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Stereochemistry

activity vsepr modeling student copy

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Chemistry
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Chemistry
Quantum chemistry
Molecular geometry
Stereochemistry
VSEPR theory
Hypervalent molecules
Sulfur tetrafluoride
Chemical bond

Name: ______________________ VSEPR Modeling Lewis Structure # Electron pair domains # Nonbonding (lone) pairs Shape Bond Angles Polar or Nonpolar CO2 BF3 SO2 CH4 NH3 H2O PF5 SF4 ClF3 XeF2 SF6 BrF5 XeF4 American Association of Chemistry Teachers |1-360
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activity vsepr modeling teachers copy

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Chemistry
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Chemistry
Molecular geometry
Stereochemistry
Chemical bonding
Quantum chemistry
VSEPR theory
Sulfur tetrafluoride
Lewis structure
Steric number
T-shaped molecular geometry

Summary In this activity, students construct physical models of molecular shapes. However, students are not told what the preferred arrangements of electron pair domains are. Instead, they derive the arrangements. Students are given the opportunity to conceptualize what is happening when one electron pair domain acts upon another, and to understand how those interactions result in the molecular geometries predicted by VSEPR theory. Grade Level High School Objectives By the end of this activity, students should be able to Conceptualize the impact of one electron pair domain acting upon another, and understand how those interactions result in the molecular geometries predicted by VSEPR theory. Describe the implications of electron pair repulsions on molecular shape.

Campbell Biology 9th Edition - Ch. 4 Organic Chem

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Biology
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Chemistry
Organic chemistry
Functional groups
Isomerism
Chemical nomenclature
Stereochemistry
Isomer
Structural isomer
Carbon
Carboxylic acid
Organic compound
Substituent

Chapter 4 Carbon and the Molecular Diversity of Life I. Importance of Carbon Organic chemistry: branch of chemistry that specializes in study of carbon compounds Organic compounds: contain Carbon (& H) Major elements of life: CHNOPS Carbon can form large, complex, and diverse molecules II. Diversity of Carbon It has 4 valence electrons (tetravalence) It can form up to 4 covalent bonds Most frequent bonding partners: H, O, N II. Diversity of Carbon Bonds can be single, double, or triple covalent bonds. II. Diversity of Carbon Carbon can form large molecules 4 classes of macromolecules: carbohydrates, proteins, lipids, nucleic acids II. Diversity of Carbon Molecules can be chains, ring-shaped, or branched II. Diversity of Carbon Forms isomers

Organic Chemistry Lecture 23

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Chemistry
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Carbohydrate chemistry
Carbohydrates
Sugar substitutes
Nutrition
Stereochemistry
Carbohydrate
Anomer
Glucose
Reducing sugar
Monosaccharide
Aldonic acid

Chapter 23 ? 2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Carbohydrates and Nucleic Acids Chapter 23 * Carbohydrates Synthesized by plants using sunlight to convert CO2 and H2O to glucose and O2. Polymers include starch and cellulose. Starch is a storage unit for solar energy. Most sugars have formula Cn(H2O)n, ?hydrate of carbon.? Chapter 23 Chapter 23 * Classification of Carbohydrates Monosaccharides or simple sugars: polyhydroxyaldehydes or aldoses polyhydroxyketones or ketoses Disaccharides can be hydrolyzed to two monosaccharides. Polysaccharides hydrolyze to many monosaccharide units. For example, starch and cellulose have > 1000 glucose units. Chapter 23 Chapter 23 * Monosaccharides Classified using three criteria:

Organic Chemistry Lecture 7

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Chemistry
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Functional groups
Chemical nomenclature
Isomerism
Stereochemistry
Alkene
Cis–trans isomerism
Saturated and unsaturated compounds
Butene
Isomer
Haloalkane

Chapter 7 ?2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Structure and Synthesis of Alkenes Chapter 7 * Introduction Alkenes are hydrocarbon with carbon-carbon double bonds. Alkenes are also called olefins, meaning ?oil-forming gas?. The functional group of alkenes is the carbon-carbon double bond, which is reactive. Chapter 7 Chapter 7 * Sigma Bonds of Ethylene Chapter 7 Chapter 7 * Orbital Description Sigma bonds around the double-bonded carbon are sp2 hybridized. Angles are approximately 120? and the molecular geometry is trigonal planar. Unhybridized p orbitals with one electron will overlap forming the double bond (pi bond) . Chapter 7 Chapter 7 * Bond Lengths and Angles sp2 hybrid orbitals have more s character than the sp3 hybrid orbitals.

Organic Chem Review

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Algebra
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VSEPR theory
World Wide Web
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organic chemistry

Molecular Geometry: VSEPR model stand for valence-shell electron-pair repulsion and predicts the 3D shape of molecules that are formed in bonding. Sigma and Pi Bonds: All single bonds are sigma(?), that occur in the overlap of hybridized orbitals. Pi (?) bonds occur when parallel, unhybridized p orbitals overlap. Double bonds contain one sigma and one pi bond; triple bonds contain one sigma and two pi bonds. ? bonds are weaker than the ? bonds, but because ? bonds are found with ? bonds they are stronger than a single ? bond. Pi bonds also prevent rotation about the bond. Hybridization: Blending of outer bonding orbitals Intermolecular Forces: London Dispersion - Weak intermolecular force, temporary attractive force that results when
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