Rutherford Model and Wave-Particle Duality
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Rutherford Model and Wave-Particle Duality

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Questions and Answers

What is the relationship between wavelength (λ) and the mass (m) and velocity (v) of a moving material particle as proposed by Louis De Broglie?

  • λ = mv/h (correct)
  • λ = h/vm
  • λ = hv/m
  • λ = h/mv
  • According to De Broglie's model, what does the equation 2πr = nλ signify?

  • The energy of the particle is a function of the radius.
  • The orbit radius is directly proportional to the wavelength.
  • The velocity of the particle is constant.
  • The total orbit length is equal to a multiple of the wavelength. (correct)
  • What kind of spectrum is produced when electromagnetic radiation is generated from discharges in low-pressure gases like hydrogen?

  • Continuous spectrum
  • Absorption spectrum
  • Discontinuous spectrum (correct)
  • Infrared spectrum
  • What does the energy (E) of a particle relate to according to De Broglie's demonstration?

    <p>E = hv</p> Signup and view all the answers

    In the context of emission spectra, what is a common characteristic observed in the spectrum of hydrogen?

    <p>It results in a set of distinct colored lines.</p> Signup and view all the answers

    What would happen to the electron according to the laws of electrodynamics when it orbits the nucleus?

    <p>It would gradually lose energy and fall into the nucleus.</p> Signup and view all the answers

    What is one issue with Rutherford's description of the atom?

    <p>It fails to explain why electrons do not fall into the nucleus.</p> Signup and view all the answers

    In the atomic model described by Rutherford, what is situated at the center of the atom?

    <p>A dense nucleus</p> Signup and view all the answers

    What electromagnetic phenomenon is expected to occur as the electron orbits the nucleus?

    <p>Emission of electromagnetic radiation</p> Signup and view all the answers

    How do electrons orbit the nucleus in Rutherford's atomic model?

    <p>In a planetary-like manner</p> Signup and view all the answers

    What is the wavelength range of visible light?

    <p>380 nm to 780 nm</p> Signup and view all the answers

    Which of the following correctly describes the particle aspect of light?

    <p>Light is composed of photons, each carrying a specific amount of energy</p> Signup and view all the answers

    What does the formula $E = hv = \frac{hc}{\lambda}$ represent in relation to light?

    <p>The relationship between light energy, frequency, and wavelength</p> Signup and view all the answers

    Which scientist is NOT associated with the wave-particle duality of light?

    <p>Isaac Newton</p> Signup and view all the answers

    Which type of electromagnetic radiation has a longer wavelength than visible light?

    <p>Infrared light</p> Signup and view all the answers

    What type of wave does light from the sun exemplify?

    <p>Electromagnetic wave</p> Signup and view all the answers

    What phenomenon explains why sunlight appears white to the naked eye?

    <p>Combination of different colors</p> Signup and view all the answers

    What is the speed of light in a vacuum?

    <p>$3 imes 10^8$ m⋅s⁻¹</p> Signup and view all the answers

    What is the definition of a wavelength?

    <p>The length of a cycle of a wave</p> Signup and view all the answers

    Which fields are present in an electromagnetic wave?

    <p>Electric field and magnetic field</p> Signup and view all the answers

    What is the speed of light in a vacuum?

    <p>3⋅10^8 m/s</p> Signup and view all the answers

    What unit is used to measure the frequency of a wave?

    <p>Hertz (Hz)</p> Signup and view all the answers

    Which type of electromagnetic radiation has very short wavelengths?

    <p>Gamma rays</p> Signup and view all the answers

    What is the wavelength range of the visible spectrum?

    <p>390 nm to 760 nm</p> Signup and view all the answers

    What is the relationship between the period and frequency of a wave?

    <p>Frequency is the inverse of the period.</p> Signup and view all the answers

    What does the first postulate of Bohr's model state about the electron in a hydrogen atom?

    <p>The electron moves in circular, stationary orbits with constant energy.</p> Signup and view all the answers

    According to the second postulate of Bohr's model, what is true about the angular momentum of the electron?

    <p>It is an integer multiple of h/2π.</p> Signup and view all the answers

    What happens when an electron transitions between stationary orbits according to the third postulate?

    <p>It absorbs or emits electromagnetic radiation.</p> Signup and view all the answers

    What is the value of Planck's constant (h) related to in Bohr's model?

    <p>Quantum unit of angular momentum.</p> Signup and view all the answers

    How does Bohr's model describe the structure of the hydrogen atom?

    <p>It is structured around quantized energy levels.</p> Signup and view all the answers

    What force is equal in magnitude but opposite in direction to the centripetal force acting on an electron in Bohr's model?

    <p>Electrostatic force</p> Signup and view all the answers

    Which equation represents the total energy of an electron in the Bohr model?

    <p>E_T = - rac{Ke^2}{2r}</p> Signup and view all the answers

    In the context of Bohr's model, what does the centripetal force depend on?

