Energy level

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Wave–particle duality

Atomic Structure Atomic structure of an atom based on energy relative to size of an electron can be measured with Einstein?s formula of e=mc2. However, energy of an electron within an atom based on how long a wavelength takes to pass can be determined with the formula of constant= wavelength x frequency. Electromagnetic Radiation is described with wavelike energy with both magnetic and electrical properties. Waves of electrons (atoms) are within radiation additionally wave measurements can be made with the wavelength, frequency, and the speed of light (constant). Wavelength= Indicated with lambda, described as the length of a wave from one crest to another. Frequency= Measured in Hz (1/s), the number of waves that pass per second

AP Chemistry Zumdahl 7E Chapter 7 Notes

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Principal quantum number

Ionization energy

Bohr model

AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 10-12 10-10 10-8 4 to 7x10-7 10-4 10-2 1 102 104 Wavelength increases Frequency decreases Energy decreases Speed is constant = 2.9979 x 108 m/sec B. Properties of EM Waves 1. Wavelength (l) a. Distance between two consecutive peaks or troughs in a wave b. Measured in meters (SI system) 2. Frequency (n) a. Number of waves that pass a given point per second b. Measured in hertz (sec-1) 3. Speed ( c ) a. Measured in meters/sec 4. Relationship of properties a. c=nl gamma xrays UV visible IR micro Radio waves FM short AM 7.2 The Nature of Matter

Raven Biology Chapter 2 Notes

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Gavin Morgan 8/31/2015 Chapter 2 2-Point Notes The Nature of Atoms Atomic structure includes a central nucleus and orbiting electrons: 1. Danish physicist Niels Bohr created the model of the atom in 1913, which is still used today. 2. An atom?s mass is measured in daltons (6.02 x 1023 daltons = 1 g). A proton and neutron each way 1 dalton. Electrons determine the chemical behavior of atoms: 1. The position of an electron cannot be determined at any given time. 2. Orbitals are predictions where electrons are most likely to be found. Atoms contain discrete energy levels: 1. Electrons contain discrete energy levels which correspond to quanta.

Principles of Chemistry Chapter 8

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Chemical bonding

Quantum chemistry

Chemical properties

intermolecular forces

Polymer

Chapter 8: Molecules and Materials Section 8.2: Condensed Phases--Solids Monday, October 13, 2014 1:00 PM Arrangements of Solids: ? Crystalline solid - solids with regular, repeating geometric arrangements of atoms, ions, or molecules Amorphous solids - noncrystalline solid with random arrangement of atoms or molecules ? **crystalline solids are more common and well-known ? Arrangements can be thought of as packing marbles together in a box (especially since atoms are spherical) We can reduce space between atoms--but not eliminate it--by rearranging the atoms in the structure "packing efficiency" - percentage of total volume that is actually occupied by atoms in a crystal lattice Affected by density of the material ? ? ? Types of Structures ? ? Cubic Crystal lattices: ? ? ?

Principles of Chemistry Chapter 6

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Hund's rule of maximum multiplicity

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electron configuration

electron

Aufbau principle

Bohr model

Chapter 6: The Periodic Table & Atomic Structure Section 6.2: The Electromagnetic Spectrum Monday, September 15, 2014 3:06 PM Visible Light - portion of electromagnetic spectrum that we can see, typically with wavelengths between 400 / 700 nanometers ? Electromagnetic Spectrum - various forms of light, consisting of oscillating electric and magnetic fields ? ? ? The Wave Nature of Light ? Wavelength - distance between corresponding points on a wave Amplitude - height of the wave from equilibrium position Frequency - number of cycles of a wave passing a certain point per second (measured in Hz) **note: amplitude corresponds with brightness, wavelength and frequency correspond with color ? Speed of light ( c ) : c = lamda x v = wavelength x frequency ? The Particulate Nature of Light

Chapter 8

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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 05 November 2012 Jespersen, Brady & Hyslop Chapter 8 The Quantum Mechanical Atom Quantum Mechanics Ch. 8.1 The physics that describes objects with wave-particle duality is called quantum mechanics or quantum theory. In the late 1800?s, scientists discovered that electrons acted like tiny charged particles in some experiments and waves in others. Quantum mechanics accurately describes the structure and reactivity of atoms and molecules. Electromagnetic Radiation Ch. 8.1 Energy can be transferred as heat or as light. Electromagnetic radiation can be carried energy through space in the form of electromagnetic waves.

Holt Biology Chapter 2 Section 1

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ion

Atom

Unit 1 Chapter 2: Chemistry of Life Section 1: Nature of Matter Atom Smallest unit of matter that can?t be broken down by chemical means Protons, Neutrons, Electrons Electron cloud Region around nucleus that electrons can occupy at any time Stable atoms usually have no charge 1 electron for every 1 proton Elements Pure substance made of one kind of atom Differ in number of protons Ex. Carbon-12 (Carbon has 6 protons) 12-6=6 Carbon-12 has 6 neutrons Compound Substance made of joined atoms of 2 or more different elements Chemical formula identifies what is in compound and those elements? proportions Ex. NaCl 1 Sodium for every 1 Chlorine Covalent Bonds Two or more atoms share electrons to form a molecule Molecule Group of atoms held together by covalent bonds

Chemistry The central science Summary Chapter 6

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Physics

Atomic orbital

electron configuration

Hot Objects and the Quantization of Energy Heated solids emit radiation (blackbody radiation) The wavelength distribution depends on the temperature (i.e., ?red hot? objects are cooler than ?white hot? objects). In 1900 Max Planck solved the problem He investigated black body radiation. He proposed that energy can only be absorbed or released from atoms in ?chucks? of some minimum size . These amounts are called quanta. A quantum (meaning ?fixed amount?) is the smallest amount of energy that can be emitted or absorbed as electromagnetic radiation. The relationship between energy and frequency is: . The Photoelectric Effect and Photons The photoelectric effect provides evidence for the particle nature of light and for quantization.

Chapter 7

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Physics

atoms

electron

Energy level

Atomic orbital

Azimuthal quantum number

Aufbau principle

Technology

Claire Rafson Chapter 7: Atomic Structure and Periodicity 7.1- 7.3 Wavelength and frequency are inversely related C= speed of light = 2.9979 X 10^8 m/s Photoelectric effect- Einstein. Phenomenon in which electrons are emitted from the surgace of a metal when light strikes it. E=mc^2 ?. M= mass Dual nature of light Diffraction- light is scattered from a regular array of points or lines. Change in E= hv 7.4- quantum model- made by Bohr. Model for the hydrogen atom. Electron in a hydrogen atom moves around the nucleus only in certain orbits. Ground state- lowest possible energy state. 7.5- quantum mechanical model- Heisenberg, Broglie, and Schrodinger probability distribution- intensity of color is used to indicate probability value near a given point in space. 7.6-

Campbell Biology Chapter 1-4 Outline

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