SCH4U1 Models of the Atom Quiz

Study Notes

John Dalton: Proposed the billiard ball model, suggesting atoms are solid and indivisible spheres. Limitations include inability to explain isotopes or chemical reactivity.
J.J. Thomson: Conducted cathode ray experiments leading to the plum pudding model, where electrons are embedded in a positive sphere. Limitations revolve around the lack of a nucleus and the structure’s failure to account for atomic behavior.
Ernest Rutherford: Gold foil experiment revealed the nuclear model, proposing a dense nucleus surrounded by electrons. Limitations include not accounting for electron stability and behaviors.
Niels Bohr: Developed the Bohr model based on electromagnetic spectra, introducing quantized orbits for electrons. Limitations found in explaining spectral lines of multi-electron atoms.
Louis de Broglie: Theorized matter waves, suggesting particles exhibit wave properties similar to light. His equation (λ = h/mv) connects wavelength, mass, and speed. This theory aligns with Bohr's findings but doesn't explain complex electron behaviors.
Erwin Schrödinger: Integrated wave-like behavior of electrons into atomic models, creating wave functions (Ψ) that illustrate probable electron locations in 3D atomic orbitals.
Werner Heisenberg: Introduced the uncertainty principle, pinpointing that one cannot simultaneously know an electron's exact position and momentum. His equation (ΔxΔmv ≥ h/4π) outlines this limitation in measurement.

Evolved from merging de Broglie’s and Einstein’s theories, establishing a model where electrons are viewed as standing waves.
Describes atomic particles using mathematical equations to express wave properties.
Electrons have discrete energy levels akin to Bohr's model, with their probable locations represented as atomic orbitals.

Quantum numbers stem from solutions to the Schrödinger wave equation, identifying properties of electrons within atoms.
Four quantum numbers summarize electron specifics:
- Principal Quantum Number (n): Indicates the energy level or shell of the electron.
- Orbital-Shape Quantum Number: Represents the shape of the orbital (sublevel).
- Magnetic Quantum Number: Identifies a specific subshell or orientation of the orbital.
- Spin Quantum Number: Indicates the electron's spin direction.
Quantum numbers can be visualized as an address for electrons: Country > City > Street > Building.

John Dalton: Proposed the billiard ball model, suggesting atoms are solid and indivisible spheres. Limitations include inability to explain isotopes or chemical reactivity.
J.J. Thomson: Conducted cathode ray experiments leading to the plum pudding model, where electrons are embedded in a positive sphere. Limitations revolve around the lack of a nucleus and the structure’s failure to account for atomic behavior.
Ernest Rutherford: Gold foil experiment revealed the nuclear model, proposing a dense nucleus surrounded by electrons. Limitations include not accounting for electron stability and behaviors.
Niels Bohr: Developed the Bohr model based on electromagnetic spectra, introducing quantized orbits for electrons. Limitations found in explaining spectral lines of multi-electron atoms.
Louis de Broglie: Theorized matter waves, suggesting particles exhibit wave properties similar to light. His equation (λ = h/mv) connects wavelength, mass, and speed. This theory aligns with Bohr's findings but doesn't explain complex electron behaviors.
Erwin Schrödinger: Integrated wave-like behavior of electrons into atomic models, creating wave functions (Ψ) that illustrate probable electron locations in 3D atomic orbitals.
Werner Heisenberg: Introduced the uncertainty principle, pinpointing that one cannot simultaneously know an electron's exact position and momentum. His equation (ΔxΔmv ≥ h/4π) outlines this limitation in measurement.

Evolved from merging de Broglie’s and Einstein’s theories, establishing a model where electrons are viewed as standing waves.
Describes atomic particles using mathematical equations to express wave properties.
Electrons have discrete energy levels akin to Bohr's model, with their probable locations represented as atomic orbitals.

Quantum numbers stem from solutions to the Schrödinger wave equation, identifying properties of electrons within atoms.
Four quantum numbers summarize electron specifics:
- Principal Quantum Number (n): Indicates the energy level or shell of the electron.
- Orbital-Shape Quantum Number: Represents the shape of the orbital (sublevel).
- Magnetic Quantum Number: Identifies a specific subshell or orientation of the orbital.
- Spin Quantum Number: Indicates the electron's spin direction.
Quantum numbers can be visualized as an address for electrons: Country > City > Street > Building.