Energy Levels in Atoms
This worksheet covers fundamental concepts of energy levels in atoms, including electron configuration, quantum numbers, and atomic spectra, suitable for Grade 12 Chemistry students.
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Energy Levels in Atoms
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Read each question carefully and answer to the best of your ability. Show all your work for calculations.
1. Which of the following describes the principal quantum number (n)?
It describes the shape of an orbital.
It indicates the energy level and size of an orbital.
It specifies the orientation of an orbital in space.
It represents the spin of an electron.
2. How many electrons can a single p-orbital hold?
1
2
3
6
3. The states that an electron occupies the lowest energy orbital that can receive it.
4. According to Hund's Rule, electrons will fill degenerate orbitals (orbitals of equal energy) before pairing up.
5. The maximum number of electrons that can be held in the n=3 energy level is .
6. Write the full electron configuration for a neutral sulfur atom (S).
7. Explain the concept of atomic emission spectra and how it relates to electron energy levels.
8. The Pauli Exclusion Principle states that no two electrons in the same atom can have the same set of four quantum numbers.
True
False
9. A photon is emitted when an electron moves from a lower energy level to a higher energy level.
True
False
10. Observe the atomic structure diagram below. Label the nucleus and at least two electron shells. Explain how the energy of electrons changes as they move further from the nucleus.
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