Write out the ground-state electron configurations of  c. Au³⁺ ,

Verified step by step guidance

1. Identify the atomic number of gold (Au), which is 79, and write its ground-state electron configuration: \([Xe] 4f^{14} 5d^{10} 6s^1\).
2. Recognize that Au³⁺ means the gold atom has lost 3 electrons.
3. Remove electrons starting from the outermost shell. First, remove the 1 electron from the 6s orbital.
4. Next, remove 2 electrons from the 5d orbital, as it is the next highest energy level after 6s.
5. Write the electron configuration for Au³⁺: \([Xe] 4f^{14} 5d^8\).

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level to the highest. The notation typically includes the principal quantum number, subshell type, and the number of electrons in each subshell, providing insight into the atom's chemical properties.

Ground State

The ground state of an atom refers to the lowest energy configuration of its electrons. In this state, electrons occupy the lowest available energy levels without any excitation. Understanding the ground state is crucial for predicting how an atom will interact chemically, as it reflects the most stable arrangement of electrons.

Ionization and Charge

Ionization involves the removal of electrons from an atom, resulting in a charged species known as an ion. For example, Au³⁺ indicates that three electrons have been removed from a neutral gold atom. This process affects the electron configuration, as the configuration must be adjusted to reflect the loss of electrons, particularly from the outermost shells.