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The Periodic Table of The Elements

The Periodic Table of The Elements. The Periodic Table. Arrangement of the known elements based on atomic number and chemical and physical properties. Divided into three basic categories: Metals Nonmetals Metalloids. Basic Organization. The periodic table is organized by:

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The Periodic Table of The Elements

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  1. The Periodic Table of The Elements

  2. The Periodic Table • Arrangement of the known elements based on atomic number and chemical and physical properties. • Divided into three basic categories: • Metals • Nonmetals • Metalloids

  3. Basic Organization The periodic table is organized by: • Atomic structure • Atomic number • Chemical and Physical Properties

  4. Uses of The Periodic Table The periodic table is useful in predicting: • chemical behavior of the elements • trends • properties of the elements

  5. Atomic Structure Review • Atoms are made of protons, electrons, and neutrons. • Elements are atoms of only one type. • Elements are identified by the atomic number (# of protons in nucleus).

  6. Energy Levels Review • Electrons are arranged in a region around the nucleus called an electron cloud. Energy levels are located within the cloud. • At least 1 energy level and as many as 7 energy levels exist in atoms.

  7. Energy Levels Review • Electrons in levels farther away from the nucleus have more energy. • Inner levels will fill first before outer levels.

  8. Energy Levels & Valence Electrons • Energy levels hold a specific amount of electrons: • 1st level = up to 2 • 2nd level = up to 8 • 3rd level = up to 8 (first 18 elements only)

  9. Energy Levels & Valence Electrons • The electrons in the outermost level are called valence electrons. • Determine reactivity - how elements will react with others to form compounds • Outermost level does not usually fill completely with electrons

  10. Due Today • Two column notes save as a PDF • Video watched with comment • Due Tomorrow • Interpreting the Periodic Table • Warm Up Log • Current Event

  11. Elements & Reactivity • Reactivity is a chemical property that determines how elements will react with others to form compounds.

  12. Elements & Reactivity • What makes an element reactive? • Number of valence electrons each atom has • When outer levels are full, atoms are stable. • When they are not full, they react: • gain, lose, or share 1 or 2 electrons.

  13. Elements & Reactivity • The most reactive metals are the elements in Groups 1 and 2. • Elements in Group 1 need seven more electrons to fill their outer level. • Elements in Group 2 need six more electrons to fill their outer level. • These groups are known as the “givers” because they easily give up their valence electrons to make a compound. Video http://www.youtube.com/watch?v=xxi6kUbvo94

  14. Elements & Reactivity • The most reactive nonmetals are the elements in Groups 16 and 17. • Elements in Group 16 only need two more electrons to fill their outer level. • Elements in Group 17 only need one more electron to fill their outer level. • These groups are known as the “takers” because they easily receive valence electrons to make a compound. Fluorite

  15. Using the Table to Identify Valence Electrons • Elements are grouped into vertical columns because they have similar properties. • These are called groups or families. • Groups are numbered 1-18.

  16. Using the Table to Identify Valence Electrons • Group numbers can help you determine the number of valence electrons: • Group 1 has 1 valence electron. • Group 2 has 2 valence electrons. • Groups 3–12 are transition metals and have 1 or 2 valence electrons.

  17. Using the Table to Identify Valence Electrons cont. • Groups 13–18 have 10 fewer than the group number. For example: • Group 13 has 3 valence electrons. • Group 15 has 5 valence electrons. • Group 18 has 8 valence electrons. Switch to Mimio

  18. Group 1: Alkali Metals • Contains: Metals • Valence Electrons: 1 • Reactivity: Very Reactive • Properties: • solids • soft • react violently with water • shiny • low density Sodium

  19. Group 2: Alkaline-Earth Metals • Contains: Metals • Valence Electrons: 2 • Reactivity: very reactive, but less reactive than alkali metals (Group 1) • Properties: • Solids • Silver colored • More dense than alkali metals Magnesium

  20. Groups 3-12 Transition Metals • Contain: Metals • Valence electrons: 1 or 2 • Reactivity: less reactive than alkali and alkaline-earth metals • Properties: • Higher density • Good conductors of heat and electricity Copper

  21. Groups 3-12 Transition MetalsBelow Main Table • Contain: The Lanthanide and Actinide Series • These two rows are pulled out of sequence and placed below the main table to keep the table from being too wide. • Lanthanides are #’s 58–71. • Actinides are #’s 90–103. Plutonium

  22. Groups 3-12 Rare Earth Elements ~ Lanthanides • Lanthanides follow the transition metal # 57 Lanthanum in Period 6. • Valence electrons: 3 • Reactivity: Very reactive • Properties: • High luster, but tarnish easily • High conductivity for electricity • Very small differences between them Cerium

  23. Groups 3-12 Rare Earth Elements ~ Actinides • Actinides follow the transition metal # 89 Actinium in Period 7 • Valence electrons: 3 (but up to 6) • Reactivity: unstable • All are radioactive • Most made in laboratories Uranium

  24. Metalloids • A zig-zag line that separates metals from metalloids • Elements from Groups 13–17 contain some metalloids. • These elements have characteristics of metals and nonmetals.

