Virtual Labs

Quantum Mechanics of the Hydrogen Atom

1. In the simulation, when you set n=2 and ℓ=1, what orbital type are you visualizing?

a: 2s orbital Explanation

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b: 2p orbital Explanation

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c: 2d orbital Explanation

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d: 1p orbital Explanation

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2. While using the simulation, you observed that the 3s orbital appears larger than the 1s orbital. This is because:

a: 3s has more electrons Explanation

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b: Higher n means the electron is farther from the nucleus on average Explanation

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c: 3s has a different shape than 1s Explanation

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d: The simulation is incorrectly scaled Explanation

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3. When you changed the visualization mode to 'Probability' in the simulation, the dots represent:

a: Actual electron positions at different times Explanation

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b: Probability density of finding the electron Explanation

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c: Electric field strength Explanation

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d: Nuclear charge distribution Explanation

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4. In the simulation, you observed that the energy becomes less negative as n increases. What does this indicate?

a: The electron loses energy Explanation

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b: The electron is less tightly bound to the nucleus Explanation

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c: The orbital becomes smaller Explanation

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d: The electron moves faster Explanation

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5. Using the simulation, you found that for n=3 and ℓ=2, the mₗ slider allows values from -2 to +2. How many distinct 3d orbitals does this represent?

a: 2 Explanation

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b: 3 Explanation

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c: 5 Explanation

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d: 7 Explanation

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6. The simulation shows that a p-orbital has a dumbbell shape with two lobes. What separates these lobes?

a: The nucleus Explanation

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b: A nodal plane where ψ = 0 Explanation

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c: An energy barrier Explanation

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d: A magnetic field Explanation

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7. When you clicked on the '4f' preset button in the simulation, which quantum numbers were automatically set?

a: n=4, ℓ=4, mₗ=0 Explanation

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b: n=4, ℓ=3, mₗ=0 Explanation

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c: n=3, ℓ=4, mₗ=0 Explanation

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d: n=4, ℓ=2, mₗ=0 Explanation

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8. After completing the simulation, which statement best describes the relationship between quantum numbers and orbital properties?

a: All quantum numbers equally affect only the energy Explanation

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b: n affects size/energy, ℓ affects shape, mₗ affects orientation Explanation

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c: Quantum numbers only affect the color of the visualization Explanation

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d: Only the principal quantum number matters for orbital properties Explanation

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9. The simulation showed that the energy of hydrogen orbitals follows E = -13.6/n² eV. What would be the energy at n = ∞ (ionization)?

a: -13.6 eV Explanation

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b: -∞ eV Explanation

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c: 0 eV Explanation

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d: +13.6 eV Explanation

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10. Based on your simulation observations, why can't a 2d orbital exist?

a: d-orbitals require at least 10 electrons Explanation

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b: Because ℓ must be less than n, so for n=2, ℓ can only be 0 or 1 Explanation

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c: d-orbitals are only found in transition metals Explanation

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d: The simulation doesn't support d-orbitals Explanation

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