Questions About Energy Levels

 Questions About Energy Levels

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 Multiple-Choice Questions: Energy Levels

1. What does the term “energy level” in an atom refer to?
   A) The velocity of an electron
   B) The orbit radius of a nucleus
   C) A quantized amount of energy an electron can have
   D) The atomic weight
   E) The number of neutrons in the nucleus

2. Which quantum number primarily determines the energy level of an electron?
   A) Spin quantum number
   B) Principal quantum number
   C) Magnetic quantum number
   D) Azimuthal quantum number
   E) Radial quantum number

3. In a hydrogen atom, the energy levels are:
   A) Equally spaced
   B) Continuously variable
   C) Closer together as $n$ increases
   D) Independent of $n$
   E) Randomly distributed

4. Which of the following best describes the ground state of an atom?
   A) The state with maximum potential energy
   B) An excited state
   C) The lowest possible energy level
   D) A temporary state
   E) A state of radioactive decay

5. When an electron moves from a higher to a lower energy level, it:
   A) Absorbs a photon
   B) Emits a photon
   C) Changes into a proton
   D) Becomes unstable
   E) Gains mass

6. Energy levels in atoms are described as:
   A) Discrete
   B) Arbitrary
   C) Continuous
   D) Variable
   E) Infinite

7. Which scientist’s model introduced the concept of quantized energy levels in atoms?
   A) Schrödinger
   B) Heisenberg
   C) Bohr
   D) Einstein
   E) Rutherford

8. The difference between two energy levels in an atom corresponds to:
   A) Atomic mass
   B) Energy of emitted or absorbed radiation
   C) Number of protons
   D) Ionization potential
   E) Gravitational force

9. Which energy transition in the hydrogen atom releases the most energy?
   A) From $n=4$ to $n=3$
   B) From $n=2$ to $n=1$
   C) From $n=5$ to $n=4$
   D) From $n=3$ to $n=2$
   E) From $n=6$ to $n=5$

10. What happens to the energy of an electron as it moves to higher energy levels?
    A) It decreases
    B) It stays the same
    C) It becomes negative
    D) It increases
    E) It becomes zero

11. Which series in the hydrogen spectrum corresponds to transitions to the $n=1$ level?
    A) Balmer series
    B) Paschen series
    C) Lyman series
    D) Brackett series
    E) Pfund series

12. In quantum mechanics, electrons occupy energy levels to:
    A) Maximize distance from the nucleus
    B) Minimize energy
    C) Maximize charge
    D) Match the number of neutrons
    E) Create light

13. The ionization energy of an atom refers to:
    A) Energy released when an atom gains a neutron
    B) Energy needed to remove an electron from the atom
    C) Energy stored in the nucleus
    D) Energy emitted during radioactive decay
    E) Total energy of all electrons

14. Which element has only one electron energy level when neutral?
    A) Helium
    B) Hydrogen
    C) Lithium
    D) Carbon
    E) Neon

15. In the Bohr model, which energy level is the most negative?
    A) $n = 1$
    B) $n = 2$
    C) $n = 3$
    D) $n = 4$
    E) $n = \infty$

16. The energy difference between levels in the Bohr model is proportional to:
    A) $1/n$
    B) $n^2$
    C) $1/n^2$
    D) $n^3$
    E) $\sqrt{n}$

17. Why can electrons not exist between energy levels in atoms?
    A) There are no forces acting there
    B) Their charge prevents it
    C) Energy levels are quantized
    D) They would lose mass
    E) They would become photons

18. When an atom is excited, it means that:
    A) It has lost an electron
    B) Its nucleus has split
    C) One or more electrons have moved to higher energy levels
    D) It becomes neutral
    E) It has become unstable

19. In multi-electron atoms, energy levels split into sublevels due to:
    A) Gravitational forces
    B) Electron-electron interactions
    C) Nucleon collisions
    D) Magnetic shielding
    E) Zero-point energy

20. As energy levels increase in hydrogen, they become:
    A) More negative
    B) Equally spaced
    C) Closer together
    D) Randomly spaced
    E) Unstable

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• Questions About the de Broglie Wave Equation
• Questions on Quantum Mechanics
• Questions on Heisenberg Uncertainty Principle

Answers and Explanations

1. C – A quantized amount of energy an electron can have
   Electrons in atoms have specific energy values they can occupy.

2. B – Principal quantum number
   It determines the main energy level or shell.

3. C – Closer together as $n$ increases
   In hydrogen, energy levels get closer as $n$ increases.

4. C – The lowest possible energy level
   The ground state is the most stable, lowest energy state.

5. B – Emits a photon
   Energy is released as light when dropping to a lower level.

6. A – Discrete
   Energy levels are not continuous; they have fixed values.

7. C – Bohr
   Niels Bohr’s model introduced quantized orbits for electrons.

8. B – Energy of emitted or absorbed radiation
   Transitions between levels correspond to photon energies.

9. B – From $n=2$ to $n=1$
   Lower levels have greater energy differences.

10. D – It increases
    Higher levels mean higher (less negative) energy.

11. C – Lyman series
    Transitions to $n=1$ emit ultraviolet radiation.

12. B – Minimize energy
    Electrons occupy levels in a way that minimizes the atom’s total energy.

13. B – Energy needed to remove an electron from the atom
    Ionization energy measures how tightly an electron is bound.

14. B – Hydrogen
    Hydrogen has only one electron in the $n=1$ level.

15. A – $n = 1$
    Lower energy levels have more negative energy.

16. C – $1/n^2$
    In Bohr's model, energy is inversely proportional to the square of $n$.

17. C – Energy levels are quantized
    Electrons can’t exist in between levels due to quantization.

18. C – One or more electrons have moved to higher energy levels
    Excitation involves absorbing energy and moving to a higher state.

19. B – Electron-electron interactions
    These cause splitting of energy levels into sublevels.

20. C – Closer together
    The higher the level, the smaller the energy difference with the next.

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Ronaldo Silva: Professor and Specialist in Science Teaching, from UFF/RJ, with more than 25 years of experience in teaching.