1. IONIC COMPOUNDS

2. Sec 8.1 Forming Chemical Bonds
The force that holds atoms together is a chemical bond
Valence electrons are involved in chemical bonds

3. Elements tend to react to acquire the stable electron structure of a noble gas (octet rule)

4. Formation of Positive Ions
Positive ions form when an atom loses one or more valence electrons in order to obtain a noble gas formation

5. A cation is a positive ion

6. Formation of Negative Ions
Negative ions form when an atom gains one or more valence electrons in order to obtain a noble gas formation

8. An anion is a negative ion formed when an atom gains one or more valence electrons

11. 1. a force that holds two atoms together
2. Atoms gain more stable electron configurations by losing or gaining electrons.
3. Noble gases are relatively unreactive because they have eight electrone I n their outermost energy
level, which is a stable configuration.
4. Positive ions form when atoms lose valence electrons. Negative ions form when valence electrons
are added to an atom.
5. a. gain 3 electrons (3- ion) or lose 5 electrons (5+ ion)
b. gain 2 electrons (2- ion)
c. lose 2 electrons (2+ ion)
d. lose 1 electron (1+ ion)
6. Models should show that the calcium atom loses two electrons forming Ca+2 and the bromine atom
gains one atom forming Br-

12. Section 8.2 The Formation and Nature of Ionic Bonds
Formation of an Ionic Bond An ionic bond is usually between a metal cation and a non-metal anion

13. Formation of an Ionic Bond
The electrostatic force that holds oppositely charged particles together in an ionic compound is called an Ionic Bond

14. Formation of an Ionic Bond
Compounds that contain ionic bonds are called ionic compounds.
Ionic bonds that occur between metals and the non metal oxygen are called oxides

15. Formation of an Ionic Bond
 Most other ionic compounds are called salts

16. Formation of an Ionic Bond
In an ionic bond the number of electrons lost must equal the number of electrons gained, Consider Ca and F

17. Formation of an Ionic Bond
In an ionic bond the number of electrons lost must equal the number of electrons gained,

18. Ionic Compounds

19. Ionic Compounds
Binary Ionic Compounds- contain only two different elements (one metallic cation and one nonmetallic anion).

20. Ionic Compounds Most ionic compounds are binary
MgO is binary, CaSO4 is not binary Why?

21. Properties of Ionic Compounds
The chemical bonds that occur between the atoms in a compound determine many of the physical and chemical properties.

22. Crystal Lattice
The strong attraction of positive and negative ions in an ionic compound result in a 3 dimensional geometric arrangement of particles called a crystal lattice.

23. Crystal Lattice

24. Melting point, Boiling Point, Hardness and Color
Ionic compounds generally have high melting points and boiling points.

25. Electrolyte
 An ionic compound whose aqueous solution conducts electric current is called an electrolyte

26. Lattice Energy
The formation of ionic compounds from positive and negative ions is always exothermic.

27. Lattice Energy
If this amount of energy is added to an ionic compound, the bonds will break. The energy required to separate one mole of the ions of an ionic compound is referred to as the Lattice Energy

28. 7. Na3N Al2S3
8. Li2O Cs2P
9. SrF2

30. 12. the electrostatic attraction between oppositely charged ions
13. Ions form from electron transfer. Oppositely charge electrons attract.
14. exist as crystals, high BP and MP, hard, rigid, conductive when dissolved or molten but not solid.
15. Each ion is surrounded by oppositely charged ions.
16. It is the energy required to separate the ions of an ionic compound and is the energy given off when positive and negative ions attract.
17. As the ionic radius of the non-metallic ion increases, the melting point and lattice energy decrease.
18. SrCl2

31. Section 8.3 Names and Formulas of Ionic Compounds
Formula Unit
The simplest ratio of the ions represented in an ionic compound.

32. Section 8.3 Names and Formulas of Ionic Compounds
Monatomic Ion
a one-atom ion, such as Mg+2 or Br-

33. Names and Formulas of Ionic Compounds
Most transition metals and some of those 3A and 4A can form several different positive ions

34. Names and Formulas of Ionic Compounds
Oxidation Number
The charge of a monatomic ion is its oxidation number. (sometimes called oxidation state)   

35. The oxidation numbers of ions are used to determine the formulas for the ionic compounds they form.

36. Writing Formulas Criss cross the oxidation numbers
Reduce subscripts if possible

38. Polyatomic Ions
Many ionic compounds contain polyatomic ions, which are ions made up of more than one atom.
The charge given to a polyatomic ion applies to the entire group of atoms.

39. Polyatomic Ions The polyatomic ion acts as an individual ion.
The chemical formula can be written following the same rules as monatomic ions

40. Polyatomic Ions
If more than one polyatomic ion is needed, place parentheses around the ion and write the appropriate subscript outside the parentheses.
EX Mg(ClO3)2

42. Naming Ionic Compounds
  Rules:
1. Name the cation first and the anion second 
2. Monoatomic cations use the element.
3. Monoatomic anions take their name from the root of the element name plus the suffix -ide.  
4. Group 1A and 2A metals have only one oxidation number. Transition metals and metals on the right side of the periodic table often have more that one oxidation number. the name and chemical formula (written as a roman numeral in parentheses after the name of the cation).
5. If the compound contains a polyatomic ion, simply name the ion.

43. Naming Ionic Compounds
  Rules:
1. Name the cation first and the anion second 
2. Monoatomic cations use the element.
3. Monoatomic anions take their name from the root of the element name plus the suffix -ide.  
4. Group 1A and 2A metals have only one oxidation number. Transition metals and metals on the right side of the periodic table often have more that one oxidation number. the name and chemical formula (written as a roman numeral in parentheses after the name of the cation).
5. If the compound contains a polyatomic ion, simply name the ion.

44. Naming Ionic Compounds
  Rules:
1. Name the cation first and the anion second 
2. Monoatomic cations use the element.
3. Monoatomic anions take their name from the root of the element name plus the suffix -ide.  
4. Group 1 and 2 metals have only one oxidation number. Transition metals and metals on the right side of the periodic table often have more that one oxidation number. the name and chemical formula (written as a roman numeral in parentheses after the name of the cation).
5. If the compound contains a polyatomic ion, simply name the ion.

46. Old, classic or common nomenclature
Suffix “ic” added to the Latin name of the element with the higher oxidation number.
Suffix “ous” added to the Latin name of the element with the lower oxidation number.

47. Section 8.4 Metallic Bonds and
 the attraction of a metallic cation for delocalized electrons

48. Section 8.4 Metallic Bonds and Properties of Metals
Electron Sea Model
 proposes that all metal atoms in a metallic solid contribute their valence electrons to form a “sea of electrons” that are not held by any specific atom and can easilly move from one atom to the next.

49. Section 8.4 Metallic Bonds and Properties of Metals  
Delocalized Electrons
 Because they are free to move, these electrons are called delocalized electrons.

50. Section 8.4 Metallic Bonds and Properties of Metals
Metal alloys 
Form when a metal is mixed with one or more other elements.

51. Section 8.4 Metallic Bonds and Properties of Metals  
Metallic Bond
Electron Sea Model
Delocalized Electrons
Properties of metals
Metal alloys 

52. 24. NaNo K2CrO4
25. Ca(Clo3) MgCO3
26. Al2(CO3)3

53. 29. sodium bromide 32. copper (II) nitrate
30. calcium chloride silver chromate
31. potassium hydroxide

58. Hydrate Lab

59. Hydrate Lab

61. Barium Chloride di hydrate
hygroscopic.