Systematic Naming

1. Systematic Naming • There are too many compounds to remember the names of them all. • Compound is made of two or more different elements that are bonded together by electrostatic forces. • Name should tell us how many and what type of atoms.

2. Cations • Positive ions. • Formed by losing electrons. • More protons than electrons. • Metals form cations. K+1 Has lost one electron Ca+2 Has lost two electrons

3. Anion • A negative ion. • Has gained electrons. • Non metals can gain electrons. • Charge is written as a super script on the right. F-1 Has gained one electron O-2 Has gained two electrons

4. Compounds • Follow the Law of Definite Proportions. It states that compounds have a constant composition (there are always the same number and types of atoms in the compound).

5. Formula Unit • The smallest whole number ratio of atoms in an ionic compound. • Ions surround each other so you can’t say which is hooked to which.

6. Charges on ions • For most of the Group A elements, the Periodic Table can tell what kind of ion they will form from their location. • Elements in the same group have similar properties. • Including the charge when they are ions.

7. +1 +2 +3 -3 -2 -1

8. Naming ions • We will use the systematic way. • Cation- if the charge is always the same (Group A) just write the name of the metal. • Transition metals can have more than one type of charge. • Indicate the charge on transition metals with roman numerals in parentheses.

9. Name these • Na+1 • Ca+2 • Al+3 • Fe+3 • Fe+2 • Li+1

10. Name these • Na+1 sodium ion • Ca+2 calcium ion • Al+3 aluminum ion • Fe+3 iron (III) ion • Fe+2 iron (II) ion • Li+1 lithium ion

11. Write Formulas for these • Potassium ion • Magnesium ion • Copper (II) ion • Chromium (VI) ion • Barium ion • Mercury (II) ion

12. Write Formulas for these • Potassium ion K+1 • Magnesium ion Mg+2 • Copper (II) ion Cu+2 • Chromium (VI) ion Cr+6 • Barium ion Ba+2 • Mercury (II) ion Hg+2

13. Naming Anions • Anions are always the same. • Change the element ending to – ide • F-1 Fluorine

14. Naming Anions • Anions are always the same. • Change the element ending to – ide • F-1 Fluorin

15. Naming Anions • Anions are always the same • Change the element ending to – ide • F-1 Fluori

16. Naming Anions • Anions are always the same • Change the element ending to – ide • F-1 Fluor

17. Naming Anions • Anions are always the same • Change the element ending to – ide • F-1 Fluori

18. Naming Anions • Anions are always the same • Change the element ending to – ide • F-1 Fluorid

19. Naming Anions • Anions are always the same • Change the element ending to – ide • F-1 Fluoride

20. Name these • Cl-1 • N-3 • Br-1 • O-2

21. Name these • Cl-1 chloride ion • N-3 nitride ion • Br-1 bromide ion • O-2 oxide ion

22. Write these • sulfide ion • iodide ion • phosphide ion • chloride ion

23. Write these • sulfide ion S-2 • iodide ion I-1 • phosphide ion P-3 • chloride ion Cl-1

24. Polyatomic ions • Groups of atoms that stay together through covalent bonding and have a charge. • You must memorize these. • Nitrate NO3-1 • Nitrite NO2-1 • Hydroxide OH-1

25. And These: Sulfate SO4-2 Sulfite SO3-2 Carbonate CO3-2 Phosphate PO4-3 Ammonium NH4+1 Polyatomic ions

26. Ions in Ionic Compounds

27. Naming Binary Ionic Compounds • Binary Compounds - 2 elements. • Ionic - a cation and an anion. • To write the names just name the two ions. • Easy with Representative elements. • Group A • NaCl = Na+ Cl- = sodium chloride • MgBr2 = Mg+2 Br- = magnesium bromide

28. Naming Binary Ionic Compounds • The problem comes with the transition metals. • Need to figure out their charges. • The compound must be neutral with the same number of + and – charges. • Use the anion to determine the charge on the positive ion.

29. Naming Binary Ionic Compounds • Write the name of CuO • Need the charge of Cu • O is -2 • copper must be +2 • You write Copper (II) oxide • Name CoCl3 • Cl is -1 and there are three of them = -3 • Co must be +3 Cobalt (III) chloride

30. Naming Binary Ionic Compounds • Write the name of Cu2S. • Since S is -2, the Cu2 must be +2, so each one is +1. • copper (I) sulfide • Fe2O3 • Each O is -2 3 x -2 = -6 • 2 Fe must = +6, so each is +3. • iron (III) oxide

31. Naming Binary Ionic Compounds • Write the names of the following • KCl • Na3N • CrN • Sc3P2 • PbO • PbO2 • Na2Se

32. Naming Binary Ionic Compounds • Write the names of the following • KCl potassium chloride • Na3N sodium nitride • CrN chromium (III) nitride • Sc3P2 scandium (II) phosphide • PbO lead (II) oxide • PbO2 lead (IV) oxide • Na2Se sodium selenide

33. Writing Formulas • The charges have to add up to zero. • Get charges on pieces. • Cations from name off the table. • Anions from table or polyatomic. • Balance the charges by adding subscripts. • Put polyatomics in parenthesis.

34. Writing Formulas • Write the formula for calcium chloride. • Calcium is Ca+2 • Chloride is Cl-1 • Ca+2Cl-1 would have a +1 charge. • Need another Cl-1 • CaCl2

35. Write the formulas for these • Lithium sulfide • tin (II) oxide • tin (IV) oxide • Magnesium fluoride • Copper (II) sulfate • Iron (III) phosphide • gallium nitrate • Iron (III) sulfide

36. Write the formulas for these • Lithium sulfide Li2S • tin (II) oxide SnO • tin (IV) oxide SnO2 • Magnesium fluoride MgF2 • Copper (II) sulfate CuSO4 • Iron (III) phosphide FeP • gallium nitrate Ga(NO3)3 • Iron (III) sulfide Fe2S3

37. Write the formulas for these • Ammonium chloride • ammonium sulfide • barium nitrate

38. Things to look for • If a cation has ( ), the roman numeral is its charge. • If anions end in -ide they are probably off the periodic table (Monoatomic) • If anion ends in -ate or -ite it is polyatomic