1. Periodic Table Unit IV

2. I History A. Mendeleev Arranged elements by their masses Arranged elements by their masses B. Moseley Arranged elements by their atomic number Arranged elements by their atomic number Modern periodic table Modern periodic table

3. II Arrangement of the Periodic Table A. Groups Columns on the table Columns on the table Contain the same number of valence electrons Contain the same number of valence electrons B. Periods Rows on the table Rows on the table Use the same energy levels Use the same energy levels

4. Groups Periods

5. III Types of Elements

6. A. Metals 1. Location a) Lower left side of the table 2. Properties a) Metals are malleable and ductile b) Metals are solids at room temperature except mercury c) Metals have luster d) Metals are good conductors e) Metals have low ionization energy and low electronegativity f) Metals lose electrons and form positive ions

7. B. Nonmetals 1. Location a) Upper right side of the table 2. Properties a) Nonmetals are brittle b) Nonmetals are gases or molecular solids at room temperature except bromine which is a liquid c) Nonmetals are dull d) Nonmetals are insulators e) Nonmetals have high ionization energy and high electronegativity f) Nonmetals gain electrons and form negative ions

8. C. Transition Metals 1. Location a) Groups 3 through 12 2. Properties a) Series of elements that fill the d-sublevel b) Transition metals have multiple oxidation states c) Transition metals form colored ions

9. D. Metalloids 1. Location a) On the “stairs” plus Ge and Sb 2. Properties a) Metalloids are brittle b) Metalloids are solid at room temperature c) Metalloids have luster d) Metalloids are semi- conductors e) Metalloids have middle ionization energy and electronegativity values f) Metalloids gain or lose electrons

10. E. Noble Gases 1. Location a) Noble Gases are in Group 18 2. Properties a) Noble gases are inert which means they do not react b) Noble gases are monatomic c) Noble gases have filled outer energy levels

11. IV Properties of Elements Ionization Energy (IE) Amount of energy to remove an electron Amount of energy to remove an electron Atomic Radius ½ distance between two nuclei ½ distance between two nuclei Ionic Radius Metals decrease in size Metals decrease in size Nonmetals increase in size Nonmetals increase in size Electronegativity (EN) Attraction for electrons Attraction for electronsReactivity Metal activity increases as you go left and down Metal activity increases as you go left and down Nonmetallic activity increases as you go up and to the right Nonmetallic activity increases as you go up and to the right

12. V Groups Hydrogen Alkali Metals Group 1 Group 1 Explosive in water Explosive in water Alkaline Earth Metals Group 2 Group 2Halogens Group 17 Group 17 All nonmetals All nonmetals All phases of matter All phases of matter F 2 and Cl 2 (gas) Br 2 (liquid) I 2 (solid) F 2 and Cl 2 (gas) Br 2 (liquid) I 2 (solid) Noble Gases Group 18 Group 18 Do not react except the largest members Do not react except the largest members

13. VI Trends As you go down a group Atomic number increases Mass increases Valence electrons remain the same Energy levels increase Metallic character increases Nonmetallic character decreases Radius increases IE and EN decrease As you go across a period Atomic number increases Mass increases Valence electrons increase Energy level is constant Metallic character decreases Nonmetallic character increases Radius decreases IE and EN increase

14. Notable Observations

15. s-electrons d-electronss p-electrons f-electrons

16. s-electrons 2s 3s 4s 5s 6s 7s

17. 2p 3p 4p 5p 6p 7p p-electrons

18. d-electrons 4d 6d 5d 3d

19. f-electrons 4f 5f