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Quizzes > Science > Physics

Atoms Quiz: Can You Identify Every Subatomic Particle?

Think you can ace this atoms quiz? Test on atoms now with our atom quiz challenge!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Illustration for atoms quiz with subatomic particles, inviting users to take part on a sky blue background.

Use this quiz to identify subatomic particles and regions of the atom. Match protons, neutrons, electrons, and parts like the nucleus or electron cloud to each prompt. You'll get instant feedback and brief notes on every answer to spot gaps before a test or just have fun; for more practice, try a follow-up quiz.

Which subatomic particle carries a positive electrical charge?
Photon
Proton
Electron
Neutron
Protons are subatomic particles with a positive electric charge, residing in the atomic nucleus. Electrons, by contrast, carry a negative charge and orbit the nucleus. Neutrons have no charge. .
Which subatomic particle has no electric charge?
Positron
Electron
Neutron
Proton
Neutrons are subatomic particles found in the nucleus that carry no net electric charge. They contribute to the mass of the atom but do not affect its charge. Protons carry a positive charge, and electrons carry a negative charge. .
Which region of the atom is primarily occupied by electrons?
Nucleus
Electron cloud
Neutron layer
Proton shell
The electron cloud is the region around an atom's nucleus where electrons are likely to be found according to quantum mechanics. This area represents a probability distribution rather than fixed orbits. Most of an atom's volume is occupied by this electron cloud, making the nucleus extremely small by comparison. .
Which property of an element is defined by its number of protons?
Atomic number
Mass number
Atomic mass
Atomic radius
An element's atomic number is defined by the number of protons in its nucleus. This number uniquely identifies each element on the periodic table. Changing the proton count alters the element itself. .
What is the electric charge of an electron?
0
+1
-2
-1
Electrons carry a fundamental charge of -1 elementary charge unit. This negative charge balances the positive charge of protons in a neutral atom. Protons have a charge of +1 and neutrons have no charge. .
In an atom's nucleus, which two subatomic particles are found?
Protons and electrons
Protons and neutrons
Neutrons and electrons
Electrons and protons
Protons and neutrons are the two types of nucleons found in the atomic nucleus. Together they account for almost all of an atom's mass. Electrons orbit outside the nucleus and are not considered part of it. .
How many quarks are found in a proton?
Three
Four
Two
One
A proton is composed of three valence quarks: two up quarks and one down quark. These quarks are held together by the strong nuclear force mediated by gluons. The combination of quark types gives the proton its overall +1 charge. .
Which subatomic particle has the smallest mass among these options?
Electron
Proton
Alpha particle
Neutron
Among the primary subatomic particles in atoms, the electron has the smallest mass. Protons and neutrons are almost 1,836 and 1,839 times heavier, respectively. Electrons therefore contribute very little to the overall mass of an atom. .
Which subatomic particle mediates the electromagnetic force?
Neutrino
Photon
Gluon
W boson
Photons are the gauge bosons responsible for mediating the electromagnetic force in quantum field theory. They are massless particles that carry electromagnetic energy between charged particles. Gluons mediate the strong force, neutrinos interact via the weak force, and W bosons also participate in weak interactions. .
What is the term for atoms of the same element that have different numbers of neutrons?
Isotopes
Allotropes
Isomers
Ions
Isotopes are variants of the same element that differ only in their neutron count. They have the same number of protons (and thus the same atomic number) but different mass numbers due to additional or fewer neutrons. Isotopes can exhibit slightly different nuclear properties. .
The mass number of an atom equals the sum of which two particles?
Neutrons and electrons
Electrons and positrons
Protons and electrons
Protons and neutrons
The mass number of an atom is the total count of protons and neutrons in its nucleus. Electrons have negligible mass by comparison and are not included. This sum determines the isotope's mass on the periodic table. .
What is the name of the electron energy levels in the Bohr model of the atom?
Quantum numbers
Electron shells
Sublayers
Orbitals
In the Bohr model, electrons occupy discrete energy levels called electron shells around the nucleus. Each shell corresponds to a principal quantum number that determines its energy. While modern quantum mechanics uses orbitals, the shell concept remains a useful simplification. .
What is the antiparticle of the electron called?
Proton
Positron
Neutron
Anti-neutron
A positron is the antiparticle counterpart of the electron, carrying the same mass but a positive charge. When a positron and electron meet, they can annihilate and produce photons. Positrons are commonly observed in certain types of radioactive decay. .
Approximately how many times more massive is a neutron compared to an electron?
About 2000 times
About 1839 times
About 1 time
About 1000 times
