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Chapter 7 Ionic Covalent and Metal Materials

Chapter 7 Ionic Covalent and Metal Materials. Types of Atoms. Ionic Compounds: 1/3 page for each. Ions (Ca+ions & Anions). Covalent (Molecular Compounds):. Two or more nonmetals. Metallic Solids:. Only metal atoms. Electron Dot structures.

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Chapter 7 Ionic Covalent and Metal Materials

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  1. Chapter 7 Ionic Covalent and Metal Materials

  2. Types of Atoms Ionic Compounds:1/3 page for each Ions (Ca+ions & Anions) Covalent (Molecular Compounds): Two or more nonmetals Metallic Solids: Only metal atoms

  3. Electron Dot structures valence electrons: as dots around the atomic symbols Ne EX.

  4. Octet Rule - atoms react until contain 8 valence e- _ F Ne (Fluorine) Ions achieve electron configuration as Noble Gas Neon

  5. Halide Ions halogen, become negative gaining 1 electron. _ F Br I _ _ Fluorine Bromine Iodine Fl0urine, Iodine and Bromine are all halogens - Halide Ions.

  6. Ionic Bonds • force binds oppositely charged ions Cl Na + - Sodium (Cation) Sodium chloride Chlorine (Anion) Sodium

  7. Electrostatic Attraction

  8. B. Two types of compounds Ionic Compounds Molecular Compounds Made from IONS ca+ion & anion atoms w/ positive or negative charges. when an atom has lost or gained electrons. • Good conductors when dissolved/melted. Electrically neutral +CrystallineSolid - Na + Cl - NaCl

  9. Ionic Compounds: Bond formation Bond formation Transfer of electrons room temperature crystalline Hard & Brittle, High Melting pt Electrostatic forces Very Strong Covalent (Molecular): Sharing of electrons solid, liquid or gas. Weak soft & low melting point Free moving valence e- Metallic Solids: Higher valence # of e- , harder metal. Soft to very hard Strong

  10. Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Cl- Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ Na+ How many Na+ surround Cl-?

  11. Compound Arrangement Ionic Compound • Oppositely charged ions close packed layers. repeating 3D pattern : Unit cell Crystal

  12. H x . C . H . . x H x H x

  13. Even at this point, there was still a Polar Covalent Bond between Sara, Johnny and Bill… Stop in the name of Love, before You break my heart. Johnny didn’t like the feeling of competing with Bill but he knew if he really wanted her, he’d have to fight for her.

  14. Covalent Compound • nonmetals bonds between molecules are weak Weak forces Water molecules

  15. CRYSTALLINE GIANTS

  16. Metals: • Low to high mt. pts. can be drawn into wires • Ductile: can be hammered into different shapes • Malleable:

  17. Electron cloud e- e- Form a bond

  18. Conductors Metallic Solids: Why? • Free-moving valence electrons Good conductors of heat Why? • Free-moving valence electrons

  19. Conductors Molecular Compounds: IonicCompounds: Poor conductors in the molten state. or as electrolytes Don’t form ions Bonds break (melt) or dissociate (dissolve). Ions separate - free to move around.

  20. Network Solids Network Solid • Consist of atoms held together by large network of covalent bonds. • Each atom is covalently bonded in a largechain or network. • There are NO moleculesin a network solid, onlyatoms bonded together. • Bonds are very strong. Example: Diamond

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