Question

The ______ elements achieve an electron configuration analogous to the previous noble gas by losing electrons from their valence shells.

Short answer

The type of elements that achieve an electron configuration analogous to the previous noble gas by losing electrons from their valence shells are \(\textbf{metals}\).

Step-by-step solution

Identify the Elements

The elements in the Periodic Table can be broadly classified as metals, non-metals, and metalloids. Metals are on the left side of the periodic table and dominate most of the periodic table. They tend to lose electrons to imitate the nearest noble gas in their electron valence shell to gain stability.

Consider the Electron Configuration

Metals have a few electrons in their outer shell (usually 1, 2, or 3), so it is easier for them to lose electrons and reach a stable configuration like the previous noble gas. The elements that commonly follow this behavior are the alkali metals (Group 1), alkaline earth metals (Group 2) and some transition metals.

Final Answer

The type of elements that achieve an electron configuration analogous to the previous noble gas by losing electrons from their valence shells are \(\textbf{metals}\).

Key concepts

Noble Gas Stability

Noble gases are unique elements found in Group 18 of the periodic table. They include helium, neon, argon, krypton, xenon, and radon. These elements are renowned for their stability and inertness. The reason behind their remarkable stability lies in their electron configuration. Noble gases possess a complete valence electron shell. For most of them, this means having eight electrons in their outermost shell, except for helium, which is stable with only two electrons. This complete outer shell makes noble gases unlikely to react with other elements, as they have no tendency to gain or lose electrons. Their stability is a natural benchmark for other elements, which often seek to mimic this electron configuration through chemical reactions.

Metals and Electron Loss

Metals, primarily located on the left side of the periodic table, encompass a variety of elements from alkali metals, alkaline earth metals, to transition metals. One of the defining characteristics of metals is their tendency to lose electrons easily. This behavior is due to their electron configurations, which generally have only a few electrons in their outermost shell. The loss of these electrons allows metals to achieve the stable electron configuration akin to their closest noble gas. This electron loss results in a positive oxidation state and transforms them into positively charged ions or cations. The energy needed for metals to lose these electrons is minimal compared to other elements, facilitating their ability to undergo this transformation swiftly.

Periodic Table Classification

The periodic table is a crucial tool in chemistry that organizes all known elements based on their atomic number, electron configurations, and recurring chemical properties. Each column, or group, typically shares valence electron similarities among its elements. Metals comprise a considerable portion of the periodic table and are generally positioned on the left and center.

• Alkali Metals (Group 1): These elements are highly reactive and tend to lose one electron.
• Alkaline Earth Metals (Group 2): These elements lose two electrons to achieve stability.
• Transition Metals: Situated in the central block, they can lose varying numbers of electrons.

Metals contrast with non-metals, which are on the right side of the table and tend to gain electrons. Understanding the classification in the periodic table helps predict the chemical behavior of elements, such as their reactivity and the type of ions they form.