2. Families of Elements Chemistry

3. Learning Objectives TLW use the Periodic Table to identify and explain the properties of chemical families (TEKS 6.B) TLW color code the periodic table we’ve been customizing

4. Agenda Ready, Set, Color Your Periodic Table How Elements are Classified Types of Metals Types of Non-Metals Review questions Independent Practice – Periodic Table Puzzle

5. I. How elements are classified A. Elements are classified as metals or non-metals 1. Metals – elements that are good conductors of heat and electricity; a. Usually shiny solids; b. Can be (can be shaped and hammered)

6. c. 88 elements are metal d. Metals have 1, 2, 3, or 4 valence electrons e. Metals tend to lose electrons in a chemical reaction ex. Rusting = iron will lose its valence electrons

7. 2. Non-metals – elements that are poor conductors of heat and electricity a. Found on the right side of periodic table b. Non-metals can be solid, liquid, or gas c. Solid non-metals are very brittle and dull

8. d. Non-metals gain electrons in a chemical reaction e. Non-metals have 5, 6, 7 or 8 valence electrons 3. Metalloids a. elements that have properties of both metals and nonmetals b. they can conduct electricity and heat, just not very well

9. B. Types of Metals 1. Alkali Metals a. All alkali metals are found in Group 1 (Column 1) b. the alkali metals include: Li, Na, K, Rb, Cs and Fr c. Alkali metals are soft and shiny d. All alkali metals react very violently with H 2 O

11. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

12. e. all alkalis have 1 valence electron; that is why they are so reactive f. Forms positive ions = lose electrons (oxidation no. 1+) g. alkali metals are only found in nature as compounds, not pure elements

13. 2. Alkaline-earth Metals a. Earth metals are in Group 2 b. Earth metals have 2 valence electrons c. Alkaline-Earth metals include: Be, Mg, Ca, Sr, Ba, Ra d. Forms positive ions = lose electrons (oxidation no. 2+) e. Ex. Of useful alkaline-earth metal – milk of magnesia

15. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

16. 3. Transition Metals a. Found in the middle of the periodic table b. In Groups 3-12 c. Not as reactive as Groups 1 and 2 d. Can be found in nature in pure form e. Since easily shaped; many transitional metals are used for jewelry, wiring and others f. Includes rare earth metals & radioactives

17. f. All transition metals lose electrons => so they form positive ions (variable number of valence e - 1 to 4) (oxidation numbers from 1+ - 4+) g. Includes 68 elements

18. h. Some examples of transitional metals include: Cu, Fe, Au, Ag, Hg, Zn, etc

19. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

20. 4. Other Metals a. Part, but not all elements of Groups 13-16 b. form positive ions = loses electrons (oxidation numbers usually 3+ or 4+) c. includes: Al, Sn, Pb and others d. some are called metalloids (metals/non-metal properties)

21. Alloys Alloys are materials that contain more than one metal element and still maintain the characteristic properties of metals Alloys can be easier to work with, more durable, hold their shape better, more corrosion resistant than any of the pure metals they contain Examples – steel (iron, chromium, nickel, and carbon), brass (copper and zinc) and solder (lead and tin)

22. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

23. C. Non-metals Groups – 13 - 18 1. Basic Non-Metals a. Group 13 – 16 and H b. Not reactive c. Include: C, N, S, O, Si, P d. Are gases or solids e. Semiconductors – elements that can conduct electricity, but aren’t metals includes: B, Si, Ge, As, Sb, Te

24. C. Types of Non-metals 1. Basic Non-Metals e. Groups 13 & 14 have 3 and 4 valence electrons, respectively. - Tend to lose electrons and become positive. (oxidation numbers 3+ and 4+, respectively) f. Groups 15 & 16 have 5 & 6 valence electrons, respectively. Tend to gain valence electrons. Oxidation numbers are 3- and 2-, respectively.

25. C. Types of Non-metals 2. Halogens a. Highly reactive elements b. Group 17 c. Halogens include: F, Cl, Br, I, At d. Are gases in nature… except Bromine which is a liquid e. Notice they all end in “ine” f. halogens gain electrons = forms negative ions (oxidation number 1-)

26. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

28. 3. Noble Gases a. Elements in Group 18 b. Located on the far right side of the periodic table c. Nobel gases are the most non-reactive elements d. All noble elements are gases e. Noble gases include: He, Ne, Ar, Kr, Xe, and Rn

29. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

30. f. All noble gases have 8 valence electrons (except He with 2) g. Since outer valence shell is filled, they don’t react with other elements (oxidation number is 0) h. Because noble gases are nonreactive they are called “inert” gases i. Noble gases are mostly found as pure elements, not in compounds

32. 2 3456789101112 13141516 17 Group # CCCCCCCCCC F Cl Br I At Non-metals (green) Alkali Metals (blue) Alkaline Earth Metals (red) Group No. Transition Metals (yellow) Noble Gases (brown) Halogens (orange) Ge Sb Po Other metals (turquoise) Metalloids (fushia) Rare Earth Metals (gold)

34. Section Questions 1. A shiny luster, can conduct electricity, is malleable and is a solid describes what? metals 2. Cannot conduct electricity, and is dull in luster describes what? nonmetals

35. 3. How many valence electrons do metals have? 1, 2, 3, or 4 4. How many valence electrons do nonmetals have? 5, 6, 7, or 8

36. 5. If an element has properties of both metals and nonmetals, it is called a what? metalloid 6. What kind of ions do metals form? positive 7. What kind of ions do nonmetals form? negative

37. 8. Where are the most reactive metals found on the periodic table? Left side – Group 1 – Alkali Metals 9. Where are the most stable, nonreactive elements found on the periodic table? Right side – Group 18 – Noble Gases 10. What are the elements in Group 17 called? halogens

38. Independent Practice Periodic Table Puzzle