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Quantum review
Quantum review

Chapter 6: Electronic Structure of Atoms Recommended Text
Chapter 6: Electronic Structure of Atoms Recommended Text

... electronic configuration of 10B differ from that of 11B? Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? Indicate three major ways in which the 1s electrons in boron differ from its 2s electrons. Elemental boron reacts with fluorine to form BF3, a gas. Write a ...
Chem 1a Review
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... When you add 1 electron (to a partially filled orbital) and 1 proton the added electrons do not completely shield the added positive charge. Thus the effective nuclear charge goes up and the electrons are held more tightly. The ionization energy, Iz, also goes up, and the atom becomes smaller. When ...
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... – Used quantum theory, and atomic spectra to fix problems with the Rutherford model. Proposed: – An electron can only occupy certain allowed orbits without radiating – Each nth orbit has a radius (rn) and an energy (En). – An electron can make a transition between two orbits through • Absorbing a Ph ...
Chapter 7 - Gordon State College
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... - We can consider the nucleus to be fixed and the electron to be revolving about it. - The force holding the electron in a circular orbit is supplied by the columbic force of attraction between the proton and the electron. ...
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Chemistry is a material science
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... ______ of atoms and molecules are present in this matter. Matter composed of _______ kind of particle such as an atom or molecule is a pure __________ or simply a substance. Substances are comprised of only one kind of ________ or ___________. Substances have _________ properties such as melting and ...
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... 3.5 Percentage yield Very few chemical reactions have a yield of 100% because: • Reaction is reversible • Some reactants produce unexpected products • Some products are left behind in apparatus • Reactants may not be completely pure • More than one product is produced and it may be difficult to sep ...
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... Classical electrodynamic theory rejected (charged particles undergoing acceleration must emit radiation) Electron assumed to travel in circular orbits. Only orbits with quantised angular momentum are allowed (as observed in spectra) h mvr = n 2π Electromagnetic radition is adsorbed or emitted only w ...
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... Any object (including atoms) can emit or absorb only certain quantities of energy. Energy is quantized; it occurs in fixed quantities, rather than being continuous. Each fixed quantity of energy is called a quantum. An atom changes its energy state by emitting or absorbing one or more quanta of ener ...
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... In 1926, the German physicist Erwin Schroedinger used de Brogli’s wave model to create a quantum theory of atom based on waves. The theory does not provide a simple planetary picture of an atom as in the Bohr model. In particular, the radius of the electron orbit is not like the radius of the orbit ...
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... (determine the charge or oxidation number using your periodic table) Write the symbol for the negative ion second (determine the charge or oxidation number using your periodic table). An oxidation number (or charge) indicates how many electrons are lost, gained or shared when bonding occurs. ...
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... bound and readily enter into metallic bond formation. The metallic radius decreased in passing from Sc to Ni. Addition of electrons might be expected to result in an increase in radius, but the electrons are being added to an inner orbital and it is the increased in nuclear charge in passing from Sc ...
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... Since the wavefunctions have different probability density distributions, the energies E+total and E-total are also different. For (y1+y2) it is more likely to find the electron between the protons, which reduces the repulsion and hence a lower energy solution results, ie. to take the electron from ...
Chemistry Midterm Review 2006
Chemistry Midterm Review 2006

... 15. A copper penny has a mass of 3.1 g and a volume of .35 cm3. What is the density? 16. A plastic ball has a volume of 19.7 cm3 and a density of .8029 g/cm3. What is the mass? 17. The density of silicon is 2.33 g/cm3. What is the volume if its mass is 62.9g? 18. Convert 157 cg into g. Convert 8.6 ...
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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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