    <p>The mass of the electron and its velocity</p> Signup and view all the answers

    From the equations presented, what does $m_e v^2 = \frac{Ke^2}{r}$ imply about the electron?

    <p>The electron's velocity changes based on its radius</p> Signup and view all the answers

    What is the relationship between potential energy and distance in the Bohr model?

    <p>Potential energy decreases as distance increases</p> Signup and view all the answers

    What is the expression for the total energy of the hydrogen atom as a function of the principal quantum number n?

    <p>$E_{T} = - rac{2K^{2} imes rac{h^{2}}{2}}{n^{2}}$</p> Signup and view all the answers

    What is the value of the first Bohr radius when n = 1?

    <p>$0.529 ext{ Å}$</p> Signup and view all the answers

    Which equation reflects Bohr's second postulate regarding angular momentum quantization?

    <p>$mev_{r} imes r = rac{n imes h}{2 heta}$</p> Signup and view all the answers

    What energy level corresponds to the ground state of the hydrogen atom?

    <p>$-13.6 eV$</p> Signup and view all the answers

    For an electron in an excited state with n > 1, what can be said about the amount of energy it has?

    <p>It has additional energy from an external source.</p> Signup and view all the answers

    What happens to the electron when it transitions from a higher energy level to a lower one?

    <p>It emits energy.</p> Signup and view all the answers

    What is the equation that relates the difference in energy levels to the emitted photon?

    <p>$|E_{n2} - E_{n1}| = ΔE = hν$</p> Signup and view all the answers

    What is the role of the constant $R_H$ in the context of the hydrogen atom?

    <p>It is used in the Ritz-Rydberg formula for wavelengths.</p> Signup and view all the answers

    Which of the following describes the absorption of energy by the electron?

    <p>Transition from $E_{n1}$ to $E_{n2}$</p> Signup and view all the answers

    Which equation accurately represents the frequency of the emitted radiation?

    <p>$ν = \frac{2Kπ^2e^4m_e}{h^3} (\frac{1}{n_1^2} - \frac{1}{n_2^2})$</p> Signup and view all the answers

    What does a higher principal quantum number (n) indicate about an electron's state?

    <p>The electron is in an excited state.</p> Signup and view all the answers

    What is the ionization energy of a hydrogen atom?

    <p>-13.6 eV</p> Signup and view all the answers

    What happens when an electron transitions to a lower energy level?

    <p>It emits radiation.</p> Signup and view all the answers

    What does the formula $E_n = \frac{-13.6}{n^2}$ represent?

    <p>The energy level of a hydrogen atom depending on n.</p> Signup and view all the answers

    What does a negative energy value indicate about an electron in the hydrogen atom?

    <p>The electron is bound to the nucleus.</p> Signup and view all the answers

    What represents the free electron state in the energy level diagram?

    <p>n = ∞</p> Signup and view all the answers

    How can the energy of emitted radiation when an electron transitions be calculated?

    <p>Using $E_n2 - E_n1 = hν$.</p> Signup and view all the answers

    Which statement best describes the energy levels of the hydrogen atom?

    <p>Electrons can occupy specific quantized energy levels.</p> Signup and view all the answers

    Study Notes

    Rutherford Model

    • Rutherford described the atom as a nucleus with orbiting electrons, like planets around the sun.
    • This model contradicts electrodynamics, as electrons should radiate energy while orbiting, causing them to spiral into the nucleus.
    • However, atoms exist, and electrons don't fall into nuclei.

    Wave-Particle Duality & De Broglie's Relationship

    • Building on work by Planck and Einstein, Louis de Broglie proposed that any moving particle with mass m and velocity v has an associated wave with wavelength λ, given by: λ = h/mv.
    • The frequency v of the associated wave relates to the particle's energy E: E = hv.
    • In the model, the orbit's total length is a whole number multiple of the de Broglie wavelength (2πr = nλ).

    Hydrogen Atom Emission Spectrum

    • When gas in a tube is excited under low pressure, it emits a line spectrum, meaning only specific wavelengths of light are seen.
    • The spectrum of hydrogen appears as a series of colored bands, representing the frequencies of light emitted when electrons transition between energy levels.

    Electromagnetic Spectrum

    • The image shows a spectrum of electromagnetic radiation, including visible light.
    • The visible light spectrum is a small portion of the electromagnetic spectrum with wavelengths ranging from approximately 380 nm to 780 nm.
    • The diagram includes gamma rays, X-rays, ultraviolet (UV) light, infrared (IR) light, microwaves, and radio waves, ordered by wavelength and energy.

    Light Characteristics

    • Light has both wave and particle aspects.
    • Wave Aspect: Light has a specific color (or a mix of colors) corresponding to its wavelength, frequency, and energy.
    • Particle Aspect: Light consists of photons, each carrying energy proportional to its frequency: E = hv = hc/λ.

