General Chemistry

General Questions

To determine the electron configuration of nickel (Ni), which has an atomic number of 28, we will follow the Aufbau principle, the Pauli exclusion principle, and Hund's rule. These principles guide the order in which electrons are distributed among the orbitals. The Aufbau principle states that electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. According to this principle, the order of orbital filling is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on. The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. As a result, each orbital can hold a maximum of two electrons with opposite spins. Hund's rule states that electrons will fill degenerate orbitals (orbitals with the same energy) singly first, and pair up only when necessary, with parallel spins. Now, let's determine the electron configuration of nickel step by step: 1. Begin filling the 1s orbital: Nickel has 28 electrons. The 1s orbital can hold 2 electrons. Electron configuration so far: \(1s^2\) 2. Fill the 2s and 2p orbitals: The 2s orbital holds 2 electrons, and the three 2p orbitals can hold a total of 6 electrons (2 electrons per orbital). Electron configuration so far: \(1s^2 2s^2 2p^6\) 3. Fill the 3s and 3p orbitals: The 3s orbital holds 2 electrons, and the three 3p orbitals hold a total of 6 electrons. Electron configuration so far: \(1s^2 2s^2 2p^6 3s^2 3p^6\) 4. Fill the 4s orbital: According to the Aufbau principle, the 4s orbital is filled before the 3d orbitals. The 4s orbital can hold 2 electrons. Electron configuration so far: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2\) 5. Fill the 3d orbitals: After the 4s orbital is filled, electrons begin to fill the 3d orbitals. There are five 3d orbitals, each capable of holding 2 electrons. Since nickel has 28 electrons, and we have already placed 18 in the previous orbitals, we have 10 electrons left to place in the 3d orbitals. Electron configuration so far: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^8\) Therefore, the complete electron configuration for nickel (Ni) is: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^8\] Alternatively, we can use the noble gas shorthand notation by recognizing that the electron configuration up to \(3p^6\) is the same as that of the noble gas Argon (Ar). Thus, the shorthand electron configuration for nickel is: \[[Ar] 4s^2 3d^8\] This notation indicates that nickel has the same electron configuration as argon, plus the additional electrons in the 4s and 3d orbitals.

Question

What is the electron configuration of nickel (Ni)?

Solution

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