Question

Element 106 has been named seaborgium, Sg, in honor of Glenn Seaborg, discoverer of the first transuranium element. a. Write the expected electron configuration for element 106. b. What other element would be most like element 106 in its properties? c. Predict the formula for a possible oxide and a possible oxyanion of element 106.

Short answer

a. The electron configuration of Seaborgium (Sg) is [Rn] 5f¹⁴ 6d⁴ 7s². b. Seaborgium is most similar to Chromium (Cr), Molybdenum (Mo), and Tungsten (W). c. A possible oxide formula is SgO₃, and a possible oxyanion formula is (SgO₄)²⁻.

Step-by-step solution

Determine the electron configuration of Seaborgium (Sg)

Seaborgium, Sg, is element 106, which means it has 106 electrons in its neutral state. Using the periodic table, we can find the electron configuration for Seaborgium as follows: 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², 4f¹⁴, 5d¹⁰, 6p⁶, 7s², 5f¹⁴, 6d⁴ So, the electron configuration of Seaborgium is [Rn] 5f¹⁴ 6d⁴ 7s².

Identify the element most similar in properties to Seaborgium

Seaborgium belongs to Group 6 in the periodic table, along with Chromium, Molybdenum, and Tungsten. These elements share similar properties because they have the same number of valence electrons. Therefore, Seaborgium would be most similar to Chromium (Cr), Molybdenum (Mo), and Tungsten (W).

Predict the formula for a possible oxide of Seaborgium

The elements in Group 6 typically form oxides with a charge of +6, i.e., they lose six valence electrons when forming an oxide compound. The oxygen atom gains two electrons and has a charge of -2. Therefore, the formula for a possible oxide of Seaborgium would be SgO₃.

Predict the formula for a possible oxyanion of Seaborgium

A common oxyanion formed by Group 6 elements is the molybdate [(MoO₄)²⁻] and chromate [(CrO₄)²⁻] ions. Following this trend, we can predict that a possible oxyanion for Seaborgium would have the formula (SgO₄)²⁻.

Key concepts

Electron Configuration

Electron configuration is a way of distributing the electrons of an atom into different atomic orbitals. Seaborgium (Sg), which is element number 106, has a specific electron configuration due to its position in the periodic table.
Understanding its configuration requires knowledge of the sequence in which electrons fill the atomic orbitals. The electron configuration for Seaborgium is given by \[1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^{10}, 4p^6, 5s^2, 4d^{10}, 5p^6, 6s^2, 4f^{14}, 5d^{10}, 6p^6, 7s^2, 5f^{14}, 6d^4\]
This can be simplified using noble gas notation as [Rn] 5f¹⁴ 6d⁴ 7s², where [Rn] denotes the electron configuration of radon, the nearest noble gas. Each shell and subshell has a specific maximum capacity: the s subshell holds 2 electrons, the p subshell holds 6, the d holds 10, and the f holds 14. Understanding these rules helps figure out the arrangement for other elements too.

Periodic Table Groups

The periodic table is organized in such a way that elements with similar properties are grouped together. Seaborgium (Sg) is part of Group 6.
This group includes Chromium (Cr), Molybdenum (Mo), and Tungsten (W). One of the main characteristics these elements share is their electron configuration in the outer shell, specifically having similar valence electrons, which leads to similar chemical properties.
These elements are known as transition metals and show a propensity for forming colored compounds, variable oxidation states, and at times acting as catalysts. Due to these shared properties, Seaborgium behaves similarly in chemical reactions and physical properties as the other elements in its group.

Oxide Formation

Oxides are compounds formed when elements react with oxygen. In the context of transition metals like Seaborgium, they often achieve stable oxidation states.
Group 6 elements, including Seaborgium, typically form oxides where they lose six valence electrons to result in a +6 oxidation state. Oxygen typically forms oxides with a -2 charge.
Thus, Seaborgium forms an oxide with the formula SgO₃. This follows the general formula for oxides in this group, where the metal (M) and oxygen has the ratio determined by the charges balancing each other out. Understanding oxide formation is crucial for predicting how these elements react in nature and industrial processes.

Oxyanion Prediction

Oxyanions are polyatomic ions that contain oxygen and another element. For Group 6 elements, common oxyanions are the molybdate (MoO₄)²⁻ and chromate (CrO₄)²⁻ ions.
These ions form when the metal is in its highest oxidation state and bonds with oxygen atoms. Seaborgium, part of the same group, would be expected to form a similar oxyanion.
The predicted formula for Seaborgium's oxyanion is (SgO₄)²⁻. This reflects the trend in the group and helps in understanding potential chemical behaviors. Predicting oxyanions is important for studying environmental interactions and reactions within biological systems.