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Chemical Bonding in Molecules

Explore the fundamentals of ionic and covalent bonding, the structure of matter, and the types of molecules. Learn about Lewis Dot Structures, metallic bonds, and polyatomic ions.

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Chemical Bonding in Molecules

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Presentation Transcript

  1. Chapter 5-2 Warm - Up • 1. What is a compound? • 2. What is the difference between bond length and bond angle? • 3. What are the 3 different types of models that represent molecules? • 4. ________ are intermolecular attractions that occur between water molecules.

  2. Chapter 5-2The Structure of Matter Ionic and Covalent Bonding

  3. Bonding • Bonded atoms usually have a stable electron configuration • Valence electrons interact • Structure similar to noble gases

  4. Bonds • Bonds can be stretched without breaking • Flexible rubber bands

  5. Ionic Bonds • Ionic Bond – formed by attraction between oppositely charged ions • Metal Elements – positive • Nonmetal Elements – negative • Network structure

  6. Ionic Bonds • Formed by the transfer of electrons • Instead of sharing outer most electrons they are transferred • Na+ ion and Cl- ion

  7. Ionic Compounds • Ionic compounds are in the form of networks, not molecules • Na+ and Cl- form to make NaCl • 1:1 Ratio for a zero charge • Ca2+ and F- form to make CaF2 • 1:2 Ratio for a zero charge

  8. Ionic Compounds • When melted or dissolved in water ionic compounds conduct electricity • Electric current – moving charges

  9. Metallic Bonds • Metallic Bond – formed by the attraction between positively charged metal ions and the electrons around them

  10. Metallic Bond • Atoms in metals • Atom’s nucleus and neighboring electrons packed tightly together • Electrons overlap and move freely • Conduct electricity

  11. Covalent Bond • Covalent Bond – formed when atoms share one or more pairs of electrons • Compounds made of molecules • Low boiling point • Water and sugar • Nonmetals

  12. Covalent Bond • Most of the molecules remain intact and do not conduct electricity • No charge

  13. Lewis Dot Structure

  14. A line shows atoms share 2 electrons

  15. Triple Covalent Bond

  16. Polyatomic Ions • Polyatomic Ion – an ion made of 2 or more atoms • Both ionic and covalent bonds

  17. Parentheses Group Polyatomic Ions • Ammonium Sulfate is written as: • (NH4)2SO4 • Act like a single ion • 2 ammonia ions • Carbonate ion: • CO32- • 2- charge

  18. Made of Oxygen • -ite • One less oxygen atom • -ate • One more oxygen atom • The charge of each ion pair is the same.

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