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Quizzes > Science

Quantum Numbers Quiz: Electron Configuration and Orbitals

Quick, free quiz to test electron configurations and quantum numbers. Instant results.

Editorial: Review CompletedCreated By: Asif KhanUpdated Aug 25, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration of electron orbitals numbers and calculator symbols on dark blue background for quantum number quiz

This quantum numbers quiz helps you practice choosing valid sets and building electron configurations. Answer short questions, get instant feedback, and fix mistakes fast as you learn how orbitals fill and pair. For more practice, try an electron configuration test, explore an orbital notation quiz, or take a focused quiz on quantum numbers.

What is the maximum number of electrons that can occupy the second energy level (n=2)?
2
4
18
8
The maximum number of electrons in any shell is given by 2n². For n = 2, 2 × (2²) = 2 × 4 = 8 electrons can occupy that level. This rule arises from the number of available orbitals and spin states. Learn more about electron shells .
Which of the following sets of quantum numbers is valid for an electron?
n=4, l=2, m?=3, m?=-1/2
n=3, l=2, m?=1, m?=+1/2
n=1, l=1, m?=-1, m?=+1/2
n=2, l=3, m?=0, m?=-1/2
Quantum numbers must satisfy: n ? 1, 0 ? l < n, ?l ? m? ? +l, and m? = ±1/2. The set n=3, l=2, m?=1, m?=+1/2 meets these criteria. The others violate one or more of these rules. Read more about quantum numbers .
What is the typical shape of a p orbital?
Toroidal
Spherical
Dumbbell-shaped
Four-lobed
P orbitals have a dumbbell shape with two lobes on opposite sides of the nucleus. This arises from the angular part of their wavefunction associated with l = 1. Each set of p orbitals has three orientations (m? = ?1, 0, +1). Further details on orbital shapes can be found .
What is the correct electron configuration for a neutral oxygen atom (Z=8)?
1s² 2s² 2p?
1s² 2s¹ 2p?
1s² 2s² 2p³
1s² 2s² 2p?
Oxygen has eight electrons. The first two fill the 1s orbital, the next two fill 2s, and the remaining four occupy the 2p orbital. Thus the configuration is 1s² 2s² 2p?. You can review electron configurations .
How many unpaired electrons are in a ground-state carbon atom (Z=6)?
1
2
0
3
Carbon's electron configuration is 1s² 2s² 2p². In the second shell, the two electrons occupy separate p orbitals with parallel spins, resulting in two unpaired electrons. Hund's rule explains this distribution. More on electron pairing and Hund's rule .
Which quantum number specifies the orientation of an orbital in space?
Magnetic quantum number (m?)
Principal quantum number (n)
Spin quantum number (m?)
Azimuthal quantum number (l)
The magnetic quantum number m? determines the orientation of the orbital around the nucleus, ranging from -l to +l. The principal quantum number n defines the energy level, and l defines the subshell shape. Spin quantum number m? specifies the electron spin direction. More on m? .
What is the correct term symbol for the ground state of the carbon atom?
¹S?
³D?
³P?
¹D?
Carbon's ground state configuration is 1s² 2s² 2p², which leads to a triplet P state with total spin S=1 and total orbital L=1, giving term symbol ³P?. The subscript 0 is the total angular momentum J. Explore term symbols in detail .
How many orbitals are in the 3d sublevel, and what is the maximum number of electrons it can hold?
7 orbitals, 14 electrons
5 orbitals, 10 electrons
3 orbitals, 6 electrons
9 orbitals, 18 electrons
A d sublevel has l = 2, so m? ranges from -2 to +2, giving five orbitals. Each orbital can hold two electrons, so the 3d sublevel can accommodate a total of 10 electrons. More on sublevels and capacities .
Which element has the electron configuration [Ne] 3s² 3p??
Argon (Ar)
Chlorine (Cl)
Sulfur (S)
Phosphorus (P)
The configuration [Ne] 3s² 3p? corresponds to element sulfur, which has atomic number 16. Neon core accounts for the first ten electrons, then 3s² and 3p? complete sulfur's valence shell. Confirm with periodic table details .
For a hydrogen-like atom, which pair of quantum numbers corresponds to the highest-energy sublevel within n=4?
n=4, l=3
n=4, l=1
n=4, l=0
n=4, l=2
Within a given principal level n, energy increases with azimuthal quantum number l. For n=4, the highest l value is 3 (4f sublevel), making it the highest-energy sublevel. This holds true for hydrogen-like atoms. More on sublevel energy ordering .
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Study Outcomes

  1. Understand Quantum Numbers -

    Learn the definitions and significance of the four quantum numbers (n, l, ml, ms) to describe electron positions within atoms.

  2. Apply Quantum Number Rules -

    Use established quantum number principles to assign valid values for electrons in specific atomic orbitals during the electron configuration quiz.

  3. Analyze Electron Configurations -

    Break down and interpret the step-by-step filling order of orbitals, reinforcing your electron configuration practice.

  4. Utilize the Quantum Number Calculator -

    Interact with the free quantum number calculator tool to receive instant feedback on your answers and correct mistakes on the spot.

  5. Evaluate Atomic Structure -

    Assess how quantum numbers and electron configurations relate to atomic properties, deepening your understanding of atomic structure quiz concepts.

  6. Interpret Periodic Table Electron Arrangement -

    Apply your knowledge in the periodic table electrons quiz by predicting and verifying electron distributions across elements.

Cheat Sheet

  1. Principal Quantum Number (n) -

    Defines the shell or energy level of an electron, where n=1,2,3… determines its relative distance from the nucleus. The maximum number of electrons in a shell is given by 2n² (e.g., n=2 holds up to 8 electrons), a fact emphasized on many university chemistry sites like MIT OpenCourseWare. Use "n=nth tier" as a quick mnemonic to recall it measures energy levels.

  2. Azimuthal Quantum Number (l) -

    Specifies the subshell or shape of the orbital, ranging from 0 to n - 1 and corresponding to s (l=0), p (l=1), d (l=2), and f (l=3) subshells. Resources such as Purdue University's ChemChain highlight how l dictates electron configuration practice when predicting chemical behavior. Remember the "speeds, pistols, dogs, foxes" phrase as a playful way to memorize s-p-d-f order.

  3. Magnetic Quantum Number (ml) -

    Indicates the orientation of an orbital in space, spanning integer values from - l to +l (for a p subshell with l=1, ml= - 1, 0, +1). This concept appears in any thorough atomic structure quiz on Britannica or Royal Society of Chemistry resources. A tip: visualize axes (x, y, z) to place p orbitals along three meridians in your mind for effective quantum number practice.

  4. Spin Quantum Number (ms) -

    Describes the intrinsic spin of an electron with only two values: +½ or - ½, ensuring no two electrons in an orbital share all four quantum numbers per the Pauli exclusion principle. This rule underpins most electron configuration quiz questions on platforms like Khan Academy and UW-Madison. Think "spin up before spin down" as a simple rule of thumb during your quantum number calculator challenges.

  5. Aufbau Principle & Hund's Rule -

    The Aufbau principle directs electrons to fill the lowest-energy orbitals first following the n + l rule, while Hund's rule states that electrons occupy degenerate orbitals singly before pairing with opposite spins. This combined guideline is foundational in electron configuration practice and is extensively covered by ACS publications. Memorize the diagonal rule diagram and the phrase "one to all, then pair to share" to breeze through the electron configuration quiz.

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