Question

Write electron configurations for each of the following. a. \(\mathrm{Ti}, \mathrm{Ti}^{2+}, \mathrm{Ti}^{\mathrm{i}+}\) b. \(\operatorname{Re}, \mathrm{Re}^{2+}, \mathrm{Re}^{3+}\) c. \(\mathrm{Ir}, \mathrm{Ir}^{2+}, \mathrm{Ir}^{3+}\)

Short answer

a. Ti: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\); Ti²⁺: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^2\); Ti³⁺: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^1\) b. Re: \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^5\); Re²⁺: \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^3\); Re³⁺: \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^2\) c. Ir: \([Xe]6s^2 4f^{14} 5d^7\); Ir²⁺: \([Xe]6s^2 4f^{14} 5d^5\); Ir³⁺: \([Xe]6s^2 4f^{14} 5d^4\)

Step-by-step solution

Identify the number of electrons for each species

Using the periodic table, we can see that Titanium (Ti) has an atomic number of 22, which means it has 22 electrons. Ti²⁺ has lost 2 electrons, so it has 20 electrons. And Ti³⁺ has lost 3 electrons, so it has 19 electrons.

Write the electron configuration for each species

Using the periodic table to fill in orbitals, we can write the electron configurations as follows: Ti (22 electrons): \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\) Ti²⁺ (20 electrons): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^2\) Ti³⁺ (19 electrons): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^1\) b. Electron configurations for Re, Re²⁺, Re³⁺

Identify the number of electrons for each species

Rhenium (Re) has an atomic number of 75, which means it has 75 electrons. Re²⁺ has lost 2 electrons, so it has 73 electrons. And Re³⁺ has lost 3 electrons, so it has 72 electrons.

Write the electron configuration for each species

Using the periodic table to fill in orbitals, we can write the electron configurations as follows: Re (75 electrons): \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^5\) Re²⁺ (73 electrons): \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^3\) Re³⁺ (72 electrons): \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^2\) c. Electron configurations for Ir, Ir²⁺, Ir³⁺

Identify the number of electrons for each species

Iridium (Ir) has an atomic number of 77, which means it has 77 electrons. Ir²⁺ has lost 2 electrons, so it has 75 electrons. And Ir³⁺ has lost 3 electrons, so it has 74 electrons.

Write the electron configuration for each species

Using the periodic table to fill in orbitals, we can write the electron configurations as follows: Ir (77 electrons): \([Xe]6s^2 4f^{14} 5d^7\) Ir²⁺ (75 electrons): \([Xe]6s^2 4f^{14} 5d^5\) Ir³⁺ (74 electrons): \([Xe]6s^2 4f^{14} 5d^4\)

Key concepts

Transition Metals

Transition metals are fascinating elements that sit in the middle of the periodic table, in groups 3 to 12. They are known for having unique properties due to their electron configurations. These metals are often shiny and conduct electricity well, thanks to delocalized electrons that move freely. Another cool feature is that they can form different ions or oxidation states because of partially filled d orbitals.

This happens when electrons from these orbitals are lost or shared in chemical reactions. The wider range of possible oxidation states compared to other elements allows transition metals to participate in many types of chemical bonding and reactions.

Moreover, their ability to transition between these various states makes them valuable in catalysts used in processes like industrial manufacturing.

Oxidation States

Oxidation states refer to the charge of an atom within a molecule or a compound. It indicates the number of electrons that an atom gains or loses to form chemical bonds. In the context of electron configurations, knowing the oxidation state helps us figure out how many electrons have been removed or added. Transition metals, for example, exhibit a variety of oxidation states which can make their chemistry both complex and diverse. When transition metals lose electrons, they typically lose them from the outer electron shells. Generally, the electrons are first removed from the outermost s orbital followed by the d orbitals.

For example, titanium (Ti) in its neutral state has an electron configuration of \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\]. In the Ti²⁺ ion, it loses two electrons, giving the electron configuration \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^2\].
The loss of electrons corresponds to an increase in positive charge, which affects how these metals interact with other substances.

Periodic Table

The periodic table is a systematic arrangement of elements in order of increasing atomic number. Every element in the table is represented with symbols, with transitions metals forming a specific block in the middle. The table is split into periods (rows) and groups (columns), with elements grouped by similar properties. Understanding the periodic table can help us predict the behaviours and properties of elements, including electron configuration and reactivity. Each position on the table gives us insight into the atomic structure, such as the number of electrons. Transition metals are located in the d-block, and this location signifies specific properties like the ability to form variable oxidation states. When determining electron configurations from the periodic table, one can see the order in which orbitals are filled.

For instance, the first two columns belong to the s-block, while the middle ones are the d-block, where transition metals reside.

Atomic Structure

Atomic structure describes the organization of particles within an atom, which includes protons, neutrons, and electrons. Protons and neutrons reside in the atom's nucleus, while electrons orbit around it. The number of protons determines the element's identity and its atomic number; for instance, titanium has 22 protons. Electrons are distributed in shells or energy levels around the nucleus, following Pauli's Exclusion Principle and Hund's Rule. The arrangement of electrons in these shells forms the electron configuration, which helps explain the chemical behavior of elements.

For transition metals, electrons add to lower energy levels first (s and p) before filling the d-subshells. The unique arrangement and ability to rearrange electrons in d-block elements lead to various oxidation states and complex bonding capabilities. Understanding atomic structure provides insight into the interaction of elements, predicting how atoms may bond or interact.