Period 3 Advanced Chemistry Bell Task-Make a Prediction: Using your Chemistry knowledge, order the following substances in order of increasing Boiling Points-Ne, HF, H2, BaCl2. Explain why you chose that order! Agenda- Complete Bell task Demo Dipole Moment/Calculations HW: Worksheet
Bell Task Answer- H2, Ne, HF, BaCl2 Substance Boiling Point H2 20 K Ne
Class Expectations: Collect HW more often for a grade Daily Assessments Labs-More lab technique needed Exams will be more comprehensive Study/Practice problems Weekly agenda will be given Calculate data before you leave on lab days Read lab prior to lab class! Do not "cram" the night before an unit exam-study often! See me for help when needed Let me know if there is anything else I should add to this list!
Guided Questions ·Examine the forces responsible for properties of Liquids and Solids ·What happens during transitions between s/l/g and the effects of temperature and pressure during these transitions
Solid/Liquid/Gas Characteristics
Develop the Idea of Bond Dipoles and Dipole Moment Why do some molecules and compounds exist as a solid, liquid or gas phases? Ideas???? Develop the Idea of Bond Dipoles and Dipole Moment
The iodine monobromide molecule, IBr, has a bond length of 2 The iodine monobromide molecule, IBr, has a bond length of 2.49 angstroms and a dipole moment of 1.21 D. Which atom of the molecule is expected to have a negative charge? Calculate the effective charges on the I and Br atoms in units of the electronic charge e
Period 3 Advanced Chemistry Bell Task-Science Trivia on your desk! Answer as many questions as you can within 5 minutes! Agenda- Bell task Review Dipole values - Table Types of Intermolecular forces
They are, however, strong enough to control physical properties such as boiling and melting points, vapor pressures, and viscosities. These intermolecular forces as a group are referred to as van der Waals forces.
Ion-Dipole Interactions Types of Intermolecular Forces Ion-Dipole Interactions
Ion-Dipole Interactions ·A fourth type of force, ion-dipole interactions are an important force in solutions of ions. ·The strength of these forces are what make it possible for ionic substances to dissolve in polar solvents.
occurs in polar covalent molecules as a result of neighboring partial + and partial - charges
London dispersion-occurs in all molecules and individual atoms and is a result of motion of e- London dispersion forces, or dispersion forces, are attractions between an instantaneous dipole and an induced dipole. ·These forces are present in all molecules, whether they are polar or nonpolar. ·The tendency of an electron cloud to distort in this way is called polarizability
Hydrogen bonding arises in part from the high electronegativity of nitrogen, oxygen, and fluorine. Also, when hydrogen is bonded to one of those very electronegative elements, the hydrogen nucleus is exposed.
Assessment Which IMF is present in the following (There may be multiple IMF present for each substance) 1. NH3 2. O2 3. Kr 4. CH3CH3 5. CH3OH 6. HCl 7. CCl4 8. CH3NH2 9. HF 10. H2O
Bell task Discrepant event-Using the beaker filled with water and ice, explain in detail why ice is less dense than liquid water! Agenda Bell task and review Review Van der waals forces Finish Hydrogen bonding notes Assemble CH3F and Methyl Amine (CH3NH2) Mini assessment Penny activity Viscosity and Surface Tension notes Quiz tomorrow section 10.1 through 10.4 including page 365
The hexagonal shape of a snowflake
Arrangement of H2O molecules in ice
Each hydrogen atom in one H2O molecule is oriented toward a nonbonding pair of electrons on an adjacent H2O molecule Its open arrangement optimizes the hydrogen bonds to 4 other H2O molecules-thus creating an open cavity. As solid ice melts the motion of the water molecule causes the structure to collapse.