Identify these elements from their atomic structure diagrams: (a) \(16 \mathrm{p}\) \(16 \mathrm{n}\) \(2 \mathrm{e}^{-} \quad 8 \mathrm{e}^{-} \quad 6 \mathrm{e}^{-}\) (b) \(\left.\begin{array}{l}28 \mathrm{p} \\ 32 \mathrm{n}\end{array}\right) 2 \mathrm{e}^{-} \quad 8 \mathrm{e}^{-} \quad 16 \mathrm{e}^{-} \quad 2 \mathrm{e}^{-}\)

Understanding the atomic number of an element is crucial for identifying it. In simple terms, the atomic number is the number of protons present in the nucleus of an atom. Each element has a unique atomic number, which distinguishes it from other elements. For example, in the exercise given, the atomic number for element (a) was found to be 16 due to the presence of 16 protons. This is a defining feature because no two elements have the same number of protons.

Therefore, the atomic number serves as an identifier and is used extensively to arrange elements in the Periodic Table. Thanks to this systematic arrangement, once you know the atomic number of an element, you can easily find it in the Periodic Table and determine many of its properties.

Electron configuration is another key to unlocking the identity of an element. This configuration describes the arrangement of electrons in an atom's various energy levels or shells. Electrons fill these shells in a specific order, generally starting with the shell closest to the nucleus. The exercise illustrates this: element (a) has its electrons arranged in a '2-8-6' format. It signifies 2 electrons in the closest shell, followed by 8 in the next one, and finally 6 in the third shell.

Knowledge of the typical electron configurations can help you predict and explain chemical properties of elements. For instance, Sulfur usually has a '2-8-6' electron configuration, matching the one provided in the exercise. It is important to note that some elements can have multiple electron configurations due to the various possible arrangements electrons can have, especially in a more complex chemistry context like bond formation or excited states.

The Periodic Table of Elements is an invaluable tool for chemists, highlighting the orderly arrangement of all known elements based on their properties. Elements are listed by increasing atomic number, but they are also grouped by common properties. For example, columns, known as groups or families, contain elements with similar chemical behaviors.

The Periodic Table also provides information about the electron configurations as you move across periods and down groups, reflected in the exercise solutions. By knowing the atomic number and electron configuration, like with Nickel (element b) with an atomic number of 28, you can locate the element's position on the Periodic Table. This not only helps identify the element but also provides insights into its potential reactivity and the types of chemical bonds it can form.