Atomic Structure of Matter
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Questions and Answers

According to Hund's Rule, how should electrons be distributed in orbitals of the same energy?

  • All electrons should be paired in the first orbital before moving to the next.
  • Electrons should fill each orbital singly before pairing. (correct)
  • Electrons can fill any orbital randomly without following a specific order.
  • All electrons must occupy the lowest energy orbital first before moving higher.

    • Why does the electron configuration for chlorine show 3p has 5 electrons rather than 6?

  • The 3p orbital can only hold a maximum of 5 electrons.
  • The chlorine atom does not have enough protons to hold more electrons.
  • Chlorine prefers to have unpaired electrons for stability.
  • The energy levels dictate that lower energy orbitals fill first. (correct)

    • What do you call atoms that have unpaired electrons in their orbital diagrams?

  • Stable atoms
  • Diamagnetic atoms
  • Paramagnetic atoms (correct)
  • Magnetically neutral atoms

    • In the orbital filling sequence for chlorine, how many total electrons are in the 3p orbital?

    <p>5</p> Signup and view all the answers

    What is the significance of the term 'Aufbau Principle' in relation to electron configuration?

    <p>It determines the order in which electrons fill atomic orbitals based on energy levels.</p> Signup and view all the answers

    What term did Democritus use to refer to the smallest indivisible objects?

    <p>Atomos</p> Signup and view all the answers

    Which scientist proposed that matter consists of indivisible atoms?

    <p>John Dalton</p> Signup and view all the answers

    What model of the atom was J.J. Thompson known for?

    <p>Plum Pudding Model</p> Signup and view all the answers

    Which experimental setup did Ernest Rutherford use to discover the nucleus?

    <p>Gold foil experiment</p> Signup and view all the answers

    What was one of the key features of the Plum Pudding Model?

    <p>Electrons are embedded in a positively charged sphere</p> Signup and view all the answers

    Which atomic model introduced the concept of nuclei containing protons and electrons?

    <p>Nuclear Model</p> Signup and view all the answers

    What is the significance of quantum numbers in atomic structure?

    <p>They describe the electron's position and energy</p> Signup and view all the answers

    What does the term 'electron configuration' refer to?

    <p>The distribution of electrons among the energy levels</p> Signup and view all the answers

    What determines the location and energy of every electron in an atom?

    <p>A set of four quantum numbers</p> Signup and view all the answers

    Which of the following is NOT a type of atomic orbital?

    <p>g orbital</p> Signup and view all the answers

    What does the principal quantum number (n) indicate?

    <p>The energy level of the electron</p> Signup and view all the answers

    How can we describe the location of electrons in an atom?

    <p>There is a certain probability of finding them in given space</p> Signup and view all the answers

    What is the significance of an atom's core?

    <p>It is composed of at least one proton</p> Signup and view all the answers

    Which statement is true regarding the probability of finding an electron?

    <p>There is a certain probability we can find an electron in a given space</p> Signup and view all the answers

    Which of the following statements about atomic orbitals is incorrect?

    <p>f orbitals are always located at the nucleus</p> Signup and view all the answers

    What is the relationship between the principal quantum number and the distance from the nucleus?

    <p>Higher principal quantum numbers indicate greater distance from the nucleus</p> Signup and view all the answers

    What behavior is characteristic of the electrons in an atom based on their energy levels?

    <p>Electrons can move freely but still have specific energy levels</p> Signup and view all the answers

    Who were the first people to propose the idea of atoms?

    <p>Democritus and Leucippus</p> Signup and view all the answers

    According to the Bohr model, how are electrons situated in an atom?

    <p>They orbit randomly like planets around the nucleus.</p> Signup and view all the answers

    What is primarily described by the Quantum Mechanical Model?

    <p>The shapes of orbitals and electron probabilities.</p> Signup and view all the answers

    Which scientist is credited with the discovery of protons?

