1. …electrons are transferred
Ionic Bonding
…electrons are transferred

2. Guiding Questions? What is that?
How do we figure out what the chemical formula is?
What does it mean to be "free of chemicals"?
Chemical formulas can be predicted from the periodic table and allow chemists to classify and predict properties of compounds
The general trend in the universe to strive for lower energy explains and allows for prediction of chemical properties of elements
Elements combine in whole number ratios and these molar ratios can be used to determine chemical formulas
More Specifically...:
Bonding Model
Use physical and chemical properties to distinguish between ionic and covalent compounds
Describe energy changes as elements combine to form an ionic compound
Describe ionic bonding as the transfer of electrons and the formation of a crystal lattice due to electrostatic attraction between ions of opposite charge
Predict the formation of cations and anions based on placement on periodic table
Relate formation of anion or cation with ionization energy and electron affinity
State that bonding occurs to increase stability
Contrast metallic and ionic bonding
Nomenclature and formulas
Learn the names and formulae of common anions and cations, including carbonate, sulfate, nitrate, hydroxide, phosphate, and ammonium
Write chemical formulas for ionic compounds given
a. Name of compound or
b. A pair of ions
Identify polyatomic ions
Classify compounds as being ionic or covalent.
Name ionic compounds using stock system (Roman numerals)
Math
Calculate molecular mass
Use dimension analysis to convert between moles, grams, atoms, ions and molecules

3. Keeping Track of Electrons
The electrons responsible for the chemical properties of atoms are those in the outer energy level.
Valence electrons - The s and p electrons in the outer energy level.
Core electrons -those in the energy levels below.

4. Keeping Track of Electrons
Atoms in the same column
Have the same outer electron configuration.
Have the same valence electrons.
Easily found by looking up the group number on the periodic table.
Group 2A - Be, Mg, Ca, etc.-
2 valence electrons

5. X Electron Dot diagrams A way of keeping track of valence electrons.
How to write them
Write the symbol.
Put one dot for each valence electron
Don’t pair up until they have to X

6. The Electron Dot diagram
for Nitrogen
Nitrogen has 5 valence electrons.
First we write the symbol. N
Then add 1 electron at a time to each side.
Until they are forced to pair up.

7. Write the electron dot diagram forNa
1s22s22p63s1 Na Mg C O F Ne He Mg
1s22s22p63s2 C
1s22s22p2 O
1s22s22p4 F
1s22s22p5 Ne
1s22s22p6 He
1s2

8. Electron Configurations for Cations
Metals lose electrons to attain noble gas configuration.
They make positive ions.
If we look at electron configuration it makes sense.
Na 1s22s22p63s1 - 1 valence electron
Na+ 1s22s22p6 -noble gas configuration

9. Electron Dots For Cations
Metals will have few valence electrons
These will come off
Forming positive ions Ca
40.078 20
1s22s22p63s2 Ca +2

10. Electron Configurations for Anions
Nonmetals gain electrons to attain noble gas configuration.
They make negative ions.
If we look at electron configuration it makes sense.
S 1s22s22p63s23p4 - 6 valence electrons
S-2 1s22s22p63s23p6 -noble gas
configuration.
(anions)

11. Electron Dots For Anions
Nonmetals will have many valence electrons.
They will gain electrons to fill outer shell. P
P-3

12. Stable Electron Configurations
All atoms react to achieve noble gas configuration.
Noble gases have two s and six p electrons.
Eight valence electrons .
Also called the octet rule. Ar

13. Ionic Bonding
Anions and cations are held together by opposite charges.
Ionic compounds are called salts.
Simplest ratio is called the formula unit.
The bond is formed through the transfer of electrons.
Electrons are transferred to achieve noble gas configuration.

14. Ionic Bonding
transfer of electron + - Na Cl
NaCl

15. Ca +2 Ca P -3 +2 Ca P -3 +2 Ionic Bonding
All the electrons must be accounted for!

16. Ca2+ Ca3P2 Ca2+ P3- Ca2+ P3- Ionic Bonding Formula Unit Ca2+ P3- Ca2+

17. Properties of Ionic Compounds
Crystalline structure.
A regular repeating arrangement of ions in the solid.
Ions are strongly bonded.
Structure is rigid.
High melting points- because of strong forces between ions.

18. Crystalline structure

19. Do they Conduct? Conducting electricity is allowing charges to move.
In a solid, the ions are locked in place.
Ionic solids are insulators.
When melted, the ions can move around.
Melted ionic compounds conduct.
First get them to 800ºC.
Dissolved in water they conduct.

20. Metallic Bonds How atoms are held together in the solid.
Metals hold onto there valence electrons very weakly.
Think of them as positive ions floating in a “sea of electrons”.

21. + Sea of Electrons Electrons are free to move through the solid.
Metals conduct electricity. +

22. + + + + + + + + + Metals are Malleable Hammered into shape (bend).
Ductile - drawn into wires.
Electrons allow atoms to slide by. + + + + + + + + +

23. Ionic solids are brittle
Strong repulsion breaks crystal apart. + -
Force + - + - + - + -