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Ionic, Covalent and Metallic Bonding

Ionic, Covalent and Metallic Bonding. Monroe December 32, 2007. Chlorine is a non-metal, and it has seven electrons in it’s outer shell, needing one more to fill it will the maximum of eight. Cl.

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Ionic, Covalent and Metallic Bonding

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  1. Ionic, Covalent and Metallic Bonding Monroe December 32, 2007

  2. Chlorine is a non-metal, and it has seven electrons in it’s outer shell, needing one more to fill it will the maximum of eight. Cl

  3. Potassium is a metal, and it will want to lose one electron, in order to have a filled outer shell of eight. It is easier to lose one, than gain seven. K

  4. Metal Atom Nonmetal Atom K Cl Before Potassium “steals” one electron, they both are neutrally charged, with equal numbers of protons and electrons.

  5. Metal Ion (+1) Nonmetal Ion (-1) K Cl After Potassium “steals” one electron, they both are electrically charged, with unequal numbers of protons and electrons. They are now attracted to each other.

  6. Ionic Unit K Cl Metal Ion (+1) Nonmetal Ion (-1) Electrons are “captured”, so it will not conduct electricity. The bonds are very strong, so the melting point is very high, and this is a crystalline structure, so it will break, and not bend.

  7. Nonmetal Atom Nonmetal Atom Nonmetal Atom H H O

  8. H H O Hydrogen and Oxygen are both acting as nonmetals. Neither one has the ability to steal an electron from the other. In true democratic and American fashion, they decide to share one of the valence electrons, and they call it a “co-valence” electron.

  9. Molecule H H O There are now two electrons in each of the Hydrogen’s orbits, filling outer shell.

  10. Molecule H H O Electrons are used cooperatively (and not free to move), so it will not conduct electricity. The bonds are not very strong, so the melting point is not very high, and this is a crystalline structure, so it will break, and not bend.

  11. Metallic Bonding (metal to metal) e- e- e- e- e- e- e- e- e- Fe e- Fe Fe Fe Fe e- Fe e- e- Fe e- Fe e- Fe e- e- e- e- e- Fe e- Fe e- e- e- e- e- Fe Fe e- Fe e- Fe Fe Fe Fe e- e- e- e- e- e- e- e- e- e- e- In this type of bonding, there is an ocean, or “sea” of electrons and atoms. Everything is just kind of floating around. Every once in a while, an atom will have too many, or too few electrons, causing short term electromagnetic bonds.

  12. e- Metallic Bonding (metal to metal) e- Fe Fe e- e- e- e- Fe Fe e- e- e- e- Fe e- e- e- e- e- Fe Fe e- e- Fe Fe Fe e- e- e- Fe e- e- e- e- e- e- Fe e- e- Fe e- Fe In this type of bonding, there is not a rigid crystalline structure, so it a malleable, or bendable. e- Fe e- Fe e- e- e- Fe e- e- e- Fe e- e-

  13. Metallic Bonding (metal to metal) e- e- e- e- e- e- e- e- e- Fe e- Fe Fe Fe Fe e- Fe e- e- Fe e- Fe e- Fe e- e- e- e- e- Fe e- Fe e- e- e- e- e- Fe Fe e- Fe e- Fe Fe Fe Fe e- e- e- e- e- e- e- e- e- e- e- In this type of bonding, electrons can easily move from atom to atom, hence; it will conduct electricity. e-

  14. Melting Temperature Electrical Conductivity Smallest Unit Bonding Type Example (from periodic table) Ionic Bonding Covalent Bonding Metallic Bonding http://ithacasciencezone.com/chemzone/lessons/03bonding/mleebonding/default.htm

  15. Melting Temperature Electrical Conductivity Smallest Unit Bonding Type Example (from periodic table) Formula Unit Ionic Bonding High None Ionic Salt None Sugar Covalent Bonding Low Molecule Covalent Metallic “Electron Sea” Metallic Bonding Low/High High Atom Iron http://ithacasciencezone.com/chemzone/lessons/03bonding/mleebonding/default.htm

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