    <p>Ernest Rutherford</p> Signup and view all the answers

    How many types of orbitals are there in the Quantum Mechanical Model?

    <p>Four</p> Signup and view all the answers

    What happens to the probability of finding an electron as the distance from the nucleus increases?

    <p>It begins to decrease after a certain distance.</p> Signup and view all the answers

    In the context of atomic structure, what does 'nucleus' refer to?

    <p>The center where protons and neutrons are concentrated.</p> Signup and view all the answers

    How did early ideas about atoms represent atomic structure?

    <p>Atoms were seen as indivisible particles.</p> Signup and view all the answers

    Which statement accurately describes the density of an electron's location near the nucleus?

    <p>Most of the electron density is located near the nucleus.</p> Signup and view all the answers

    What was a significant contribution of Niels Bohr to atomic theory?

    <p>Developed the first quantum model of the atom.</p> Signup and view all the answers

    What does the angular momentum quantum number (l) describe?

    <p>The shape of the orbital</p> Signup and view all the answers

    If an electron has a principal quantum number (n) of 3, which of the following values can l take?

    <p>0, 1, or 2</p> Signup and view all the answers

    Which orbital corresponds to l = 1?

    <p>p-orbital</p> Signup and view all the answers

    The magnetic quantum number (ml) can take values based on l. What are the possible values when l = 2?

    <p>-2, -1, 0, 1, 2</p> Signup and view all the answers

    How many electrons can the d-orbitals hold?

    <p>10</p> Signup and view all the answers

    According to the Pauli Exclusion Principle, what is true about electrons in an atom?

    <p>No two electrons can have the same set of quantum numbers</p> Signup and view all the answers

    Which quantum number indicates the spin of an electron?

    <p>ms</p> Signup and view all the answers

    What is the maximum number of electrons that can occupy f-orbitals?

    <p>14</p> Signup and view all the answers

    Which of the following electric properties is wrong regarding the quantum numbers?

    <p>ml can be equal to l</p> Signup and view all the answers

    Study Notes

    Atomic Structure of Matter

    • Democritus proposed the concept of "atomos" (uncuttable particles) with varying sizes and shapes.
    • Dalton's atomic model (1808) posited atoms as indivisible particles combining to form different compounds.
    • The Plum Pudding model (1904) depicted atoms with negatively charged electrons embedded in a positively charged "dough".
    • Rutherford's nuclear model (1911) suggested a dense, positively charged nucleus at the center of the atom, with electrons orbiting around it, largely empty space.
    • Bohr's model (1913) illustrated electrons orbiting the nucleus in specific energy levels and pathways, similar to planets orbiting a star.
    • The Quantum Mechanical Model (1920s), developed by Schrödinger, describes electrons as existing in orbitals, defined regions of space where there's a high probability of finding them.
    • Subatomic particles include protons (positively charged), neutrons (neutral), and electrons (negatively charged). Protons and neutrons reside in the nucleus.
    • Atomic orbitals are described by quantum numbers, which dictate the shape, size, and energy of orbitals.
    • Principal quantum number (n) represents the energy level.
    • Angular momentum quantum number (l) describes the shape.
    • Magnetic quantum number (ml) specifies the orientation in space.
    • Spin quantum number (ms) describes the spin of the electron, either +1/2 or -1/2.
    • The Aufbau principle dictates electron filling order in orbitals, starting from the lowest energy level.
    • Hund's rule suggests that electrons fill each orbital individually before doubling up.
    • Paramagnetic atoms have unpaired electrons and are attracted to magnetic fields.
    • Diamagnetic atoms have all paired electrons and are not significantly affected by magnetic fields

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    Science Grade 9 Week 2 Quarter 2 PDF

    Description

    Explore the evolution of atomic theory from Democritus to Schrödinger. This quiz covers key models including Dalton's, Rutherford's, Bohr's, and the Quantum Mechanical model. Test your understanding of the structure of atoms and subatomic particles.

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