Write the ground state electron configuration for each atom...

Write the ground state electron configuration for each atom and ion pair.
$${ a. } \mathrm \ {Zr}, \mathrm{Zr}^{2+} \quad \text { b. } \mathrm{Co}, \mathrm{Co}^{2+} \quad \text { c. } \mathrm{Tc}, \mathrm{Tc}^{3+} \quad \text { d. } \mathrm{Os}, \mathrm{Os}^{4+}$$

Key Concepts

Transition Metals

Transition metals have partially filled d orbitals that lead to unique electron configurations. Their electron removal during ionization can involve the higher energy s electrons initially, highlighting the subtle interplay between s and d orbital energies in these elements.

Orbital Energy Levels

Orbital energy levels describe the hierarchy of energy in atomic orbitals (s, p, d, f), which determines the order of electron filling and removal. This concept is essential for constructing both neutral atom configurations and configurations for ions.

Ionization and Oxidation States

Ionization involves the removal or addition of electrons to create ions, and the oxidation state indicates the number of electrons removed relative to the neutral atom. Understanding these concepts is critical to predicting how the electron configuration changes when atoms form ions.

Aufbau Principle

The Aufbau principle is a guideline used to determine the order in which electrons populate orbitals. It states that electrons occupy the lowest energy orbitals first before moving to higher energy levels, allowing us to construct the electron configuration step by step.

Electron Configuration

Electron configuration refers to the orderly arrangement of electrons in an atom’s orbitals, following quantum mechanical rules. It explains how electrons fill various orbitals in order of increasing energy and is fundamental to understanding an element's chemical properties.

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