1. Chemical Bonding and Nomenclature
Chapter 5
Chemical Bonding and Nomenclature

2. 5.1 Ionic Bonding Quick Review!
Explain the formation of NaCl from Na and Cl atoms with respect to how many electrons are exchanged, what forms and how they form a compound….

3. 5.1 Ionic Bonding (Continued)
Ionic compounds
How are ionic compounds formed?
What is the relative strength of these bonds?

4. 5.1 Ionic Bonding (Continued)
Ionic bond- between ions of opposing charges
What types of elements?
What’s a lattice?
Lattice types:

5. 5.1 Ionic Bonding (Continued)
What are the properties of ionic compounds?
What is lattice energy and how does it affect melting point of ionic compounds?

6. 5.1 Ionic Bonding (Continued)
Other Ionic Compound Properties
What is cleaving and why can it happen in ionic compounds?

7. 5.2 Molecules—What Are They?
Molecule : What are they?
What are molecular substances?

8. 5.3 Holding Molecules Together— The Covalent Bond
What happens in a covalent bond?
How is it different than an ionic bond?

9. 5.3 Holding Molecules Together— The Covalent Bond (Continued)
What are three ways to show covalent bonding in a hydrogen molecule?
How does covalent bonding satisfy each hydrogen atom’s need for electrons?

10. 5.4 Molecules, Dot Structures, and the Octet Rule
What’s this chart all about?

11. 5.4 Molecules, Dot Structures, and the Octet Rule (Continued)
How does covalent bonding satisfy each atom’s need for electrons?

12. 5.4 Molecules, Dot Structures, and the Octet Rule (Continued)
Octet rule and Lewis dot structures
How do Lewis structures show an atoms need for electrons?
How do Lewis structures show how covalent bonding makes atoms obey the octet rule?

13. Steps to draw a molecular dot diagram:
5.5 Part 2 Multiple Bonds
Steps to draw a molecular dot diagram:
Determine total number of valence electrons.
Connect atoms with a single bond.
Place remaining electrons as lone pairs.
First on terminal atoms, then the central atom
If each atom does not have an octet, change lone pairs to bonding pairs.
This is the easiest way to draw the Lewis structure for any molecular compound!

14. 5.5 Multiple Bonds Diatomic Oxygen
Draw Lewis structures for each atom and the diatomic oxygen molecule…

15. 5.5 Multiple Bonds (Continued)
Differentiate among the different bond types:
Single:
Double:
Triple:

16. 5.5 Multiple Bonds (Continued)
Draw the dot diagrams for the ethylene (C2H4) and acetylene molecules C2H2

17. 5.5 Multiple Bonds (Continued)
Draw the dot diagram for the carbon dioxide molecule, CO2

18. 5.5 Multiple Bonds (Continued)
Resonance Structures
Valid dot diagrams that differ by electron placement
Each is correct, but one is usually more common
Draw resonance structures for CO2:

19. Lewis Structures for Ions
5.5 Ion Structures
Lewis Structures for Ions
Atoms with too few or too many electrons
Draw the correct number of dots to fit the ions’ charge…
Draw Sodium and chloride ions below:

20. 5.5 Ion Structures Polyatomic ions
Ions made up of multiple nonmetal atoms
Account for the charge with the correct number of electrons…
Draw the Lewis structure for ammonium, NH4+

21. 5.5 Ion Structures Polyatomic ions
Draw the Lewis structure for carbonate, CO32-

22. Chapter 5 Summary
Chapter 5 HW:
Practice Problems: , ,
Summarize the naming of ionic and molecular compounds that we learned in lab.
You must also know how to draw Lewis structures and figure out molecular geometry
Complete the practice worksheets for naming and drawing Lewis structures.

23. 5.7 Nomenclature—Naming Chemical Compounds
Binary compound naming
Compound made of only two elements
Binary ionic compounds—comprised of a metal and a nonmetal
Binary covalent compounds—comprised of two nonmetals or metalloids

24. 5.7 Nomenclature—Naming Chemical Compounds (Continued)
Naming binary ionic compounds
Metal is considered the cation.
Written as element name
Nonmetal is the anion.
Add suffix –ide to the elemental name.

25. 5.7 Nomenclature—Naming Chemical Compounds (Continued)
Transition metals
Can carry multiple charges
Use roman numeral to show charge
Iron (II) chloride is Fe2+ and Cl-.
Iron (III) chloride is Fe3+ and Cl-.

26. 5.7 Nomenclature—Naming Chemical Compounds (Continued)

27. 5.7 Nomenclature—Naming Chemical Compounds (Continued)
Naming binary covalent compounds
Use prefixes to indicate how many atoms of each types are present.
Mono- prefix is left off if only one atom of least electronegative element is present.

28. 5.7 Nomenclature—Naming Chemical Compounds (Continued)

29. 5.7 Nomenclature—Naming Chemical Compounds (Continued)

30. 5.7 Nomenclature—Naming Chemical Compounds (Continued)