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Chapter 3: Problem 17

For each of the questions, four choices have been provided. Select the correct alternative. Among the following, the orbital that has the lowest energy is (a) \(5 \mathrm{f}\) (b) \(4 \mathrm{f}\) (c) \(6 \mathrm{~s}\) (d) \(6 \mathrm{p}\)

Short Answer

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Answer: (c) 6s

Step by step solution

01

Common Understanding of Quantum Numbers

The principal quantum number (n) denotes the energy level and the distance from the nucleus (higher n, higher energy levels). The azimuthal quantum number (l) represents the shape of the orbital, where, for example, l=0 is designated as "s," l=1 as "p," and l=2 as "d."
02

Assign Quantum Numbers to the Given Options

Assign the principal quantum number (n) and azimuthal quantum number (l) for each option: (a) 5f: n=5, l=3 (b) 4f: n=4, l=3 (c) 6s: n=6, l=0 (d) 6p: n=6, l=1
03

Calculate the Sum n+l for Each Option

Determine the sum n+l for each option: (a) 5f: 5+3=8 (b) 4f: 4+3=7 (c) 6s: 6+0=6 (d) 6p: 6+1=7
04

Determine the Orbital with the Lowest Energy

The orbital with the lowest energy corresponds to the option with the smallest sum n+l. In this case, it is option (c) 6s with n+l=6. Therefore, among the given orbital options, the orbital with the lowest energy is (c) 6s.

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Most popular questions from this chapter

For each of the questions, four choices have been provided. Select the correct alternative. (1) The probability of finding an electron is maximum at certain places in space. (2) Energy change takes place only during excitation or deexcitation of electrons. (3) Electron has both particle and wave nature. (4) Angular momentum of the electrons revolving in different elliptical orbits is quantized. Arrange the above statements of different models or principles in the chronological order, which ultimately led to the development of modern structure of the atom. (a) \(1,2,3,4\) (b) \(2,4,3,1\) (c) \(4,3,2,1\) (d) \(2,3,1,4\)

Bohr's model introduced the concept of quantization of _______.

For each of the questions, four choices have been provided. Select the correct alternative. Which of the following sets of quantum numbers represent electron in hydrogen atom? (a) \(1,1,0,+1 / 2\) (b) \(1,0,0,+1 / 2\) (c) \(3,0,0,-1 / 2\) (d) \(4,2,1,-1 / 2\)

For each of the questions, four choices have been provided. Select the correct alternative. In the following pairs, identify the pair having a different \((\mathrm{n}+\ell)\) value: (a) \(4 \mathrm{~s}, 3 \mathrm{p}\) (b) \(3 \mathrm{~d}, 4 \mathrm{p}\) (c) 4s, \(3 \mathrm{~d}\) (d) \(4 \mathrm{~d}, 5 \mathrm{p}\)

Direction for questions: State whether the following statements are true or false. Any two electrons in an atom can have maximum of three quantum numbers same.
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