'Pauli exclusion principle' presentation slideshows

Announcement

Announcement. Homework is due at the beginning of class. Put it on your desk during the first two minutes. HW detentions emailed at the beginning of class.

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Chapter 1: Structure and Bonding

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Chemistry Taboo

Chemistry Taboo. Fall Final Review. liquid. VOLUME WATER CHEMICAL SLIDES FLOWS. periodic table. ELEMENTS ORGANIZED ATOMIC NUMBER PROPERTIES DIFFERENT. physical change. BURN CUT CHEMICAL REACTION ALTER. period. PERIODIC TABLE COLUMNS ROWS GROUPS VALENCE ELECTRON.

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Chem C1403 Lecture 11. Wednesday, October 12, 2005 End of Chapter 16, into Chapter 17

Chem C1403 Lecture 11. Wednesday, October 12, 2005 End of Chapter 16, into Chapter 17. Magic (Quantum) numbers from the solutions of the wave equation: orbitals of the H atom: n, l and m l . The size, shape and orientation of orbitals. Electron spin. Multielectron atoms.

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The color of the light emitted depends upon the D E as the electron(s) move from higher to lower energy levels.

Chapter 6. The color of the light emitted depends upon the D E as the electron(s) move from higher to lower energy levels. . Ne. He. The shorter the wavelength ( ?) , the higher the frequency ( ?) . Energy of the wave increases as frequency increases. Electromagnetic spectrum.

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To learn about the shapes of the s, p and d orbitals To review the energy levels and orbitals of the wave mechanical

Objectives. To learn about the shapes of the s, p and d orbitals To review the energy levels and orbitals of the wave mechanical model of the atom To learn about electron spin . A. Electron Location . Energy Level Called principal energy levels Corresponds to row on periodic table

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Science Jeopardy

Science Jeopardy. Biology. Chemistry. Physics. Earth/Space Sci. Health. 100. 100. 100. 100. 100. 200. 200. 200. 200. 200. 300. 300. 300. 300. 300. 400. 400. 400. 400. 400. 500. 500. 500. 500. 500. Final Jeopardy. Help. (1) Save a duplicate of this template.

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CHAPTER 8 Atomic Electron Configurations and Chemical Periodicity

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Learning Objectives

Learning Objectives. Who was involved? Which experiments were used to help us understand? What are atomic line spectra? Which models were used to represent the atom? Which equations are fundamental? Which ones are handy to know?! What have been the successes of quantum theory?

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Atomic Structure

Atomic Structure. www.lab-initio.com. Standards. Modern Atomic Theory. All matter is composed of atoms Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions . However, these changes CAN occur in nuclear reactions!

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The Emergence of Everything(?)

The Emergence of Everything(?). Alan Baker Philosophy, Swarthmore College Dec 2nd 2003. What is emergence?. 3 basic approaches; (to clarifying a concept, F) (i) Formulate a definition of F. (ii) Give examples where F applies.

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Semi-Empirical Mass Formula Applications - I

Semi-Empirical Mass Formula Applications - I. [Sec. 4.2 Dunlap]. Pairing Energy. ? - particle. Deuteron. Triton.

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Molecular Orbital Theory and Charge Transfer Excitations

Molecular Orbital Theory and Charge Transfer Excitations. Chemistry 123 Spring 2008 Dr. Woodward. Molecular Orbital Diagram H 2. Antibonding Molecular Orbital (Orbitals interfere destructively). Energy. H 1s Orbital. H 1s Orbital. Bonding Molecular Orbital

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8.1 Atomic Structure and the Periodic Table 8.2 Total Angular Momentum 8.3 Anomalous Zeeman Effect

CHAPTER 8 Atomic Physics. 8.1 Atomic Structure and the Periodic Table 8.2 Total Angular Momentum 8.3 Anomalous Zeeman Effect. What distinguished Mendeleev was not only genius, but a passion for the elements. They became his personal friends; he knew every quirk and detail of their behavior.

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The Applications of Nano Materials

The Applications of Nano Materials. Department of Chemical and Materials Engineering San Jose State University. Zhen Guo, Ph. D. Final Review. Traditional theme mainstreaming materials science for last 5000+ years. Part I. Basic Materials Science Principles. Microstructure. Materials.

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III. Quantum Model of the Atom (p. 98 - 104)

Ch. 4 - Electrons in Atoms. III. Quantum Model of the Atom (p. 98 - 104). A. Electrons as Waves. Louis de Broglie (1924) Applied wave-particle theory to e - e - exhibit wave properties. QUANTIZED WAVELENGTHS. A. Electrons as Waves. QUANTIZED WAVELENGTHS. VISIBLE LIGHT. ELECTRONS.

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Chemistry Chapter 5

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To learn about the shapes of the s, p and d orbitals To review the energy levels and orbitals of the wave mechanical

Objectives. To learn about the shapes of the s, p and d orbitals To review the energy levels and orbitals of the wave mechanical model of the atom To learn about electron spin . A. The Hydrogen Orbitals . Orbitals do not have sharp boundaries. . 90% boundary. A. The Hydrogen Orbitals .

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Quantum Mechanical Model Electron Placement

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Where is the Electron Located?

Where is the Electron Located?. The Quantum Model of the Atom. Heisenberg uncertainty principle : It is impossible to determine both the position and velocity of an electron or any other particle. What is the Address of the Electron?.

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