Chemical Bonding and Nomenclature Chapter 5 Chemical Bonding and Nomenclature

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….

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

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

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?

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

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

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

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?

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

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

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?

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!

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

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

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

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

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:

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:

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+

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

Chapter 5 Summary Chapter 5 HW: Practice Problems: 5.10-5.18, 5.19-5.22, 5.23-5.36 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.

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

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.

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-.

5.7 Nomenclature—Naming Chemical Compounds (Continued)

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.

5.7 Nomenclature—Naming Chemical Compounds (Continued)

5.7 Nomenclature—Naming Chemical Compounds (Continued)

5.7 Nomenclature—Naming Chemical Compounds (Continued)