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Chemical Bonds: Ionic, Covalent, and Metallic Bonding Explained

Learn about the different types of chemical bonds - ionic, covalent, and metallic - and how atoms are attracted to each other to form stable molecules. Discover the importance of valence electrons and the octet rule in bonding. Understand the characteristics and properties of compounds formed by these bonds.

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Chemical Bonds: Ionic, Covalent, and Metallic Bonding Explained

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  1. Chemical Bonds

  2. s Chemical Bond 8 Bonding, the way atoms are attracted to each other to form molecules, determines nearly all of the chemical properties we see. And, as we know, the number “8” is very important to chemical bonding. I want you to meet a friend of mine?

  3. Pure Substances- COMPOUNDS • What is a compound? • 2 or more elements chemically bound together BONDS

  4. We will Cover 3 Types of Chemical Bonds • Ionic • Covalent • Metallic

  5. Why Bonds Form

  6. BONDSBonds form between elements to become stable atoms…. It’s all about the valence electrons baby!

  7. OCTET RULE –Special # 8!!!! • Which group has 8 valence electrons? • What is that group called? • How do they act?

  8. OCTET RULE –Special # 8!!!! • Elements want to be like the Noble Gases STABLE… • Elements need full valence shells to feel happy (STABLE) • they want 8 (like the noble gases) • Atoms will Get as close to 8 valence e- as possible by forming bonds

  9. How do they do it? How do they get those valence shells full? Making bonds with other elements…

  10. IONIC BONDbond formed between cation(+) and anion(-) Electrons: transferred from one element to anotherLet’s see how it happens….http://www.youtube.com/watch?v=lODqdhxDtHM

  11. Ionic Compounds Compounds formed by Ionic Bonds-attraction between opposite charges • Alwayshave at least 1 metal • Neutral charge + equal - • Very Strong Bonds • High Melting Point • They Conduct Electricity Why do you think they do this??

  12. Ionic Bonds (Compounds) Elements try to get 8e- in their valence shell METALS will give up electrons and become cations(+) Most NON-METALS take/gain electrons Become anions(-)

  13. Polyatomic Ions • A compound (group of atoms) with a charge- this ion sticks together and can bond with other ions • Ex: CO3 has -2 charge • Ex: NH4 has a +1 charge Polyatomic = Poly (many) Atomic (atoms)

  14. Now, on your periodic table you are going to write the Charge (oxidation) Numbers above the Groups – what ion they normally form We call the charge number the Oxidation Number………..

  15. Oxidation Number-tells you what charge the element has when it becomes an ion

  16. Ionic Bond Rules Your compound must be neutral (balanced) • Make 5 different compounds (ionic bonds) • Cation always goes first, Anion goes after • Polyatomic ions carry 1 charge for the group • Your compounds may only contain 1 type of positive ion and 1 type of negative • See example sheet • Show me what you have made, then draw these on your sheet

  17. Chemical Bonds

  18. COVALENT BONDBond between non metals/metalloidsbond formed by the sharing of electrons

  19. Covalent Bonds

  20. Covalent Compounds Compounds formed by SHARING ELECTRONS • Non-metals and/or metalloids only • Weaker Bonds • Low Melting Point • Do not Conduct Electricity Why do you think they don’t conduct?

  21. Bonding and the elements in GROUP 14 ….. • Elements with 4 valence electrons only SHARE their valence electrons.

  22. CoF H2O NaCl Ionic or Covalent? • MgBr2 • SiO4 • CO2

  23. METALLIC BONDbond betweenmetals

  24. Metallic Bond • Formed between atoms of metallic elements • Good conductors at all states, lustrous, very high melting points • Examples; Na, Fe, Al, Au, Co

  25. In Summary • Atoms bond to become stable (they lose, gain or share electrons)

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