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# Class Note for CHEM 121 at UMass(12)

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This 2 page Class Notes was uploaded by an elite notetaker on Friday February 6, 2015. The Class Notes belongs to a course at University of Massachusetts taught by a professor in Fall. Since its upload, it has received 17 views.

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Date Created: 02/06/15
CHEM121H Honors General Chemistry 1 Mass Terms and Units Used in Describing Atoms Atomic Mass 1mg 7 The rest mass of an atom in its electronic and nuclear ground state NonSI unit The most common unit used is the uni ed atomic mass unit amu or u defined as 112 the mass ofa carbon12 atom in its ground state1 u 11661 x 103924 g For example the atomic mass ofa 10B isotope is 1001294 u and the atomic mass ofa 11B isotope is 1100931 u Mass or Nucleon Number 1A17 The total number of protons and neutrons collectively called nucleons in the nucleus of the atom The mass number is always a whole number For example the mass number oflOB is 10 5 protons 5 neutrons Atomic Weight 0r Relative Atomic Mass Ar 7 The weighted average mass of all naturally occurring isotopes of that element For example boron has two naturally occurring isotopes 10B 199 and 11B 801 The weighted average ofthese is 10799 u Mass Defect 7 The difference between the calculated mass of an atom based on the rest masses of atomic particles and the experimentally determined atomic mass The mass defect is converted into binding energy BE upon formation of the atom Atomic 0r Proton Number 1Z17 The number of protons in the atomic nucleus Always a whole number This is the basis for element ordering in the periodic table For example Z 1 for H Z 6 for C and Z 109 for Mt Meitnerium From Mills 1 et al Quantities units and symbols in physical chemistry The Green Book IUPAC Blackwell Publications Oxford 1988 and McNaught A D Wilkinson A Compendium of chemical terminology 2e The Gold Book IUPAC Blackwell Publications Oxford 1997 D L Adams 882005

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