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Chem 105 Ch 2

Quiz yourself by thinking what should be in each of the black spaces below before clicking on it to display the answer.
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Term
Definition
Subatomic particles   protons, neutrons, and electrons  
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Thomson cathode ray tube experiment   found mass-to-charge ratio of election  
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Cathode rays   beam of electrons  
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Electrons   negatively charged subatomic particle with a very small mass (9.109x10^-31g)  
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Millikan oil drop experiment   mass of an electron  
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Cations and anions   positive and negative ions respectively  
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Rutherford gold foil experiment   shot positive helium nuclei at gold foil, most go through, some reflected a little, some completely; found most of atom is empty space with a dense nucleus  
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Atomic nucleus   nucleus contains protons and neutrons, protons always the same for an element, neutrons may differ  
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Atomic mass units   one twelfth the mass of carbon 12  
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1 amu   1.66054x10^-27 kg  
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Nuclide/isotope   different number of neutrons  
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Atomic number   number of protons  
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Mass number   sum of protons plus neutrons  
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Periodic table   chart of elements in order of atomic number, reflect physical  
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Periods   rows  
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Groups   columns  
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Main group elements   everything but  
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Metals   everything left of metalloids  
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Alkali metals   group 1  
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Alkaline earth metals   group2  
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Transition metals   d level  
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Metalloids   steps  
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Nonmetals   not a metal, right of metalloids  
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Halogens   group 17  
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Noble gases   group 18  
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Atomic mass   weighted average of natural abundance of isotopes  
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Natural abundances   percentage of  
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Formula mass   for formula unit  
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Mole   chemist's dozen  
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Avogadro’s number   6.0221x10^-23  
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Molar mass   mass per mole of an element  
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