Question

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

Short answer

The electron configuration for element 113 is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s² 5f¹⁴ 6d^9. Its valence electrons are found in the 7s², 5f¹⁴, and 6d^9 orbitals. The possible oxidation states for element 113 are from +2 up to +8, as higher oxidation states are extremely rare.

Step-by-step solution

Aufbau Principle

The Aufbau Principle states that electrons in an atom fill the orbitals in order of increasing energy. To find the order in which to fill the orbitals, we can use the diagonal rule. The order is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

Fill orbitals

Now we will fill the orbitals with electrons for element 113. As there are 113 electrons, we start filling the orbitals based on the Aufbau Principle. The electron configuration is formed as follows (we stop once we've placed all 113 electrons): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s² 5f¹⁴ 6d^9

Identify valence electrons

From the electron configuration, we can identify the valence electrons. Valence electrons are the electrons in the outermost energy level and are involved in chemical bonding. In this case, valence electrons are found in the outermost energy levels: 7s² 5f¹⁴ 6d^9

Predict oxidation states

Oxidation states for an element are determined by the number of valence electrons it has, which are involved in forming chemical bonds and can be gained, lost, or shared. In element 113, the valence electrons are 7s², 5f¹⁴, and 6d^9. The 7s² orbitals can lose two electrons, the 5f¹⁴ orbitals can lose up to fourteen electrons, and the 6d^9 orbitals can lose up to nine electrons. This gives us the possible oxidation states: +2, +3, +4, +5, +6, +7, +8, +9, +10, +11, +12, +13, +14, +15, and +16. However, it should be noted that oxidation states higher than +8 are extremely rare and usually not observed. So the most likely oxidation states for element 113 could be from +2 up to +8, depending on the specific chemical environment and the elements it forms compounds with.

Key concepts

Aufbau Principle

The Aufbau Principle is a fundamental guideline used in chemistry to determine the electron configuration of an atom. Every atom is made up of protons, neutrons, and electrons. The electrons inhabit specific regions around the nucleus called orbitals. According to the Aufbau Principle, electrons fill these orbitals starting from the lowest energy level to the highest. This way, the atom remains stable.
To visualize this filling sequence, the diagonal rule—also known as the "Madelung rule"—can be a handy tool. It demonstrates the order in which orbitals are filled based on increasing energy levels. Some key points about the Aufbau Principle include:

• Electrons fill the 1s orbital first, then the 2s, then the 2p, and so on.
• The goal is to achieve a stable, lowest-energy state for the atom.
• Element 113 would have electrons placed meticulously following this principle up to 6d and 7s orbitals.

If you imagine the orbitals as boxes and electrons as arrows, each orbital can hold a maximum of two arrows, indicating two electrons with opposite spins. Understanding this process is vital in predicting how element 113 behaves and interacts with other elements.

Valence Electrons

Valence electrons are the electrons located in the outermost shell of an atom. These electrons are vital because they are the ones involved in chemical bonding and reactions. For example, in element 113, the valence electrons are found in the 7s, 5f, and 6d orbitals. Knowing the count and configuration of these electrons can predict how an element reacts with others.
These valence electrons help determine:

• The atom's ability to form bonds with other atoms.
• Its chemical properties.
• Possible oxidation states (more on this in the next section).

In many cases, atoms are most stable when they have eight valence electrons (a full outer shell), which is known as the "octet rule." However, element 113 doesn't strictly follow this rule due to its position in the periodic table and its unique electron configuration. For elements like 113, focusing on the outermost s, f, and d orbital electrons helps predict their chemical behavior. This thing is particularly helpful when determining the element's reactivity.

Oxidation States

Oxidation states represent the total number of electrons an atom can gain, lose or share during chemical reactions. These states are crucial for balancing redox reactions and predicting the outcomes of complex chemical processes. For element 113, the potential oxidation states are deduced from its electron configuration, especially focusing on its valence electrons.
Element 113 can exhibit various oxidation states, ranging theoretically from +2 to +16. However, realistic oxidation states are much lower, usually not exceeding +8. This limitation arises because high oxidation numbers are rarely stable in real-world conditions. Some essential points about oxidation states include:

• Oxidation states are typically written as positive or negative integers.
• The most stable oxidation states are usually used in chemical calculations.
• Element 113, in particular, would likely exhibit oxidation states from +2 to +8 under suitable conditions.

Understanding these oxidation states helps in predicting the type of compounds element 113 could form, such as oxides and halides. This knowledge provides a framework for imagining new chemical interactions and potential applications.