Chemistry 1: Sub-atomic Particles Quiz
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Questions and Answers

What was the overall charge of the atom in Thomson's Plum-Pudding Model?

  • Electrically neutral (correct)
  • Variable charge
  • Negatively charged
  • Positively charged
  • Which particle did J.J. Thomson consider to be a fundamental particle?

  • Electron (correct)
  • Proton
  • Neutron
  • Nucleus
  • Who discovered radioactivity and coined the term?

  • Henri Becquerel
  • Ernest Rutherford
  • J.J. Thomson
  • Marie and Pierre Curie (correct)
  • What significant contribution did Rutherford make regarding atomic structure?

    <p>He introduced the concept of a central nucleus.</p> Signup and view all the answers

    What experiment did Rutherford use to demonstrate the shortcomings of Thomson's model?

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

    What did J.J. Thomson conclude about cathode rays?

    <p>They consist of negatively charged particles.</p> Signup and view all the answers

    What experimental method did Robert Millikan use to determine the charge of an electron?

    <p>Charged oil droplets.</p> Signup and view all the answers

    What was the main feature of Thomson's Plum-Pudding Model?

    <p>Electrons were uniformly distributed in a positive matrix.</p> Signup and view all the answers

    Which of the following did Thomson conduct in 1897?

    <p>Charge-to-mass ratio calculation.</p> Signup and view all the answers

    What did the mass-to-charge ratio allow Thomson to determine?

    <p>The properties of electrons.</p> Signup and view all the answers

    What analogy was used to describe Thomson's Plum-Pudding Model?

    <p>Plum pudding dessert.</p> Signup and view all the answers

    Which discovery is attributed to J.J. Thomson?

    <p>The identification of the electron.</p> Signup and view all the answers

    How were electrons thought to be arranged in the Plum-Pudding Model?

    <p>Uniformly distributed throughout the atom.</p> Signup and view all the answers

    What primarily contributes to the positive charge of an atom?

    <p>Protons in the nucleus</p> Signup and view all the answers

    According to Rutherford’s model, how do electrons move around the nucleus?

    <p>In fixed, discrete energy levels</p> Signup and view all the answers

    What did Rutherford's model imply about the structure of the atom?

    <p>It is mostly empty space.</p> Signup and view all the answers

    What makes an atom electrically neutral?

    <p>Equal numbers of protons and electrons</p> Signup and view all the answers

    What were neutrons discovered to be in Chadwick’s experiment?

    <p>Electrically neutral particles</p> Signup and view all the answers

    What was the target material used in Chadwick’s Beryllium-Paraffin experiment?

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

    What characteristic of neutrons explains why they were not deflected in experiments?

    <p>They are electrically neutral.</p> Signup and view all the answers

    In Rutherford's Nuclear Model, what happens to the mass of the atom?

    <p>Most of it is concentrated in the nucleus.</p> Signup and view all the answers

    Study Notes

    Discovery of Electrons

    • J.J. Thomson conducted experiments in 1897 using cathode rays, revealing they could be deflected by magnetic and electric fields, indicating they were composed of charged particles.
    • Thomson calculated the mass-to-charge ratio of these particles and found they possessed a net negative charge, coining the term "electron" for these subatomic particles.

    Robert Millikan's Experiment

    • Between 1906 and 1914, Robert Millikan used electrically charged oil droplets to determine the charge of a single electron.
    • Utilized Thomson’s mass-to-charge ratio to calculate the mass of an electron.

    J.J. Thomson's Plum-Pudding Model

    • Proposed in 1904, suggested that atoms consist of a positively charged matrix that holds most of the atom's mass, akin to "pudding."
    • Negatively charged electrons were embedded within this matrix like "plums" in a pudding, distributed uniformly, yielding an overall electrically neutral atom.
    • Asserted that electrons were fundamental particles that could not be further divided.

    Radiation Discovery

    • Henri Becquerel discovered that uranium salts emitted a new form of energy.
    • Marie and Pierre Curie introduced the term "radioactivity" to describe this emission of energy rays.
    • Ernest Rutherford identified multiple distinct types of radiation emitted by compounds containing uranium and other elements.

    Discovery of Protons

    • Ernest Rutherford's gold foil experiment demonstrated that Thomson's atomic model was inaccurate.
    • Introduced the nuclear model of the atom in 1911, featuring a dense, positively charged nucleus at its center, containing most of the atom’s mass.

    Rutherford's Nuclear Model

    • Proposed that electrons orbit a central nucleus in fixed energy levels similar to planets around the sun.
    • Established the concept that atoms are mostly empty space, with orbiting electrons occupying this volume around the nucleus.
    • Emphasized that the atom remains electrically neutral, as the positive charge of the nucleus balances the negative charge of the electrons.

    Discovery of Neutrons

    • James Chadwick utilized beryllium as a target in experiments, bombarding it with alpha particles and observing a penetrating radiation that was neither electrically charged nor affected by electric/magnetic fields.
    • Concluded these neutral particles, with a mass slightly greater than protons, are known as neutrons and possess no electrical charge.

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    Description

    Test your knowledge on the fundamental aspects of sub-atomic particles, particularly focusing on J.J. Thomson's Cathode Ray Experiment. This quiz covers essential concepts in General Inorganic Chemistry as part of Quarter 1 Week 2b. Dive into the world of electrons and discover their significance in atomic theory.

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