Balmer Series and Atomic Absorption Spectrometry Quiz
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Questions and Answers

What is the main difference between an energy level and an atomic orbital?

  • Energy level refers to the fixed energy of an electron, while atomic orbital refers to a region in space where there is high probability of finding an electron. (correct)
  • Energy level refers to the region in space where there is high probability of finding an electron, while atomic orbital refers to a fixed energy of an electron.
  • Atomic orbital determines the energy of an electron, while energy level indicates the position of the electron.
  • Energy level is the same as atomic orbital.
  • What is the electron configuration (s, p) of an atom of silicon in its ground state?

  • 1s² 2s² 2px² 2py² 2pz² 3s² 3px¹ 3py¹ (correct)
  • 1s² 2s² 2px² 2py² 2pz² 3s² 3px⁰ 3py¹
  • 1s² 2s² 2px² 2py² 2pz² 3s² 3px¹ 3py⁰
  • 1s² 2s² 2px² 2py² 2pz² 3s² 3px¹ 3py¹ (correct)
  • How many main energy levels are occupied in the ground state of a silicon atom?

  • 5
  • 3 (correct)
  • 4
  • 2
  • How many atomic orbitals are occupied by a silicon atom in its ground state?

    <p>8</p> Signup and view all the answers

    What was the purpose of Millikan’s 'oil drop' experiments from 1908 to 1913?

    <p>To measure the magnitude of the charge on an electron</p> Signup and view all the answers

    Which term refers to a fixed energy value of an electron in an atom?

    <p>Main energy level</p> Signup and view all the answers

    How many electrons are present in the 3d subshell of an iron atom?

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

    Which subshell is filled after the 4s subshell in an iron atom's electron configuration?

    <p>(3d)</p> Signup and view all the answers

    In which subshell does the last electron reside in an iron atom's ground state configuration?

    <p>(5s)</p> Signup and view all the answers

    'To measure the magnitude of the charge on an electron' describes the purpose of which experiment?

    <p>'Oil drop' experiments</p> Signup and view all the answers

    How many electrons are present in each p orbital when all three p orbitals are half-filled?

    <p>2</p> Signup and view all the answers

    Study Notes

    Bohr's Contribution to Atomic Theory

    • Niels Bohr provided insights into electron arrangement in atoms through his study of atomic spectra.
    • When white light passes through a prism, it produces a continuous spectrum; Bohr focused on hydrogen's emission spectrum, which consists of narrow colored lines.
    • Each element has a unique emission spectrum, important for element identification.

    Spectroscopy Tools

    • A spectrometer measures light wavelength; a spectroscope observes spectra without measuring wavelengths.
    • Flame tests can identify metals based on the color they produce when burned:
      • Lithium: Crimson
      • Potassium: Lilac
      • Barium: Green
      • Strontium: Red
      • Copper: Blue-green
      • Sodium: Yellow

    Bohr's Theory of Electron Energy Levels

    • Electrons possess fixed energy values called quanta, moving in defined paths or orbits (energy levels).
    • Energy levels are labeled with 'n', starting with n=1 as the lowest.
    • Atoms in the ground state have electrons at the lowest energy levels; they absorb energy to jump to excited states.

    Ground and Excited States

    • Ground state: Electrons occupy the lowest energy levels available.
    • Excited state: Electrons occupy higher energy levels, becoming unstable and eventually returning to the ground state while emitting energy as light.
    • Energy difference between levels corresponds to emitted light frequency, defined by the equation E2 – E1 = hf, where 'h' is Planck's constant, and 'f' is frequency.

    Emission Spectra and the Balmer Series

    • Electrons falling to the n=2 energy level produce visible light, called the Balmer Series, identifiable by specific colored lines in the emission spectrum.

    Atomic Absorption Spectrometry (AAS)

    • Atoms also absorb specific wavelengths of light, creating an Atomic Absorption Spectrum where certain wavelengths are missing.
    • Ground state atoms absorb the same wavelengths they emit when excited.
    • AAS is utilized for analyzing metals in water, blood samples, and forensic applications, reflecting the absorbed light's correlation with the element's concentration.

    Energy Sublevels

    • Energy levels above n=1 include sublevels, subdivisions containing orbitals of identical energy.
    • The number of sublevels matches the energy level’s principal quantum number (n), e.g., n=2 has 2 sublevels.

    Wave-Particle Duality

    • Louis de Broglie proposed that all moving particles, including electrons, have associated wave motion.
    • Werner Heisenberg formalized this with the Uncertainty Principle, stating simultaneous measurement of an electron's velocity and position is impossible, challenging Bohr's model.

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    Description

    Test your knowledge on the Balmer Series of emission lines, where electrons transition from n=2 energy level, and the principles of Atomic Absorption Spectrometry (AAS) in analyzing samples. Explore the relationship between energy levels, frequency of emitted light, and Planck's constant.

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