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Questions and Answers
What aspect of atomic structure does the Rutherford model fail to explain?
Why is the Rutherford model compared to a solar system?
What is a significant drawback of using classical mechanics to describe electron motion?
What issue arises from considering electrons as stationary around the nucleus?
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How does the Rutherford model relate to ion formation?
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What is a black body characterized by?
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How does the intensity of radiation emitted by a black body vary with wavelength?
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What is the phenomenon whereby electrons are ejected from certain metals when exposed to light?
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What type of equipment is used in the study of the photoelectric effect?
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Which of the following factors does not affect the distribution of black body radiation?
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What is the threshold frequency (ν₀) for the metal described in the content?
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Using Einstein's equation, which of the following represents the process of an electron emitting radiation?
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What happens to atoms and molecules after they absorb energy from electromagnetic radiation?
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What type of spectrum is produced when a substance emits radiation after absorbing energy?
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What does ν represent in the equation for kinetic energy of an emitted electron?
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What is the fundamental unit of electrical charge represented by in the equation q = n e?
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What determines the charge to mass ratio of positively charged particles discovered in canal rays?
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Which of the following statements about positively charged particles in canal rays is true?
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What type of force is NOT mentioned as acting on the oil droplets in Millikan's apparatus?
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Which statement accurately describes the behavior of positively charged particles compared to electrons?
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What is the formula for angular momentum of an electron moving in a circular orbit?
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Which of these statements is true regarding the principal quantum numbers of an electron in a hydrogen atom?
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What is the expression for the radius of the nth stationary state in a hydrogen atom according to Bohr's theory?
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What determines the stationary orbits that an electron can occupy?
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How is the frequency of radiation absorbed or emitted during transitions between stationary states calculated?
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Study Notes
Discovery of Protons and Neutrons
- Modified cathode ray tubes enabled the identification of positive charges, termed canal rays.
- Millikan's experiments demonstrated that the charge (q) on oil droplets is an integral multiple of the elementary charge (e); q = n*e (where n = 1, 2, 3...).
- Canal rays are positively charged gaseous ions, their charge-to-mass ratio varies by gas type.
- The smallest positive ion identified is the proton, derived from hydrogen.
- Rutherford's model suggests stability is questionable under classical mechanics due to electron movement.
Drawbacks of Rutherford Model
- The Rutherford atomic model likens an atom to a miniature solar system, where electrons orbit a dense nucleus.
- The model neglects the electronic structure, particularly how electrons are distributed around the nucleus.
- Classical mechanics predicts instability since electrostatic attraction would lead to electrons spiraling into the nucleus.
Black Body Radiation
- Black body radiators emit radiation based solely on temperature, characterized by a maximum intensity at specific wavelengths.
- The intensity of radiation increases with temperature but decreases as wavelength shortens beyond a certain point.
Photoelectric Effect
- In 1887, Hertz discovered that exposing specific metals (like potassium, rubidium, cesium) to light emitted electrons, termed the photoelectric effect.
- A critical frequency (threshold frequency) is required for electron ejection; below this threshold, no electrons are emitted.
- Light of higher frequency can liberate electrons with measurable kinetic energy, governed by the equation: KE = (h*(ν - ν₀)) where ν₀ is the threshold frequency.
Emission and Absorption Spectra
- When substances absorb energy, they emit radiation, forming an emission spectrum.
- Excited atoms or molecules transition to lower energy states, releasing radiation at characteristic frequencies.
Angular Momentum in Electron Orbits
- Angular momentum (L) for an electron in circular motion around a nucleus is quantized and defined as: L = mevr (where v is linear velocity).
- Only certain orbits are permissible, associated with integer multiples of h/2π (Planck constant).
- The Bohr model sets fixed orbits (n = 1, 2, 3...) corresponding to principal quantum numbers, with the first radius at r₁ = 52.9 pm (a₀).
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Description
Test your knowledge on the discovery of protons and neutrons, along with the limitations of the Rutherford model. This quiz covers key experiments and concepts, such as canal rays and black body radiation. Evaluate your understanding of atomic structure and its implications in classical mechanics.