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The Periodic Table: Mendeleev to Modern Trends

A journey through the development of the Periodic Table from Mendeleev to modern innovations like Bohr's proposal and the Mayan Table. Understand the organization, properties, and classifications of elements, including metals, nonmetals, and metalloids. Explore groups, periods, and families, and discover the significance of valence electrons and ion formation.

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The Periodic Table: Mendeleev to Modern Trends

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  1. Periodic Table(video – Mendeleev’s PT)

  2. The Periodic Table

  3. John Dalton’s Symbols (1808)

  4. Periodic Table proposed by Neils Bohr

  5. Mayan Periodic Table

  6. Spiral Periodic Table

  7. Stowe Periodic Table

  8. Chinese Periodic Table

  9. Periodic Table • Dmitri Mendeleev organized the elements by similar properties and it resulted in increasing atomic mass • Predicted undiscovered elements

  10. Moseley • 40 years after Mendeleev, Moseley arranged elements by atomic number

  11. (Periodic law: predictable patterns of physical and chemical properties in columns when elements are arranged in order of increasing atomic number)

  12. The majority of the elements are…? • Metals • Nonmetals • Metalloids

  13. Most Elements are Metals

  14. Blocks • Main Group Elements • Transition Metals • Inner Transition Metals

  15. Identify Family name

  16. Columns • vertical columns (18) are called groups or families • Elements in the same column have similar properties or characteristics because they have the same number of valence electrons

  17. Rows • Horizontal rows are called periods. • Elements in a period do NOT have similar properties

  18. Alkali Metals • Group I • One valence electron • Soft • highly reactive Alkali metals in water, accurate! - YouTube

  19. Alkaline earth metals • Located in Group 2 and have 2 valence electrons Alkaline and Alkaline Earth Metals - YouTube

  20. Transition metals • Located in groups 3-12 • All have 2 valence electrons Mercury - Periodic Table of Videos - YouTube

  21. Rare earth elements/ Inner transition metals • Last two rows • Known as Lanthanide and Actinide series

  22. Metalloids/Semi-conductors • Characteristics of both metals and nonmetals

  23. Nonmetals • Not able to conduct heat or electricity • Brittle, no metallic luster • Can exist in either solid (Carbon) or gas (Oxygen)

  24. Halogens • Located in group 17 and have 7 valence electrons • Highly reactive Comparing the four halogens (2/8) - YouTube

  25. Noble gases • Located in group 18, have 8 valence electrons so they are stable • Gases at room temperature • Nonreactive Noble Gases - YouTube

  26. Ions Atoms are neutral (protons and electrons are equal) Ions – have a charge – different number of electrons • Octet – 8 valence electrons – Full outer shell. • elements will bond in order to complete octet.

  27. Losing electrons * positive * cation * 3 or less valence electrons * metals

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