'Principal energy levels' presentation slideshows

Chapter 11 Modern Atomic Theory

Chapter 11 Modern Atomic Theory. This chapter helps us understand why chemicals do the things they do!!. What are atoms like? What is the structure of one? We learned a little about them earlier, and how they were grouped (on the Periodic Table)

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Ch 3: Elements, atoms, ions, and the periodic table

Ch 3: Elements, atoms, ions, and the periodic table. Right now our picture of the atom: protons (+1) and neutrons (()) in nucleus and electrons (-1) in region outside the nucleus.

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Chapter 7; Electronic Structure of Atoms

Chapter 7; Electronic Structure of Atoms. Electromagnetic Radiation Flame Test/ Emission Spectra Quantized Energy Levels Bohr Model/ Rydberg Equation Principal Energy Levels, n First Ionization Energy 2 nd , 3 rd , 4 th , etc Ionization Energy. Chapter 7; Electronic Structure of Atoms.

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Types of bonding

Types of bonding. There are three types of bond that can occur between atoms:. an ionic bond occurs between a metal and non-metal atom (e.g. NaCl). a covalent bond occurs between two non-metal atoms (e.g. I 2 , CH 4 ). a metallic bond occurs between atoms in a metal (e.g. Cu).

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Periodic Trends

Periodic Trends. Periodic Trends. What is a trend? A trend is the general direction in which something tends to move. Periodic Trends. The elements on the Periodic Table of Elements show many trends in their physical and chemical properties. Across the rows (periods or series)

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Electrons in Atoms

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Chapter 11 Modern Atomic Theory

Chapter 11 Modern Atomic Theory. Electromagnetic Radiation. Light is a form of electromagnetic (EM) radiation All forms of EM radiation are types of kinetic energy See page 306. EM Radiation. EM radiation can be described as traveling in waves or as packets of energy called photons.

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10/17/2011 Standards : 1 O bjectives :

10/17/2011 Standards : 1 O bjectives : a. Be able to distinguish bright line spectra from continuous spectra b. Be able to recognize the difference between light as wave and light as particle . c. Be able to describe the Bohr atom. D O NOW :

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Electron Location: Part III

Electron Location: Part III. Electron Configuration. 4f 4d 4p 4s. 14 (7). 10 (5). = sub-level = max. # of electrons = # of electrons = number of orbitals. 6 (3). 32. 2 (1). 3d 3p 3s. 10 (5). 6 (3). 2 (1). 18. 2p 2s. 6 (3). 2 (1). 8. 1s. 2 (1). 2.

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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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Chapter 2- Atoms

Chapter 2- Atoms. HW-2.10, 2.11, 2.15, 2.17, 2.25, 2.29, 2.45, 2.48, 2.53, 2.54, 2.66, 2.79. Ancient Thinkers. Pondered what matter was made of Democritus and followers believed matter was composed of tiny particles Called particles atoms

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KING FAHD UNIVERSITY OF PETROLEUM AND MINERALS

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Quantum Theory and the Atom

Quantum Theory and the Atom. Objectives: AOD C.3.1 Define atomic radii, ionization energy, electronegativity, and energy levels. AOD C.3.2 Recognize periodic trends of elements, including the number of valence electrons, atomic size, and reactivity. . Niels Bohr and Energy States.

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Electron configurations

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Ch. 13 Electrons in Atoms

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Development of the Periodic Table

Development of the Periodic Table. Johann Doberiener (1829). Arranged elements in groups of three (triads) For example: Cl (mass 35) Br (mass 80) I (mass 127) Note: Average mass of the extreme elements =mass of the middle element. John Newland (1865).

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Atomic Orbitals

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Valence electrons, Lewis dot structures, and ionic charge

Valence electrons, Lewis dot structures, and ionic charge. Stable atoms have. 8 electrons (or 2 or 0 if they are small). Metal: sodium. Electron configuration: 1s 2 2s 2 2p 6 3s 1 Sketch of principal energy levels: (Na)2)8)1) Lewis dot structure: (see the board)

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