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Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
Metals, Non Metals And Oxidation
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Metals, Non Metals And Oxidation

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  • 1. Periodic Table Metals, Non-Metals, Groups and Periods
  • 2. Metals • Metals are located left of the black line on the periodic table. • Metals become cations, they lose electrons. Positive charge. • Metals are maleable and ductile and they are also conductors of heat and electricity.
  • 3. Non-Metals • Located right of the black line on the periodic table. • Non-Metals gain electrons and become negatively charged. • Not conductors, brittle (if solid), not ductile.
  • 4. Metaloids • Located along the line on the periodic table. • Share properties of metals and non- metals. • Typically used in electronics.
  • 5. Groups • Group IA has a +1 charge, lose 1 electron. Also known as the Alkali Metals. • Soft and white and highly reactive. • Group IIA has a +2 charge, lose 2 electrons. Also known as the Alkaline Earth Metals. React easily with the halogens to form salts.
  • 6. More Groups • Group VIIA has a -1 charge. They gain one electron. This group is known as the halogens. Highly reactive, fluorine is one of the most reactive elements in existence. • Group VIIIA are known as the Noble Gases. Full valence electron shell. Non- reactive. Important for use in welding, lighting, and space exploration.
  • 7. Oxidation-Reduction • Oxidation is the losing of an electron in a reaction. Original meaning was combining with oxygen. • Reduction is the gaining of an electron in a reaction. Original meaning was removing oxygen. • LEO says GER or OIL RIG
  • 8. Examples of Oxidation
  • 9. Examples of Oxidation
  • 10. Reduction
  • 11. Oxidation Characteristics • Complete loss of electrons • Shift of electrons away from an atom • Gain of oxygen • Increase in oxidation number
  • 12. Characteristics of Reduction • Complete gain of electrons • Shift of electrons toward an atom • Loss of oxygen • Decrease in oxidation number
  • 13. Rules for Assigning Oxidation #’s • 1. Oxidation number of a monatomic ion is equal to its charge. Ex: Br1- is -1 and Fe3+ is +3. • 2. Oxidation number of hydrogen in a compound is +1, except in metal hydrides like NaH then it is +1. • Oxidation number of oxygen in compounds is -2.
  • 14. continuted • 4. The oxidation number of an atom in an uncombined elemental form is 0. • 5. For any neutral compound the sum of the oxidation numbers must equal zero. • For a polyatomic ion, the sum of the oxidation numbers must equal the ionic charge of the ion.

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