Atomic Calculations and Mass Spectrometry

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Presentation transcript:

Atomic Calculations and Mass Spectrometry Quantum Orbital Video

Atomic Mass – Atomic Number = # Neutrons (p + n) - (p) = (n)

Complete the following chart: protons electrons neutrons H Zr Ca2+ P3- Al3+ Cl- 1 1 0 40 40 51 20 18 20 15 18 16 13 10 14 17 18 19

Isotopes- same atomic number but different mass For example, there are 3 types of hydrogen atoms. 1H 2H 3H Not all atoms of the same element are identical.

Mass Spectrometers Are used to determine the abundance and mass of the isotopes of elements

Mass Spectrometers A device known as a mass spectrometer can be used to determine the relative abundance and the mass of the isotopes of elements. In the graph the isotopes of a sample of the element zirconium can be seen in their relative abundances.

The data can be summarized as follows: Isotope Mass` Abundance 90Zr 90.00 amu 51.5 % 91Zr 91.00 amu 11.2 % 92Zr 92.00 amu 17.1 % 94Zr 94.00 amu 17.4 % 96Zr 96.00 amu 2.80 % atomic mass of isotope 100 %

Calculate the weighted average mass of zirconium using the data above. Change each percent to a decimal by dividing by 100. Multiply by the mass. Add it all together. 0.515(90.00) + 0.112(91.00) + 0.171(92.00) + 0.174(94.00) + 0.0280(96.00) = 91.3 amu 3 sig figs! Look up the mass on the periodic chart. The unit amu describes how many times heavier than the mass of H = 91.2 amu They are the same with uncertainty

Calculate the average atomic mass for Germanium 36.54 % 73.92115 amu 27.43 % 71.92174 amu 20.52 % 69.92428 amu 7.76 % 75.9214 amu 7.76 % 72.9234 amu (0.2052)(69.92428) + (0.2743)(71.92174) + (0.0776)(72.9234) + (0.3654)(73.92115) + (0.0776)(75.9214) = = 72.6 amu Periodic Table = 72.6 amu

Quantum orbitals