column = group (or family) • Similar physical & chemical properties • Identified by number (1 - 18)

4. Periods

5. Groups/Families

6. Areas of the periodic table Three classes of elements are: • Metals • Nonmetals 3. Metalloids Notice the heavy, stair-step line? • This is the dividing line between the Metals and Non-Metals

7. On the Left side of the table Does not include hydrogen Solids at room temperature (except for Mercury) Shiny Ductile: can be made into wires Malleable: can be pounded & easily shaped, like knives and swords Most are silver/grey in color Conducts heat and electricity Will loseelectrons to form (+) ions (cations) Properties of Metals

8. On the right sideof the periodic table Most are gases (H, He, Ne, etc.) Brittle, or break easily Dull texture Poor conductorsof heat and electricity Will Gainelectrons to become negative ions (anions) Come in a variety of colors Properties of Non-metals

9. Properties of Metalloids • Properties are intermediatebetween metals and nonmetals • Also called semi-metals • They are on the stair step line in between the metals and non-metals • They have a combination of both metallicandnon-metallic properties • Ex: they are shiny but don’t conduct electricity • Semiconductors – conduct electricity under certain circumstances (some used in computer technology)

10. Metallic Character • Metals • Nonmetals • Metalloids

11. Blocks • Main Group Elements – groups 1, 2 &13-18 • Transition Metals – groups 3-12 • Inner Transition Metals

12. Sublevel Blocks

13. 1 2 3 4 5 6 7 • Each row (or period) is the energy level for s and p orbitals. Period Number

14. Elements in the s - blocks s1 s2 He • Group 1 metals all end in s1 • Group 2 metals all end in s2 • really should include He, but it fits better in a different spot, since He has the properties of the noble gases, and has a full outer level of electrons. 1s1 2s2 7s1 7s2

15. The P-block – groups 13 - 18 p1 p2 p6 p3 p4 p5 2p6 2p1 3p1 6p1 6p6

16. Transition Metals - d block Groups 3 - 12 d9 d4 d1 d2 d3 d5 d6 d7 d8 d10 3d1 3d10 4d1 5d1

17. f6 f13 f1 f2 f3 f4 f5 f7 f8 f10 f12 f14 f11 f9 F - block • Called the “inner transition elements” 4f1 5f1

18. 1 2 3 4 5 6 7 • f orbitals start filling at 4f, and are 2 less than the period number 4f 5f

19. The “f” Block

20. The “d” orbitals fill up in levels 1 less than the period number, so the first d is 3d even though it’s in row 4. 1 2 3 4 5 6 7 3d 4d 5d

21. Writing Electron Configuration from the Periodic Table • The way an electron configuration ends will tell you what element you have. Examples: • 3d5 • 5s1 • 4p2 Mn Rb Ge

22. Chemistry Crash Course video - Periodic Table