The Periodic Table of Elements

1. The Periodic Table of Elements E.Ray Period 3 November 30, 2009 Joy Period 6 November 30, 2009

2. The History of the Periodic Table: Who Contributed

3. Antointe Lavoisier • Known as the “Father of Chemistry” • Made a system for naming the elements. • Named approximately 23 elements including: oxygen, silver, gold, and carbon. • Found that water is made up of hydrogen and oxygen. • Defined the nature of elements.

4. John Newlands • Organized the first fourteen elements by their chemical properties. • He called this system the law of octaves.

5. Lothar Meyer • Created a periodic table much like the modern one. Based upon atomic mass and physical properties. • Much of the credit was given to Mendeleev because Mendeleev published a book of these ideas first.

6. Dmitri Mendeleev • Designed one of the first periodic tables with the known elements by their atomic mass and chemical properties. • Predicted properties of many undiscovered elements like scandium, gallium, and germanium.

7. Henry Moseley • Found that each element has their own number of protons and that the number equaled the atomic number. • Came up with the periodic law…which is when the elements are arranged by atomic number instead of mass, there is a repetition of physical and chemical properties.

8. The Modern Periodic Table: Organization

9. Groups: A vertical column of elements in the periodic table. Can also be called a family. Periods: A horizontal row of elements in the modern periodic table. Column or Row??? Definitions from textbook page 154.

10. Valence Electrons: The electrons in an atom’s outermost orbitals. Determines the chemical properties of an elements. Orbitals: S three-dimensional region around the nucleus. Describes the electron’s probable location. Determines What??? Definition from textbook page 140 Definition from textbook page 132

11. Trends: Moving Through the Periodic Table

12. Atomic Radius • Defined as half the distance between adjacent nuclei in a crystal of the element. (Textbook page 163) • When looking from the left side of the periodic table to the right, the atomic radii decreases. • When traveling downward on the periodic table the atomic radii will increase.

13. Ionic Radius • Atoms can gain or lose electrons. These electrons will come together to make positive or negative ions. • As atoms lose their negatively charged electrons and become positive ions, the ionic radius will always become smaller. • As atoms gain electrons and form negative ions, the ionic radius will always become larger. • As you travel left through the Periodic Table, periods will increase. • As you travel downward through the table, the groups will increase.

14. Ionization Energy • Ionization energy = the energy required to remove an electron from a gaseous atom. • As you move left through the periods, the ionization energies increase. • As you move down through the groups, the ionization energies decrease. Definition from textbook page 167

15. Electronegativity • The electronegativity of an element indicates the relative ability of its atoms to attract electrons on a chemical bond. • The units used are called Paulings. • Electronegativity usually decreases as you move down through a group and increases as you move left through a period. Definition from textbook page 168

16. The Elements Themselves!

17. Have valence configuration of s1 or s2. The block consists of the first two columns in the table. Have similar chemical and physical properties. Referred to as the representative elements. Made up of Hydrogen, Group 1A and 2A. S Block is broken down into three main categories: Hydrogen Alkali Metals Alkaline Earth Metals S Block Elements Block in yellow!

18. Hydrogen • Abbreviation: H • Atomic Number: 1 • Atomic Weight: 1.01 • State of Matter: Gas • Uses: • Manufacture of ammonia • Hydrogenation of vegetable oils • Rocket fuels

19. Consists of six elements: Lithium~ Li Sodium~ Na Potassium~ K Rubidium~ Rb Cesium~ Cs Francium~ Fr Composed of Group 1A. Elements react with water to form alkaline solutions. Easily lose a valence electron and form ion with +1 charge. Very soft. Highly reactive. Naturally found combined with other elements. Good conductors of heat and electricity. Alkali Metals

20. Lithium • Abbreviation: Li • Atomic Number: 3 • Atomic Weight: 6.94 • State of Matter: Solid • Uses: • Batteries • Dehumidifiers • When combined, used as a bipolar treatment drug. • Airplane parts

21. Sodium • Abbreviation: Na • Atomic Number: 11 • Atomic Weight: 22.99 • State of Matter: Solid • Uses: • Table salt

22. Potassium • Abbreviation: K • Atomic Number: 19 • Atomic Weight: 39.09 • State of Matter: Solid • Uses: • Fertilizers • In large fireworks. • Bananas

23. Rubidium • Abbreviation: Rb • Atomic Number: 37 • Atomic Weight: 85.47 • State of Matter: Solid • Uses: • Vacuum systems • TV and cathode-ray tubes

24. Cesium • Abbreviation: Cs • Atomic Number: 55 • Atomic Weight: 132.91 • State of Matter: Solid • Uses: • Vacuum systems • Apparatus of emergency workers • Atomic clocks

25. Francium • Abbreviation: Fr • Atomic Number: 87 • Atomic Weight: 223 • State of Matter: Solid • Uses: • No known use

26. Consists of five elements: Beryllium ~ Be Magnesium ~ Mg Calcium ~ Ca Strontium ~ Sr Barium ~ Ba Radium ~ Ra Shiny and hard. Naturally found in Earth’s crust. Lose two electrons to form +2 ions. When exposed to oxygen, form a thin oxide coating. Don’t dissolve easily in water. Alkaline Earth Metals

27. Beryllium • Abbreviation: Be • Atomic Number: 4 • Atomic Weight: 9.01 • State of Matter: Solid • Uses: • Tools • Petroleum refineries • Alloy • Window for x-ray tubes

28. Magnesium • Abbreviation: Mg • Atomic Number: 12 • Atomic Weight: 24.31 • State of Matter: Solid • Uses: • Backpack frames • Bicycle frames • “Mag” wheels on sports cars. • Line furnaces. • Human muscle functions and metabolism. • Hard water

29. Calcium • Abbreviation: Ca • Atomic Number: 20 • Atomic Weight: 40.08 • State of Matter: Solid • Uses: • Antacid tablets • Abrasive in toothpaste • Maintains strong human teeth and bones. (Milk, Fish) • Steel • Paper • Glass • Mortar Only when calcium carbonate decomposes and forms oxide of calcium.

