1. Ionic Compounds

2. Ionic bond: bond formed by attraction between + and - ions
Ionic Bonding
Electrons are transferred from one atom to another so that each has 8 valence electrons
- called the octet rule +
Cation -
Anion
Ionic Compound
Ionic bond: bond formed by attraction between + and - ions 2

3. Ionic Bonding Ionic bonds occur between metals and non-metals H He LiF Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Lr Rf Db Sg Bh Hs Mt
Uun
Uuu
Uub
Uut
Metals
Metalloids
Non-metals

4. The “magic number” is 8! 4

5. Binary Ionic Compounds Formula to Name

6. The Language of Chemistry
Chemistry has a language all of its own
Chemistry
English
Element Symbols
Letters
Chemical Formulas
Words
Chemical Equations
Sentences
Each element symbol starts with a capital letter

7. Binary Ionic: Formula to Name
These compounds have:
2 elements (“binary”)
A metal & a non-metal (“ionic”)
To name:
Name of the metal (the cation)
Name of the non-metal (the anion) with the suffix “-ide”
The subscripts in the formula do not matter when naming this type

8. Example
CaBr2

9. Example
K2O

10. Write the name for the following compounds
Let’s Practice
CaF2
Na3P
NaI
SrBr2
Example:
Write the name for the following compounds

11. Write the name for the following compounds
Let’s Practice
CaF2
Na3P
NaCl
SrBr2
Calcium fluoride
Sodium phosphide
Sodium chloride
Strontium bromide
Example:
Write the name for the following compounds

12. Binary Ionic Compounds Name to Formula

13. Binary Ionic: Name to Formula
These compounds:
End in “-ide” (except “hydroxide and cyanide”)
Do NOT contain covalent prefixes
To write:
Draw Lewis dot diagrams of each element and transfer electrons.
Use subscripts to show how many of each type of ion you have.

14. Example
Sodium fluoride

15. Write the following chemical formulas
Let’s Practice
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
Example:
Write the following chemical formulas

16. Write the following chemical formulas
Let’s Practice
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
CsCl
K2O
CaS
Li3N
Example:
Write the following chemical formulas

17. Multivalent Ionic Compounds Formula to Name

18. Multivalent (Transition) Metals
Multivalent Metal: a metal that has more than one possibility for cationic (positive) charge
The Appendix of your book (Page A-2) has the following chart
Common multivalent metals and their charges
Cobalt Co Co+3
Copper Cu Cu+2
Iron Fe Fe+3
Lead Pb Pb+4
Manganese Mn+2 Mn+3
Mercury Hg2+2 Hg+2
Tin Sn Sn+4 18

19. Multivalent Metals: Formula to Name
To identify:
Have a transition metal
To name:
Name of the metal cation
Name of the anion
Determine total negative charge in the compound
Total negative charge must = total positive charge
Determine the charge on each metal atom
Write the charge in roman numerals in parenthesis after the metal’s name 19

20. Total negative charge in compound Total positive charge in compound
Example
Anion
Total negative charge in compound
Total positive charge in compound
Cation
Name
CuCl2 20

21. Total negative charge in compound Total positive charge in compound
Example
Anion
Total negative charge in compound
Total positive charge in compound
Cation
Name
Fe2O3 21

22. Write the name for the following compounds
Let’s Practice
PbCl2
PbCl4
MnO
Mn2O7
Example:
Write the name for the following compounds 22

23. Write the name for the following compounds
Let’s Practice
PbCl2
PbCl4
MnO
Mn2O3
Lead (II) chloride
Lead (IV) chloride
Manganese (II) oxide
Manganese (VII) oxide
Example:
Write the name for the following compounds 23

24. Multivalent Ionic Compounds Name to Formula

25. Multivalent Metals: Name to Formula
To identify:
Will have roman numerals
To write:
Same as binary!
Roman numerals tell the charge of the metal cation 25

26. Example
Iron (III) oxide 26

27. Example
Copper (I) nitride 27

28. Write the following chemical formulas
Let’s Practice
Iron (II) nitride
Copper (I) chloride
Lead (IV) sulfide
Tin (II) oxide
Example:
Write the following chemical formulas 28

29. Write the following chemical formulas
Let’s Practice
Iron (II) nitride
Copper (I) chloride
Lead (IV) sulfide
Tin (II) oxide
Fe3N2
CuCl
PbS2
SnO
Example:
Write the following chemical formulas 29

30. Polyatomic Ionic Compounds

31. Polyatomic Ions
Polyatomic Ion: a group of atoms that has lost or gained electrons. Therefore, it has a charge!
Polyatomic Ionic Compound: compound containing at least one polyatomic ion -
Polyatomic
Anion
Polyatomic Ionic
Compound +
Cation 31

32. Identifying Polyatomic Ions
Only one cation: NH4+
All others are anions (second part of formula)
Subscripts must match exactly as it appears on your list
If there are parenthesis, the polyatomic ion is inside 32

33. Practice Identifying Polyatomic Ions
NaNO3
NH4Cl
Ca(OH)2
(NH4)3PO4
K2CO3
Example:
Identify and name the polyatomic ion in each compound 33

34. Practice Identifying Polyatomic Ions
NaNO3
NH4Cl
Ca(OH)2
(NH4)3PO4
K2CO3
Nitrate
Ammonium
Hydroxide
Ammonium & phosphate
Carbonate
Example:
Identify and name the polyatomic ion in each compound 34

35. Polyatomic Ionic Compounds Name to Formula

36. Polyatomic Ionic: Name to Formula
To identify:
Do not end with “-ide” (except hydroxide & cyanide)
Do not use covalent prefixes
To write these formulas:
Write the symbol & charge of the cation & anion
Add additional cations or anions to have a neutral compound
Use subscripts to show the number of ions
- When using subscripts with a polyatomic ion, you must put the polyatomic ion in parenthesis. 36

37. Example
Sodium carbonate 37

38. Example
Magnesium nitrate 38

39. Write the following chemical formulas
Let’s Practice
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
Example:
Write the following chemical formulas 39

40. Write the following chemical formulas
Let’s Practice
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
NaNO3
Ca(ClO3)2
K2SO3
Ca(OH)2
Example:
Write the following chemical formulas 40

41. Polyatomic Ionic Compounds Formula to Name

42. Polyatomic Ionic: Formula to Name
To identify:
More than 2 capital letters (not starting with H)
at least 1 metal & 1 non-metal
To name:
Name of the cation
If the anion is a polyatomic ion, write the polyatomic ion’s name just as it is
If the anion is a single non-metal element, use “-ide” 42

43. Example
NaNO3 43

44. Example
Fe(OH)2 44

45. Write the name for the following compounds
Let’s Practice
Ca(NO3)2
Na3PO4
NH4ClO
K2CO3
Example:
Write the name for the following compounds 45