Write the electron configuration for each of the following ions, and determine which ones possess noble-gas configurations: a. Rb+ b. Rh3+ c. P3− d. Sc3+ e. S2− f. V2+.

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Identify the atomic number of each element to determine the number of electrons in the neutral atom.

For each ion, adjust the electron count by adding electrons for negative charges or removing electrons for positive charges.

Write the electron configuration for the neutral atom, then modify it according to the charge of the ion.

Compare the resulting electron configuration to that of the nearest noble gas to determine if it matches.

List the ions that have electron configurations identical to a noble gas.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom or ion's atomic orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons, following the Aufbau principle, Pauli exclusion principle, and Hund's rule. Understanding how to write electron configurations is essential for predicting chemical behavior and reactivity.

Ionic Charge and Electron Loss/Gain

Ionic charge refers to the net electrical charge an atom or ion carries due to the loss or gain of electrons. Cations (positively charged ions) are formed by losing electrons, while anions (negatively charged ions) are formed by gaining electrons. Knowing how to adjust the electron configuration based on the ionic charge is crucial for determining the correct configuration of ions.

Noble-Gas Configuration

Noble-gas configuration refers to the electron arrangement of noble gases, which have full outer electron shells, making them stable and unreactive. Atoms or ions that achieve a noble-gas configuration typically have eight electrons in their outermost shell (octet rule), which is a key factor in chemical stability. Identifying ions with noble-gas configurations helps in understanding their stability and reactivity.

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