Exploring the Bohr Atomic Model

What are the main characteristics of electron orbits in the Bohr model?

• Electrons do not have specific energy levels in orbits.

• Electrons can only exist in one orbit at a time without transitioning.

• Electron orbits are quantized, fixed paths with specific energy levels, and electrons can transition between these orbits by absorbing or emitting energy.

• Electron orbits are random and unpredictable.

How does the Bohr model define energy levels for electrons?

• Electrons can exist in any energy level without restriction.

• Energy levels are determined solely by the electron's mass.

• Electrons are not restricted to specific distances from the nucleus.

• Electrons occupy quantized energy levels defined by their distance from the nucleus, determined by the principal quantum number.

What is the formula used to calculate the energy levels in a hydrogen atom according to the Bohr model?

• E_n = - (13.6 eV) / n^2

• E_n = - (6.8 eV) * n^2

• E_n = - (27.2 eV) / n^3

• E_n = (13.6 eV) / n

What are the limitations of the Bohr model when applied to multi-electron atoms?

• The Bohr model can predict the exact energy levels of all multi-electron atoms.

• The Bohr model incorporates relativistic effects for multi-electron systems.

• The Bohr model accurately describes electron interactions in multi-electron atoms.

• The limitations of the Bohr model in multi-electron atoms include neglecting electron-electron interactions, inability to explain fine structure, and lack of quantum mechanical principles.

How does the Bohr model explain the emission spectrum of hydrogen?

• The spectrum is a result of chemical reactions in the hydrogen gas.

• The emission spectrum is caused by the movement of protons in the nucleus.

• Electrons emit energy continuously without quantization.

• The emission spectrum of hydrogen is explained by electron transitions between quantized energy levels, emitting photons of specific wavelengths.

What is the significance of the principal quantum number in the Bohr model?

• The principal quantum number indicates the mass of the electron.

• The principal quantum number determines the color of the emitted light.

• The principal quantum number is related to the charge of the nucleus.

• The principal quantum number signifies the energy level and size of an electron's orbit in the Bohr model.

How does the concept of quantization relate to electron orbits in the Bohr model?

• Quantization has no effect on the stability of electron orbits.

• Electron orbits are determined solely by their mass in the Bohr model.

• Quantization restricts electron orbits to specific energy levels in the Bohr model.

• Quantization allows electrons to occupy any orbit freely.

What experimental evidence supports the Bohr model of the hydrogen atom?

• Continuous spectrum observed in hydrogen's emission spectrum.

• Absence of spectral lines in hydrogen's emission spectrum.

• Discrete spectral lines in hydrogen's emission spectrum.

• Spectral lines observed in other elements only.

In what ways does the Bohr model differ from classical physics?

• Electrons can exist in any orbit without restrictions.

• The Bohr model eliminates the concept of energy levels entirely.

• The Bohr model differs from classical physics by introducing quantized energy levels and stable electron orbits, preventing electrons from spiraling into the nucleus.

• Electrons are treated as particles with no wave-like properties.

What role does the concept of angular momentum play in the Bohr model?

• Angular momentum is irrelevant in the Bohr model.

• Angular momentum quantization determines the allowed electron orbits and energy levels in the Bohr model.

• Angular momentum only affects the nucleus, not the electrons.

• Angular momentum is a concept that applies only to classical mechanics.