What is wrong with the following electron configurations? a. Ni 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 b. N 1s^2 2p^5 c. Si 1s^2 2s^2 2p d. Mg 1s^2 2s^2 2p^6 3s

Verified step by step guidance

1. Identify the correct electron configuration for each element using the periodic table.
2. For Ni (Nickel), check if the configuration accounts for all 28 electrons and follows the order of filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d.
3. For N (Nitrogen), ensure the configuration accounts for all 7 electrons and follows the order of filling: 1s, 2s, 2p.
4. For Si (Silicon), verify the configuration accounts for all 14 electrons and follows the order of filling: 1s, 2s, 2p, 3s, 3p.
5. For Mg (Magnesium), confirm the configuration accounts for all 12 electrons and follows the order of filling: 1s, 2s, 2p, 3s.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It follows specific rules, such as the Aufbau principle, which states that electrons fill lower-energy orbitals before higher-energy ones. Understanding the correct order of filling and the maximum number of electrons per orbital is essential for identifying errors in configurations.

Pauli Exclusion Principle

The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of four quantum numbers. This principle implies that an orbital can hold a maximum of two electrons, which must have opposite spins. Recognizing this principle helps in determining if an electron configuration is valid or if it violates this fundamental rule.

Hund's Rule

Hund's Rule states that electrons will occupy degenerate orbitals (orbitals of the same energy) singly before pairing up. This means that for orbitals like p, d, and f, each orbital must have one electron before any can have two. Understanding this rule is crucial for correctly filling electron configurations and identifying any discrepancies in the provided examples.