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Ionic Bonds and Ionic Compounds

Ionic Bonds and Ionic Compounds. Properties of Ionic Compounds. Solids at room temperature Atoms arranged in a 3D pattern High melting points Conduct an electric current when melted or dissolved in water. Fluorite CaF2. Pyrite FeS2. Review.

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Ionic Bonds and Ionic Compounds

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  1. Ionic Bonds and Ionic Compounds

  2. Properties of Ionic Compounds • Solids at room temperature • Atoms arranged in a 3D pattern • High melting points • Conduct an electric current when melted or dissolved in water Fluorite CaF2 Pyrite FeS2

  3. Review • Compound: two or more elements chemically combined in a fixed ratio

  4. Formation of Ionic Compounds • Composed of (non-metal) anions and (metal) cations • Example: Sodium Chloride

  5. Formation Continued • Electrically neutral Metal gives their electrons to the non-metal creating an ionic bond

  6. So What’s Happening? Na Cl +1 +1 Na Cl Cation Anion Opposites Attract

  7. Ionic Bonds • Want 8 valence/full outer shell • Example: Sodium Chloride • Sodium: 1s22s2sp63s1  Na • Chlorine: 1s22s22p63s23p5  Cl

  8. Practice: Hydrogen and Bromine

  9. Practice: Potassium and Iodine

  10. Practice: Magnesium and Oxygen

  11. Practice: Hydrogen and Oxygen (you may need more than one of each type of atom)

  12. Practice: Hydrogen and Carbon (you may need more than one of each type of atom)

  13. Practice: Potassium and Nitrogen (you may need more than one of each type of atom)

  14. Practice: Calcium and Sulfur (you may need more than one of each type of atom)

  15. One of the following pairs will form an ionic bond, one won’t. Draw out the one that will form the bond and describe why the other pair won’t bond. Lithium and Magnesium Zinc and Oxygen

  16. Chemical Formula • A written representation of a substance using symbols for its elements • Subscripts • Show how many of each TYPE of atom are in the compound • Example: Water H2O

  17. Naming and Writing Formulas For Ionic Compounds

  18. Binary Compound • Composed of two elements • Can be ionic or molecular

  19. Cinnabar HgS Chemical Formula forIonic Compounds • Formula Units • Lowest whole-number ratio of the ions in a compound • Example: • Sodium Chloride NaCl

  20. Magnesium Chloride

  21. Calcium Nitride

  22. Naming Ionic Compounds • Cation FIRST • Keeps name of element • Anion SECOND • Add an –ide ending • Number of each element DOES NOT MATTER • Example: NaCl MgCl2 Sodium Chloride Magnesium Chloride

  23. Hand out Common Ion List

  24. What’s Going On?! Copper (i) Oxide Copper (ii) Oxide

  25. Is it Cu+1 or Cu+2? CuS Cu2S

  26. Grab a whiteboard and let’s practice!

  27. Chemical Formula Practice: • What is the formula for Aluminum Bromide?

  28. Practice: • Predict the formula if Oxygen and Potassium form an ionic bond.

  29. Practice: • Predict the formula if Copper(ii) and Nitrogen form and ionic bond.

  30. One of the following pairs will form an ionic bond, one won’t. Draw out the one that will form the bond and describe why the other pair won’t bond. Argon and Oxygen Barium and Carbon

  31. Practice: Write the correct formula for the compounds formed from each pair of ions Potassium and Sulfur Calcium and Oxygen

  32. Practice: Write the formulas for each compound Barium Chloride Lithium Oxide

  33. Practice: Which pairs of elements are likely to form ionic compounds? • A. Cl and Br • B. Li and Cl • C. K and He • D. I and Na

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