Chemical Formulas & Compounds

1. Chemical Formulas & Compounds Chapter 7

2. Formulas tell you the number of atoms of each element in a compound . . .

3. Formulas tell you the number of atoms of each element in a compound . . . • How many atoms of each element are in the compounds below? • H2O • NaCl • CaCl2 • Ca(CO3)2 • NaCO3

4. Formulas tell you the number of atoms of each element in a compound . . . • How many atoms of each element are in the compounds below? • H2O . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • NaCl • CaCl2 • Ca(CO3)2 • NaCO3

5. Formulas tell you the number of atoms of each element in a compound . . . • How many atoms of each element are in the compounds below? • H2O . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • NaCl . . . . . . . . . . . . . . . . . . . . . . . . . . 2 • CaCl2 • Ca(CO3)2 • NaCO3

6. Formulas tell you the number of atoms of each element in a compound . . . • How many atoms of each element are in the compounds below? • H2O . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • NaCl . . . . . . . . . . . . . . . . . . . . . . . . . . 2 • CaCl2 . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • Ca(CO3)2 • NaCO3

7. Formulas tell you the number of atoms of each element in a compound . . . • How many atoms of each element are in the compounds below? • H2O . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • NaCl . . . . . . . . . . . . . . . . . . . . . . . . . . 2 • CaCl2 . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • Ca(CO3)2 . . . . . . . . . . . . . . . . . . . . . . . 9 • NaCO3

8. Formulas tell you the number of atoms of each element in a compound . . . • How many atoms of each element are in the compounds below? • H2O . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • NaCl . . . . . . . . . . . . . . . . . . . . . . . . . . 2 • CaCl2 . . . . . . . . . . . . . . . . . . . . . . . . . . 3 • Ca(CO3)2 . . . . . . . . . . . . . . . . . . . . . . . 9 • NaCO3 . . . . . . . . . . . . . . . . . . . . . . . . . 5

9. Monatomic: Contain only one atom Carry a charge because of gaining or losing valence electrons Polyatomic: Contain more than one atom bonded together Usually written with parentheses (talk more later) List on p. 210 Monatomic v. Polyatomic Ions

10. S & P Block elements Number of valence electrons helps to determine charge D block elements Can have any charge ranging from +1 to +4 When naming, which ion being used must be indicated using Roman numerals See table on p. 205 Monatomic Ions

11. Naming Monatomic Ions • No changes are made to the name of the cation (Cation is almost always a metal) • If cation is a d-block metal, add a roman numeral indicating the charge after the name • Anion must have the –ide ending added (Anion is always a nonmetal)

12. Na+1 S-2 Al+3 Fe+2 Br-1 P-3 Naming Practice

13. Na+1 S-2 Al+3 Fe+2 Br-1 P-3 Sodium Naming Practice

14. Na S Al Fe+2 Br P Sodium Sulfide Naming Practice

15. Na S Al Fe+2 Br P Sodium Sulfide Aluminum Naming Practice

16. Na S Al Fe+2 Br P Sodium Sulfide Aluminum Iron (II) Naming Practice

17. Na S Al Fe+2 Br P Sodium Sulfide Aluminum Iron (II) Bromide Naming Practice

18. Na S Al Fe+2 Br P Sodium Sulfide Aluminum Iron (II) Bromide Phosphide Naming Practice

19. Binary Ionic: Composed of a cation (usu. metal) bonded to an anion (usu. nonmetal) Cation gives electron to anion Positive charges must balance negative charges Binary Molecular Usually composed of 2 nonmetals Electrons are shared between atoms Prefixes or Roman numerals must be used Ionic v. Molecular Compounds

20. Binary Ionic Compounds • Because positive charges must balance negative charges, use criss-cross method to make formulas: Al 3+ O 2-

21. Binary Ionic Compounds • Because positive charges must balance negative charges, use criss-cross method to make formulas: Al 3+ O 2- Al2O3

22. Binary Ionic Compounds • When naming binary ionic compounds, you name the cation first (using a Roman numeral if needed) and the anion second with the –ide ending Al2O3

23. Binary Ionic Compounds • When naming binary ionic compounds, you name the cation first (using a Roman numeral if needed) and the anion second with the –ide ending Al2O3 Aluminum Oxide

