Atomic Orbitals Worksheet
Explore the shapes, energies, and quantum numbers associated with atomic orbitals in Grade 12 Chemistry.
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Atomic Orbitals Worksheet
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Read each question carefully and provide the best answer based on your understanding of atomic orbitals and quantum mechanics.
1. What is the maximum number of electrons that can occupy a single atomic orbital?
1
2
6
10
2. Which quantum number describes the shape of an atomic orbital?
Principal quantum number (n)
Angular momentum quantum number (l)
Magnetic quantum number (ml)
Spin quantum number (ms)
3. The states that no two electrons in the same atom can have the same set of four quantum numbers.
4. A p-orbital has a shape.
5. The principal quantum number (n) primarily determines the and of an electron.
6. All orbitals within a given subshell have the same energy in a multi-electron atom.
True
False
7. The spin quantum number (ms) can have values of +1/2 or -1/2.
True
False
8. Draw and label the shapes of the 2s and 2p orbitals.
9. Explain the difference between an orbital and an orbit.
Match each quantum number with the property it describes.
10. Principal quantum number (n)
a. Orientation of the orbital in space
11. Angular momentum quantum number (l)
b. Energy level and size of the orbital
12. Magnetic quantum number (ml)
c. Shape of the orbital
13. Describe the Aufbau principle, Hund's rule, and the Pauli exclusion principle, and explain how they are used to determine the electron configuration of an atom.