30. Strontium • Abbreviation: Sr • Atomic Number: 38 • Atomic Weight: 87.62 • State of Matter: Solid • Uses: • Crimson color in fireworks. • Medical research

31. Barium • Abbreviation: Ba • Atomic Number: 56 • Atomic Weight: 137.33 • State of Matter: Solid • Uses: • Paints • Glasses • Radiology • Photography paper • Vacuum system

32. Radium • Abbreviation: Ra • Atomic Number: 88 • Atomic Weight: 226.02 • State of Matter: Solid • Uses: • Cancer therapy

33. Made up of groups 3A – 8A. Valence configuration of p1, p2, p3, p4, p5, or p6. Metals, metalloids, and nonmetals. Solids and gases. P Block Elements Block in pink-red! • Broken down into six categories: • Boron Group • Carbon Group • Nitrogen Group • Oxygen Group • Halogens • Noble Gases

34. Consists of: Boron~ B Aluminum~ Al Gallium~ Ga Indium~ In Thallium~ Tl Naturally found combined with other elements. Some found in earth’s crust. Lose three valence electrons to form +3 ions. Boron Group

35. Boron • Abbreviation: B • Atomic Number: 5 • Atomic Weight: 10.81 • State of Matter: Solid • Uses: • Transistors in high- tech industry • Nuclear reactors

36. Aluminum • Abbreviation: Al • Atomic Number: 13 • Atomic Weight: 26.98 • State of Matter: Solid • Uses: • High-voltage transmission lines • Various reflectors • Airplane wings • Alloys • Foil • Pots/pans

37. Gallium • Abbreviation: Ga • Atomic Number: 31 • Atomic Weight: 69.72 • State of Matter: Liquid • Uses: • Laser diodes • Supercomputers • Neutrino detectors

38. Indium • Abbreviation: In • Atomic Number: 49 • Atomic Weight: 114.82 • State of Matter: Solid • Uses: • Alloys with other elements • Nuclear reactors • Solders

39. Thallium • Abbreviation: Tl • Atomic Number: 81 • Atomic Weight: 204.37 • State of Matter: Solid • Uses: • Treat skin disorders • Photoelectric cells and infrared detectors • The diagnosis of diseases

40. Consists of the following: Carbon~ C Silicon~ Si Germanium~ Ge Tin~ Sn Lead~ Pb Consists of a nonmetal, metalloids, and metals. Wide range of properties and few number of rules that apply. Is called group 4A: The Carbon Group Carbon Group

41. Carbon • Abbreviation: C • Atomic Number: 6 • Atomic Weight: 12.01 • State of Matter: Solid • Uses: • Industry for abrasive purposes • Lead pencils • For fuel in industry and the home

42. Silicon • Abbreviation: Si • Atomic Number: 14 • Atomic Weight: 28.09 • State of Matter: Solid • Uses: • Microelectronics industry • Glass • Ceramics • Solar cells • Microphones • Computer chips

43. Germanium • Abbreviation: Ge • Atomic Number: 32 • Atomic Weight: 72.59 • State of Matter: Solid • Uses: • Transistors

44. Tin • Abbreviation: Sn • Atomic Number: 50 • Atomic Weight: 118.69 • State of Matter: Solid • Uses: • Foil sheets • As alloy agent to make bronze • Solder • Electrical connections • Cans

45. Lead • Abbreviation: Pb • Atomic Number: 82 • Atomic Weight: 2047.19 • State of Matter: Solid • Uses: • Storage batteries • Solder • Television screens • Paint • Crystal glass • Pipes

46. Consists of five elements: Nitrogen~ N Phosphorus~ P Arsenic~ As Antimony~ Sb Bismuth~ Bi Each have five valence electrons. Their physical and chemical properties are different. Is group 5A. Nonmetals, metalloids, and a metal make up this category. Nitrogen Group

47. Nitrogen • Abbreviation: N • Atomic Number: 7 • Atomic Weight: 14.01 • State of Matter: Gas • Uses: • Freeze foods and biological specimens • Industry as a blanketing gas • Making ammonia

48. Phosphorus • Abbreviation: P • Atomic Number: 15 • Atomic Weight: 30.97 • State of Matter: Solid • Uses: • Fertilizers • Television tubes • Detergents

49. Arsenic • Abbreviation: As • Atomic Number: 33 • Atomic Weight: 74.92 • State of Matter: Solid • Uses: • Herbicide and insecticide • Medical products • Solid-state electronics

50. Antimony • Abbreviation: Sb • Atomic Number: 51 • Atomic Weight: 121.75 • State of Matter: Solid • Uses: • Safety matches • Alloys • Flame retardant