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Solutions to the exam itself are now available.
Solutions to the exam itself are now available.

... (f) The Cr4+ ion in the compound CrO2 is exploited in magnetic audio and video recording tape. The electron configuration of Cr4+ is [Ar] 3d2. The question here is simple: which four electrons does Cr with the [Ar] 4s1 3d5 configuration lose? There are two obvious possibilities for Cr4+ that make se ...
IntroQuantumNuclearp..
IntroQuantumNuclearp..

... J.J. Thomson’s model predicted α particles pass through Particles were scattered! Rutherford assumed that positively charges grouped together in a nucleus caused scattering Proposed “planetary model” – but not stable in classical physics—electron orbits would lose energy and decay Proposed existence ...
Questions
Questions

... Problem 3: Spectrum of Alkali Atoms (10 points) We have seen that the spectrum of hydrogen has an “accidental” degeneracy – states with the same principle quantum number n, but different angular momentum quantum number l are degenerate. This was an artifact of the pure 1/r Coulomb potential associa ...
Modern Physics
Modern Physics

... Dual Nature of Light  Light exhibits wave phenomena as a light wave is propagated by interchange of energy between varying electric and magnetic fields (Maxwell)  Light acts like particles composed of kinetic energy and momentum when light interacts with matter  Both wave and particle 1. Wave Nat ...
Physics 12 Assignmen.. - hrsbstaff.ednet.ns.ca
Physics 12 Assignmen.. - hrsbstaff.ednet.ns.ca

... 2. In Rutherford’s planetary model of the atom, what keeps the electrons from flying off into space? In Rutherford’s planetary model of the atom, the Coulomb (or electrostatic) force keeps the electrons from flying off into space. Since the protons in the center are positively charged, the negativel ...
Solution - UMD Physics
Solution - UMD Physics

... a. Write down the time-independent differential wave equation governing the energy of this system. (1) b. Solve this equation for the stationary-state wavefunctions Ψ ,  , and determine all the allowed energies, using quantum numbers nx and ny. What is the lowest “groundstate” energy?(2) c. Calcul ...
Name Objective 1: Matter and Energy C3H8 + 5O2 → 3CO2 + 4H2O
Name Objective 1: Matter and Energy C3H8 + 5O2 → 3CO2 + 4H2O

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Ch.3 lecture

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Bohr`s atomic model

... An orbiting electron must have a whole number of wavelengths around the circumference of its orbit (6), otherwise the wave will interfere destructively with itself. This approach predicts the same energy levels as Bohr’s model. (You can use Box 2 to show that Equations 1 and 2 are equivalent.) ...
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Quantum Model of the Atom Power point

Chapter 4 Arrangement of Electrons in Atoms
Chapter 4 Arrangement of Electrons in Atoms

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... Quantum Hall edge states with a Bose gas Ultracold atomic systems can be used to model condensed-matter physics, providing precise control of system variables often not achievable in real materials. This involves inducing charge-neutral particles to behave as if they were charged particles in a magn ...
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Nuclear Chemistry

... • Produces even more energy per gram of fuel than fission. • Produces less nuclear waste than fission. • Fusion fuel is easy to get. (Heavy hydrogen is found in ...
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Chapter 7_01042016

... Pauli exclusion principle In a given atom no two electrons can have the same set of four quantum numbers (n, l, ml, ms). ...
Chemistry DCA Review Sheet
Chemistry DCA Review Sheet

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... one kind of atom that cannot be broken down into other substances by chemical or physical means. Atoms are the smallest units of an element that has the properties of that element. Atoms are made of subatomic particles (protons, neutrons, and electrons): ...
Mid-Term OR Study Guide
Mid-Term OR Study Guide

... Be able to complete an AUFBAU CHART: Consider the element barium. Answer the following questions: (A) What is the element symbol? How many electrons are in a neutral atom of barium? (B) Draw the orbital notation for barium using up and down arrows. (C) Write the complete electron configuration for b ...
All That Matters - Teach-n-Learn-Chem
All That Matters - Teach-n-Learn-Chem

... We need to be able to identify the materials we see every day so that we can use them correctly. We do this by observing physical and chemical properties and comparing them to what we know from personal experience. Physical properties include such things as boiling point, color, density, hardness, m ...
Name Period Nuclear Study Packet Set 1 1. What subatomic
Name Period Nuclear Study Packet Set 1 1. What subatomic

... 1.   What subatomic particles are involved in nuclear reactions? 2.   What subatomic particles are involved in chemical reactions? 3.   If an atom undergoes a reaction and attains a more stable form, how do you know if the reaction was chemical or nuclear? 4.   Draw a lithium-6 atom. This includes d ...
ChemicalBondingPowerpoint
ChemicalBondingPowerpoint

... KEY CONCEPTS  Water is a small, highly polar molecule. As a result, it is an extremely efficient solvent and has a high capacity for absorbing energy. ...
PHYSICS 4E QUIZ 4 SPRING QUARTER 2010 PROF. HIRSCH
PHYSICS 4E QUIZ 4 SPRING QUARTER 2010 PROF. HIRSCH

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Electrons in Atoms

... 1. Aufbau Principle Electrons enter orbitals of the lowest energy first, s
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Electrons in Atoms

... 1. Aufbau Principle Electrons enter orbitals of the lowest energy first, s
Biochemistry I (CHE 418 / 5418)
Biochemistry I (CHE 418 / 5418)

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SCIENCE 9

... has its own distinct properties and cannot be broken down into simpler substances by means of a chemical change. COMPOUNDS- are pure substances that are made up of two or more elements chemically combined together. Compounds can be broken down into elements again by chemical means DALTON’S ATOMIC TH ...
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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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