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CHEMICAL BONDS

CHEMICAL BONDS. I. Chemical Compounds. Compounds Are made from more than one type of atom (element) Are made during a chemical chg Have properties different from the elements they are made of Have constant compositions. I. Chemical Compounds. Fe 2 O 3.

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CHEMICAL BONDS

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  1. CHEMICAL BONDS

  2. I. Chemical Compounds • Compounds • Are made from more than one type of atom (element) • Are made during a chemical chg • Have properties different from the elements they are made of • Have constant compositions

  3. I. Chemical Compounds Fe2O3 • Chemical Formulas • Use symbols to represent the ratios of elements in a particular compound. • Element symbols • Subscripts

  4. B.Chemical Formulas 3. Practice Interpreting Formulas • NaCl 1 sodium atom; 1 chlorine atom • H2O 2 hydrogen atoms; 1 oxygen atom • Al2(SO4)3 • 2 aluminum atoms • 3 sulfur atoms • 12 oxygen atoms

  5. Your Turn! Interpret each of the following Fe2O3 Pb(C2H3O2)2 2 iron atoms 3 oxygen atoms 1 lead atom 4 carbon atoms 6 hydrogen atoms 4 oxygen atoms

  6. I. Chemical Compounds C. Atoms Combine • To become Stable • Atoms are stable when they have a full valence energy level • Octet rule: Usually 8 e- • Exception: He is stable w/ 2 e- • Atoms gain, lose or share e- to achieve a full valence level c. Atoms are held together by achemical bond

  7. I. Chemical Compounds C. Atoms Combine • Noble gases • Are inert • do not react because they already have a full valence energy level (stableoctet)

  8. II. Ions A. Ions are atoms which 1. Have gained or lost e- ELementsto the Left of the Line Lose eLectrons Neither LOSE GAIN

  9. II. Ions A. Ions are atoms which 1. Have gained or lost e-

  10. II. Ions A. Ions are atoms which 1. Have gained or lost e- • You can predict the # of e- which will be gained or lost by looking at the family

  11. Lose 1 e- Gain 1 e- Lose 2 e- Gain 2 e- Gain 3 e- Varies Lose 3 e- Will P gain or lose electrons when forming an ion? How many? Gains 3 e-

  12. A. Ions are atoms which • Another name for charge is oxidation number • The formula for an ion includes its charge (oxidation number) • Na ion • Lost 1 e- Formula= Na1+ • Cl ion • Gained 1 e- Formula= Cl1-

  13. Ions have a charge, atoms do not Review it Now! • What is the difference between an atom and an ion? • What is an oxidation number? • Write the oxidation number for each of the following ions: a. Li f. Al b. K g. S c. Mg h. Cl d. P i. Ne e. B j. N The charge on an ion 1+ 3+ 1+ 2- 2+ 1- 3- 0 3- 3+

  14. III.Compounds with Ionic Bonds • Ionic Bonds 1.Are formed a.between (+) and (-) ions b.When one atom gains e- while the other loses e- 2.Compounds with ionic bonds are called ionic compounds

  15. III.Compounds with Ionic Bonds • Ionic Bonds 3. Ionic bonds are formed between a metal and a nonmetal!

  16. Check Your Understanding! Which of the following are ionic compounds? 1. KCl 2. CO2 3. LiF 4. CaCl2 Ionic Not ionic Ionic Ionic

  17. B. Formulas for Binary Cmpds Step 1:Write the symbol of the (+) ion first, followed by the symbol of the (-) ion Step 2: Determine the ox.# for each ion and write it above the symbols. Step 3: Crisscross the charges and write them as subscripts. Step 4: If the charges can be reduced, do so.

  18. B. Formulas for Ionic Cmpds Example #1: Ba and Cl

  19. B. Formulas for Ionic Cmpds Example #2: Be and P Be3P2

  20. B. Formulas for Ionic Cmpds Example #3: Ba and S BaS Ba2S2 note subscripts can be reduced; do so!

  21. Your Turn! Write the formula for each of the following compounds 1. calcium with chlorine 2. potassium with bromine 3. lithium with sulfur 4. magnesium with phosphorus 5. aluminum with nitrogen CaCl2 KBr Li2S Mg3P2 AlN

  22. C. Naming Binary Cmpds Step 1:Write the name of the positive element 1st. Step 2:Write the name of the negative element 2nd. Step 3:Add the ending -ide to the root of the second element.

