Hund's Rule Demystified: Electron Configuration Challenge

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Hunds Rule Demystified: Electron Configuration Challenge - Quiz

Welcome to "Hund's Rule Demystified: Electron Configuration Challenge," where we unravel the mysteries of electron configurations and put your knowledge to the test. Hund's Rule is a fundamental principle in quantum mechanics that dictates how electrons fill the orbitals of an atom. This rule helps us understand the arrangement of electrons in atoms and why certain elements exhibit unique properties.
In this quiz, you'll face 10 thought-provoking questions that delve into the intricacies of electron configurations and Hund's Rule. Can you grasp the concept of electron filling order and Hund's Rule exceptions? Are you familiar with the rules governing electron Read morespin and the Pauli Exclusion Principle? Can you navigate the periodic table with confidence, knowing the electron configurations of various elements?Whether you're a student of chemistry, a science enthusiast, or someone eager to unravel the mysteries of atomic structure, our quiz offers an engaging and educational experience. Test your comprehension of these fundamental concepts and gain valuable insights into the behavior of atoms. With questions spanning theory, examples, and practical applications, you'll embark on an enlightening journey through the fascinating realm of electron configurations.
So, are you ready to take on the Hund's Rule Demystified: Electron Configuration Challenge? Dive into the quiz, explore the intricacies of electron arrangements, and enhance your knowledge of atomic structure. Challenge yourself, have fun, and unlock the secrets of electron configurations!


Questions and Answers
  • 1. 

    What is Hund's rule?

    • A.

      Electrons will always occupy the lowest energy level available.

    • B.

      Electrons will pair up in the same orbital only when all orbitals have at least one electron.

    • C.

      Electrons will fill orbitals of the same energy level one at a time with parallel spins before pairing up.

    • D.

      Electrons will populate higher energy orbitals before filling lower energy orbitals.

    Correct Answer
    C. Electrons will fill orbitals of the same energy level one at a time with parallel spins before pairing up.
    Explanation
    Hund's rule states that electrons will fill orbitals of the same energy level one at a time with parallel spins before pairing up. This rule ensures the maximum spin alignment and therefore the maximum stability for the atom or ion.

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  • 2. 

    Which of the following statements is true regarding electron configuration?

    • A.

      Electrons fill orbitals from lower to higher energy levels.

    • B.

      Electrons fill orbitals from higher to lower energy levels.

    • C.

      Electrons fill orbitals randomly without following any particular order.

    • D.

      Electrons fill orbitals only when all higher energy levels are filled completely.

    Correct Answer
    A. Electrons fill orbitals from lower to higher energy levels.
    Explanation
    Electrons fill orbitals from lower to higher energy levels. This is known as the Aufbau principle and is based on the idea that electrons seek the most stable configuration by filling the lowest energy levels first.

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  • 3. 

    Which electron configuration violates Hund's rule?

    • A.

      1s2 2s2 2p6

    • B.

      1s2 2s2 2p5

    • C.

      1s2 2s2 2p4

    • D.

      1s2 2s2 2p3

    Correct Answer
    B. 1s2 2s2 2p5
    Explanation
    Electron configuration '1s2 2s2 2p5' violates Hund's rule because it pairs up electrons in the same orbital (2p) without filling all the orbitals with parallel spins first.

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  • 4. 

    How many electrons can be accommodated in the s orbital?

    • A.

      2

    • B.

      4

    • C.

      6

    • D.

      8

    Correct Answer
    A. 2
    Explanation
    The s orbital can accommodate a maximum of 2 electrons. This is because the s orbital has a single orientation and can hold two electrons with opposite spins.

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  • 5. 

    Which of the following electron configurations is correct for oxygen (atomic number 8)?

    • A.

      1s2 2s2 2p2

    • B.

      1s2 2s2 2p3

    • C.

      1s2 2s2 2p4

    • D.

      1s2 2s2 2p5

    Correct Answer
    C. 1s2 2s2 2p4
    Explanation
    The correct electron configuration for oxygen (atomic number 8) is '1s2 2s2 2p4'. Oxygen has 8 electrons, and following the Aufbau principle, we fill the lowest energy levels first, with the s orbital being filled before the p orbital. Each orbital can hold a maximum of 2 electrons, and thus, the p orbital will be filled with 4 electrons.

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  • 6. 

    Which electron configuration exists for an atom in an excited state?

    • A.

      1s2 2s2 2p6 3s1

    • B.

      1s2 2s2 2p6 3s2

    • C.

      1s2 2s2 2p6 3s2 3p1

    • D.

      1s2 2s2 2p6 3s2 3p2

    Correct Answer
    D. 1s2 2s2 2p6 3s2 3p2
    Explanation
    The electron configuration '1s2 2s2 2p6 3s2 3p2' represents an atom in an excited state. An excited state occurs when an electron has absorbed energy and moved to a higher energy level or a higher energy orbital within the same level. In this case, the atom has one electron in the 3p orbital, which is higher in energy compared to the 3s orbitals.

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  • 7. 

    Which principle explains the filling order of atomic orbitals?

    • A.

      Hund's rule

    • B.

      Pauli exclusion principle

    • C.

      Aufbau principle

    • D.

      Octet rule

    Correct Answer
    C. Aufbau principle
    Explanation
    The filling order of atomic orbitals is explained by the Aufbau principle. According to this principle, electrons fill the lowest energy levels first before moving to higher energy levels. This principle helps in determining the electron configuration of atoms and their stability.

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  • 8. 

    When writing electron configurations, which quantum number describes the shape of the orbital?

    • A.

      Principal quantum number (n)

    • B.

      Azimuthal quantum number (l)

    • C.

      Magnetic quantum number (m)

    • D.

      Spin quantum number (s)

    Correct Answer
    B. Azimuthal quantum number (l)
    Explanation
    The shape of the orbital is described by the azimuthal quantum number (l). It determines the subshell (s, p, d, f) to which an orbital belongs. The value of l ranges from 0 to (n-1), where n is the principal quantum number.

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  • 9. 

    Which electron configuration is correct for a neutral sulfur atom (atomic number 16)?

    • A.

      1s2 2s2 2p6 3s2 3p4

    • B.

      1s2 2s2 2p6 3s2 3p5

    • C.

      1s2 2s2 2p6 3s2 3p6

    • D.

      1s2 2s2 2p6 3s2 3p7

    Correct Answer
    A. 1s2 2s2 2p6 3s2 3p4
    Explanation
    The correct electron configuration for a neutral sulfur atom (atomic number 16) is '1s2 2s2 2p6 3s2 3p4'. Sulfur has 16 electrons, and following the Aufbau principle, we fill the lowest energy levels first, with the s orbital being filled before the p orbital. The 3p orbital will be filled with 4 electrons.

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  • 10. 

    Which of the following electron configurations violates the Pauli exclusion principle?

    • A.

      1s1

    • B.

      1s2

    • C.

      2s2 2p6

    • D.

      2s2 2p5

    Correct Answer
    D. 2s2 2p5
    Explanation
    The electron configuration '2s2 2p5' violates the Pauli exclusion principle. This principle states that no two electrons in an atom can have the same four quantum numbers, meaning they must have opposite spins. In this configuration, two electrons are paired up with the same spin in the 2p orbital, violating the principle.

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  • Current Version
  • Sep 22, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Sep 22, 2023
    Quiz Created by
    Amit Mangal
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