1. Unit 3 Bonding & Chemical Rxns

2. OBJECTIVES SWBAT:
Identify the properties of ionic, covalent, and metallic bonds.
Write the name of ions.
Name ionic compounds given their formulas.
Write the formula of ionic compounds given their names.

3. Notes #1: Types of Bonding Ionic Bonding
Electrostatic force between a cation (positive ion, metal) and an anion(negative ion, non- metal) created by the transfer of electrons.

4. Sodium Chloride Lattice Structure
Examples
NaCl - Sodium Chloride
CaO - Calcium Oxide

5. Ionic Bonding
Ionic compounds form from ions. Ions are created when a metal loses electrons and a non-metal gains electrons.

6. Ionic Bonding
Ionic substances form giant ionic lattices containing positive and negative charged ions.

7. Ionic Bonding
They have high melting and boiling points because the intermolecular forces are very strong.

8. Ionic Bonding
They conduct electricity when melted or dissolved in water.

9. Covalent Bonding
Bonds form between nonmetal atoms. The nonmetals are connected by the sharing of valence electrons.

10. Covalent Bonding
Covalent bonds are overlapping; that is, they are inside the molecule and hold the atoms together to make the molecule.

11. Valence electrons are shared when orbitals over lap each other.

12. Covalent Bonding
Covalent bonds are strong bonds and it is difficult and requires a lot of energy to break a molecule apart into its atoms.  However, since molecules are neutral one molecule does not have a strong electrical attraction for another molecule.  

13. Electrolysis is sending a high voltage current through water.

14. Covalent Bonding
The attractions between molecules are called intermolecular and these are weak forces.

15. Hydrogen bonding is a type of intermolecular force.

16. Covalent Bonding
Some nonmetals never exist as single atoms, they exist as diatomic elements.  This means they are covalently bonded to another atom of itself.

17. Diatomic Molecules
Hydrogen: H-H Nitrogen: N-N
Oxygen: O-O Fluorine: F-F
Chlorine: Cl-Cl Bromine: Br-Br
Iodine: I-I

18. Covalent Bonding
Covalent substances have Low melting points and boiling points because the intermolecular forces are weaker than in ionic compounds and metals

19. Covalent Bonding
At room temperature, covalent substances can be solids, liquids or gases.

20. States of matter for covalent bonds
Solid
Liquid
Gas

21. Covalent Bonding
Do not conduct electricity as solids or when molten and usually do not conduct when dissolved in water.

22. Metallic Bonding
Metallic bonding is found in elemental metals and in mixtures of metals called alloys.

23. Metallic Bonding
Delocalized Sea of Electrons allow for the properties of metals
Examples:
Copper
Steel
Brass
Silver
Gold

24. Common Alloys

25. Metallic Bonding
The electrical attractions of the cations for the electrons are strong and hard to break so metals have high melting points and form crystalline solids.

26. Metallic Bonding
The electrical attractions of the cations for the electrons are strong and hard to break so metals have high melting points and form crystalline solids.

27. Because the electrons are free to move metals are Terminator
Good Conductors
Exist as Solids
Exist as Liquids