Chapter 5

• Focus on slides 31 to end.

• Be sure you understand the information and are able to complete the activities on slides 35, 43, 44, 46, 53, 57, 62, 63, 64

• You will be asked to draw out orbital diagrams and electron configurations.

• You must understand the concept of valance electrons.

Write the orbital diagrams for

1. Nitrogen

1s 2s 2p 3s 3p

2. Oxygen

1s 2s 2p 3s 3p

3. Magnesium

1s 2s 2p 3s 3p

Learning Check

Chapter 6

• Rule of 8, the octet• Using arrows show the exchange or sharing of

electrons to form compounds. see the following slides

• Study the naming of ionic and covalent compounds from the formulas and writing formulas from compound names

• Memorize the names and formulas for the polyatomic ions and how to use them to write formulas and compound names

• The formulas of ionic compounds are determined from the charges on the ions.

atoms ions –

Na + F : Na+ : F : NaF

sodium fluorine sodium fluoride

The overall charge of NaF is zero (0).

Na+ F- = NaF

(1+ ) + (1-) = 0

Charge Balance in NaF

Using Lewis Electron Dot Symbols

Br

Ca + →

Br

Using Lewis Electron Dot Symbols

Al + N →

Writing Ionic Formulas from Charges

Charge balance is used to write the formula for

sodium nitride, a compound containing Na+ and

N3−.

Na+

3 Na+ + N3− = Na3N

Na+

3(+1) + 1(3-) = 0

Note: the subscript 3 for three sodium ions.

Charges of Representative Elements

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Formula Ions Name

NaCl Na+ Cl- sodium chloride

K2S K+ S2- potassium sulfide

MgO Mg2+ O2- magnesium oxide

CaI2 Ca2+ I- calcium iodide

Al2O3 Al3+ O2- aluminum oxide

Some Ionic Compounds with Two Elements

More Ionic Compounds

Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

Nick the Camel Craved and ate a Clam Supper in Phoenix.

Molecular Geometries or Shapes

• Be able to draw out electron dot foumulas for simple covalent compounds like those in your lecture notes.

• Know how to use the table of electronegativities.• Be able to distinguish between ionic bonding,

covalent bonding, hydrogen bonding, dipole dipole or polar bonding, and non polar dispersion forces of attraction.

• Be able to use arrows to describe the dipole in a polar molecule.

• For Chapter 8 see the items listed on the study guide.