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lecture_CH1-2review_chem121pikul
lecture_CH1-2review_chem121pikul

...  Distinguish the difference between chemical and physical properties & changes  We represent uncertainty with significant figures  You do not need to memorize Sig Fig rules  Scientific Notation  Conversions within the metric system and non metric units  Temperature conversions  Density & Spec ...
Electron Configurations
Electron Configurations

... you may want some extra information on the subject. Most of this below is “borrowed” from Sparknotes.com. The first and most important rule to remember when attempting to determine how electrons will be arranged in the atom is Hund’s rule, which states that the most stable arrangement of electrons i ...
Evolution of Atomic Models
Evolution of Atomic Models

... Down the wrong path… •400 BC – Democritus proposed that atoms make up substances •Aristotle disagreed with him and thought matter was uniform throughout •This was accepted for the next 2,000 years! ...
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C:\Documents and Settings\Travis D. Fridgen\My Documents

... classical physics predicted that a charged particle travelling in a circular orbit would emit light, losing energy, and spiral into the nucleus. The atom and thus matter would be unstable. ii) Bohr used the idea of quantization to overcome the problem with Rutherford’s model. He postulated that the ...
Mastering the Ultra-Cold
Mastering the Ultra-Cold

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Honors Chemistry

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Physics 107 Exam #3 October 13, 1994 Your name: Multiple Choice

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Lecture 12

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Quantum Notes (Chapter 16)(Powerpoint document)

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... • When the elements are listed in order of atomic number, elements with similar chemical and physical properties recur at regular interval, known as the periodical law. • Elements with similar properties form the groups shown as vertical columns in the table. • The horizontal rows in the table are c ...
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chapter 7: atomic structure and periodicity
chapter 7: atomic structure and periodicity

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Electron Configuration

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... ii. h = Planck’s constant = 6.626 x 10 -34 J.s iii. v = frequency (Hertz) b. Energy of radiation increases as the radiation’s frequency increases. 4. According to Planck’s theory, for a given frequency, matter can emit or absorb energy only in whole-number multiples of hv. b. The Photoelectric Effec ...
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PowerPoint Template

... matter usually occurs as mixtures, such as air, seawater, soil, and organisms A heterogeneous mixture has one or more visible boundaries between the components Example: rocks A homogeneous mixture has no visible boundaries because the components are mixed as individual atoms, ions, and ...
Solute
Solute

... electrons Protons – have a positive charge Neutrons – no charge Electrons – negative charge In a neutral atom, #protons = #electrons ...
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... dipole or two dipoles where the (+) charge attracts the (-) charge (purely electrostatic) • H-bonding : a special type of dipole-dipole interaction that results from the bonding between a H atom which is partially (+) charged and a highly electronegative atom such as O, F, N, Cl, (directional) ...
Electronic structure (download)
Electronic structure (download)

... Electrons are waves too! Life at the electron level is very different Key to unlocking the low door to the secret garden of the atom lay in accepting the wave properties of electrons De Broglie wave-particle duality All particles have a wavelength – wavelike nature. – Significant only for very smal ...
Presentation - University of Colorado Boulder
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... 1. Scalable array of well defined qubits. 2. Initialization: ability to prepare one certain state repeatedly on demand. 3. Universal set of quantum gates: A system in which qubits can be made to evolve as desired. ...
Atomic Structure and Chemical Bonding
Atomic Structure and Chemical Bonding

The Pauli exclusion principle states that no two fermions
The Pauli exclusion principle states that no two fermions

... the way atoms share electrons. It explains the variety of chemical elements and their ...
The Quantum Model of the Atom
The Quantum Model of the Atom

... • Electron can neither gain nor lose energy • “the single electron of hydrogen orbits the nucleus only in allowed orbits, each with a fixed energy” ...
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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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