6.3 Naming Compounds and Writing Formulas

1. 6.3 Naming Compounds and Writing Formulas Chapter 6 Chemical Bonds

2. What are we going to learn? • How to write the name and formula of ionic and covalently bonded compounds

3. Naming Ionic Compounds • Ionic compound name: distinguishes the compound from other ionic compounds containing the same elements • Name =words (ex: calcium chloride)

4. Ionic compound formula: describes the ratio of the ions in the compound • Formula = numbers of elements(ex: CaCl2)

5. Binary Compounds • If a compound is made from only two elements is a binary compound (Ex: salt is a binary compound made of sodium and chlorine - sodium chloride)

6. What’s in a Name? • To name a binary compound: list the name of the cation (+ ion) followed by the name of the anion (- ion)

7. Cations – First in Naming • Cation: simply the name of the metal (no changes) • Ex: sodium atom and sodium ion

8. This works for groups 1A, 2A and Aluminum • Group 1A has a 1+ charge • Group 2A has a 2+ charge • Aluminum (Group 3A) has a 3+ charge

9. Transition metals with more than one possible charge have a different naming strategy • Name of the ion contains a Romannumeral to indicate the charge • Ex: copper (II) ion

10. Anions – The Followers • Anion: use name of the nonmetal with the suffix –idereplacing –ine (ex: chlorine atom and chloride ion) • Nonmetals are on the right side of the periodic table • Ex: sodium chloride (cation) (anion)

11. Formulas • If you know the name of an ionic compound, you can write its chemical formula • Chemical formula includes chemical symbols of the elements and numbers (indicating amounts of each element)

12. How do you write a formula? • Write the symbol of the cation first • Follow with the symbol of the anion • Use subscripts to show the ratio of the ions in the compound

13. Polyatomic Ions • A covalently bonded group of atoms that has a positive or negative charge and acts as a unit • Ex: nitrate (NO)3-, sulfate (SO4)2-, phosphate (PO4)3-

15. Molecular Compounds • Name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound • These elements are usually on the right side of the periodic table • Elements in the compound share electrons

16. The molecules in the top row bond by sharing electrons. The compounds in the bottom row join in polar covalent bonds.

17. Naming a Molecular Compound • Most metallic element name appears first (most left in the periodic table) • Name of the second element is changed to end in the suffix -ide • Ex: carbon dioxide

18. Prefixes indicate amount of atoms in the molecule • Ex: di shows that there are two carbon atoms in the molecule

19. Molecular Formula • Write the symbols for the elements in the order the elements appear in the name • Prefixes in the compound name indicate the number of atoms of each element in the molecule • Prefixes appear as subscripts in the formula

21. Writing Chemical Formulas for Binary Compounds Practice • 1 - Write the symbols for the elements.2 - Look up element ion charges and write them as superscripts to the right of the elemental symbols.3 - Use the correct combination of ions to produce a compound with a net charge of zero. Multiple ions are indicated with subscripts. • lithium oxide • potassium chloride • calcium oxide • barium bromide

22. Writing Chemical Formulas for Binary Compounds Practice • 1 - Write the symbols for the elements.2 - Look up element ion charges and write them as superscripts to the right of the elemental symbols.3 - Use the correct combination of ions to produce a compound with a net charge of zero. Multiple ions are indicated with subscripts. • lithium oxide Li2O • potassium chloride KCl • calcium oxide CaO • barium bromide BaBr2

23. Writing Chemical Formulas for Binary Compounds with Polyatomic Ions  • lithium carbonate • calcium nitrate • ammonium sulfide • sodium sulfate

24. Writing Chemical Formulas for Binary Compounds with Polyatomic Ions  • lithium carbonate Li2CO3 • calcium nitrate Ca(NO3) 2 • ammonium sulfide (NH4) 2S • sodium sulfate Na2SO4

25. Writing Chemical Formulas for Transition Metals Practice • Lead (IV) carbonate • Copper (II) nitrate • Iron (III) oxide • Tin (IV) fluoride

26. Writing Chemical Formulas for Transition Metals Practice • Lead (IV) carbonate Pb(CO3)2 • Copper (II) nitrate Cu(NO3)2 • Iron (III) oxide Fe2O3 • Tin (IV) fluoride SnF4

27. Writing Chemical Names for Transition Metals Practice • Fe(NO3)2 • CuF2 • NiS • FeCl2

28. Writing Chemical Names for Transition Metals Practice • Fe(NO3)2 iron (II) nitrate • CuF2 copper (II) fluoride • NiS nickel (II) sulfide • FeCl2iron (II) chloride

29. Writing Chemical Formulas Practice • zinc carbonate • barium oxide • cadmium fluoride • magnesium sulfide • lithium phosphate

30. Writing Chemical Formulas Practice • zinc carbonate ZnCO3 • barium oxide BaO • cadmium fluoride CdF2 • magnesium sulfide MgS • lithium phosphate Li3PO4

31. Writing Chemical Names Practice • FeF2 • FeF3 • Hg2Br2 • HgBr2

32. Writing Chemical Names Practice • FeF2 iron (II) fluoride • FeF3 iron (III)fluoride • Hg2Br2 mercury (I) bromide • HgBr2mercury (II) bromide

33. Writing Chemical Names Practice • BaSO4 • FeF2 • CuCO3 • CaS • MgO • KCl

34. Writing Chemical Names Practice • BaSO4 barium sulfate • FeF2 iron (II) fluoride • CuCO3 copper (II) carbonate • CaS calcium sulfide • MgO magnesium oxide • KCl potassium chloride

35. NO • N2O • NO2 • N2O5 • N2O3

36. NO nitrogen monoxide • N2O dinitrogen monoxide • NO2nitrogen dioxide • N2O5dinitrogen pentoxide • N2O3dinitrogen trioxide