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energy levels
energy levels

... Bohr’s theory of hydrogen (1913): • An obsolete theory which has been replaced by quantum mechanics. • The model can still be used to develop ideas of energy and angular momentum quantization in atomic-sized systems. Assumption 1: The electron moves in circular orbits around the proton under the ele ...
Lecture notes 2: Quantum mechanics in a nutshell
Lecture notes 2: Quantum mechanics in a nutshell

... can be built up by neglecting electron spin (but do keep the exclusion principle). This means any electron configuration can have two electrons — one with spin up, the other with spin down. Assume further that each electron moves in a central field which is the combined field of the nucleus and all ...
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Slide 1

... 4. Some of these photons run in a direction parallel to the ruby's axis, so they bounce back and forth off the mirrors. As they pass through the crystal, they stimulate emission in other atoms. ...
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General Chemistry - Review for final exam: (Make sure you bring

... 74. What types of products are you likely to find in a double-replacement reaction? 75. How can you identify a Combustion reaction by the reactants and products? 76. What values in a chemical equation are used to calculate molar ratios between different compounds? 77. What values are used to calcula ...
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Physical and Chemical Properties

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Atomic Structure Notes

... where n is an integer, h is Planck’s constant and ν is the frequency of the electromagnetic radiation absorbed or emitted. 2. Energy is in fact quantized and can only occur in discrete units of size hv. Each of these small "packets" of energy is called a quantum (or a photon when we are talking abou ...
Some Quantum Considerations II
Some Quantum Considerations II

... Which of the following statements is false? a. Longer wavelength radiation carries higher energies. b. Light can be considered to be made up of particles called photons. c. All material objects have some wave characteristics. d. Electrons can be viewed as standing waves in an atom. e. Bohr’s model o ...
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... 8. Trace the changes in atomic theory starting with Dalton and ending with the modern quantum mechanical model. 9. Describe the basic properties of alpha, beta, and gamma radiation. 10. Explain why some atomic nuclei are unstable 11. Predict the type of nuclear decay that will occur given the compos ...
Atoms
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Chemical reactions revision

... Atoms are the units that elements are built from Atoms are so tiny that they cannot be seen even with powerful microscopes The atoms of each element are different to each other, but have a similar structure. ...
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File - Mr. Holz`s Website

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2A Final Exam Review Worksheet

... 1. If the density of aviation fuel is 1.77 lb/L, how many liters must be added to a tank to give 16,131 kg (1 kg= 2.205 lb)? 2. Count the total number of protons, neutrons, and electrons: protons neutrons electrons ...
AP Chem II Instructor: Mr. Malasky Name Period ______ Due Date
AP Chem II Instructor: Mr. Malasky Name Period ______ Due Date

... ____ 1. The Heisenberg uncertainty principle states that a. electrons have no momentum b. the position of an electron is impossible to determine c. the faster an electron moves, the more unreliable is its energy d. the momentum and the position of an electron cannot be precisely defined simultaneous ...
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Section 4.2 The Quantum Model of the Atom

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Electron Configuration and New Atomic Model

... •  It was also shown that interference occurs when waves overlap, causing a slight decrease in energy. ...
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Electron Configuration - Warren County Public Schools

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CHEMISTRY CHAPTER 5 OUTLINE NOTES 5.1 – Light and

... the same manner as Earth is in orbit around the sun. This is sometimes called the planetary atomic model or Bohr’s Model. o So a hydrogen atom should be similar to a solar system consisting of a sun and one planet. o Scientists began to unravel the puzzle of chemical behavior in the early 1900’s and ...
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Quantum Mechanics Problem Set

... (b) De Broglie states that electrons demonstrate the properties of both particles and waves and that each moving particle has a wave associated with it. A wave function is the mathematical description of the matter wave of an electron. (c) Although we cannot predict he exact location of an electron ...
Lecture 29B - UCSD Department of Physics
Lecture 29B - UCSD Department of Physics

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6.1 Organizing the Periodic Table

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Shapes of the Charge Clouds

... •These areas are cloud-like with a fairly large space being filled by a few tiny electrons (e.g. fan blades) •Therefore, the electron cloud takes up most of the space of the atom, while the small, dense nucleus fills the center. ...
Quantum Mechanical Model - Elmwood Park Memorial Middle School
Quantum Mechanical Model - Elmwood Park Memorial Middle School

... •  These  slides  are  on  the  webpage  if  you  would   like  them.   ...
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Atom

An atom is the smallest constituent unit of ordinary matter that has the properties of a chemical element. Every solid, liquid, gas, and plasma is made up of neutral or ionized atoms. Atoms are very small; typical sizes are around 100 pm (a ten-billionth of a meter, in the short scale). However, atoms do not have well defined boundaries, and there are different ways to define their size which give different but close values.Atoms are small enough that classical physics give noticeably incorrect results. Through the development of physics, atomic models have incorporated quantum principles to better explain and predict the behavior.Every atom is composed of a nucleus and one or more electrons bound to the nucleus. The nucleus is made of one or more protons and typically a similar number of neutrons (none in hydrogen-1). Protons and neutrons are called nucleons. Over 99.94% of the atom's mass is in the nucleus. The protons have a positive electric charge, the electrons have a negative electric charge, and the neutrons have no electric charge. If the number of protons and electrons are equal, that atom is electrically neutral. If an atom has more or fewer electrons than protons, then it has an overall negative or positive charge, respectively, and it is called an ion.Electrons of an atom are attracted to the protons in an atomic nucleus by this electromagnetic force. The protons and neutrons in the nucleus are attracted to each other by a different force, the nuclear force, which is usually stronger than the electromagnetic force repelling the positively charged protons from one another. Under certain circumstances the repelling electromagnetic force becomes stronger than the nuclear force, and nucleons can be ejected from the nucleus, leaving behind a different element: nuclear decay resulting in nuclear transmutation.The number of protons in the nucleus defines to what chemical element the atom belongs: for example, all copper atoms contain 29 protons. The number of neutrons defines the isotope of the element. The number of electrons influences the magnetic properties of an atom. Atoms can attach to one or more other atoms by chemical bonds to form chemical compounds such as molecules. The ability of atoms to associate and dissociate is responsible for most of the physical changes observed in nature, and is the subject of the discipline of chemistry.Not all the matter of the universe is composed of atoms. Dark matter comprises more of the Universe than matter, and is composed not of atoms, but of particles of a currently unknown type.
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