  25. Group 13: Boron Group • Group 13: Boron Group • Contains: 1 metalloid and 4 metals • Valence Electrons: 3 • Reactivity: Reactive • Other shared properties: • Solid at room temperature Boron

  26. Group 14: Carbon Group • Contains: 1 non-metal, 2 metalloids, and 3 metals • Valence Electrons: 4 • Reactivity: Varies • Other shared properties: • Solid at room temperature Carbon

  27. Group 15: Nitrogen Group • Contains: 2 non-metals, 2 metalloids, and 1 metal • Valence electrons: 5 • Reactivity: Varies • Other shared properties: • All but N are solid at room temperature Nitrogen

  28. Group 16: Oxygen Group • Contains: 3 non-metals, 1 metalloid, and 2 metals • Valence Electrons: 6 • Reactivity: Reactive • Other shared properties: • All but O are solid at room temperature. Oxygen

  29. Groups 17 : Halogens • Contain: Nonmetals • Valence Electrons: 7 • Reactivity: Very reactive • Other shared properties • Poor conductors of electric current • React violently with alkali metals to form salts • Never found uncombined in nature Chlorine Gas

  30. Group 18 Noble Gases • Contains: Nonmetals • Valence Electrons: 8 (2 for He) • Reactivity: Unreactive (least reactive group) • Other shared properties: • Colorless, odorless gases at room temperature • Outermost energy level full • All found in atmosphere Neon

  31. Hydrogen Stands Apart • H is set apart because its properties do not match any single group. • Valence electrons: 1 • Reactivity: very, but loses the 1 electron easily • Properties: • Similar to those of non-metals rather than metals Hydrogen in it’s Plasma state

  32. Warm Up • WAIT TO TURN THIS IN!!!!!!!!!!!!!!!!

  33. Due Today • Due Today • Two column notes save as a PDF • Warm Up Log saved as a PDF • Current Event • Video watched with comment • Interpreting the Periodic Table

  34. Periods • Periods run horizontally across the Periodic Table • Periods are numbered 1–7 • All the elements in a period will have the same number of energy levels, which contain electrons. Examples: • Period 1 atoms have 1 energy level. • Period 2 atoms have 2 energy levels. • Period 5 atoms have 5 energy levels. Mimio

  35. Periods Continued • Moving from left to right across a period, each element has one more electron in the outer shell of its atom than the element before it. • This leads to a fairly regular pattern of change in the chemical behavior of the elements across a period. Mimio

  36. Quiz Quiz Trade

  37. Brief History of the Periodic Table

  38. Brief history of the periodic Table

  39. Ancient Greece • In Ancient Greece, people believed that there were only four elements….. • Earth • Fire • Water • Air

  40. What were scientist looking for when they found the first element • Alchemists • They were looking for the philosopher’s stone, which reputedly could change base metals into gold

  41. Hennig Brand • 1649 • Made the first scientific discovery of an element • Phosphorus • He isolated from urine, a white, waxy material and named it phosphorus (“light bearer”), because it glowed in the dark.

  42. A.E. Beguyer de Chancourtois • 1817 • Listed elements on a cylinder in order of increasing atomic mass

  43. Johann Dobereiner • 1862 • Proposed there were triads of three elements in nature with the mass of the middle element being the average of the other two • Law of Triads • Found that the properties of bromine seem halfway between those of chlorine and iodine. He showed that in each triad the mean of the lightest and heaviest atomic weights approximated the atomic weight of the middle element. • In other words…. 4………6.......8

  44. John Newlands • 1863 • Classified the 56 known elements into a table with 11 groups based on properties. He proposed that any element will behave similar to the 8th element following it. • Law of Octaves

  45. Lothar Meyer • 1864, German • Developed a shortened version of the table only showing half of the known elements. • Elements were listed in order of atomic mass and differences in behavior were due to mass. • He published a longer version in 1869 but it wasn’t published until 1870

  46. Dmitri Ivanovich Mendeleev • 1869, Russian • Rearranged elements in order of their properties. • He showed a vertical, horizontal and diagonal relationship between the 63 known elements • Predicted three yet-to-be-discovered elements including eke-silicon and eke-boron

  47. Lord Rayleigh • 1895 • Discovered argon and found it didn’t fit in the current groups. • In 1898 he proposed a new group to be called zero group because argon was unreactive (inert)

  48. Ernest Rutherford • 1911 • Studied nuclei which led to the concept of nuclear charge • Positive Charge and Protons

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