1. Chapter 8 Ionic Compounds
I. Forming Chemical Bonds – How do Compounds Form?
Why do atoms form bonds?
Stability
Like the noble gases, every element wants to be inert
Not a nerd

2. I. Why do atoms form bonds?
Chemical Bond - strong attractive force between atoms or ions in a compound.
stability - goal is to reach the most energetically favorable condition
bond energy - energy involved in process of bond forming or bond breaking
Valence Electrons outermost electrons

3. Highest Energy Level
Valence Electrons?
3s23p6

4. How do you represent Valence Electrons?
Watch the video clip and fill in examples that you can in your notes

6. 1. What is the atomic number of this element?
How do you represent Valence Electrons?
Electron Dot Structures Video Clip
1.       What is the atomic number of this element?
2.       Write the electron configuration.
3.       Identify just the valence electrons (hint use the “A” roman numerals on the periodic table).

7. 4. Write the symbol for the element.
How do you represent Valence Electrons? Electron Dot Structures
4.       Write the symbol for the element.
5.       Use a dot for each valence electron. s orbitals on one side p orbitals on remaining three sides of element.
Try these examples:
Li B N F Be C O Ne

8. 1. shows valence electrons, for example lets try these……
Li B N F Be
C O Ne
Valence electron

9. Stable Octet (new words, octet rule): 8 electrons in valence shell, stable configuration

10. II. Ionic Bonding: process by which one or more electrons are transferred from the valence shell of one atom to the valence shell of another atom. (usually forms salts)

11. 3s1
3p5
Unstable
3s2
Electons Transferred = ionic bond
full octets
Electrostatic attraction
Stable
11P+
17P+
10e-
18e-
1+charge
1- charge

12. Ionic Bonding

13. 8.3. Names and Formulas for Ionic Compounds (8.3 pgs. 221-227)
A. Formulas tell: 1. which elements make up the compound (qualitative) 2. ratios of atoms contained (quantitative)
H2O
Hydrogen & Oxygen in element
# of H’s and O’s in molecule

14. B. Made from a metal + a nonmetal
1. metals form (+) ions - cations
2. nonmetals form (-) ions - anions

15. C. Using ion charge to write formulas
1. write the chemical symbol
2. using the periodic table assign a charge
(to be written as a subscript)
Group IA, IIA, IIIA, VA, VI, VIIA

16. 4. when subscripts are equal they reduce to 1
3. add charges together to equal zero, use charge of one ion as subscript for the other ion, or use criss-cross method
4. when subscripts are equal they reduce to 1
5. for polyatomics (more than one atom combined that has an overall charge)
use parenthesis when subscript is 2 or more

17. examples:
Calcium chloride
Ca2+
+ Cl1- + Cl1- = 0
CaCl2

18. examples: MgS +Al3+ + O2- + O2- + O2- = 0 Al3+ Al2O3 Mg2+ S2- CaCl2
Calcium chloride
Aluminum oxide
Magnesium sulfide
CaCl2
+Al3+
+ O2- + O2- + O2- = 0
Al3+
Al2O3
Mg2+
S2-
MgS

19. examples:
Magnesium phosphate
Mg PO43- 3 2
Mg3(PO4)2

20. examples: Ba2+ SO2- NH41+ Cl1- Ammonium chloride BaSO4 NH4Cl
Barium sulfate
Ammonium chloride
BaSO4
Ba2+
SO2-
NH41+
Cl1-
NH4Cl

21. D. Naming ionic compounds
1. binary compounds - two different kinds of atoms
a. name the first element
b. name the second element, drop the last syllable, add -ide.

22. examples:
Na2S =
MgO =
Sodium Sulfide
Magnesium Oxide

23. Naming ternary compounds
2. ternary compounds - name the first element, then name the polyatomic ion

24. examples:
Ca(NO3)2 =
Na2SO4 =
Calcium Nitrate
Sodium Sulfate

25. E. atoms that form more than one type of ion
(examples: Cu, Fe, Hg, Pb, Sn)
1. old system - call the ion with the greater charge -ic, and the ion with the lesser change -ous. (use Latin names as roots)

26. Old System Cu+2 cupric CuF2 cupric fluoride
Cu+1 cuprous CuF cuprous fluoride
Cu+2 cupric CuF2 cupric fluoride
Fe+2 ferrous FeF2 ferrous fluoride
Fe+3 ferric FeF3 ferric fluoride

27. New System – Stock System
2. new system (or stock system), name ion by atom. The name is followed by roman numeral telling its charge.

