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FTCE Chemistry SAE Preparation Course

FTCE Chemistry SAE Preparation Course. Session 3. Lisa Baig Instructor. Course Outline. Session 1 Review Pre Test Competencies 1 & 2 Session 2 Competency 5 Session 3 Competency 3 Session 4 Competency 4 Session 5 Competencies 6, 7 and 8 Post Test. Session Norms. Respect

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FTCE Chemistry SAE Preparation Course

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  1. FTCE Chemistry SAEPreparation Course Session 3 Lisa Baig Instructor

  2. Course Outline Session 1 Review Pre Test Competencies 1 & 2 Session 2 Competency 5 Session 3 Competency 3 Session 4 Competency 4 Session 5 Competencies 6, 7 and 8 Post Test

  3. Session Norms • Respect • No side bars • Work on assigned materials only • Keep phones on vibrate • If a call must be taken, please leave the room to do so

  4. Homework Review Any questions from last night?

  5. Chemistry Competencies • Knowledge of the nature of matter (11%) • Knowledge of energy and its interaction with matter (14%) • Knowledge of bonding and molecular structure (20%) • Knowledge of chemical reactions and stoichiometry (24%) • Knowledge of atomic theory and structure (9%) • Knowledge of the nature of science (13%) • Knowledge of measurement (5%) • Knowledge of appropriate laboratory use and procedure (4%)

  6. Electronegativity • Fluorine is the most electronegative element. • Pattern of increasing electronegativity moves from bottom to top, and from left to right across the periodic table.

  7. Chemical Bond Mutual electrical attraction between the nuclei and valence electrons of different atoms that bind the atoms together Atoms would like to have 8 Valence electrons. These bonds help the atoms to achieve their full valence shells Three Types Ionic Covalent Metallic

  8. Force of attraction between oppositely charged ions Occurs between Metal and Non-Metal elements The Non-metal “steals” the valence electron(s) from the Metal Forms a crystalline structure of these positive and negative charges Typically solids at room temperature Ionic Bond

  9. Ionic Character • Ionic Bonds are bonds with > 50% ionic character • Difference in Electronegativity of involved atoms is >1.7

  10. Covalent Bond • Sharing of valence electron pairs by 2 atoms • Occurs between 2 Non-metal elements • Or the SAME non-metal element • Can share one, two or three pairs of electrons • Single Bond = 1 pair (1 sigma) • Double Bond = 2 pairs (1 sigma, 1 pi) • Triple Bond = 3 pairs (1 sigma, 2 pi) • Sharing can also be “unequal” • Called a POLAR covalent bond • Typically liquids or gases at room temperature

  11. Character • Ionic Character: • Polar Covalent Bonds have between 5% and 50% ionic Character • Non-Polar Covalent Bonds have less than 5% ionic character • Difference in Electronegativities • Polar Covalent Bonds have between 0.3 and 1.7 as a difference in electronegativities • Non-Polar Covalent bonds have less than 0.3 difference in electronegativities

  12. Break Time Take a 10 minute break

  13. Ionic Compounds • Ion names are used in combination • Cation- same as the element • Transitional Metals use Roman Numerals to represent Charge • Anion- replace the ending syllable of the element name with –ide • Polyatomic Ions- use the name of that ion- do not try to rename. Use “criss-cross” to determine charges

  14. CuCl2 Copper (II) Chloride CuO Copper (II) Oxide NaCl Sodium Chloride KI Potassium Iodide Mg3N2 Magnesium Nitride PbO2 Lead (IV) Oxide

  15. Lewis Structures • A way to show the octet rule in molecules

  16. Practice • Draw the lewis structures for • Ammonia (NH3) • Water (H2O) • Phosphorus Trifluoride (PF3) • Hydrogen Cyanide (HCN) • Ozone (O3) • Formaldehyde (CH2O)

  17. VSEPR • AB5 • Trigonal bipyramidal • AB6 • Octahedral

  18. VSEPR • AB4 • Tetrahedral • 109.50 Bond Angles • AB3 • Trigonal Planar • 1200 Bond Angles • AB2 • Linear • 1800 Bond Angles

  19. VSEPR • AB2E • Bent or Angular • AB2E2 • Bent or Angular • AB3E • Trigonal Pyramidal

  20. Polarity? • The potential for opposite charges at different areas of a molecule

  21. Shape and Polarity? • What is the shape and polarity of the following molecules? • Water • Ammonia • Carbon Tetrachloride • Carbon Dioxide • Hydrogen Chloride

  22. Hybrids • Atoms “don’t like” to have empty orbitals • Hybridization • Mixing of 2 or more atomic orbitals of similar energies to produce new hybrid orbitals of equal energies • It works like this • Methane: CH4 Normally: 1s22s22p2 • Through hybridization- it forms an “sp” orbital, with 4 electrons total • New arrangement: 1s22(sp3) 4

  23. Hybrid Orbitals

  24. What type of hybrid? • Beryllium fluoride • BeF2 • sp • Ammonia • NH3 • sp2 • Methane • CH4 • sp3

  25. Break Time Take a 10 minute break

  26. Spectroscopy • Devices that measure the interaction between matter and energy • Absorption • Measures the wavelengths of electromagnetic waves absorbed by a substance • X-Ray spectroscopy • Used to determine elemental composition and types of bonding

  27. Spectroscopy • UV • Used to quantify DNA and Protein concentration • Infrared • Used to determine bond type • Bonds resonate when exposed to the radiation • Nuclear Magnetic Imaging (NMR) • Used to determine bond structure

  28. Simple Organics • Alkanes (end in –ane) • Containing only single bonds • CnH2n+2 • Alkenes (end in –ene) • Containing at least one double bond • CnH2n • Alkynes (end in –yne) • Containing at lease one triple bond • CnH2n-2

  29. Simple Organics

  30. Functional Groups

  31. Naming and Formulas • Numbers are used in the name to designate locations of the following • Types of bonds • Branches • Attached functional groups • For Example • 2,2,4- trimethylpentane • 1-pentyne • 2,3,4- trimethylnonane • 2-methyl 3-hexene • 2- propanol

  32. Macromolecules • Carbohydrates • Chains of carbon, hydrogen and oxygen. • Isomers • Lipids • Fatty acids- Chains of Carbon and Hydrogen • Proteins • Chains of Amino acids • Differ in their R group • Nucleic Acids • Chains of Nucleic Acids

  33. Organic Compound Naming • Numbers are used in the name to designate locations of the following • Types of bonds • Branches • Attached functional groups • For Example • 2,2,4- trimethylpentane • 1-pentyne • 2,3,4- trimethylnonane • 2-methyl 3-hexene • 2- propanol

  34. Homework • Diagnostic Exam in your AP Chem Prep book- Page 17-26 • Only answer the questions for these Chapters & Questions • Chapter 5 #1,3 • Chapter 11 #41-43, 46 • Chapter 18, #86

  35. Bibliography • VSEPR Theory GIF’s • Rindge, R. (Artist). (1998). Shapes of molecules. [Web]. Retrieved from http://chemmybear.com/shapes.html

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