Transcript Unit 2.2- Metallic and Covalent Bonding

Unit 2.1: Metallic and
Covalent Bonding
Bell Work October 15
Agenda:
1. Turn in Lewis Dot Structure
HW
2. Planner: Read Lab and be
ready to start tomorrow
1. Finish Pre-Lab
2. Quiz Monday
3. Bell Work
4. Notes
Bell Work:
•What types of atoms make
ionic bonds (metal,
nonmetal, metalloid)?
•Draw the Lewis Dot
Structure for GaBr3
Bell Work October 16
Agenda:
1. Place Pre-lab on Desk
2. Planner: TBD
1. Quiz Monday
3. Bell Work
4. Lab
Bell Work:
•Review your pre-lab with
the members of your table
Bell Work October 17
Agenda:
1. Planner: Lab Due Monday
1. Quiz Monday
2. Bell Work
3. Finish Lab
Bell Work:
•When are ionic
compounds conductive?
Bell Work October 20
Agenda:
1. Turn in Ionic Properties Lab
2. Planner:
3. Bell Work
4. Quiz
5. Notes
Bell Work:
•Draw the 2 Lewis Dot
structures for BaI2
•What is the name of the
Ba ion? What is the name
of the I ion? Are they
cations or anions?
Metallic Bonds
• Metals + Metals
• Electromagnetic interaction between
delocalized electrons and the metallic
nuclei within metals (electrons attracted
to metal cations)
• The sharing of “free” electrons among a
lattice of cations
• “Electron Sea”
Metallic Bonds
• Metals are very giving
Metallic Properties
• Conductive: Since electrons are in a sea, there are free flowing ions
and charges making it easy for metals to carry electrical currents
• Ductile: The ability to be pulled into thin strands or wires
• Malleable: Moldable, able to roll into thin sheets
• Shape Memory Alloys Video
Bell Work October 21
Agenda:
1. Planner:
2. Bell Work
3. Notes
4. Covalent Bonding Lewis Dot
Structure Practice
Bell Work:
Covalent Bonding
• Non-Metals + Non-metals
• SHARING of electrons so everyone is a happy octopus
• H has a full valence shell at 2 ve-, everything else needs 8 ve• The force that holds atoms together in a covalent bond is the
attraction of each atom’s nucleus for the shared pair of electrons
• Nucleus is positive, electrons are negative
Covalent Bond Practice
• H2O
• CH4
• NH3
Single Bonds, Double Bonds, and Triple Bonds
• Single Bond: 2 atoms share a pair of electrons (2 total)
• Double Bond: 2 atoms share 2 pairs of electrons (4 total)
• Triple Bond: 2 atoms share 3 pairs of electrons (6 total)
Double and Triple Bond Practice
• CO2
• CH2
• CH4
Diatomic Atoms:
• Diatomic = “2
atoms”
• These atoms do
not exist in nature
alone
• BrINClHOF
• Bromine
• Iodine
• Nitrogen
• Chlorine
• Hydrogen
• Oxygen
• Fluorine
Diatomic Lewis Structures
•Br2
•H2
•I2
•O2
•N2
•F2
•Cl2
Molecular Compound
• Molecular Compound- compound composed of molecules (covalently
bonded atoms)
• Have lower melting points, boiling points, and do not conduct
electricity when dissolved in water (unlike ionic compounds)
Melting and Boiling Points
• Covalent bonds are weaker than ionic bonds
• Melting and boiling involves breaking those bonds
• The bonds are weaker so they take less energy/heat to break
• = lower melting and boiling point