Grade 12 Chemistry: Orbital Diagrams
A Grade 12 Chemistry worksheet covering electron configurations and orbital diagrams, including Hund's Rule and the Pauli Exclusion Principle.
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Grade 12 Chemistry: Orbital Diagrams
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Read each question carefully and provide the best answer. Show all your work for calculations and orbital diagrams.
1. According to the , no two electrons in an atom can have the same set of four quantum numbers.
2. Hund's Rule states that electrons will occupy separate orbitals within a subshell with spins before pairing up.
3. The maximum number of electrons that can occupy a 'p' subshell is .
4. The principle states that electrons fill orbitals starting with the lowest energy level.
Match each term with its definition.
1. Principal Quantum Number
a. Describes the orientation of an orbital in space
2. Angular Momentum Quantum Number
b. Describes the main energy level of an electron
3. Magnetic Quantum Number
c. Describes the shape of an orbital
4. Spin Quantum Number
d. Describes the intrinsic angular momentum of an electron
1. Write the full electron configuration and draw the orbital diagram for Nitrogen (N).
2. Write the full electron configuration and draw the orbital diagram for Sulfur (S).
3. Explain how Hund's Rule applies when filling the 3d orbitals of an atom like Iron (Fe).
4. Describe the significance of the Pauli Exclusion Principle in terms of electron pairing within an orbital.
1. Which of the following elements has an electron configuration ending in 3p⁵?
Oxygen
Chlorine
Fluorine
Bromine
1. All orbitals within a given subshell have the same energy level.
True
False