Grade 12 Electron Configuration Worksheet
This worksheet covers advanced concepts in electron configuration, including orbital diagrams, quantum numbers, and exceptions to the Aufbau principle for Grade 12 Chemistry students.
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Electron Configuration Review
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Read each question carefully and provide detailed answers based on your knowledge of electron configurations and quantum mechanics. Show all your work for calculations.
1. Write the full electron configuration and orbital diagram for a neutral atom of Manganese (Mn).
2. Explain Hund's Rule and the Pauli Exclusion Principle in your own words, providing an example for each.
3. Which of the following sets of quantum numbers (n, l, ml, ms) is NOT possible for an electron in an atom?
(3, 2, -1, +1/2)
(2, 2, 0, -1/2)
(4, 0, 0, +1/2)
(1, 0, 0, -1/2)
4. What is the maximum number of electrons that can occupy a 'd' subshell?
2
6
10
14
5. The Aufbau principle states that electrons fill atomic orbitals of the energy levels first.
6. The electron configuration of an element describes how electrons are distributed among the orbitals.
7. For an electron in the 3p subshell, the possible values for the magnetic quantum number (ml) are .
8. The electron configuration for Chromium (Cr) is [Ar] 4s² 3d⁴.
True
False
9. All orbitals within a given subshell have the same energy in a multi-electron atom.
True
False
10. Consider the illustration of the atom electron cloud below. If this represented an electron in a 2p orbital, what are the possible values for its quantum numbers (n, l, ml, ms)?
11. Discuss the concept of 'shielding' and 'penetration' in multi-electron atoms and how these factors influence the effective nuclear charge experienced by valence electrons. How does this relate to the order of filling orbitals (e.g., why 4s fills before 3d)?