ftce chemistry sae preparation course session 3 lisa baig instructor
TRANSCRIPT
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FTCE Chemistry SAEPreparation Course
Session 3
Lisa BaigInstructor
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Course OutlineSession 1
Review Pre TestCompetencies 1 & 2
Session 2Competency 5
Session 3Competency 3
Session 4Competency 4
Session 5Competencies 6, 7 and 8
Post Test
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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
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Homework Review
Any questions from last night?
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Chemistry Competencies
1. Knowledge of the nature of matter (11%)2. Knowledge of energy and its interaction with
matter (14%)
3. Knowledge of bonding and molecular structure (20%)
4. Knowledge of chemical reactions and stoichiometry (24%)
5. Knowledge of atomic theory and structure (9%)6. Knowledge of the nature of science (13%)7. Knowledge of measurement (5%)8. Knowledge of appropriate laboratory use and
procedure (4%)
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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.
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Chemical BondMutual 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 TypesIonic
CovalentMetallic
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Ionic Bond• 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
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Ionic Character
• Ionic Bonds are bonds with > 50% ionic character
• Difference in Electronegativity of involved atoms is >1.7
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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
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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
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Break Time
Take a 10 minute
break
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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
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CuCl2
Copper (II) ChlorideCuO
Copper (II) OxideNaCl
Sodium ChlorideKI
Potassium IodideMg3N2
Magnesium NitridePbO2
Lead (IV) Oxide
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Lewis Structures
• A way to show the octet rule in molecules
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Practice
• Draw the lewis structures for– Ammonia (NH3)
– Water (H2O)
– Phosphorus Trifluoride (PF3)– Hydrogen Cyanide (HCN)– Ozone (O3)
– Formaldehyde (CH2O)
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VSEPR
•AB5
•Trigonal bipyramidal
•AB6
•Octahedral
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VSEPR• AB4
– Tetrahedral– 109.50 Bond Angles
• AB3– Trigonal Planar– 1200 Bond Angles
• AB2– Linear– 1800 Bond Angles
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VSEPR• AB2E
– Bent or Angular
• AB2E2
– Bent or Angular
• AB3E– Trigonal Pyramidal
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Polarity?
• The potential for opposite charges at different areas of a molecule
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Shape and Polarity?
• What is the shape and polarity of the following molecules?– Water– Ammonia– Carbon Tetrachloride– Carbon Dioxide– Hydrogen Chloride
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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
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Hybrid OrbitalsAtomic Orbitals
Type of Hybrid
Number of
Orbitals
MolecularGeomet
rys p sp 2 1800
Linear
s p p sp2 3 1200
Trigonal Planar
s p p p sp3 4 109.50
Tetrahedral
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What type of hybrid?
• Beryllium fluoride– BeF2
– sp• Ammonia
– NH3
– sp2
• Methane– CH4
– sp3
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Break Time
Take a 10 minute
break
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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
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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
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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
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Simple OrganicsName Number of Carbons
Meth- 1
Eth- 2
Prop- 3
But- 4
Pent- 5
Hex- 6
Hept- 7
Oct- 8
Non- 9
Dec- 10
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Functional GroupsCompound
Type Image Suffix or Prefix
Alcohol - -OH -ol
Haloalkane -X Halo-
Amine -CN- -amine
Aldehyde -COH -al
Ketone -COC- -one
Carboxylic Acid -COOH -oic acid
Ester -COOC- -oate
Amide -CON- -amide
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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
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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
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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
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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
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Bibliography
• VSEPR Theory GIF’s– Rindge, R. (Artist). (1998). Shapes of molecules.
[Web]. Retrieved from http://chemmybear.com/shapes.html