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Summary Stoichiometry
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Summary of 3rd chapter from Chemical Principles: Zumdahl and Decoste. Notes containing key concepts from the chapter and thorough explanations of the terminology. Also includes formulas and relevant course-related information.

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  • Chapter 3
  • July 19, 2019
  • 3
  • 2018/2019
  • Summary

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Stoichiometry
3.1 Atomic Masses

 All the masses in the modern periodic table are relative to Carbon, where C
is given a mass exactly of 12 atomic mass units (amu).
 Mass spectrometer is used to compare the masses of atoms, it is an
instrument which delocalizes electrons from a sample atom using a beam of
high speed electrons, which is later accelerated through a magnetic field;
the deviation from the path formed by original C-12 is measured as a ratio,
which is later multiplied by C-12 mass to give the relative mass of the atom.
 Atomic mass is an average value based on isotopic composition of an
element.
 A mass spectrometer is also used to determine the isotope composition of
a natural element.

3.2 The Mole

 A mole is the number equal to the number of Carbon atoms in exactly 12g
of Pure C-12.
 Avogadro’s number, known as the mol, is 6.022x1023
 A mole can also be considered as the ratio between the mass of an atom in
grams to its molar mass.

3.3 Molar Masses

 Molar mass is the mass in grams of 1 mole of a compound.
 For ionic compound, the term formula weight is utilized, as there is no
actual covalent relation between multiple elements in an ionic substance.

3.4 Conceptual Problem Solving

 First, we should read the problem and decide where we are going, what are
we seeking for.
 Next, we must sort out the key facts given in the information of the
problem.
 Develop a procedure either back-to-forth or from reactants to products to
approach the problem. Recall any formulas or relations we must express in
order to solve the problem.
 Verify the solution that we have reached to.

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