Question

Consider element \(113,\) Nh. What is the expected electron configuration for Nh? What oxidation states would be exhibited by Nh in its compounds?

Short answer

The expected electron configuration for Nihonium (Nh) is \(1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \ 4s^2 \ 3d^{10} \ 4p^6 \ 5s^2 \ 4d^{10} \ 5p^6 \ 6s^2 \ 4f^{14} \ 5d^{10} \ 6p^6 \ 7s^2 \ 5f^{14} \ 6d^{10} \ 7p^1\). Nh is in group 13 of the periodic table, and elements within this group commonly exhibit the +3 oxidation state. However, Nh may also display a +1 oxidation state due to relativistic effects and lanthanide contraction. In summary, Nh is expected to exhibit the oxidation states +3 and +1 in its compounds.

Step-by-step solution

Identify the element and its atomic number

Element 113 is Nihonium (Nh), and its atomic number is 113. This means it has 113 electrons orbiting the nucleus. We will use this information to construct the electron configuration.

Determine the electron configuration

To determine the electron configuration for Nihonium, we will follow the aufbau principle, which states that electrons fill orbitals in increasing order of energy. We will use the periodic table to establish the order of the orbitals. The electron configuration for Nh is: \(1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \ 4s^2 \ 3d^{10} \ 4p^6 \ 5s^2 \ 4d^{10} \ 5p^6 \ 6s^2 \ 4f^{14} \ 5d^{10} \ 6p^6 \ 7s^2 \ 5f^{14} \ 6d^{10} \ 7p^1\)

Analyze the electron configuration

Now that we have the electron configuration for Nihonium, we can use it to predict the oxidation states Nh can exhibit in its compounds. The valence electrons are those in the outermost orbitals, which in the case of Nh are: - 7s: 2 electrons - 5f: 14 electrons - 6d: 10 electrons - 7p: 1 electron These orbitals determine the chemical properties and reactivity of Nh.

Predict the oxidation states

To predict the oxidation states for Nh, we will analyze the valence orbitals. The oxidation states represent the number of electrons an atom can lose, gain, or share while forming chemical bonds with other atoms. Generally, the elements in the same group exhibit the same oxidation states. Nh is in group 13, which includes elements like boron (B), aluminum (Al), gallium (Ga), indium (In), and thallium (Tl). The common oxidation state for these elements is +3, as they tend to lose three electrons in their compounds. Nh can lose its 7p electron and two 7s electrons to achieve the +3 oxidation state. However, considering the relativistic effects and lanthanide contraction, Nh might also exhibit lower oxidation states, such as +1, similar to thallium (Tl), which is also in the same group and is known to exhibit the +1 oxidation state besides +3. In summary, Nh is expected to exhibit the oxidation states +3 and +1 in its compounds.

Key concepts

Oxidation States

The concept of oxidation states is essential for understanding the behavior of elements in chemical compounds. Oxidation states represent the number of electrons an atom either loses, gains, or shares when forming chemical bonds. For Nihonium (Nh), an element in group 13 of the periodic table, the oxidation states are primarily influenced by its position. Group 13 elements typically exhibit a +3 oxidation state. This is because they usually lose three electrons to attain stability. In Nh, the +3 oxidation state is achieved by losing the 7p electron and two 7s electrons. This is similar to other group 13 elements like boron (B), aluminum (Al), and indium (In). However, Nihonium might also exhibit different oxidation states like +1. This is due to relativistic effects and lanthanide contraction, which influence the size and energy levels of its orbitals. Thallium (Tl), another group 13 element, is known to commonly exhibit both +1 and +3 oxidation states, hinting at similar possibilities for Nihonium.

Valence Electrons

Valence electrons determine the chemical reactivity and bonding behavior of an element. In the electron configuration of Nihonium (Nh), the valence electrons are found in its outermost energy levels. Specifically, these are the:

• 7s: 2 electrons
• 7p: 1 electron
• 5f: 14 electrons
• 6d: 10 electrons

Valence electrons hold pivotal roles, as they are involved in the formation of chemical bonds. For Nihonium, the presence of one electron in the 7p orbital makes it reactive and capable of forming bonds with other elements. The involvement of these specific orbitals reflects the common group characteristics in group 13, where the tendency to reach a stable state by losing electrons is pronounced. Understanding valence electrons helps predict the potential compounds Nihonium can form, which could involve various oxidation states ranging from +1 to +3.

Lanthanide Contraction

Lanthanide contraction refers to the unexpected trend observed among the elements of the periodic table, particularly after the lanthanide series. This effect results in elements like Nihonium (Nh) having atoms smaller than expected. Lanthanide contraction occurs because the 4f orbitals are not very effective at shielding the increased nuclear charge. Hence, after the lanthanide series, elements have more tightly held electrons, which leads to a smaller atomic radius than one might predict by simply looking at the periodic table. In the case of Nihonium, this contraction impacts its electronic structure and oxidation states. The stronger hold on its electrons can lead to the element exhibiting lower oxidation states, similarly seen in thallium within its group. Nihonium's behavior, influenced by this contraction, allows for oxidation states such as +1 besides the common +3, showcasing the nuances of chemical bonding and reactivity trends driven by lanthanide contraction.