Ch. 5 - The Periodic Table

1. Ch. 5 - The Periodic Table I.History of the Periodic Table Mendeleev Mosely Periodic Law

2. A. Dmitri Mendeleev • Dmitri Mendeleev (1869, Russian) • Organized elements by increasing atomic mass. • Predicted the existence of undiscovered elements.

3. B. Henry Mosely • Henry Mosely (1913, British) • Organized elements by increasing atomic number. • Fixed problems in Mendeleev’s arrangement.

4. C. Periodic Law • Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements into groups.

5. Key Concept How is the modern periodic table organized? In the modern periodic table, elements are arranged by increasing number of protons.

6. Ch. 5 - The Periodic Table II.Organization Metallic Character Rows & Columns Table Sections

7. A. Terms • Periodic Law • Properties of elements repeat periodically when the elements are arranged by increasing atomic number.

8. A. Metallic Character • Metals • Nonmetals • Metalloids

9. A. Metallic Character The majority of the elements on the periodic table are classified as metals. • Metalsare elements that are good conductors of electric current and heat. • Except for mercury, metals are solid at room temperature. • Most metals are solids. • Many metals are ductile; that is, they can be bent or drawn in to wires. .

10. A. Metallic Character Nonmetals generally have properties opposite to those of metals. • Nonmetalsare elements that are poor conductors of heat and electric current. • Nonmetals have low boiling points – many nonmetals are gases at room temperature. • Nonmetals that are solids at room temperature tend to be brittle. If they are hit with a hammer, they shatter or crumble.

11. A. Metallic Character Metalloid elements are located on the periodic table between metals and nonmetals. • Metalloidsare elements with properties that fall between those of metals and nonmetals. • For example, a metalloid’s ability to conduct electric current varies with temperature. Silicon (Si) and Germanium (Ge) are good insulators at low temperatures and good conductors at high temperatures.

12. B. Rows and Columns • Representative Elements • Transition Metals

13. B. Rows and Columns • Group (Family) • Period

14. B. Rows and Columns Each column in the periodic table is called a Group or Family. • The elements in a group have the same number of valence electrons, so members of the same group in the periodic table have similar chemical properties. • This pattern of repeating properties is the periodic law.

15. C. Family/Group Names • Group 1 • Alkali Metals • All have 1 valance electron • All form +1 charged ions • Hydrogen is NOT a metal and can also form -1 charged ion. • One of the most reactive groups on periodic table

16. Family/Group Names • Group 2 • Alkaline Earth Metals • All have 2 valance electrons • All from +2 charged ion

17. Family/Group Names • Group 3 to 12 • Transition Metals • All form positive ions but with different values (+1 to +6)

18. Family/Group Names • Group 13 • Boron Family • All have 3 valance electrons • All from +3 charged ions • Mixture of metalloids and metals

19. Family/Group Names • Group 14 • Carbon Family • All have 4 valance electrons • Form +4 or -4 charged ion • Mixture of metals, metalloids, and non metals.

20. Family/Group Names • Group 15 • Nitrogen Family • All have 5 valance electrons • All form -3 ion • Mixture of metals, metalloids, and non metals.

21. Family/Group Names • Group 16 • Oxygen Family • All have 6 valance electrons • All form -2 charged ions • Mostly nonmetals though 1 metal and one metaloids

22. Family/Group Names • Group 17 • Halogens • All have 7 valance electrons • All form -1 charged ion • Mostly nonmetals though 1 metalloid • One of the most reactive groups on the periodic table

23. Family/Group Names • Group 18 • Noble Gases • All have (except He) have 8 valance electrons • Most don’t react at all • They are “noble” • All are nonmetal • All are gases at room tempature

24. 1A 8A 2A 3A 4A 5A 6A 7A A. Terms • Group # = # of valence e- (except He) • Families have similar chemical characteristics . • Period # = # of energy levels

25. A. Terms • Valence Electrons • e- in the outermost energy level • Representative elements the number of valance electrons equals the ones digit • Group 13 = 3 valance electrons

26. B. Rows and Columns Each column in the periodic table of elements is a Group. • Elements in group 1 have ___ valence electron. • Elements in group 2 have ___ valence electrons. • Elements in group 13 have ___ valence electrons. • Elements in group 14 have ___ valence electrons. • Elements in group 15 have ___ valence electrons. • Elements in group 16 have ___ valence electrons. • Elements in group 17 have ___ valence electrons. • Elements in group 18 have ___ valence electrons. 1 2 3 4 5 6 7 8

27. Horizontally Into Periods B. Rows and Columns Each row in the table of elements is a Period. • Elements in period __ have one energy level. • Elements in period __ have two energy levels. • Elements in period __ have three energy levels. • Elements in period __ have four energy levels. • Elements in period __ have five energy levels. • Elements in period __ have six energy levels. • Elements in period __ have seven energy levels. 1 2 3 4 5 6 7

28. B. Lewis Dot Diagrams • Dots represent the valence e-. • Ex.: Sodium • Ex.: Chlorine

29. B. Lewis Dot Diagrams • Start by putting one dot on each side of elements symbol. • Once all 4 side have one dot they can double up

30. Review There are four pieces of information for each element. 1. _______________ 2. _______________ 3. _______________ 4. ______________

31. Which element is a halogen?

32. Which element has 4 valance electrons?

33. Which element is a alkaline earth metal with 4 energy levels?

34. Which element forms a charge of -1 ?

35. Which element forms a charge of +1 ?