'Diatomic molecules' presentation slideshows

Chapter 22 Chemistry of The NonMetals

Chapter 22 Chemistry of The NonMetals. Descriptive chemistry of the elements is consistent with the various principles discussed earlier. We will focus on trends in and explanations for the observed behavior of the elements. 22.1 General Concepts: Periodic Trends.

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Reversible Process

Grains of sand. In limit of infinitesmal changes, system moves through equilibrium states during transition-->reversible process. Reversible Process. Remove one grain of sand at a time. Allow system to equilibrate. Pressure decreases by very small amount.

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8.2 Energy level and its degeneracy

0 1 2 3 4 5 . 8.2 Energy level and its degeneracy. Energy levels are said to be degenerate , if the same energy level is obtained by more than one quantum mechanical state. They are then called degenerate energy levels.

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Chem. 355B - 2010 Molecular Properties & Structure II (Molecular Spectroscopy)

Chem. 355B - 2010 Molecular Properties & Structure II (Molecular Spectroscopy) Prof. W. Galley email: william.galley@mcgill.ca Lectures: MWF 10:30AM OM 217 Tutorial: 1/wk to be arranged

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Covalent Bonding

Covalent Bonding. Chapter 9. The Covalent Bond Section 9.1. Why do atoms bond? To achieve full outer electron shells Octet Rule- atoms gain, lose, or share electrons to achieve the electron configuration of noble gases Gain and Lose ? IONIC BONDING Share ? COVALENT BONDING.

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The Heat Capacity of a Diatomic Gas

The Heat Capacity of a Diatomic Gas. 15.1 Introduction. Statistical thermodynamics provides deep insight into the classical description of a MONATOMIC ideal gas.

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Molecular Orbital Theory

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Climate-Greenhouse Effect

Climate-Greenhouse Effect. Greenhouse. Glass, the material that greenhouse is made of, 1) transmit short-wavelength visible light, 2) absorbs and redirects the longer wavelengths of energy. These two aspects make the greenhouse warmer than outside air temperature.

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Chapter 2: Atoms, Molecules and Ions

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Chemistry 445. Lecture 4. Molecular Orbital Theory of diatomic molecules

Chemistry 445. Lecture 4. Molecular Orbital Theory of diatomic molecules. The non-existent He 2 molecule (bond order = 0). BO = (2-2)/2 = 0. The MO diagram for the He 2 molecule is similar to that for the H 2 molecule,

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Introduction to the Periodic Table

Introduction to the Periodic Table. Dmitri Mendeleev. The elements were first arranged in the periodic ta ble in 1869 by Dmitri Mendeleev.

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CH 4: Chemical Foundations

CH 4: Chemical Foundations. The Elements and the Periodic Table. The Elements. Information found on the periodic table Symbol Carbon Oxygen Cobalt. The Elements. Information found on the periodic table State of matter Color of symbol indicates state of matter Black = solid

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Molecular Orbital Theory

Molecular Orbital Theory. Diatomic molecules: Heteronuclear molecules.

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Lecture 14: Molecular structure

Lecture 14: Molecular structure. Rotational transitions Vibrational transitions Electronic transitions. Bohn-Oppenheimer Approximation. Born-Oppenheimer Approximation is the assumption that the electronic motion and the nuclear motion in molecules can be separated.

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Redox & Electrochemistry

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Naming Compounds, cations and anions

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Periodic table families and valence electrons

Periodic table families and valence electrons. Valence electron. Valence electrons are the electrons contained in the outermost, or valence, electron shell of an atom

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