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Chemical Bonding Ionic and Metallic

Learn about chemical bonding in elements, including diatomic molecules and compounds, the octet rule, ionic bonding, and metallic bonding. Discover how atoms form strong attractions to achieve stability in compounds.

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Chemical Bonding Ionic and Metallic

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  1. Chemical BondingIonic and Metallic Chemistry

  2. Elements • Some elements never exist by themselves • These are called diatomic molecules • There are seven of them and they make a seven on the periodic table

  3. The Diatomic Molecules • These would still be said by their elemental name but would be written with a subscript of 2 • H2 • N2 • F2 • O2 • I2 • Cl2 • Br2 • BrINClHOF

  4. Compounds • Most elements are not found separately but combined in a compound with something else • Chemical bonds are strong attractions between atoms or ions in a compound • The reason for this is the octet rule We want 8…eight is great!

  5. Octet Rule • Noble gases are what all elements aspire to be like electronically • These elements have 8 electrons in highest energy level

  6. Na Cl Ionic Bond DEFINITION: • Chemical bond formed by the electrostatic attraction between a cation and an anion. • Atoms will either give up or take electrons in order to have eight in their highest energy level

  7. Na Cl Hey, can you help me out and gimme an electron?

  8. Na Cl Why certainly, I have one I don’t want anyway.

  9. Na Cl Give up/take away electrons

  10. Charges • Sodium now has a +1 charge since it has lost an electron • Chlorine now has a -1 charge since it gained an electron - + Na Cl

  11. Ionic Compound • The combination of Na+ and Cl- form the compound NaCl • An ionic compound will always consist of: • A metal ion (called a CATION, the + one) • A non-metal ion (called an ANION, the - one) • CATION ALWAYS COMES BEFORE THE ANION; both in the name and the formula

  12. CATION vs ANION • Positively charged ions • Lose electrons • Smaller than the parent atom • Usually metals (left side of the table) • Negatively charged ions • Gain electrons • Larger than the parent atom • Usually nonmetals (right side of table)

  13. Properties of Ionic Bonds • High melting point • Conducts electricity • Soluble in water

  14. Lewis Dot Diagrams • Diagram that shows the valence electrons • Shows ions or compounds or atoms

  15. Metallic Bonds • DEFINITION: Attraction of free floating valence electrons for the positively charged metal cations. “Sea of electrons”

  16. Properties of Metallic Bonds • Malleable/Ductile • Conduct electricity and heat • Solid at room temp and shiny luster

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