1. Chapter 5: Ions and Ionic Compounds

2. 5.1 Ions

3. Ion
Ion: an atom or group of atoms that has a charge as a result of losing or gaining one or more electrons

4. Cation Ca+ion: positively charged ion
Formed from a metal atom losing electrons

5. Anion Anion: negatively charged ion
Formed from a nonmetal atom gaining electrons

6. Ions -1 +1 -3 +2 -2
+/- 4 +3

7. Metals and Roman Numerals
Metals can have various charges, so you MUST specify which one you have!
The charge of a metal is indicated by a Roman Numeral.
Exceptions: Groups 1 & 2, Silver (Ag), and Zinc (Zn) have only one charge, so they do not get Roman numerals in their names!
Examples:
1.) Copper (II) = Cu+2
2.) Iron (III) = Fe+2

8. Practice: Metals and Roman Numerals
Name the following transition metal ions:
1.) Cr+2
2.) Cr+3
3.) Mn+2
4.) Mn+3
5.) Pt+2
6.) Pt+4

9. Practice: Metals and Roman Numberals
Name the following transition metal ions:
1.) Cr Chromium (II)
2.) Cr Chromium (III)
3.) Mn Manganese (II)
4.) Mn Manganese (III)
5.) Pt Platinum (II)
6.) Pt Platinum (IV)

10. Practice: Ions
Determine if the following ions are cations (metal) or anions (nonmetal):
1.) Calcium ion
2.) Nitrogen ion
3.) Potassium ion
4.) Bromine ion
5.) Oxygen ion
6.) Lead (IV) ion

11. Practice: Ions Determine if the following ions are cations or anions:
1.) Calcium ion: cation
2.) Nitrogen ion: anion
3.) Potassium ion: cation
4.) Bromine ion: anion
5.) Oxygen ion: anion
6.) Lead (IV) ion: cation

12. Practice: Ions Element Symbol and Charge Metal or Nonmetal?
Anion or Cation?
Sodium
Na+1
Metal
Cation
Fluorine
Magnesium
Copper (II)

13. Practice: Ions Element Symbol and Charge Metal or Nonmetal?
Anion or Cation?
Sodium
Na+1
Metal
Cation
Fluorine
F-1
Nonmetal
Anion
Magnesium
Mg+2
Copper (II)
Cu+2

14. Calculating #p and #e of Ions
# of protons
# of electrons
S-2
Al+3
Fe+2
N-3
Ca+2
C-4

15. Calculating #p and #e of Ions
# of protons
# of electrons
S-2 16 18
Al+3 13 10
Fe+2 26 24
N-3 7
Ca+2 20
C-4 6

16. Calculating #p and #e of Ions
# of protons
# of electrons
Na+1
O-2
Zn+2
F-1
Mg+2
P-3

17. Calculating #p and #e of Ions
# of protons
# of electrons
Na+1 11 10
O-2 8
Zn+2 30 28
F-1 9
Mg+2 12
P-3 15 18

18. Octet Rule
Octet Rule: Atoms lose or gain electrons to match the valence electron configuration of a noble gas.
Atoms gain or lose electrons because they want to be more stable.
Full valence shells = stable atoms

19. Electron Configurations of Ions
1.) Determine number of electrons 2.) Write electron configuration Example: Fluorine ion = F-1 Fluorine ion has 10 electrons Electron configuration is 1s22s22p6 Neon also has 10 electrons and has the same electron configuration, so F-1 and neon are isoelectronic.

20. Practice
Determine the electron configuration of the following ions and write which noble gas they are isoelectronic with.
1.) Lithium ion
2.) Magnesium ion
3.) Calcium ion

21. Practice
Determine the electron configuration of the following ions and write which noble gas they are isoelectronic with.
1.) Lithium ion (2 electrons): 1s2
isoelectronic with helium
2.) Magnesium ion (10 electrons): 1s22s22p isoelectronic with neon
3.) Calcium ion (18 electrons): 1s22s22p63s23p6
isoelectronic with argon

22. 5.2 Ionic Bonds and Ionic Compounds

23. Ionic Bond Transfer of electrons Metal + Nonmetal
Ions come together due to electrostatic attraction (opposites attract)

24. Examples Determine if the following compounds are ionic:
NaCl : metal and nonmetal = ionic
CO2 : metal and nonmetal = not ionic

25. Practice Determine if the following compounds are ionic: 1.) CO
2.) MgCl2
3.) CaBr2
4.) H2O
5.) LiF

26. Practice Determine if the following compounds are ionic:
1.) CO = nonmetal + nonmetal = not ionic
2.) MgCl2 = metal + nonmetal = ionic
3.) CaBr2 = metal + nonmetal = ionic
4.) H2O = metal + metal = not ionic
5.) LiF = metal + nonmental = ionic

27. Ionic Bond
Na (1 valence e-) + Cl ( 7 valence e-)  Na+ ion (8 valence e-) + Cl- ion (8 valence e-):
The result is a positively charged sodium ion (left) and a negatively chorline atom (right). Both have full outer shells!
Soidum (on the left) loses its one valence electron to chlorine (on the right)

28. Crystal Lattice
Ionic compounds organize in characteristic crystal lattice of alternating positive and negative ions.
Unit Cell: The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice.
Image from:

29. Lattice Energy
When ionic bonds are formed, the energy that is released is called the lattice energy.
Alternatively, you can think of it as the amount of energy required to break the ionic bonds of a compound.

