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Understanding the Periodic Table: GROUPS

Understanding the Periodic Table: GROUPS. Look at your periodic table. Write 10 observations on your paper. What are the 3 main groups we’ve learned about so far?. Metals 1. Ductile : conduct electricity very well. 2. Malleable : hammered, bent without breaking. 3. Shiny Examples :

JasminFlorian
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Understanding the Periodic Table: GROUPS

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  1. Understanding the Periodic Table:GROUPS

  2. Look at your periodic table Write 10 observations on your paper. What are the 3 main groups we’ve learned about so far?

  3. Metals 1. Ductile: conduct electricity very well. 2. Malleable: hammered, bent without breaking. 3. Shiny • Examples: Silver (Ag) Gold (Au) Copper (Cu) Aluminum (Al)

  4. Nonmetals 1. Dull: not shiny 2. Brittle: breaks easily 3. Poor conductors of electricity and heat. • Examples: Hydrogen (H) Sulfur (S) Chlorine (Cl) Helium (He)

  5. Semimetals or Metalloids • Have properties of both metals and nonmetals. • Only conduct electricity under certain conditions. • Examples: Silicon (Si) Boron (B)

  6. Metals, Nonmetals, and Semi-metals on the Periodic Table semi-metals nonmetals metals Color the metals, non-metals and semi-metals VERY LIGHTLY.There’s more……….

  7. B A Also called Families 18 Columns 8 Columns labeled A (colors) 10 Columns labeled B (gray) Each group has unique properties Elements in the same group have similar properties.

  8. Group 1A – Alkali Metals silvery white metal(except cesium, which is liquid golden) Highly reactive. Examples: Sodium (Na) Potassium (K) Cesium (Cs)

  9. Group 1A – Alkali Metals Bohr Diagram Lewis Dot Diagram H Li Na K 1 electron in each outer shell. Energy levels increase by the period

  10. Group 2A – Alkaline Earth Metals Malleable and ductile metals. Very reactive. Examples: Magnesium Calcium (Ca) Radium (Ra)

  11. Group 2A – Alkaline Earth Metals Be: Mg: Ca: 2 3 4 2 electrons in outer shell Energy levels increase by the period

  12. Groups 1B-8B: Transition Metals Brightly colored, ductile metals. Less reactive. Different columns –different numbers of electrons in outer shell. Examples: Chromium (Cr) Nickel (Ni) Gold (Au) Copper

  13. Semimetals: Groups 3A-6A (along the zig zag line) Properties of both metals and non-metals Some are semi-conductors Group number indicates how many electrons in the outer shell. Examples: Boron (B) Silicon (Si) Germanium (Ge) Antimony (Sb)

  14. B Si Ge Sb Semimetals: Groups 3A-6A (along the zig zag line) Boron (B) Silicon (Si) Germanium (Ge) Astatine (As) Antimony (Sb)… Group number indicates the number of electrons in the outer shell. As Group 3 Group 4 Group 4 Group 5 Group 5

  15. Group 7A: Halogens Nonmetals Brittle, dull, poor conductors of electricity. Very reactive ionsForm salts with Group 1 elements 7 electrons in the outer shell. Examples: Chlorine (Cl) Fluorine (F) Bromine (Br) Iodine (I)

  16. F Cl Br Group 7A: Halogens 7 electrons in the outer shell. As you look down the group the number of energy levels increases.

  17. Group 8A: Inert Gases Also called Noble gases Inert means inactive 8 electrons in the outer shell, which makes them non-reactive Examples:

  18. He Ne Ar Kr Group 8A: Inert Gases Bohr Lewis full outer shell, which makes them non-reactive He only has the possibility of 2 electrons in outer energy level. All the others have 8. Each next period brings another energy level.

  19. Lanthanide, Actinide, TransUranium Lanthanide also called Rare Earth Metals Actinide and Transuranium are radioactive All part of IIIB group Examples: Cesium Uranium Plutonium

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