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