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Quantum chemistry

Chapter 9: Covalent Bonding: Orbitals

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Campbell Biology Chapter 2

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? 2017 Pearson Education, Inc. Lecture Presentations byNicole Tunbridge and Kathleen Fitzpatrick Chapter 2The Chemical Context of Life 1 A Chemical Connection to Biology Biology is the study of life Organisms and their environments are subject to basic laws of physics and chemistry One example is the use of formic acid by ants to protect themselves against predators and microbial parasites ? 2017 Pearson Education, Inc. 2 Concept 2.1: Matter consists of chemical elements in pure form and in combinations called compounds Organisms are composed of matter Matter is anything that takes up space and has mass ? 2017 Pearson Education, Inc. 3 Elements and Compounds Matter is made up of elements An element is a substance that cannot be broken down to other substances by chemical reactions

activity vsepr modeling student copy

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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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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.

hybrization

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Worksheet ? Hybridization One model to explain bonding in molecules is called the valence bond theory. It is based on the concept of hybridized molecular orbitals. Atomic orbitals (s,p,d) are mathematically mixed to form molecular orbitals with defined shapes and energy levels. In organic chemistry, we need only look at the hybridization of the one 2s and three 2p orbitals containing the valence electrons of C,O and N. When four equivalent molecular orbitals are needed, all four atomic orbitals are mixed to give sp3 hybridization. When three equivalent molecular orbitals are needed, three of the atomic orbitals are mixed to give sp2 hybridization. In this case, one unhybridized p atomic orbital remains, with its shape and energy level

Periodic Table Notes

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Trends: 1. Across? ?the? ?period ? There? ?is? ?a? ?general? ?decrease? ?in? ?atomic? ?radius? ?across? ?the? ?period. - Across? ?a? ?period,? ?proton? ?number? ?increases? ?and? ?electrons? ?are? ?being? ?added? ?to? ?the? ?same? ?outermost principal? ?quantum? ?shell - Forces? ?of? ?attraction? ?between? ?the? ?valence? ?electron? ?and? ?nucleus? ?increases? ?as? ?nucleus? ?becomes more? ?positively? ?charged - Distance? ?between? ?the? ?valence? ?electron? ?and? ?nucleus? ?decreases. 2. Down? ?the? ?group ? There? ?is? ?a? ?general? ?increase? ?in? ?atomic? ?radius? ?down? ?the? ?group - Number? ?of? ?filled? ?principal? ?quantum? ?shell? ?increases

Biochemistry powerpoint

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Chapter 2 The Chemical Context of Life Basic Terms Element = cannot be broken down to other substances Examples: Na, O, C, Cl Compound = combination of 2 or more different elements Examples: NaCl, CO2, CH4 Requirements for Life 92 natural elements? 25 are essential to life Carbon, oxygen, hydrogen, and nitrogen make up 96% of living matter Trace elements are needed, too, though Iodine?lack of = goiter!! Atomic Structure Atom = smallest possible amount of an electron that retains the element?s properties Subatomic particles: Protons = + charge Electrons = - charge Neutrons = neutral charge Atomic Structure Atomic Number: # of protons (also equals # of electrons?) Mass Number: # of protons + # of neutrons Examples Isotopes

Organic Chemistry Lecture 15

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Chapter 15 ? 2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy Chaper 15 * Conjugated Systems Conjugated double bonds are separated by one single bond. Isolated double bonds are separated by two or more single bonds. Conjugated double bonds are more stable than isolated ones. Chaper 15 Chaper 15 * Heat of Hydrogenation of Conjugated Bonds For conjugated double bonds, the heat of hydrogenation is less than the sum for the individual double bonds. The more stable the compound, the less heat released during hydrogenation, Conjugated double bonds have extra stability. Chaper 15 Chaper 15 * Relative Stabilities twice 1-pentene more substituted Chaper 15 Chaper 15 * Structure of 1,3-Butadiene

Organic Chemistry Lecture 15

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Chapter 15 ? 2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy Chaper 15 * Conjugated Systems Conjugated double bonds are separated by one single bond. Isolated double bonds are separated by two or more single bonds. Conjugated double bonds are more stable than isolated ones. Chaper 15 Chaper 15 * Heat of Hydrogenation of Conjugated Bonds For conjugated double bonds, the heat of hydrogenation is less than the sum for the individual double bonds. The more stable the compound, the less heat released during hydrogenation, Conjugated double bonds have extra stability. Chaper 15 Chaper 15 * Relative Stabilities twice 1-pentene more substituted Chaper 15 Chaper 15 * Structure of 1,3-Butadiene

Inert pair effect

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Trying to explain the trends in oxidation states There's nothing surprising about the normal Group oxidation state of +4. All of the elements in the group have the outer electronic structure ns2npx1npy1, where n varies from 2 (for carbon) to 6 (for lead). The oxidation state of +4 is where all these outer electrons are directly involved in the bonding. As you get closer to the bottom of the Group, there is an increasing tendency for the s2 pair not to be used in the bonding. This is often known as the inert pair effect - and is dominant in lead chemistry. However, just giving it a name like "inert pair effect" explains nothing. You need to look at two different explanations depending on whether you are talking about the formation of ionic or covalent bonds.

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