Practice Quantum Numbers And Orbital Shapes (2.6)

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6 sample questions

Question 1.
What is the maximum number of electrons that can fit in the n=2 energy level?
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Use the formula 2n².
Question 2.
What shape is represented by the azimuthal quantum number ℓ=2?
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Think about the shapes associated with each ℓ value.
3Question 3.
What is the principal quantum number for an electron in the n=3 shell?
- 0
- 1
- 3
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Look for the number specifying the shell directly.
4Question 4.
True or False: The magnetic quantum number can have a value of +2 for a p orbital.
- True
- False
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Confirm the range of values for m_ℓ.
Question 5.
Consider an electron in a 4f orbital. What are the values and implications of its quantum numbers?
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Remember how ℓ relates to the type of subshell.
Question 6.
Describe how an increase in effective nuclear charge affects the electron holding in the outermost shell.
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Consider how charges from protons versus shielding from inner electrons change.

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