Nuclear Chemistry. Deals with the nucleus of the atom (protons & neutrons) Matter is changed into energy by the breaking up of the nucleus of an atom Mass defect – The difference in the calculated mass of an atom and the measured mass of an atom Mass of neutron = 1.67493x10 -27 kg
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Calculate the binding energy of for carbon -12 (atomic mass 12.000) and uranium-235 (atomic mass 235.0439). The atomic mass of 11H is 1.00782 amu and the mass of a neutron is 1.00866 amu.
Looks at the proton/neutron ratio
Atoms with a high p+/n0 - emit- particles
Atoms with a low p+/n0 - +emission or e-capture
Atomic #s 84+ - emission
2. - - beta particle – 0-1e
3. - gamma ray – energy
4. + - positron – 0+1e
1. 0-1e – electron is taken in
116C 115B + 01 116C + 0-1e 115B
146C 147N + 0-1 19278Pt 18876Os + 42He
(nuclear fission) 23592U + 10n 9336Kr + 14056Ba + 310n
Shortened notation = 23592U (10n, 310n) 9336Kr, 14056Ba
Complete the following nuclear equations.
One type of commerical smoke detector contains a minute amount of radioactive americium-241 which decays by particle production. The particles ionize molecules ini the air, allowing it to conduct an electric current. When smoke particles enter, the conductivity of the air is changed and the alarm buzzes.
b. The complete decay of 241Am involves successively , , , , , , , , , , , and . What is the final stable nucleus produced in this decay series?