    Wave-Particle Duality

    • Planck and Einstein established the wave-particle duality of light.
    • Louis de Broglie extended this concept to include electrons.

    Electromagnetic Wave

    • A wave with both an electric field E and a magnetic field B oscillating at the same frequency (ν).
    • These fields propagate perpendicularly to each other in a medium, with speed equal to $3 \cdot 10^{8}$ m⋅s⁻¹ in a vacuum.
    • A wave is characterized by wavelength (λ), period (T), and frequency (v).

    Wavelength, Period & Frequency

    • Wavelength (λ): Length of one wave cycle, the distance between two successive peaks.
    • Period (T): Time for one wave cycle.
    • Frequency (v): Number of cycles per unit time (Hertz, Hz).
    • v = 1/T = c/λ (where c is the speed of light).

    Electromagnetic Spectrum

    • The range of wavelengths and frequencies of electromagnetic radiation.
    • Includes gamma rays (short wavelengths), radio waves (long wavelengths), and many others in between.
    • Most of the electromagnetic spectrum is invisible to the human eye; only a visible portion is seen.

    Visible Spectrum

    • The portion of the electromagnetic spectrum visible to humans, with wavelengths roughly from 390 nm to 760 nm.
    • Includes the colors of the rainbow, from violet to red.

    Bohr's Model of the Atom

    • The atomic model introduced in 1913 that explains the structure of the hydrogen atom and its emission spectrum based on energy quantization.
    • Bohr's Postulates:
      • Electrons in a hydrogen atom orbit the nucleus in circular, stationary orbits with constant energy.
      • The electron's angular momentum (mvr) is quantized, being an integer multiple of h/2π: mvr = nh/2π.
      • When changing orbits, electrons absorb or emit electromagnetic radiation (hv) according to ΔE = |En1 − En2| = hv.

    Bohr Model Forces & Energies

    • The text describes the forces and energies involved in the Bohr model of the atom.
    • The equations show relationships between centripetal force, electrostatic force, kinetic energy, potential energy, and total energy of an electron orbiting an atomic nucleus.

    Bohr Model of the Hydrogen Atom

    • Constants:
      • k = 1 / 4πε₀
      • ε₀ = 8.85 × 10⁻¹² C²N⁻¹m⁻² (permittivity of free space)
    • Equations:
      • $E_{T} = -\frac{Ke^{2}}{r} + \frac{Ke^{2}}{2r} = -\frac{Ke^{2}}{2r}$
      • $mev^{2} = \frac{Ke^{2}}{r}$
      • $mev^{2} = \frac{Ke^{2}}{2r}$

    Orbital Radius & Energy Levels

    • Combining equations leads to the formula for the radius of the orbit: $r = \frac{n^{2}\times h^{2}}{4\pi^{2} \times K \times m \times e^{2}}$.
    • For n = 1, r = 0.529 Å (the first Bohr radius).
    • The total energy as a function of n is: $E_{T} = -\frac{2K^{2} \pi^{2} m e^{4}}{h^{2}} \times \frac{1}{n^{2}}$.
    • For n = 1: $E_{T} = -\frac{2K^{2} \pi^{2} m e^{4}}{h^{2}}$.
    • $E_{n} = E_{1} = -\frac{2K^{2}\pi^{2} \times m \times e^{4}}{h^{2} \times n^{2}} = -21.76 \times 10^{-19} J = -13.6 eV$. (Ground state energy of hydrogen)

    Energy Levels of the Hydrogen Atom

    • States with higher n values correspond to excited states of the electron.
    • The formula $E_n = \frac{E_1}{n^2}$ calculates the energy of a state with quantum number n.
    • The ionization energy of hydrogen (E1) is -13.6 eV.

    Energy Level Diagram

    • The diagram shows the energy levels of the hydrogen atom, with negative energies indicating a bound electron.
    • The energy levels are discrete, meaning the electron can only exist at specific energy values.
    • Ionization energy is the energy required to remove the electron completely from the atom.

    Electron Behavior

    • Electrons stay in a specific energy level without emitting energy.
    • When the electron moves to a lower energy level, it emits radiation, with energy equal to the energy difference between the levels.
    • The energy of emitted radiation can be calculated using Planck's equation: $E_n2 − E_n1 = hν = \frac{hc}{\lambda}$.

    Bohr Model Summary

    • Bohr's model successfully explains the hydrogen atom's emission spectrum and the concept of quantized energy levels.
    • It serves as a foundation in understanding atomic structure and how energy is related to electron transitions.

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    Description

    Explore the Rutherford model of the atom, which describes electrons orbiting a nucleus, and understand the implications of wave-particle duality as proposed by Louis de Broglie. This quiz also covers the emission spectrum of hydrogen, highlighting its unique line spectrum and energy relationships.

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