Put the following elements in order from smallest to largest...

Put the following elements in order from smallest to largest mass:
(a) $3.79 \times 10^{24}$ atoms Fe
(e) 9.221 mol $\mathrm{Na}$
(b) $19.921 \mathrm{mol} \mathrm{H}_{2}$
(f) $4.07 \times 10^{24}$ atoms Al
(c) 8.576 mol $C$
(g) 9.2 mol $\mathrm{Cl}_{2}$
(d) $7.4 \mathrm{mol} \mathrm{Si}$

Key Concepts

Molar Mass

Molar mass is the mass of one mole of a substance and is expressed in grams per mole. It allows chemists to translate between the amount of substance (in moles) and its mass (in grams), providing a way to directly compare different substances based on the mass of their constituent particles.

Conversion Between Atoms and Moles

Converting between a count of atoms (or molecules) and moles is crucial in chemical calculations. When a sample’s particle number is given, dividing by Avogadro's number yields the amount in moles, which can then be used alongside molar mass for further conversions to mass.

Mass Comparison and Ordering

When comparing masses of different substances given in units of moles or numbers of particles, converting all quantities to a common measure like mass requires using both the mole concept and molar mass. This standardization makes it possible to order substances from smallest to largest mass effectively.

Mole Concept

The mole is a central unit in chemistry used to count particles, such as atoms, molecules, or ions, in a given sample. It provides a bridge between the atomic scale and macroscopic amounts of a substance by defining an amount that contains exactly 6.022 × 10^23 elementary entities.

Avogadro's Number

Avogadro's number, 6.022 × 10^23, is the constant that defines the number of particles in one mole of any substance. It is essential for converting between the number of atoms or molecules and the corresponding amount in moles, facilitating quantitative chemical analysis.

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