30. Examples Sodium chloride (NaCl) dissolves in water: low lattice energy
Magnesium oxide (MgO) does not dissolve in water: high lattice energy

31. Properties of Ionic Compounds
Solid at room temperature
High boiling/melting points
Dissolve in water
Conduct electricity
Hard (the crystal is able to resist a large force applied to it)
Brittle (applied force results in fracture, not dents)

32. How to Identify an Ionic Compound
1.) Identify the state of matter -should be a solid at room temperature 2.) Tap it -will not break (hard) OR -will fracture if it breaks (brittle) 3.) Heat it -will only melt at high temperatures 4.) Shock it -will conduct electricity 5.) Dissolve it in water -will dissolve in water

33. Is it Ionic?
You tap the crystal and they shatter but still retain their sharp edges.
You heat the substance and after 2-3 minutes of heating it does not melt.
It dissolves in water and conducts electricity.

34. Is it Ionic?
You tap the crystal and they shatter but still retain their sharp edges.
Yes
You heat the substance and after 2-3 minutes of heating it does not melt.
It dissolves in water and conducts electricity.

35. Is it Ionic?
You tap the crystal and they shatter but still retain their sharp edges.
Yes
You heat the substance and after 2-3 minutes of heating it does not melt.
It dissolves in water and conducts electricity.

36. Is it Ionic?
You tap the crystal and they shatter but still retain their sharp edges.
Yes
You heat the substance and after 2-3 minutes of heating it does not melt.
It dissolves in water and conducts electricity.

37. 5.3 Names and Formulas of Ionic Compounds

38. Binary Ionic Compounds
Writing Formulas
Binary Ionic Compounds

39. Ionic Compounds Metal + Nonmetal Cation = positive charge
Anion = negative charge

40. Writing Ionic Formulas
Write the symbol of the cation.
Write the charge of the cation.
Write the symbol of the anion.
Write the charge of the anion.

41. 5. Criss-cross the charges and write as subscripts without the signs. 6. Rewrite the formula. 7. Reduce the subscripts. 8. Check your answer (the compound should be neutral).

42. Examples
Sodium oxide
Aluminum sulfide
Barium chloride
Magnesium oxide

43. Examples Sodium oxide = Na2O Aluminum sulfide = Al2S3
Barium chloride = BaCl2
Magnesium oxide = MgO

44. Recall: Metals & The Stock System
The metal will have its charge listed behind its name as a roman numeral in parentheses.
Example:
Iron(III) bromide = FeBr3
Exceptions: Groups 1&2, Ag, and Zn don’t have Roman numerals because they have only one charge!

45. Examples
Copper(II) chloride
Tin(IV) iodide
Chromium(III) oxide

46. Examples Copper(II) chloride = CuCl2 Tin(IV) iodide = SnI4
Chromium(III) oxide = Cr2O3

47. Polyatomic Ionic Compounds
Writing Formulas
Polyatomic Ionic Compounds

48. Monatomic Ion
An ion made up of one atom.

49. Polyatomic Ion
A charged group of 2 or more covalently bonded atoms.

50. Writing Formulas with Polyatomic Ions
When writing the polyatomic ion, put parentheses around the formula.
When criss-crossing the charges, drop the subscript behind the parentheses.

51. NEVER change any subscripts inside the parenthesis.

52. Examples Sodium Phosphate Calcium Nitrate Magnesium Hydroxide
Potassium Sulfate
Calcium Acetate
Chromium (III) Nitrite
Magnesium Hydrogen Carbonate

53. Examples Sodium Phosphate: Na3PO4 Calcium Nitrate: Ca(NO3)2
Magnesium Hydroxide: Mg(OH) 2
Potassium Sulfate: K2SO4
Calcium Acetate: Ca(C2H3O2) 2
Chromium (III) Nitrite: Cr(NO2) 3
Magnesium Hydrogen Carbonate: Mg(HCO3)2

54. Binary Ionic Compounds
Naming Compounds
Binary Ionic Compounds

55. Naming Ionic Compounds
Write the name of the cation.
Write the name of the anion, change the ending to –ide.
Examples: RbCl = rubidium chloride
K2S = potassium sulfide

56. Examples
CaBr2
MgS
NaBr
AlP

57. Examples CaBr2 = calcium bromide MgS = magnesium sulfide
NaBr = sodium bromide
AlP = aluminum phosphide

58. Stock System for Transition Metals
Write the name of the cation.
Write the charge of the cation using a roman numeral inside of parentheses.
Write the anion, change the ending to –ide.

59. Exceptions
Metals in Groups 1 and 2, Zinc and Silver are the only metals that will not follow the stock system because they only ever have one charge.

60. Examples
CuCl2 = copper(II) chloride
FeCl2
CuBr
Cu2O

61. Examples CuCl2 = copper(II) chloride FeCl2 = iron(II) chloride
CuBr = copper(I) bromide
Cu2O = copper(I) oxide

62. Polyatomic Ionic Compounds
Naming Compounds
Polyatomic Ionic Compounds

63. Compounds with Polyatomic Ions
Name the cation.
Name the anion.
If the anion is monatomic, change the ending to –ide.
Note: Only one polyatomic ion is a cation.

64. Examples
Ca3(PO4) 2
NaOH
Ba(C2H3O2)2
MgSO4
(NH4)2S

65. Examples Ca3(PO4) 2 : Calcium Phosphate NaOH : Sodium Hydroxide
Ba(C2H3O2)2 : Barium Acetate
MgSO4 : Magnesium Sulfate
(NH4)2S : Ammonium Sulfide