Question

In what main group(s) of the periodic table do element(s) have the following number of filled p orbitals in the outermost principal level? (a) 0 (b) 1 (c) 2 (d) 3

Short answer

Question: Identify the main group(s) of the periodic table in which elements have the following numbers of filled p orbitals in their outermost principal level: (a) 0 filled p orbitals (b) 1 filled p orbital (c) 2 filled p orbitals (d) 3 filled p orbitals Answer: (a) Groups 1 and 2 (b) Group 13 (c) Group 14 (d) Group 18

Step-by-step solution

Understand the p orbitals and their relationship with outermost principal level

The p orbitals are three-dimensional orbitals (denoted as px, py, and pz) that can accommodate up to 6 electrons in total, with 2 electrons in each orbital. They are one of the types (s, p, d, and f) of atomic orbitals that electrons occupy in an atom. The outermost principal level is the highest energy level that contains electrons, and the number of filled p orbitals refers to the number of p electrons in the outermost principal level, also known as the valence shell.

Identify the main groups with the given number of filled p orbitals

We will now identify the main groups of the periodic table that have the given number of filled p orbitals for each case: (a) 0 filled p orbitals: In this case, the elements have no p electrons in their valence shell. s-block elements (groups 1 and 2) have only s electrons in their outermost shell, while d- and f-block elements don't have a filled p orbital as well. However, since the exercise asks for the main groups of the periodic table, we will only consider the s-block elements. So, Main group: Groups 1 and 2 (b) 1 filled p orbital: Here, the elements have 2 p electrons in their valence shell. These elements correspond to Group 13 or the Boron group since the general electronic configuration for this group is ns^2np^1. So, Main group: Group 13 (c) 2 filled p orbitals: In this case, the elements have 4 p electrons in their valence shell. These elements belong to Group 14 or the Carbon group, as the general electronic configuration for this group is ns^2np^2. So, Main group: Group 14 (d) 3 filled p orbitals: For elements with 6 p electrons in their valence shell, they belong to Group 18 or the Noble gases group (except Helium, with 2 s electrons only). The general electronic configuration for these elements is ns^2np^6. So, Main group: Group 18

Key concepts

P Orbitals

When diving into the world of atomic chemistry, one of the essential concepts is understanding 'p orbitals'. These orbitals are critical in determining the chemical properties and reactivity of an element. P orbitals, shaped like dumbbells, exist in three orientations: px, py, and pz. They can collectively hold up to six electrons, with a maximum of two electrons per orbital occupying these spaces in pairs with opposite spins. As we visualize the atom in layers, we find that these p orbitals exist in the second and higher principal energy levels (starting at n=2).

When elements have electrons in their p orbitals, these electrons can participate in chemical bonding. The configuration of these p electrons plays a significant role in determining how the atoms interact with each other. For instance, oxygen, with its four p electrons, is highly reactive, while neon, with a full set of six p electrons in its outer p orbitals, is inert. Knowing which orbitals are filled allows us to predict the group to which an element belongs and its typical reactions.

Valence Shell

The 'valence shell' is effectively the outermost shell of an atom that can contain electrons. It is crucial in defining an element's chemical properties, as the electrons in the valence shell are the ones involved in forming bonds with other atoms. These electrons determine the reactivity and the type of bonds an element can form. The number of electrons in this shell can vary, but elements with similar valence shell configurations are grouped together in the periodic table because of their similar chemical properties.

For a clearer understanding, consider sodium (Na), which has one electron in its valence shell. This single electron is easier to remove, making sodium an excellent conductor and highly reactive—it's eager to lose that one electron to reach a stable configuration. The valence shell is the foundation for understanding how elements interact and combine to form compounds, and thus, a solid grasp of its implications is vital for anyone studying chemistry.

Electronic Configuration

Every element on the periodic table has a unique 'electronic configuration', a specific arrangement of electrons in its atomic orbitals. This configuration follows a set of principles, such as the Aufbau principle, Hund's rule, and Pauli's exclusion principle, to achieve the most stable arrangement. The electronic configuration is often written in a shorthand notation that indicates the number of electrons in each shell and subshell (e.g., 1s² 2s² 2p⁶ for neon).

Understanding an element’s electronic configuration can give us a lot of information about its properties and behavior. For example, elements in the same group share similar valence electron configurations which dictate their reactivity and bonding patterns. When determining the group an element belongs to, one can usually look at the highest-energy electrons, or the outermost configuration, as these will be the ones participating in chemical bonds. By studying the electronic configuration, we gain insights into the periodic trends and the nature of the elements.