Question

Only trace amounts of the synthetic element darmstadtium, atomic number 110 , have been obtained. The element is so highly unstable that no observations of its properties have been possible. Based on its position in the periodic table, propose three different reasonable valence electron configurations for this element.

Short answer

Three reasonable valence electron configurations for darmstadtium (Ds) are 6d^9 7s^1, 6d^10 7s^0, and 6d^8 7s^2 based on its position in the periodic table and comparison with homologous elements.

Step-by-step solution

Identify the Group of Darmstadtium

Darmstadtium (Ds) has the atomic number 110, which places it in group 10 of the periodic table. Elements in this group are transition metals and typically show various oxidation states.

Suggest the First Valence Electron Configuration

The first reasonable valence electron configuration for darmstadtium, considering its position, would be similar to its lighter homologs like platinum (Pt). Platinum has a valence shell configuration of 5d^9 6s^1. Thus, for darmstadtium, an analogous configuration would be 6d^9 7s^1.

Propose the Second Valence Electron Configuration

The second suggested configuration could be one where the s electron is transferred to the d-orbital, potentially due to the stability provided by a completely filled d-orbital; this would be 6d^10 7s^0.

Consider an Alternate Valence Electron Configuration

Another possible valence electron configuration for darmstadtium could show two electrons in the s-orbital, like its lighter group 10 homolog, nickel (Ni), which has the outer electronic configuration of 3d^8 4s^2. Analogously, darmstadtium could potentially have a valence configuration of 6d^8 7s^2.

Key concepts

Understanding the Periodic Table

The periodic table acts as a universal reference that organizes all the known elements based on their atomic numbers, electron configurations, and recurring chemical properties. Elements are arranged in rows called periods and columns known as groups.
The periodic table is divided into several blocks, with the 'd-block' containing the transition metals. Understanding an element's position in the periodic table can provide insights into its chemical behavior, including possible valence electron configurations and oxidation states. Darmstadtium, for instance, falls into group 10 of the periodic table, suggesting it shares certain properties with other elements in this group.

Transition Metals and Their Properties

Transition metals, which occupy the d-block of the periodic table, are characterized by the presence of electrons in the 'd' orbitals. They are known for their ability to exhibit a variety of oxidation states and form colorful compounds. Transition metals typically have partially filled d-orbitals, which allows them to bond with other elements in multiple ways, leading to diverse chemistry.

As a member of the transition metals, darmstadtium's valence electron configuration is likely similar to that of other elements in group 10, although it's largely theoretical due to the element's instability and scarcity.

Oxidation States of Elements

The oxidation state, or oxidation number, describes the degree of oxidation of an element in a compound. It is an indicator of the hypothetical charge an atom would have if all bonds to atoms of different elements were fully ionic.

Transition metals, such as darmstadtium, can have multiple oxidation states because of their complex electron configurations. This versatile behavior is due to the energy closeness of their s- and d-electron orbitals which allow for various electron arrangements depending on the chemical environment.

Electron Configuration Explained

An element's electron configuration is a description of the distribution of its electrons in atomic or molecular orbitals. For transition metals, these configurations can be more complex due to the involvement of d-orbitals. The valence electrons, those found in the outermost shell, play a significant role in chemical bonding and reactions.

Darmstadtium's supposed valence electron configurations, such as 6d^9 7s^1, 6d^10 7s^0, and 6d^8 7s^2, demonstrate this complexity. These configurations are patterned after the known configurations of lighter homologs in group 10, indicating that darmstadtium may behave similarly in terms of bonding and reactivity.