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NAME PRACTICE: QUANTUM CONFIGURATIONS 1) Each of the
NAME PRACTICE: QUANTUM CONFIGURATIONS 1) Each of the

... ___20) The ground-state configuration for the atoms of a transition element ___21) The ground-state configuration of a negative ion of a halogen ___22) The ground-state configuration of a common ion of an alkaline earth element Use these answers for questions 23-25. (1) Heisenberg uncertainty princi ...
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chapter 7: atomic structure and periodicity

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Bohr Model, Quantum Mechanical Model
Bohr Model, Quantum Mechanical Model

... b. energy is involved in moving an electron from one level to another. 4. Heisenberg Uncertainty Principle- It is impossible to know the momentum (mass of electron times velocity) of an electron and its position in space at the same time. One or the other. 5. Quantum Mechanical Model- a mathematical ...
Nuclear Fission sim
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... Why do fission and fusion produce so much energy? • In nuclear reactions, energy comes from converting tiny amounts of mass lost when the bonds between protons and neutrons are broken and made. These bonds are due to the strong force. • The strong force is a thousand times stronger than the electri ...
Bohr vs. Correct Model of Atom
Bohr vs. Correct Model of Atom

... • h (Planck’s constant) = 6.63 x 10-34 J-s • 1 eV = kinetic energy of an electron that has been accelerated through a potential difference of 1 V 1 eV = q x V = 1.6 x 10-19 J ...
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ionization energies

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Periodic Trends/Patterns

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... The Bohr Model • Niels Bohr (1885 – 1962) – Danish Physicist/ Student of Rutherford – An electron is found only in specific circular paths, or orbits, around the nucleus. – The energy of an atom changes when it absorbs or emits light. – Each orbit has a fixed energy (each orbital is a different ene ...
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Atomic Structure and Electron Configurations Multiple Choice PSI

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... Atomic Structure and Electron Configurations Multiple Choice PSI Chemistry Name:________________________ 1. Rutherford’s Nuclear Model of the atom A. is the currently accepted atomic model. B. explains the unique emission spectra of different elements. C. does not account for the stability of most a ...
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Unit 3 – Quantum Mechanical Model of the Atom

... energy, it jumps from its ground state to an excited state. • When the electron falls back to the ground state, energy is given off in the form of light. • Bohr used Planck’s equation, E = hv, to verify this theory for hydrogen. ...
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... In every atom there is a balance between the attraction of the positively charged nucleus for the negatively charged electrons and repulsion between the electrons. The outer electrons (valence electrons) do not experience the full attraction of the positive nucleus because of the presence of inner e ...
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Chapter 7 Section 1 - School District 27J

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... • Each orbital, in each energy level can only hold a maximum of 2 e-. • s sublevel  1 orbital, 2 e• p sublevel  3 orbitals, 6 e• d sublevel  5 orbitals, 10 e• f sublevel  7 orbitals, 14 e- ...
Electronic Structure of Atoms (i.e., Quantum Mechanics)
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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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