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Molecular physics

Atomic Structure

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Emission spectrum
Photoelectric effect
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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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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

ap chem semester final

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Valence electron
Ionization energy
Resonance
Chemistry
electron
ion
Chemical reaction

AP/IB Chem 1st Semester Exam Review Questions?????????????????? Multiple Choice: 1. When 12 grams of methane (CH4) is burned, the quantity of energy released is most nearly: Heat of combustion for CH4 is -891 KJ/mol. a)? 0.75 kJ?b)? 56 kJ?c)? 420 kJ?d)? 600 kJ?e)? 800 kJ 2.? The reaction of sodium bicarbonate with sulfuric acid is shown below.? 2 NaHCO3?? +?? H2SO4?? ??? Na2SO4?? +?? 2 H2O?? +?? 2 CO2???????? ?H? =? + 25 kJ/mol NaHCO3

Principles of Chemistry Chapter 6

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Hund's rule of maximum multiplicity
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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electron configuration
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Energy level
Technology
behavior
Human development
Interpersonal relationships
Love
Psychoanalysis
Human behavior
Attachment theory
Evolutionary biology
Personal life

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.

Semester 1 Final Study Guide

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Chemistry Final Exam Study Guide, Chapters 1-8 Chapter 1. Matter and Change Chemistry ? the study of matter and its changes Branches of Chemistry ? 1. Organic Chemistry ? substances containing carbon 2. Inorganic Chemistry ? substances not containing carbon 3. Biochemistry ? chemistry of living things DNA, protein, lipids, carbohydrates 4. Physical Chemistry ? properties and changes of matter with respect to energy 5. Analytical Chemistry ? identification of components and composition of matter. 6. Theoretic Chemistry ? creates mathematical models of chemical behavior Chemical ? any substance with a definite composition Mass ? amount of matter Matter ? takes up space and has mass

Chemistry The central science Summary Chapter 6

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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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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-

Chapter 8 Solutions

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Periodic Properties of the Elements Review Questions 8.1 A periodic property is one that is predictable based on the element's position within the periodic table. 8.2 The relative size of the sodium and potassium ions is important to nerve signal transmission. The pumps and channels within cell membranes are so sensitive that they can distinguish between the sizes of these two ions and selectively allow only one or the other to pass. The movement of ions is the basis for the transmission of nerve signals in the brain and throughout the body. 8.3 The first attempt to organize the elements according to similarities in their properties was made by the German chemist Johann Dobereiner. He grouped elements into triads; three ele-

Chapter 8 Test Banks

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? Chemistry: A Molecular Approach (Tro) ? Chapter 8 ?? Periodic Properties of the Elements ? 1) ?? Give the ground state electron configuration for Se. ? A) ?? [Ar]4s23d104p4 ? B) ?? [Ar]4s24d104p4 ? C) ?? [Ar]4s23d104p6 ? D) ?? [Ar]4s23d10 ? E) ?? [Ar]3d104p4 ? Answer: ?? A ? 2) ?? Give the ground state electron configuration for I. ? A) ?? [Kr]5s24d105p6 ? B) ?? [Kr]5s24d105p5 ? C) ?? [Kr]4d105p6 ? D) ?? [Kr]5s25p6 ? E) ?? [Kr]5s25d105p6 ? Answer: ?? B ? 3) ?? Give the ground state electron configuration for Sr. ? A) ?? [Kr]5s24d2 ? B) ?? [Kr]5s24d105p2 ? C) ?? [Kr]5s2 ? D) ?? [Kr]5s25d105p2 ? E) ?? [Kr]5s24d10 ? Answer: ?? C ? 4) ?? Give the ground state electron configuration for Pb. ? A) ?? [Xe]6s26p2 ? B) ?? [Xe]6s25d106p2 ? C) ?? [Xe]6s25f146d106p2 ? D) ??

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