Chapter 6

1. Chapter 6 Developing The Periodic Table

2. Each element has its own symbol that begins with a capital letter. Any other letters in the symbol are lower case.

3. Latin Names

4. Lead (Pb)“The Metal That Destroyed Rome” • According to some toxicologists “Lead poisoning contributed to the fall of Rome,”

5. Plumbum (Pb) Plumber Lead (Pb) Z = 82

6. The Lost Franklin Expedition

8. Its New, Its Canned, Its Poisoned This old tin can was full of potatoes and was part of the food supply on Sir John Franklin's ships. Many of these tin cans, discarded by the sailors, have been found on Beechey Island. In those days, cans were just starting to be used as a means of preserving food. People did not understand that the lead from the solder seam would give a person lead poisoning and could kill them. It is believed that many of the men of the Franklin Expedition died in this way.

9. Mendeleev • In 1869, Dmitri Mendeléev created the first version of the periodic table. • He arranged the elements in order of increasing atomic mass and grouped them by similarity of properties. • This allowed him to predict the properties of new elements.

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13. Henry Moseley • Developed method of measuring the atomic number of elements.

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16. Henry Moseley • Developed method of measuring the atomic number of elements. • The Modern Periodic Table is organized by increasing atomic number. • Predicted the existence of elements 43, 61, 72, and 75.

17. Gallipoli

18. Moseley • At the age of 27, having volunteered to serve in the British Army in WWI, Moseley was killed by a sniper at Gallipoli. • When WWI started, he volunteered for active duty. At the time of his death, he was the most promising physicist of his time.

19. “Ein schwerer Verlust” “A heavy loss”

20. Metals, Nonmetals, Metalloids • The periodic table can be used to determine the metallic/nonmetallic nature of an element.

21. Metals, Nonmetals, Metalloids

22. Groups and Periods • The vertical columns in the periodic table are called groups. • Rows in the periodic table are termed periods. • Elements with similar properties within the periodic table are grouped into a family.

23. Families on the Periodic Table • Columns in the periodic table can be grouped into families. • Families may be one column, or several columns put together. • Families have names rather than numbers. (Just like your family has a common last name.)

24. Alkali Metals

25. Alkali Metals • 1st column on the periodic table (Group 1) not including hydrogen. • Most reactive family of metals, always combined with something else in nature (table salt). • Low density metals (Li, Na and K are less dense than water). • that are soft enough to cut with a knife.

26. Alkaline Earth Metals Ca

27. Alkaline Earth Metals • Second column on the periodic table. (Group 2) • Second most reactive family of metals, always combined with nonmetals in nature. • All of the alkaline earth metals are found in compound form within the earth's crust. • Several of these elements are important mineral nutrients (such as Mg and Ca).

28. Calcium and Magnesium Two Important Minerals

29. Magnesium & Calcium are essential minerals for your health • CalciumFound primarily in dairy foods such as milk, cheese and yogurt. Your bones eagerly absorb and store calcium necessary for your body's growth and maintenance until you reach your mid 20's. After that, your body rapidly uses up the calcium to help keep your bones strong. Failure to get enough calcium can lead to osteoporosis (holes in the bones), brittle and easily breakable bones, and tooth loss. • MagnesiumMagnesium is one of the most important minerals your body needs, and fortunately, it can be found in many of the foods we eat, including many fruits, vegetables and dairy products. Failure to get enough magnesium can lead to muscle soreness, heart and blood pressure problems, as well as nervous disorders.

30. Magnesium Keeps the Doctor at Bay Recently, a healthy 18-year-old basketball player and health-conscious jogger died suddenly. The initial diagnosis was death from coronary artery disease due to high blood cholesterol. But the cause of death eventually proved to be magnesium deficiency.

31. Transition Metals • Elements in groups 3-12 • Less reactive harder metals • Includes metals used in jewelry and construction. • Metals used “as metal.”

32. Less reactive but can still react Iron (Fe) Rust (Fe2O3)

33. Oxygen Family or Chalcogens • Elements in group 16 • Oxygen is necessary for respiration. • Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

34. Halogens • Elements in group 17 • Most reactive of the nonmetals. • Always found combined with other elements in nature. • Have a strong unpleasant odor and are poisonous (have been used as chemical weapons). • In low doses can be used as disinfectants (chlorine in drinking water and in pools).

35. The Noble Gases • Elements in group 18 • All are gases. • VERY non-reactive. • Have a full outer energy level.

36. The Octet Rule • The octet rule states that an atom's outer energy level is full and most stable when it contains eight electrons. • This stability is the reason that the noble gases are so non-reactive. • All noble gases other than helium follow the octet rule.

37. Exception to the Octet RuleThe “Duet Rule” • The first energy level can only hold two electrons. • Elements such as Hydrogen and Helium that only have one energy level follow a “duet rule”. • The duet rule states that two electrons will stabilize an atom with only one energy level.

38. Rare Earth Elements • The thirty rare earth elements are composed of the lanthanide and actinide series. • The rare earth elements are metals. • Many of these elements are synthetic or man-made. (Primarily elements after plutonium) 0

39. Homework • Chapter 6 – Worksheet 1 • Study Guide for Chapter 6 is now assigned.