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, propse three different reasonable valence electron configurations for this element.

Short answer

The three reasonable valence electron configurations for darmstadtium (Ds), based on its position in group 10 of the periodic table, could be d(10), d(9)s(1), or d(8)s(2).

Step-by-step solution

Identify the Group of Darmstadtium

Analyze the periodic table and locate darmstadtium (Ds) with the atomic number 110. Identify the group to which it belongs, which is the same group as platinum and nickel. Darmstadtium is a member of group 10, which means it should have similar characteristics and valence electron configurations to other elements in that group.

Refer to the Known Electron Configurations

Consider the known electron configurations of other group 10 elements and their common oxidation states. For example, nickel (Ni) can have a valence electron configuration of d(8)s(2), platinum (Pt) can have d(9)s(1), and in their most stable forms, they often exhibit +2 oxidation states, meaning two valence electrons can be lost.

Propose Valence Electron Configurations

Based on its group, darmstadtium is expected to have similar valence electron configurations to its lighter homologs. The reasonable valence configurations could include d(10), which is fully filled d-orbitals, as seen in the noble gas-like ending, d(9)s(1), following platinum's configuration, or d(8)s(2), which follows the configuration of nickel providing multiple oxidation states. These configurations take into account the likelihood of electron loss due to oxidation.

Key concepts

Atomic Number 110

The atomic number of an element is a fundamental characteristic that defines its position on the periodic table and its chemical properties. The atomic number, denoted by the symbol 'Z', represents the number of protons in the nucleus of an atom of the element. For darmstadtium, the atomic number is 110. This places darmstadtium in the category of superheavy elements—those with atomic numbers greater than 104.

Because of its high atomic number, darmstadtium is a synthetic element, meaning it does not occur naturally and must be created in a laboratory environment. These synthetic elements are typically produced in minute quantities and are highly unstable, resulting in very short half-lives. The synthesis of darmstadtium involves a complex process of particle collisions, usually involving the bombardment of heavier targets like lead or bismuth with high-energy ion beams. The instability and rarity of darmstadtium mean that its chemical properties are not well understood, but its place in the periodic table gives us important clues about its potential behavior.

Periodic Table Group Analysis

Understanding the periodic table is essential when predicting the properties of elements, especially ones as elusive as darmstadtium. The periodic table is arranged in a way that elements with similar properties fall within the same columns, known as groups. Darmstadtium, with the atomic number 110, falls into group 10, which it shares with elements like nickel (Ni), palladium (Pd), and platinum (Pt).

Group 10 elements are characterized by certain similarities in their electron configurations, especially in the highest occupied energy levels, or valence shells. These similar electron configurations lead to similar properties among the elements within the group. For instance, elements in group 10 are generally capable of forming compounds in which they exhibit a +2 oxidation state. This commonality offers a starting point for hypothesizing the behavior of darmstadtium, even though it has not been extensively observed. We can reasonably infer that its valence electron configuration might mimic those of its lighter homologs, influencing its potential chemical reactions and stabilities in various oxidation states.

Oxidation States

Oxidation states, also known as oxidation numbers, play a critical role in chemistry, as they help in understanding the electronic structure of elements and their capacity to form certain compounds. An oxidation state is an indicator of the degree of oxidation of an atom in a substance; it reflects the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic.

Oxidation states are important when discussing transition metals like darmstadtium, which typically exhibit multiple oxidation states. This multiplicity arises due to the variable occupancy of d-orbitals in their valence shells. In the case of darmstadtium, we may anticipate oxidation states that are common to group 10 elements, such as +2, due to the potential configurations like d(8)s(2) or d(9)s(1). The hypothetical +2 oxidation state would imply that darmstadtium has two valence electrons that can be removed or shared when forming compounds. However, due to the element's instability and rapid decay, these predicted oxidation states remain largely speculative.