  23. C. Naming Binary Cmpds Example #1: What is the formula name for CaCl2? Step 1:calcium Step 2:calcium chlorine Step 3:calcium chloride calcium chloride

  24. C. Naming Binary Cmpds Example #2: What is the formula name for Mg3P2? Step 1:magnesium Step 2:magnesium phosphorus Step 3:magnesium phosphide Magnesium phosphide

  25. Your Turn! Name each of the following 1. Li2S 2. KBr 3. BaS 4. Al2O3 5. Na3N Lithium sulfide Potassium bromide Barium sulfide Aluminum oxide Sodium nitride

  26. D. Formulas for Polyatomic Ionic Cmpds • Binary compounds are made of two kinds of elements. • Example: BaCl2 • Polyatomic (ternary) compounds are made of three or more elements. • Examples: K2SO4 Mg(ClO3)2

  27. D. Formulas for Polyatomic Ionic Cmpds • Polyatomic ions are a group of covalently bonded atoms that act as one atom with a charge.

  28. D. Formulas for Polyatomic Ionic Cmpds • Rules for Writing Formulas Step 1:Write the symbol and ox. # Step 2: Crisscross the charges and write them as subscripts. Step 3: Make sure you put polyatomic ions in parentheses (if you need more than one). Step 4: Make sure the subscripts are reduced.

  29. D. Formulas for Ionic Cmpds Ca2+ and NO31- Ca2+ and (NO3) 2 Example #1: Calcium Nitrate Ca2+ and NO31- 2 Ca(NO3)2

  30. D. Formulas for Polyatomic Ionic Cmpds Ca2+ and PO43- Example #2: Calcium Phosphate Ca2+ and PO43- 3 2 Ca3 and (PO4)2 Ca3(PO4)2

  31. Your Turn! Write the formula for each of the following compounds 1. Sodium sulfate 2. Calcium hydroxide 3. Beryllium phosphate 4. Aluminum nitrate Na2SO4 Ca(OH)2 Be3(PO4)2 Al(NO3)3

  32. E. Naming Polyatomic Ionic Compounds • Rules for Naming Polyatomic Compounds Step 1:Write the name of the positive ion. Step 2: Write the name of the negative ion .

  33. E. Naming Polyatomic Ionic Cmpds Example #1: Ca(NO3)2 Calcium nitrate Calcium nitrate

  34. E. Naming Polyatomic Ionic Cmpds Example #2: AlPO4 Aluminum phosphate Aluminum phosphate

  35. Your Turn! Potassium sulfate Name each of the following compounds 1. K2SO4 2. CaCO3 3. NaOH 4. NH4C2H3O2 Calcium carbonate Sodium hydroxide Ammonium acetate

  36. G. Special case ionic bonds: ACIDS Acids are easy to recognize as compounds as they begin with the element hydrogen. As with other ionic bonds, acids fall into 2 categories, binary and ternary.

  37. G. Special case ionic bonds: ACIDS Examples of binary acids would include things like: HF, HI, H2S and HCl Examples of ternary acids would include things like: H2SO4 and HNO3

  38. G. Special case ionic bonds: ACIDS Naming of binary acids Step 1:Name the anion, changing the ending to “-ic” Step 2: Add the prefix “hydro-” Step 3: Slap acid on the end

  39. G. Special case ionic bonds: ACIDS Example #1: HF

  40. G. Special case ionic bonds: ACIDS Example #1: HF “flourine” becomes

  41. G. Special case ionic bonds: ACIDS Example #2: HF “flourine” becomes “flouric” becomes

  42. G. Special case ionic bonds: ACIDS Example #1: HF “flourine” becomes “flouric” becomes “hydroflouric” becomes

  43. G. Special case ionic bonds: ACIDS Example #1: HF “chlorine” becomes “chloric” becomes “hydrochloric” becomes “hydroflouric acid”

  44. G. Special case ionic bonds: ACIDS Example #2: HCl

  45. G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes

  46. G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes “chloric” becomes

  47. G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes “chloric” becomes “hydrochloric” becomes

  48. G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes “chloric” becomes “hydrochloric” becomes “hydrochloric acid”

  49. G. Special case ionic bonds: ACIDS Naming of ternary acids Step 1:Name the polyatomic Step 2: Change “-ate” to “-ic” or “-ite” to “-ous” Step 3: Slap acid on the end

  50. G. Special case ionic bonds: ACIDS Example #1: H2SO4 “sulfate” becomes “sulfuric” becomes “sulfuric acid”

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