Question

give the correct box associated with each subshell

1. 1s²
2. 2s¹
3. 2p¹
4. 2p³
5. 3d⁵

Explanation:

Step1: Recall electron - filling rules

Electrons fill orbitals according to the Pauli - exclusion principle and Hund's rule. s - subshells have 1 orbital and p - subshells have 3 orbitals, d - subshells have 5 orbitals. Each orbital can hold a maximum of 2 electrons with opposite spins.

Step2: Analyze \(1s^{2}\)

The 1s subshell has 1 orbital. When it has 2 electrons, they have opposite spins. So it is represented by a single box with 2 electrons of opposite spins, which is option c.

Step3: Analyze \(2s^{1}\)

The 2s subshell has 1 orbital. With 1 electron, it is represented by a single box with 1 electron, which is option b.

Step4: Analyze \(2p^{1}\)

The 2p subshell has 3 orbitals. With 1 electron, it can go in any of the 3 orbitals. It is represented by one of the three - box diagrams with 1 electron, for simplicity, we can choose the first box filled, which is one of the single - electron in 3 - box diagrams (not all are shown here but conceptually correct), and among the given options, we assume the basic representation of a single - electron in a 2p orbital, and it can be considered as a single - electron in one of the 3 - box set. But if we consider the most basic form, it is like having one of the p - orbitals filled with 1 electron, and among the given options, we can assume it is a single - electron in one of the 3 - box set similar to the basic representation, and we can match it with a single - electron in a 3 - box set option. Let's assume the first box filled, and it can be related to a single - electron in a 3 - box set option. Among the given options, we assume it is a single - electron in one of the 3 - box set and it matches with the single - electron in a 3 - box set option, say option o (assuming the first box of the 3 - box set is filled).

Step5: Analyze \(2p^{3}\)

According to Hund's rule, electrons fill degenerate orbitals singly first with parallel spins. So for \(2p^{3}\), there are 3 electrons in the 3 p - orbitals with parallel spins. It is represented by option ee.

Step6: Analyze \(3d^{5}\)

According to Hund's rule, for \(3d^{5}\), 5 electrons fill the 5 d - orbitals singly with parallel spins. It is represented by option ee (as the pattern of singly - filled orbitals with parallel spins is the same conceptually as the \(2p^{3}\) case but with 5 orbitals instead of 3).

Answer:

1. c
2. b
3. o
4. ee
5. ee