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Questions and Answers
Who is recognized as the father of Modern Chemistry?
In what year did John Dalton present his theory?
According to Dalton's theory, what is true about all atoms of a given element?
Which statement is consistent with John Dalton's atomic theory?
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What aspect of atoms did John Dalton emphasize in his theory?
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What is the mass of an electron in kilograms?
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Who discovered the neutron?
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Which particle has a charge of +1.602 × 10-19 C?
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How is the radius of an atom typically measured?
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When was the electron discovered?
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What does the nucleus of an atom contain?
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What surrounds the nucleus of an atom in Rutherford's model?
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In Rutherford's atomic model, what term is used for the paths electrons follow around the nucleus?
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What happens to the alpha particles when they hit the thin gold foil in the diagram?
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What is indicated by the '*' symbol in the scattering diagram?
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What determines the angular momentum of an electron in the Bohr model?
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Which constant is NOT part of the angular momentum equation in the Bohr model?
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How does the Bohr model explain the stability of an atom?
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What is the relationship between energy change ($\Delta E$) and frequency ($ u$) when an electron transitions between energy levels?
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What does the equation $\Delta E = h u$ represent in the context of the Bohr model?
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What describes the orbits in which electrons revolve around the nucleus?
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How does an electron move from a lower energy level to a higher energy level?
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What is the relationship between emitted or absorbed energy and the energy levels?
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In the equation $ rac{E_{higher}}{E_{lower}} = hv$, what does 'h' represent?
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Which letter represents the lowest energy level in Bohr's Theory?
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What does $ rac{h}{4 ext{π}}$ represent in the uncertainty principle?
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Which of the following variables represents the uncertainty of momentum?
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In what year was the uncertainty principle proposed?
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What limitation of Bohr's atomic model relates to the effect of a magnetic field on atomic spectra?
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Which effect, related to electric fields, is a limitation of Bohr's atomic model?
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What does $ ext{Δx}$ represent in the context of the uncertainty principle?
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Who proposed the uncertainty principle?
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Which principle does Bohr's atomic model violate?
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Which of the following phenomena can Bohr's model not explain?
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What aspect of atomic behavior is not addressed by Bohr's atomic model?
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What does the principal quantum number (n) describe?
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Which of the following expresses the subsidiary quantum number (l)?
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Which type of orbitals corresponds to l = 1?
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What is another name for the subsidiary quantum number?
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What does the spin quantum number (s) represent?
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What does the Rutherford atomic model incorrectly imply about electron motion?
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According to calculations based on Rutherford's model, how quickly would an electron collapse into the nucleus?
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What is a key limitation of the Rutherford atomic model?
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Which theory conflicts with the Rutherford model regarding electron behavior?
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What aspect of atomic structure was not addressed in the Rutherford model?
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What does the wave function ψ represent in the Schrödinger equation?
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Which constant is represented by 'h' in the Schrödinger equation?
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In the equation, which variable represents the total energy?
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What does the term V represent in the Schrödinger equation?
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What does the equation indicate about the relationship between energy and wave function?
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Study Notes
Atomic Radius
- Measured in nanometers (nm), with 1 m equating to 10^9 nm or 0.1 m or 1 Ångström (Å).
Stationary Fundamental Particles
- Electron (e-): Discovered by J.J. Thomson in 1897, mass is 9.107 × 10^-28 kg, charge is -1.602 × 10^-19 C.
- Proton (P or H+): Discovered by E. Goldstein in 1836, mass is 1.672 × 10^-27 kg, charge is +1.602 × 10^-19 C.
- Neutron: Discovered by James Chadwick in 1932, mass is 1.672 × 10^-24 g, no charge.
John Dalton's Atomic Theory
- Introduced in 1803, known as the father of Modern Chemistry.
- Postulated that all atoms of a given element are identical in mass and properties.
Rutherford Atomic Model
- Became known as the nuclear model of the atom.
- Composed of a dense nucleus made of protons and neutrons, surrounded by negatively charged electrons in fixed circular paths called orbits.
Diagram of Rutherford's Model
- Depicts alpha particles emitted from a He2+ source, scattering on thin gold foil.
- Indicates large-angle scattering of alpha particles and uses shading to indicate where they hit the foil.
Limitations of Rutherford's Atomic Model
- Predicted that electrons should emit energy and spiral into the nucleus, which contradicts Maxwell's theory.
- Could not explain the stability of the atom or the arrangement of electrons.
Bohr's Theory
- Electrons revolve in discrete circular orbits around the nucleus without radiating energy, preventing collapse into the nucleus.
- Energy levels are represented as K, L, M, N, or n = 1, 2, 3...
- Electrons can transition between energy levels by absorbing or emitting energy, described by ΔE = hv, where h is Planck’s constant and v is the frequency.
Bohr Model
- Angular momentum of an electron is quantified as mvr = nh/2π, where variables represent mass, velocity, and radius of orbit, with h being Planck's constant and n as a positive integer.
- Successfully explains atom stability and the hydrogen atom's line spectrum.
Limitations of Bohr's Model
- Unable to explain the Zeeman Effect (magnetic field effects on spectra).
- Failed to address the Stark Effect (electric field effects on spectra).
- Violates Heisenberg Uncertainty Principle.
Heisenberg Uncertainty Principle
- Expressed as ΔxΔp ≥ h/4π, where Δx is position uncertainty and Δp is momentum uncertainty.
Quantum Numbers
- Describe an electron's state including its distance from the nucleus, orbital orientation and type, and spin.
- Four types include Principal Quantum Number (n), Subsidiary Quantum Number (l), Magnetic Quantum Number (m), and Spin Quantum Number (s).
Principal Quantum Number
- Denotes the size of the orbital, with n values of 1, 2, 3...
Subsidiary Quantum Number
- Indicates orbital shape, expressed in terms of l with values from 0 to n-1.
- Orbitals are represented as s, p, d, f with corresponding l values.
Schrödinger Equation
- Represents a mathematical model for the wave function of a quantum system, describing the probability of a particle's position and momentum.
- Written as:
[ \frac{d^2\psi}{dx^2} + \frac{d^2\psi}{dy^2} + \frac{d^2\psi}{dz^2} + \frac{8\pi m}{h^2}(E-V)\psi = 0 ] - Variables include wave function (ψ), mass (m), Planck constant (h), total energy (E), and potential energy (V).
Erwin Schrödinger
- Austrian physicist instrumental in the development of quantum mechanics, formulated the Schrödinger equation in 1926.
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Description
Explore the fundamental concepts of atomic structure, including atomic radius, stationary fundamental particles, and key atomic theories. This quiz covers the contributions of notable scientists like John Dalton and Ernest Rutherford, and how their models shaped modern chemistry. Test your understanding of atomic physics today!
