Question

Element 106 has been named seaborgium, \(\mathrm{Sg}\), 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

The electron configuration for Seaborgium (Sg) is \[ \mathrm{1s^{2}}\mathrm{2s^{2}}\mathrm{2p^{6}}\mathrm{3s^{2}}\mathrm{3p^{6}}\mathrm{4s^{2}}\mathrm{3d^{10}}\mathrm{4p^{6}}\mathrm{5s^{2}}\mathrm{4d^{10}}\mathrm{5p^{6}}\mathrm{6s^{2}}\mathrm{4f^{14}}\mathrm{5d^{10}}\mathrm{6p^{6}}\mathrm{7s^{2}}\mathrm{5f^{14}}\mathrm{6d^4} \]. Chromium (Cr) will have similar properties to Seaborgium. The predicted formula for a possible oxide of Seaborgium is SgO₃, and for a possible oxyanion is H₂SgO₄.

Step-by-step solution

a. Electron Configuration for Element 106

In the periodic table, seaborgium (Sg) is located in the 6th period and group 6. To find the electron configuration, we need to follow the filling order of atomic orbitals, which is as follows (using \( (n + l) \)-rule): 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p... With the element being in the 6th period and 6th group, the electron configuration will be: \[ \mathrm{1s^{2}}\mathrm{2s^{2}}\mathrm{2p^{6}}\mathrm{3s^{2}}\mathrm{3p^{6}}\mathrm{4s^{2}}\mathrm{3d^{10}}\mathrm{4p^{6}}\mathrm{5s^{2}}\mathrm{4d^{10}}\mathrm{5p^{6}}\mathrm{6s^{2}}\mathrm{4f^{14}}\mathrm{5d^{10}}\mathrm{6p^{6}}\mathrm{7s^{2}}\mathrm{5f^{14}}\mathrm{6d^4} \]

b. Similar Element Properties

To identify an element with similar properties to seaborgium, we have to find an element from the same group. Since Sg is in group 6, the element with the most similar properties will be chromium (Cr), which has the electron configuration: \[ \mathrm{1s^{2}}\mathrm{2s^{2}}\mathrm{2p^{6}}\mathrm{3s^{2}}\mathrm{3p^{6}}\mathrm{4s^{1}}\mathrm{3d^{5}} \] Elements in the same group tend to have similar chemical properties due to their valence electron configurations.

c. Predicting Oxide and Oxyanion Formulas

To predict the formula for a possible oxide and oxyanion of seaborgium, we can analyze its valence electrons and oxidation states. Seaborgium, being in group 6, typically has a +6 oxidation state. However, it could also possibly have other oxidation states like +2, +3, and +4. The most common oxidation state in this group is +6. For the oxide, we can expect seaborgium to form a compound with oxygen (-2 oxidation state) where it can reach its most common oxidation state +6. So, the formula for the oxide would be SgO₃, in which seaborgium's oxidation state is +6. For the oxyanion, we can follow the same logic. When Sg has an oxidation state of +6, it can form an oxyanion with oxygen and a counter ion (like hydrogen) to neutralize the charge. The possible oxyanion formula would be H₂SgO₄, like CrO₄²⁻ and H₂CrO₄ for chromium.

Key concepts

Understanding the Periodic Table

At the heart of chemistry lies the periodic table, a comprehensive chart organizing elements by atomic number and similar properties. The layout of the table is such that it provides a wealth of information about the elements, including their electron configurations. Elements are listed in rows called periods, and columns known as groups or families.

Each element in a group has the same number of electrons in its outer shell—these are known as valence electrons. These electrons primarily determine the chemical behavior of the element. For instance, seaborgium (Sg), with element number 106, falls into the 6th period and group 6 of the periodic table. Elements in the same group share similar properties because their valence electron configurations are alike. For instance, chromium (Cr) in group 6, much like seaborgium, will have similarities in its chemical behavior due to having the same number of valence electrons.

• Groups are vertical columns that indicate the number of valence electrons.
• Periods are horizontal rows that correlate with the highest energy level of an electron within an atom.

The application of periodic trends, such as atomic radius, electronegativity, and ionization energy, helps us comprehend why certain elements react or behave similarly. As students explore the periodic table, they can anticipate properties of elements and their ions, such as expected oxidation states or types of chemical bonds they might form.

Oxidation States and Chemical Reactivity

Oxidation states indicate the degree of oxidation of an atom, essentially the hypothetical charge an atom would have if all its bonds were ionic and not covalent. Different elements can have various oxidation states, affecting how they combine with other elements to form compounds.

Oxidation states are particularly useful for predicting the formulas of compounds. For example, the valence electrons of seaborgium can undergo reactions to give it a +6 oxidation state, especially since it's in group 6 of the periodic table, which other elements in this group notably exhibit.

Predicting Compound Formulas

Using oxidation states, we can predict that seaborgium (Sg) would form an oxide with the formula SgO₃, where Sg is in the +6 state and oxygen is in the -2 state, reflecting how the charges balance with three oxygen atoms needed per seaborgium atom.

• Oxidation states can vary depending on the chemical environment.
• The +6 state is common for group 6 elements but isn't the only possible state.

Understanding the concept of oxidation states not only helps students to deduce the formulas of compounds but also to predict the reactivity and types of reactions elements might undergo. For example, the capability to form certain oxides or oxyanions is closely linked to an element's oxidation states.

Valence Electrons and Element Properties

Valence electrons are the electrons present in the outermost shell of an atom. These electrons are key players in chemical reactions and bond formation because they can be lost, gained, or shared with other atoms. The number of valence electrons influences an element's chemical properties, including its reactivity and the types of bonds it can form.

In seaborgium (Sg), which is a transition metal, the valence electrons are found in the s and d orbitals of the highest principal quantum number. These electrons in the d subshell can lend seaborgium unique properties compared to other elements. Transition metals typically show a range of oxidation states due to the varying availability of s and d electrons for bonding.

Significance in Reactions

For group 6 elements like seaborgium, the typical number of valence electrons allows for multiple oxidation states which directly correlate to its reactivity. Seaborgium's electron configuration suggests it can exhibit a +6 oxidation state, due to six valence electrons, enabling it to form compounds like SgO₃ and oxyanions like H₂SgO₄.

• Valence electrons determine the types of chemical bonds.
• They explain periodic trends in element reactivity and interactions.

Grasping the understanding of valence electrons helps clarify why elements such as seaborgium mimic the behavior of their group counterparts. With valence electron knowledge, predicting reactivity and product formation in chemical reactions becomes more intuitive for students.