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Quantum-Mechanical Model of the Atom - General Chemistry

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Terms in this set (20)

  • What is the wave–matter duality concept?
    Subatomic particles like electrons exhibit both particulate (mass, volume) and wave-like energy characteristics depending on experimental conditions.
  • Why can't electrons in atoms be directly observed?
    Electrons are so small that observing them changes their behavior, even shining light on them affects their state.
  • What does the quantum mechanical model say about electrons in atoms?
    Electrons are not particles orbiting the nucleus but exist as a cloud of most probable positions described by wave nature.
  • What are the two perpendicular components of electromagnetic radiation?
    Electric field component and magnetic field component oscillate perpendicular to each other and the direction of travel.
  • Define wavelength and amplitude of a wave.
    Wavelength (λ) is the distance between successive crests; amplitude is the wave's height, related to light intensity.
  • How do wavelength and amplitude affect light properties?
    Wavelength determines color; amplitude determines brightness.
  • What is frequency (ν) of a wave?
    The number of waves passing a point per second, measured in hertz (Hz).
  • What is the relationship between wavelength and frequency?
    They are inversely proportional; as wavelength decreases, frequency increases, with speed of light constant: \(\nu \lambda = c\).
  • What is the electromagnetic spectrum?
    Range of all electromagnetic radiation wavelengths, from radio waves (long wavelength, low energy) to gamma rays (short wavelength, high energy).
  • What is the photoelectric effect?
    Emission of electrons from a metal surface when light of sufficient frequency shines on it.
  • What did Einstein propose about light energy in the photoelectric effect?
    Light energy is delivered in packets called quanta or photons, with energy proportional to frequency.
  • Write the formula relating photon energy to wavelength.
    Photon energy: \(E = \frac{hc}{\lambda}\), where h is Planck's constant and c is speed of light.
  • What is the threshold frequency in the photoelectric effect?
    Minimum frequency of light required to eject electrons from a metal surface.
  • What is the Bohr model's key idea about atomic energy?
    Atomic energy is quantized; electrons orbit the nucleus in fixed energy levels or stationary states.
  • What is de Broglie's hypothesis about electrons?
    Particles like electrons have wave-like properties, with wavelength inversely proportional to momentum: \(\lambda = \frac{h}{mv}\).
  • What does Heisenberg's uncertainty principle state?
    It is impossible to simultaneously know both the exact position and velocity of a particle like an electron.
  • What are the four quantum numbers and what do they represent?
    Principal (n): energy level; Angular momentum (l): orbital shape; Magnetic (m_l): orbital orientation; Spin (m_s): electron spin direction.
  • What shapes correspond to l = 0, 1, 2, and 3 orbitals?
    l=0: s (spherical), l=1: p (dumbbell), l=2: d (cloverleaf), l=3: f (complex lobed shapes).
  • How many orbitals are in a subshell with angular momentum quantum number l?
    Number of orbitals = 2l + 1.
  • What causes the lines in atomic emission spectra?
    Electrons transitioning between energy levels emit photons with energy equal to the difference between levels, producing discrete spectral lines.