Give the numerical values of n and l corresponding to each of the following orbital designations: (d) 5d.

검증된 단계별 안내

Identify the principal quantum number (n) from the given orbital designation. In this case, the number before the letter 'd' is 5, so n = 5.

Determine the azimuthal quantum number (l) based on the type of orbital. For a 'd' orbital, l = 2.

Combine the values to express the quantum numbers for the 5d orbital: n = 5 and l = 2.

Remember that the principal quantum number (n) indicates the energy level and size of the orbital, while the azimuthal quantum number (l) indicates the shape of the orbital.

Review the quantum number rules: n is a positive integer (1, 2, 3, ...), and l can be any integer from 0 to n-1, where l = 0 (s), l = 1 (p), l = 2 (d), l = 3 (f), etc.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

55s

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Quantum Numbers

Quantum numbers are a set of numerical values that describe the unique quantum state of an electron in an atom. They include the principal quantum number (n), which indicates the energy level, and the azimuthal quantum number (l), which defines the shape of the orbital. Each orbital designation corresponds to specific values of these quantum numbers.

Principal Quantum Number (n)

The principal quantum number (n) indicates the main energy level of an electron in an atom. It can take positive integer values (1, 2, 3, ...), with higher values corresponding to higher energy levels and greater distances from the nucleus. For the 5d orbital, n is 5, indicating it is in the fifth energy level.

Azimuthal Quantum Number (l)

The azimuthal quantum number (l) determines the shape of the orbital and can take integer values from 0 to (n-1). Each value of l corresponds to a specific type of orbital: 0 for s, 1 for p, 2 for d, and 3 for f. For the 5d orbital, l is 2, indicating it is a d-type orbital.