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Understanding moles and Avogadro's number is key to tackling problems involving quantities of atoms in a substance. A "mole" is a unit used by chemists to count atoms, much like a "dozen" is used to count eggs. One mole contains exactly \(6.022 \times 10^{23}\) particles—whether they are atoms, molecules, or ions. This extremely large number is known as Avogadro's number. To find the number of moles in the gold ring, we divide its mass by the atomic mass of gold. For example:

• Mass of the gold ring: 17.7 grams
• Atomic mass of gold: 197 grams/mole

Hence, the moles of gold in the ring is \(\frac{17.7}{197} \approx 0.0898\) moles. Once moles are calculated, we use Avogadro's number to find the number of atoms. In this case, \(0.0898 \text{ moles} \times 6.022 \times 10^{23} \text{ atoms/mole} \approx 5.40 \times 10^{22} \text{ atoms}\). This calculation allows us to understand the scale of particles present even in a small jewelry item.

Each element on the periodic table is defined by its atomic number, which tells us the number of protons in the nucleus of an atom. Protons are positively charged particles that reside in the nucleus. For gold, the atomic number is 79, indicating each gold atom has 79 protons. The atomic number is fundamental as it determines the element's identity. Considering the gold ring with \(5.40 \times 10^{22}\) atoms, the number of protons can be calculated as:

• \(79 \times 5.40 \times 10^{22} \approx 4.27 \times 10^{24} \text{ protons}\)

The importance of protons extends beyond just counting particles; they contribute to the chemical properties and overall structure of the element. In this exercise, knowing the protons helps us calculate the total positive charge of the gold ring.

The concept of electric charge is vital in understanding atomic interactions. Protons have a positive charge of \(1.602 \times 10^{-19}\) Coulombs each, which is fundamental to their role in atomic structure. In our example, once we calculate the number of protons in the gold ring, we can find the total positive charge by multiplying the number of protons by the charge of a single proton:

• Total positive charge: \(4.27 \times 10^{24} \text{ protons} \times 1.602 \times 10^{-19} \text{ C/proton} \approx 6.84 \times 10^{5} \text{ C}\)

If the gold ring has no net charge, this implies the number of electrons equals the number of protons. Since electrons carry a negative charge equal in magnitude to that of protons, but negative, their presence balances out the total charge of the gold ring. Thus, we see that the number of electrons also amounts to \(4.27 \times 10^{24}\), ensuring electronic neutrality.