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Questions and Answers
What is the fundamental charge of an electron?
What is the fundamental charge of an electron?
- $3 \times 10^8$ ms$^{-1}$
- $9.11 \times 10^{-31}$ kg
- 1 in 20,000 were deflected
- $1.602 \times 10^{-19}$ C (correct)
What did Ernest Rutherford's experiment with alpha particles lead to the discovery of?
What did Ernest Rutherford's experiment with alpha particles lead to the discovery of?
- The nuclear model of the atom (correct)
- The analysis of light emitted or absorbed by substances
- The mass of an electron
- The speed of light
What is the speed of light in a vacuum?
What is the speed of light in a vacuum?
- $1.602 \times 10^{-19}$ C
- $3 \times 10^8$ ms$^{-1}$ (correct)
- $9.11 \times 10^{-31}$ kg
- 1 in 20,000 were deflected
What did J.J. Thomson's cathode ray experiment lead to the discovery of?
What did J.J. Thomson's cathode ray experiment lead to the discovery of?
What is the trend for atomic radius across a period in the periodic table?
What is the trend for atomic radius across a period in the periodic table?
Which statement about ionic radius is correct?
Which statement about ionic radius is correct?
What is the general trend for ionization energy across a period?
What is the general trend for ionization energy across a period?
Which statement about electron affinity is true?
Which statement about electron affinity is true?
What is the Inert-Pair Effect?
What is the Inert-Pair Effect?
What are the properties of s-block elements?
What are the properties of s-block elements?
What are the properties of p-block elements?
What are the properties of p-block elements?
What are the properties of d-block elements?
What are the properties of d-block elements?
What is the minimum energy needed to remove an electron from a neutral atom in the gas phase?
What is the minimum energy needed to remove an electron from a neutral atom in the gas phase?
What is the energy released when an electron attaches to a gas-phase atom?
What is the energy released when an electron attaches to a gas-phase atom?
What is the trend for first ionization energies down a group?
What is the trend for first ionization energies down a group?
What is the trend for successive ionization energies?
What is the trend for successive ionization energies?
What did Max Planck propose to solve the ultraviolet catastrophe in classical physics?
What did Max Planck propose to solve the ultraviolet catastrophe in classical physics?
What does the de Broglie relation $\lambda = \frac{h}{p}$ illustrate?
What does the de Broglie relation $\lambda = \frac{h}{p}$ illustrate?
What does the uncertainty principle proposed by Heisenberg highlight?
What does the uncertainty principle proposed by Heisenberg highlight?
What phenomenon does quantum theory explain?
What phenomenon does quantum theory explain?
What concept did Max Planck introduce in his solution to the ultraviolet catastrophe?
What concept did Max Planck introduce in his solution to the ultraviolet catastrophe?
What did the photoelectric effect demonstrate about electromagnetic radiation?
What did the photoelectric effect demonstrate about electromagnetic radiation?
What did Johann Balmer and Johannes Rydberg contribute to the understanding of spectral lines in the hydrogen spectrum?
What did Johann Balmer and Johannes Rydberg contribute to the understanding of spectral lines in the hydrogen spectrum?
What does the Bohr frequency condition introduced by Einstein support?
What does the Bohr frequency condition introduced by Einstein support?
What are atomic spectra produced by?
What are atomic spectra produced by?
What does the electromagnetic spectrum include?
What does the electromagnetic spectrum include?
What gives rise to spectral lines in atoms?
What gives rise to spectral lines in atoms?
What does the de Broglie relation illustrate about matter?
What does the de Broglie relation illustrate about matter?
What does Heisenberg's Uncertainty Principle state?
What does Heisenberg's Uncertainty Principle state?
What does Schrödinger's wavefunction, Ψ, describe?
What does Schrödinger's wavefunction, Ψ, describe?
What does the Particle in a Box model demonstrate?
What does the Particle in a Box model demonstrate?
What determines the energy and existence of discrete energy levels in the Hydrogen Atom?
What determines the energy and existence of discrete energy levels in the Hydrogen Atom?
How are atomic orbitals described?
How are atomic orbitals described?
What is true about the ground state wavefunction for the hydrogen atom?
What is true about the ground state wavefunction for the hydrogen atom?
How many quantum numbers are needed to label each wavefunction for 3-dimensional Schrödinger’s equation?
How many quantum numbers are needed to label each wavefunction for 3-dimensional Schrödinger’s equation?
How do the orbitals of a shell with principal quantum number n fall into subshells?
How do the orbitals of a shell with principal quantum number n fall into subshells?
What does the value of l determine for atomic orbitals?
What does the value of l determine for atomic orbitals?
What does the magnetic quantum number, ml, specify?
What does the magnetic quantum number, ml, specify?
How are the orbitals of a shell with principal quantum number n distributed?
How are the orbitals of a shell with principal quantum number n distributed?
What is true about the energy of all orbitals of a given shell for atoms with 1 electron?
What is true about the energy of all orbitals of a given shell for atoms with 1 electron?
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Study Notes
Quantum Mechanics and Atomic Structure
- Heisenberg's Uncertainty Principle states that the product of the uncertainties in position and momentum is greater than or equal to Planck's constant divided by 2π.
- Schrödinger's wavefunction, Ψ, describes the probability of finding a particle and satisfies the Schrödinger equation, which calculates the wavefunction and energy for a particle.
- The Particle in a Box model demonstrates quantization of energy levels, where only certain wavelengths fit into the box, resulting in discrete energy levels.
- The Hydrogen Atom's energy levels are quantized, with the principle quantum number, n, determining the energy and existence of discrete energy levels.
- Atomic orbitals are described by spherical polar coordinates, with radial and angular wavefunctions determining the probability density of an electron at each point.
- The ground state wavefunction for the hydrogen atom is spherically symmetric and has the highest probability density closest to the nucleus.
- Three quantum numbers (n, l, ml) are needed to label each wavefunction for 3-dimensional Schrödinger’s equation, determining the size, shape, and orientation of the orbital.
- The orbitals of a shell with principal quantum number n fall into n subshells, and the value of l determines the orbital angular momentum and shape of the orbital.
- The magnetic quantum number, ml, distinguishes individual orbitals within a subshell and specifies the orientation of the orbital motion of the electron.
- The combination of the three quantum numbers specifies an individual orbital, and each shell has 2s-orbital and multiple p, d, and f orbitals, with specific orientations and shapes.
- For atoms with 1 electron, all orbitals of a given shell have the same energy, regardless of their orbital angular momentum, making them degenerate.
- The Schrödinger equation and quantum mechanics provide a detailed understanding of atomic structure, energy quantization, and the behavior of particles at the quantum level.
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