Question

Assume that element 113 has been produced. What is the expected electron configuration for element \(113 ?\) What oxidation states would be exhibited by element 113 in its compounds?

Short answer

The expected electron configuration for element 113, nihonium (Nh), is \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{10} 4p^{6} 5s^{2} 4d^{10} 5p^{6} 6s^{2} 4f^{14} 5d^{10} 6p^{6} 7s^{2} 5f^{14} 6d^{10} 7p^{1}\). Nihonium is likely to exhibit oxidation states of +1 and +3 in its compounds due to its position in group 13 of the periodic table.

Step-by-step solution

Identify the element

Element 113 is nihonium (Nh), which belongs to the 7th period and group 13 in the periodic table. It is a post-transition metal and a member of the boron family.

Determine the electron configuration

To find the electron configuration for nihonium (Nh), we will follow the order of orbitals, filling in electrons as we go along. The order is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p Since nihonium has 113 electrons, we will fill each orbital until we reach the 113th electron. The electron configuration is: \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{10} 4p^{6} 5s^{2} 4d^{10} 5p^{6} 6s^{2} 4f^{14} 5d^{10} 6p^{6} 7s^{2} 5f^{14} 6d^{10} 7p^{1}\)

Predict the oxidation states

To predict the oxidation states of nihonium, we can consult its position on the periodic table. As a member of group 13, nihonium most likely has a +3 oxidation state due to losing three electrons from both its 7s and 7p subshells. However, elements in the boron family can also exhibit a +1 oxidation state by losing only one electron from their outermost p orbital. Thus, the oxidation states of nihonium in its compounds are likely to be: +1 and +3

Key concepts

Nihonium Oxidation States

Nihonium, symbolized as Nh and known as element 113 on the periodic table, is still a relatively new addition to our list of chemical elements. Its position in group 13 implies certain chemical properties, especially regarding its oxidation states, which are crucial to understand for predicting its reactivity and the types of compounds it may form. Like its group mates including boron, aluminum, gallium, indium, and thallium, nihonium is expected to typically exhibit a +3 oxidation state. This oxidation state results from the loss of three electrons — one from its 7p orbital and two from its 7s orbital.

However, nihonium might also demonstrate a +1 oxidation state in certain compounds. This is because elements in group 13 have the capacity to lose an electron from the outermost p orbital, leading to a stable electronic configuration reminiscent of noble gases. Since nihonium is a heavier element with a potentially more complex electron cloud configuration, predicting oxidation states is based largely on trends observed in lighter group 13 elements, although relativistic effects might influence its chemistry substantially.

Periodic Table Group 13

Group 13 of the periodic table is home to the boron family, a group that includes both metals and metalloids. As we look at nihonium's position in this family — amidst its lighter counterparts — we can glean insights into its potential behaviors and similarities to its group relatives. Nihonium, being a post-transition metal, still retains the common oxidation state of +3 which is characteristic of group 13 elements. However, members of this group are known for their versatility in their oxidation states. The lighter member boron often forms covalent compounds due to its small size and high electronegativity, while metals such as aluminum are predominantly found in the +3 state because of their tendency to lose all three electrons from their p orbital and one s orbital.

It's important to remember that as we move down the group, the elements tend to become more metallic. Therefore, nihonium, being heavier, could possibly display more metallic character than its lighter group 13 counterparts. Still, only limited experimental data is available because nihonium and its isotopes are synthesized in very small amounts and have short half-lives.

Electron Orbital Filling Order

Understanding the electron orbital filling order is crucial for determining the electron configuration of elements, which in turn informs us about their chemical properties. The orbitals are filled according to the Aufbau principle, which states that electrons occupy orbitals of lower energy first before moving to higher energy ones. The sequence is as follows:

• 1s
• 2s
• 2p
• 3s
• 3p
• 4s
• 3d
• 4p
• 5s
• 4d
• 5p
• 6s
• 4f
• 5d
• 6p
• 7s
• 5f
• 6d
• 7p

For nihonium, with its 113 electrons, following this order allows for the arrangement: \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{10} 4p^{6} 5s^{2} 4d^{10} 5p^{6} 6s^{2} 4f^{14} 5d^{10} 6p^{6} 7s^{2} 5f^{14} 6d^{10} 7p^{1}\). This process accounts for all electrons from the lowest energy level to the highest until all 113 electrons have been placed.

This filled order is essential for any chemical element because it not only controls the electron configuration but ultimately the chemical and physical properties of the element. While nihonium itself is unstable and difficult to experiment on, these principles remain foundational in our understanding of the natural world at an atomic level.