24. NaF CaBr2 CoCl2 SnO2 Li2O Naming Binary Ionic Compounds Practice

25. NaF CaBr2 CoCl2 SnO2 Li2O Sodium Fluoride Naming Binary Ionic Compounds Practice

26. NaF CaBr2 CoCl2 SnO2 Li2O Sodium Fluoride Calcium Bromide Naming Binary Ionic Compounds Practice

27. NaF CaBr2 CoCl2 SnO2 Li2O Sodium Fluoride Calcium Bromide Cobalt(II) Chloride Naming Binary Ionic Compounds Practice

28. NaF CaBr2 CoCl2 SnO2 Li2O Sodium Fluoride Calcium Bromide Cobalt(II) Chloride Tin(IV) Oxide Naming Binary Ionic Compounds Practice

29. NaF CaBr2 CoCl2 SnO2 Li2O Sodium Fluoride Calcium Bromide Cobalt(II) Chloride Tin(IV) Oxide Lithium Oxide Naming Binary Ionic Compounds Practice

30. Binary Molecular Compounds • Usually consists of two nonmetals bonded together. • Naming requires either prefixes (p. 212) or Roman numerals (p. 219) • You will only be required to know prefix method

31. Naming Binary Molecular Compounds • Name the less electronegative (EN) element first • Give first element a prefix only if there is more than one atom present • Name more EN element 2nd and give it the –ide ending • Second element ALWAYS gets a prefix

32. CO2 H2O ICl3 PBr5 SO3 . . . and here’s some more practice!

33. CO2 H2O ICl3 PBr5 SO3 Carbon dioxide . . . and here’s some more practice!

34. CO2 H2O ICl3 PBr5 SO3 Carbon dioxide Dihydrogen monoxide . . . and here’s some more practice!

35. CO2 H2O ICl3 PBr5 SO3 Carbon dioxide Dihydrogen monoxide Iodine trichloride . . . and here’s some more practice!

36. CO2 H2O ICl3 PBr5 SO3 Carbon dioxide Dihydrogen monoxide Iodine trichloride Phosphorus pentabromide . . . and here’s some more practice!

37. CO2 H2O ICl3 PBr5 SO3 Carbon dioxide Dihydrogen monoxide Iodine trichloride Phosphorus pentabromide Sulfur trioxide . . . and here’s some more practice!

38. What if there are more than 2 elements? • If compound has more than 2 elements, then there is probably a polyatomic ion present (p. 210) • Most polyatomic ions are anions • Exceptions are Ammonia (NH4+1) and dimercury (Hg2+2) • Oxyanions are polyatomic ions with oxygen in them

39. Naming Polyatomic Compounds • As usual, name the cation first, using Roman numerals when needed. • Then the anion is named second, using the –ide ending if needed

40. Ca(OH)2 KClO3 NH4OH FeCrO4 It’s practice time! 

41. Ca(OH)2 KClO3 NH4OH FeCrO4 Calcium Hydroxide It’s practice time! 

42. Ca(OH)2 KClO3 NH4OH FeCrO4 Calcium Hydroxide Potassium Chlorate It’s practice time! 

43. Ca(OH)2 KClO3 NH4OH FeCrO4 Calcium Hydroxide Potassium Chlorate Ammonium Hydroxide It’s practice time! 

44. Ca(OH)2 KClO3 NH4OH FeCrO4 Calcium Hydroxide Potassium Chlorate Ammonium Hydroxide Iron(II) Chromate It’s practice time! 

45. Writing Polyatomic Formulas • Similar to writing formulas for binary ionic compounds (criss-cross method) • If you have more than 1 polyatomic ion, you must enclose the ion in parentheses and place the subscript outside the parentheses . . .

46. Lithium Hydroxide Magnesium Nitrate Ammonium Nitride Aluminum Sulfate Here we go!

47. Lithium Hydroxide Magnesium Nitrate Ammonium Nitride Aluminum Sulfate LiOH Here we go!

48. Lithium Hydroxide Magnesium Nitrate Ammonium Nitride Aluminum Sulfate LiOH Mg(NO3)2 Here we go!

49. Lithium Hydroxide Magnesium Nitrate Ammonium Nitride Aluminum Sulfate LiOH Mg(NO3)2 (NH4)3N Here we go!

50. Lithium Hydroxide Magnesium Nitrate Ammonium Nitride Aluminum Sulfate LiOH Mg(NO3)2 (NH4)3N Al2(SO4)3 Here we go!