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Lecture 1.6 PowerPoint
Lecture 1.6 PowerPoint

... level of the s, p, d, and f orbitals. Furthermore, I can draw the s and p orbitals. • 1.8 – I can write the electron configuration and orbital diagram for any element on the Periodic Table using the Pauli Exclusion Principle and Hund’s ...
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Chapter 7 - Chemical Quantities

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... classical mechanics a particle can possess any amount of energy between zero and infinity. Also, the position and velocity of the particle can be determined simultaneously. Newton’s law of motion and Maxwell’s electromagnetic wave theory successfully explained most of the phenomena known then. But w ...
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Lecture 21 revised (Slides) October 12

... Transition Metals – Electron Configurations • Transition metals have surprisingly rich chemistry. The electronic configurations of the neutral atoms are relatively complex since d subshells (with 5 orbitals) are being filled. For the first series of transition metals the 4s and 3d subshells have si ...
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PHYS150-Ch27

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Department of Physics and Astronomy University of Georgia —

... (a) If the atoms are sodium (A = 23) and derive from a thermal ensemble that has been lasercooled to a temperature of 1 mK, what is the RMS (root-mean-square) speed of the atoms in the beam? (b) What is the deBroglie wavelength of an atom traveling at the RMS speed? (c) By treating the laser beam st ...
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Assignment 8 - Duke Physics

... Note that this problem is an important historical insight from the early days of quantum mechanics, it suggested that when an electron is emitted by radioactive decay of some nucleus, the electron could not have already existed in the nucleus but had to be created by the decay process. (Does this ar ...
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PPT format - Columbia University

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Atomic Structure - The Student Room

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...  This half filled, or filled d orbital, is used most of the time to explain this, but other transition metals do not follow this trend.  AUFBAU exceptions of chromium and copper as a half full sublevel are more stable than a full 4 s sublevel, or for copper that a full d-sublevel is more stable th ...
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Wave Props of Particles - Chemistry at Winthrop University

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Monday, March 3, 2014

... Importance of Bohr’s Model • Demonstrated the need for Plank’s constant in understanding the atomic structure • Assumption of quantized angular momentum which led to quantization of other quantities, r, v and E as ...
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NSS Physics Curriculum - VII Atomic World Intention Intention Intention

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... The lowest energy levels of the atom are due to excitations of electrons between outer levels (where the smallest energy gaps and the first vacancies exist). For electrons in the n=3 electron orbitals, the nuclear charge (Z=+11e) is screened by the inner 10 electrons from the n=1 and n=2 shell (Q=-1 ...
Structure of Atom
Structure of Atom

... Consider the hydrogen atom to be a proton embedded in a cavity of radius a o (Bohr radius) whose charge in neutralized by the addition of an electron to the cavity in vacuum, infinitely slowly. Estimate the average total energy of an electron in its ground state in a hydr5ogen atom as the work done ...
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chapter 1 - College Test bank - get test bank and solution manual

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1. Review (MC problems, due Monday) 2. - mvhs

... 20. Account for each of the following in terms of principles of atomic structure, including the number, properties, and arrangements of subatomic particles. (a) The second ionization energy of sodium is about three times greater than the second ionization energy of magnesium. (b) The difference betw ...
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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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