ftce chemistry sae preparation course
DESCRIPTION
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 - PowerPoint PPT PresentationTRANSCRIPT
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
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
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%)
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.
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
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
Ionic Character
• Ionic Bonds are bonds with > 50% ionic character
• Difference in Electronegativity of involved atoms is >1.7
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
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
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
CuCl2
Copper (II) ChlorideCuO
Copper (II) OxideNaCl
Sodium ChlorideKI
Potassium IodideMg3N2
Magnesium NitridePbO2
Lead (IV) Oxide
Practice
• Draw the lewis structures for– Ammonia (NH3)
– Water (H2O)
– Phosphorus Trifluoride (PF3)– Hydrogen Cyanide (HCN)– Ozone (O3)
– Formaldehyde (CH2O)
VSEPR• AB4
– Tetrahedral– 109.50 Bond Angles
• AB3– Trigonal Planar– 1200 Bond Angles
• AB2– Linear– 1800 Bond Angles
Shape and Polarity?
• What is the shape and polarity of the following molecules?– Water– Ammonia– Carbon Tetrachloride– Carbon Dioxide– Hydrogen Chloride
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
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
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
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
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
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
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
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
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
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
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