Pick the electron structures that represent elements in the same chemical family: (a) \(1 s^{2} 2 s^{1}\) (b) \(1 s^{2} 2 s^{2} 2 p^{4}\) (c) \(1 s^{2} 2 s^{2} 2 p^{2}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}\) (g) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) (h) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{1}\)

Understanding electron configurations is essential for recognizing how atoms will interact and bond with each other. An electron configuration is a way of arranging the electrons of an atom in its atomic orbitals. Think of it as a miniature city where electrons live in various neighborhoods (orbitals) such as the 's', 'p', 'd', and 'f' blocks.

For instance, consider an electron configuration like (b) in the exercise: \(1s^{2} 2s^{2} 2p^{4}\). The numbers represent the energy levels (like the floors in an apartment building), while the letters indicate the type of orbital (like the shape of an apartment), and the superscripts show the number of electrons in each orbital (the number of residents in each apartment). An element's chemical properties are predominantly determined by its valence electrons, which are the outermost electrons. They are the ones who 'socialize' with other atoms during chemical bonding. By understanding electron configurations, one can predict how an element will behave chemically.

When analyzing the configurations in the given exercise, it is crucial to pinpoint the valence electrons to determine the chemical family, as elements in the same family share similar electron configurations in their outermost shells.

A chemical family, also known as a group, comprises elements that have similar chemical behaviors. This kinship stems from the fact that they all have the same number of valence electrons. The periodic table is kind of like a family tree, classifying elements by their chemical lineage. For example, in our exercise, configurations (b) \(1s^{2} 2s^{2} 2p^{4}\) and (d) \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{4}\) are part of the same chemical family because both have 6 valence electrons.

Valence electrons are responsible for an element's ability to form bonds and are located on the element's outermost shell. When elements share the same number of valence electrons, they exhibit similar bonding characteristics and reactivities. In classrooms and textbooks, you might often come across terms such as noble gases, halogens, or alkali metals. These are all names of different chemical families, each with unique and characteristic properties, making them motif characters in the story of chemistry.

The periodic table is more than just a list of elements; it's a map of chemical properties patterned in rows and columns known as periods and groups, respectively. The elements in each group or column share common characteristics, like actors playing similar roles across different movies. This is because, within a group, they all have the same number of valence electrons. These outer electrons dictate an element's chemical behavior.

In our exercise, elements that were in the same group were (a) with (g), having 1 valence electron, and (f) with (h), having 2 valence electrons, indicating that they belong to the same respective columns on the periodic table. These groups are also known by family names. For example, group 1 contains the alkali metals, notorious for their reactivity with water, while group 17 contains the halogens, which are equally reactive but in different ways. Understanding the groupings within the periodic table helps us forecast the properties and behaviors of the elements without needing to memorize the attributes of each one individually.

The periodic table is a magnificent puzzle, and each group is a piece of the story. By learning the layout and the patterns, you can start to see how each piece fits together and why elements behave the way they do.