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Atoms, molecules and stoichiometry

Atoms, molecules and stoichiometry

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Chapter Summary

  • Learning Outcomes 🎯:

    • Define and use terms such as relative atomic mass, isotopic mass, empirical formula, molecular formula, and the mole in terms of the Avogadro constant.

    • Analyze and use mass spectra to calculate the relative atomic mass of an element.

    • Calculate empirical and molecular formulas using combustion data or composition by mass.

    • Write and construct balanced equations.

    • Perform calculations involving the mole concept, reacting masses, volumes of gases, and volumes and concentrations of solutions.

    • Deduce stoichiometric relationships from calculations involving reacting masses, volumes of gases, and volumes and concentrations of solutions.

  • Relative Atomic Mass and the Mole 🧮:

    • Relative atomic mass is the weighted average mass of naturally occurring atoms of an element on a scale where an atom of carbon-12 has a mass of exactly 12 units.

    • The mole is a unit used to count the number of particles in a substance and is based on the Avogadro constant.

  • Empirical and Molecular Formulas 📝:

    • Empirical formulas show the simplest whole-number ratio of atoms in a compound.

    • Molecular formulas show the total number of atoms of each element present in one molecule or one formula unit of the compound.

  • Balancing Chemical Equations ⚖️:

    • Chemical equations must be balanced to ensure that the number of atoms of each element on the reactants side is equal to the number on the products side.

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