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The Periodic Table

The Periodic Table. Chemistry I: Matter and Change. BellRinger 9/6/11. How is the periodic table arranged? What is a Metalloid? Elements are classified as metals,____________, and ________________. The Periodic Table. LOTS on INFORMATION!!! Columns = Groups = Families = up and down,

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The Periodic Table

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  1. The Periodic Table Chemistry I: Matter and Change

  2. BellRinger 9/6/11 • How is the periodic table arranged? • What is a Metalloid? • Elements are classified as metals,____________, and ________________.

  3. The Periodic Table • LOTS on INFORMATION!!! • Columns = Groups = Families = up and down, • # 1-18 • Main groups : 1, 2, 13-18 • Transition metals: 3-10 • Inner Transition metals: at bottom of chart • Members of the same group have similar physical and chemical properties • Rows = “Periods”

  4. Main groups Transition metals Inner transition metals

  5. Periodic Table • Period: elements in the row • The number of elements per period varies because the number of available orbitals increases from energy level to energy level

  6. Periodic Table • Groups: Each column on the periodic table • Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements in groups

  7. Periodic Table • An element’s electron configuration determines its chemical properties.

  8. Metals • Groups 1,2,3-10, some in 14 and 15 (blue) • Malleable (Can be pressed into different shapes without breaking) • Ductile (Can be drawn into thin wires) • Conductive (Conduct electric current and heat)

  9. Metals

  10. Metalloids • Elements on “step” between metals and non-metals • Form compounds with distinctive colors • Intermediate properties • (semi-conductors)

  11. Metalloids

  12. Non-metals • Rest of chart (yellow) • Nonconductive • usually form anions

  13. Non-metals • Rest of chart (yellow) • Poor conductors of heat and electricity • Many are gas at room temperature • Low Boiling Points • If solid they are brittle • usually form anions (negative ions)

  14. Valence Electrons • Valence Electrons: is an electron that is in the highest occupied energy level • These electrons play a key role in chemical reactions • Elements in a group have similar properties because they have the same number of electrons

  15. Group 1- alkali metals • Very soft • not found in nature in uncharged atom form (find as cation) • VERY reactive with nonmetals and water

  16. Group 2- alkali earth metals • Harder, more dense vs. group 1 • Less reactive than group 1 • All react with oxygen to form metal oxides

  17. Group 17- Halogens • “salt-producing” • React with metals to form salts • Exist as diatomic molecules in nature (F2, Cl2, etc.)

  18. Group 18- Noble Gases • Colorless gases • Exist as single atoms • Very Unreactive • Some limited reactivity of Xe, Kr, Rn

  19. What is it about elements that explain the reactivity and other properties? • -arranged by atomic # (# protons), for UNCHARGED elements (#p = #e-) • So as #P increases, #e- increases • Thus– reactivity based on ARRANGEMENT OF ELECTRONS around the nucleus

  20. Electron Organization • Look at how electrons are positioned around the nucleus • Not in any one place, but fill different regions of space around the nucleus

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