## Two Ways

One can calculate atom weight from knowing the weights of the constituent electrons, protons, and neutrons. If you know the weight of each of those and the number of each in an atom, you can readily calculate its weight. Yet, there is an easier and a better way. Let’s pick an element out of the hat. Let’s take gold (If we can’t afford it, at least we can talk about it.). To calculate atom weight by method two, we need to look at the*Periodic Table of the Elements*. There we see gold, chemical symbol Au, as element number 79. At the bottom of the little square, we see the number 196.97. This is the atomic weight of gold. The atomic weight in grams of an element equals the weight of an Avogadro’s number of that element. Huh? What?

## Avogadro’s Number

Avogadro was a 19th century Italian chemist who studied the physical properties of gases. He stated that the volume of a gas at a given temperature and pressure does not depend upon the nature of the gas, but is the same for all gases. A constant was derived, which was later named in his honor. That number is currently placed atNav = 6.022 x 10²³ moles⁻¹

Although this was derived in connection with gases, the number is the same for solids and liquids, also, as it is in terms of weight, and not volume. There is an Avogadro’s number of atoms of an element in a mole of that element.## Calculate Atom Weight – Gold

That being the case, the weight of a gold atom becomes,w = (196.97 grams/mole) / 6.022 x 10²³ moles⁻¹

Since the mole units cancel out, we are left with the weight of the gold atom in grams. The math gives usResult: w = 3.27 x 10⁻²² grams per atom.

## Checking by Method One

We’ve just learned the simplest way to determine the weight of an atom of any particular element. Let’s perform the check using the weights of electrons, protons, and neutrons. This would not be so easy if gold had a number of isotopes. Gold has only one stable isotope however. What does this mean? An isotope is an element that has the same number of protons and electrons as any other atom of an element, but a differing number of neutrons. What makes it more difficult is that percentages of isotopes found in nature vary for different elements. Does this make it clear why method two is much simpler to use in determining the weight of an atom of an element than method one? If we want to know the weight of a particular isotope, however, the first method is superior, since the Periodic Table assumes a mixture of isotopes. Gold found in nature has 79 protons, 79 electrons, and 118 neutrons. The weight of a proton in grams is 1.673 x 10⁻²⁴ grams. The weight of a neutron is 1.675 x 10⁻²⁴ grams. The weight of an electron is 1/1836th the weight of a proton, so it weighs 9.11 x 10⁻²⁸ grams. This gives us,w = (79 x 1.673 x 10⁻²⁴) + (79 x 9.11 x 10⁻²⁸) + (118 x 1.675 x 10⁻²⁴) grams

This gives,w = (132.2 + 0.0720 + 197.7) x 10⁻²⁴ grams

Result: w = 3.30 x 10⁻²² grams/atom

The results are the same to within one percent.## Why the One-Percent Difference?

It ought first to be noted that for most purposes, this one-percent difference is quite acceptable. As to why there is a difference? There are a number of reasons for it. We rounded off Avogadro’s number down. We rounded the weights of the subatomic particles. Also, the weight of an atom is not strictly equal to the weight of all its subatomic particles. The reader is doubtless well aware that atomic fission is sometimes called “atom splitting.” The energy given off by the splitting of an atom is tremendous. Curiously, the energy weighs something. In fact, how much it weighs can also be calculated according to Einstein’s equation,E = mc²

The mass, or for our purposes, the weight of energy can be found by changing this around to,m = E/c²

This weight (actually, mass) is added to the weight (mass) of an atom. The combination of adjustments should put the result much closer to the mark than even the one percentage point of error.

**Note:**You may also enjoy Total Energy in One Hydrogen Atom**References:**

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