28. New System – Stock System
Cu+1 copper(I)
CuF copper (I) fluoride
Cu+2 copper(II)
CuF2 copper (II) fluoride
Fe+2 Iron(II) FeF2 iron (II) fluoride
Fe+3 Iron(III) FeF3 iron (III) fluoride

29. Crystal Lattice- three dimensional arrangement of cations & anions
III. Properties of Ionic Compounds:
Crystal Lattice- three dimensional arrangement of cations & anions
List Properties here
Crystal shape
Hard & brittle
High melting pt
High boiling pt
When dissolved,
or molten, conducts
electricity

30. Properties of Ionic Solids

31. Electrons transferred = ionic bond
Electrostatic Attraction

32. Crystal shape
Unit cell – simplest, repeating unit

33. IV. Energy and the Ionic Bond:
During any chemical or physical reaction energy is neither created or destroyed
Energy that is absorbed is called endothermic
Energy that is release is called exothermic
The formation of ionic compounds from positive and negative ions is always exothermic. The compound formed is more stable and of lower energy.

34. IV. Energy and the Ionic Bond:
The energy required to separate one mole of the ions of an ionic compound is referred to as the lattice energy.
The more negative the lattice energy, the stronger the force of attraction.
Which would have more negative lattice energy, lithium chloride or lithium bromide?
Lithium chloride
MgO is almost four times greater then the lattice energy of NaF, why?
MgO, charge of the ions is greater

35. V. Names and Formulas for Ionic Compounds(8. 3 pgs
V. Names and Formulas for Ionic Compounds(8.3 pgs )(see previous notes)
Describe a Pot of Gold (physical and chemical properties of the pot and the gold coins)
High luster High Melting/Boiling Pt. Malleable Ductile Solid Conductive

36. VI. Metallic Bonds and Properties of Metals (8.4 pgs. 228-231)
Metals form a lattice with eight to 12 other metal atoms surrounding each metal atom.
metals have at least one valence electron, they do not form ions or share their electrons
metals are crowded with electrons and the outer energy levels of the metal atoms overlap

37. VI. Metallic Bonds and Properties of Metals (8.4 pgs. 228-231)
The electron sea model proposed that all the metal atoms in a metallic solid contribute their valence electrons dot form a “sea” of electrons.

38. Electrons are not held tightly by any specific atom, electron are free to move around and are referred to delocalized electrons.

39. The attraction of a metallic cation for delocalized electrons is called a metallic bond.

40. Properties of Metallic Bonding

41. III. How do you name Salts?
A. Formulas tell: 1. which elements make up the compound (qualitative) 2. ratios of atoms contained (quantitative) H2O

42. B. Made from a metal + a nonmetal
1. metals form (+) ions - cations
2. nonmetals form (-) ions - anions

43. C. Using ion charge to write formulas
1. write the chemical symbol
2. using the periodic table assign a charge
(to be written as a subscript)
Group IA, IIA, IIIA, VA, VI, VIIA

44. 4. when subscripts are equal they reduce to 1
3. add charges together to equal zero, use charge of one ion as subscript for the other ion, or use criss-cross method
4. when subscripts are equal they reduce to 1
5. for polyatomics (more than one atom combined that has an overall charge)
use parenthesis when subscript is 2 or more

45. examples: CaCl2 Mg3(PO4)2 Al2O3 BaSO4 MgSO4 NH4Cl
Calcium chloride Magnesium phosphate
Aluminum oxide Barium sulfate
Magnesium sulfide Ammonium chloride
CaCl2
Mg3(PO4)2
Al2O3
BaSO4
MgSO4
NH4Cl