Which of the following statements is/are TRUE concerning the "mole"?

(a) One mole of a substance contains as many particles as exactly 12 amu of
carbon-12.
(b) One mole of a substance contains 6.022 x 1023 particles of that substance.
(c) There are 6.022 x 1023 carbon atoms in 12.00 g of carbon-12.
(d) Because it is heavier, a mole of iodine atoms contains more atoms than a
mole of bromine atoms.

C

Explanation: the clumsy definition of the mole obscures its utility.  It is nearly analogous to defining a dozen as the mass of a substance that contains the same number of fundamental units as are contained in 733 g of Grade A large eggs.  This definition completely obscures the utility of the dozen: that it is 12 things!  Similarly, a mole is NA things. The mole is the same kind of unit as the dozen -- a certain number of things.  But it differs from the dozen in a couple of ways.  First, the number of things in a mole is so huge that we cannot identify with it in the way that we can identify with 12 things.  Second, 12 is an important number in the English system of weights and measures, so the definition of a dozen as 12 things makes sense. However, the choice of the unusual number, 6.022 x 1023, as the number of things in a mole seems odd. Why is this number chosen?  Would it not make more sense to define a mole as 1.0 x 1023 things, a nice (albeit large) integer that everyone can easily remember? To understand why the particular number, 6.022 x 1023 is used, it is necessary to resurrect an older, in some ways more sensible and useful, definition of the mole, which is grounded in the atomic weight scale addressed above.

The atomic weight scale defines the masses of atoms relative to the mass of an atom of 12C, which is assigned a mass of exactly 12.000 atomic mass units (amu). The number 12 is chosen so that the least massive atom, hydrogen, has a mass of about 1 (actually 1.008) on the scale.  The atomic mass unit is a very tiny unit of mass appropriate to the scale of single atoms.  Originally, of course, chemists had no idea of its value in laboratory-sized units like the gram.  The early versions of the atomic weight scale were established by scientists who had no knowledge of the electron, proton, or neutron.  When these were discovered in the late 19th and early 20th centuries, it turned out that the mass of an atom on the atomic weight scale was very nearly the same as the number of protons in its nucleus.  This is a very useful correpondence, but it was discovered only after the weight scale had been in use for a long time.

In their desire to be able to count atoms by weighing, chemists gradually developed the concept of the "gram-atomic weight", which was defined in exact correspondence with the atomic weight scale:

    1 atom of 12C weighs 12.000 amu

    1 gram-atomic weight of 12C weighs 12.000 g

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