A neutron's mass (1.675×10?²? kg) is roughly 1,839 times that of an electron (9.109×10?³¹ kg). This large difference underpins why electrons contribute minimally to atomic mass. Protons have a similar mass to neutrons but differ in charge. .
In the quantum mechanical model, what name is given to the region where there is a high probability of finding an electron?
Shell
Orbital
Nucleus
Cloud
In quantum mechanics, an orbital is a mathematical function that describes the region where there is a high probability of finding an electron. Orbitals have distinct shapes (s, p, d, f) and energy levels. This concept replaces the older Bohr model's fixed orbits. .
Which fundamental force is responsible for holding the atomic nucleus together?
Electromagnetic force
Gravitational force
Strong nuclear force
Weak nuclear force
The strong nuclear force is the fundamental interaction that binds protons and neutrons together in the nucleus. It overcomes the electromagnetic repulsion between positively charged protons at very short distances. This force is mediated by gluons between quarks. .
What two spin quantum numbers can an electron have in an atom?
1/2 and 3/2
+1 and -1
+1/2 and -1/2
0 and 1
Electrons in atoms have a spin quantum number of either +1/2 or -1/2, reflecting their intrinsic angular momentum. Paired electrons in the same orbital must have opposite spins to satisfy the Pauli exclusion principle. This property leads to magnetic effects in materials. .
What is the quark composition of a neutron?
Three strange quarks
One up quark and two down quarks
One down quark and two strange quarks
Two up quarks and one down quark
A neutron is composed of one up quark (charge +2/3e) and two down quarks (each - 1/3e), resulting in a net charge of zero. Quarks are bound together by gluons via the strong force. This combination differentiates a neutron from a proton. .
According to the Pauli exclusion principle, no two electrons in an atom can share the same set of what?
Orbitals
Quantum numbers
Spin states
Energy levels
The Pauli exclusion principle states that no two electrons in an atom can share the same set of four quantum numbers. This principle explains the structure of the periodic table and electron shell filling. It arises from the antisymmetric nature of fermion wavefunctions. .
Which principle states that the more precisely a particle's position is known, the less precisely its momentum can be known?
Heisenberg uncertainty principle
Boyle's law
Archimedes' principle
Pauli exclusion principle
Heisenberg's uncertainty principle asserts that the more precisely one knows a particle's position, the less precisely one can know its momentum, and vice versa. Mathematically, the product of these uncertainties has a lower bound. This principle is fundamental to quantum mechanics. .
Which of these particles is classified as a fermion rather than a boson?
Photon
Gluon
Electron
Higgs boson
Fermions are particles with half-integer spin that obey the Pauli exclusion principle, while bosons have integer spins and can occupy the same quantum state. An electron, with spin 1/2, is a classic example of a fermion. Photons, gluons, and the Higgs boson are bosons. .
What is the approximate radius of an atomic nucleus?
1×10?¹² meters
1×10?¹? meters
1×10?¹? meters
1×10?? meters
The approximate radius of an atomic nucleus is on the order of 1×10?¹? meters (1 femtometer). This size scales approximately as R ? R? A¹?³, where A is the mass number. By contrast, the atomic radius is around 1×10?¹? meters. .
The weak nuclear force is mediated by which bosons?
Photon
Graviton
W+, W?, and Z0 bosons
Gluon
The weak nuclear force is mediated by three gauge bosons: the W+, W?, and Z0 particles. These bosons are massive and responsible for processes like beta decay. Their discovery confirmed the electroweak theory. .
What concept describes particles exhibiting both wave and particle properties?
Quantum entanglement
Wave-particle duality
Complementarity
Superposition
Wave-particle duality describes how quantum objects such as electrons and photons exhibit both wave-like and particle-like properties. This duality is a core concept of quantum mechanics, demonstrated in experiments like the double-slit experiment. It challenges classical intuition about the nature of matter. .
Which equation is used to calculate the probability density of an electron's position according to quantum theory?
Maxwell's equations
Boltzmann equation
Navier - Stokes equation
Schrödinger equation
The Schrödinger equation is the fundamental equation of non-relativistic quantum mechanics that describes how the quantum state of a system evolves over time. Its solutions yield the wavefunctions whose squared magnitudes give probability densities. It is essential for predicting electron distributions in atoms. .
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Study Outcomes

  1. Identify subatomic particles and atomic regions -

    Recognize protons, neutrons, electrons, and the spaces they occupy within the atom. You'll master the primary structure components by pinpointing each element accurately.

  2. Differentiate particle characteristics -

    Distinguish between the mass, charge, and location of subatomic particles in various atomic models. This skill helps you apply precise descriptions during analysis.

  3. Apply knowledge in an atoms quiz -

    Engage with interactive questions to test your understanding of atomic structure. Instant feedback guides you toward correct answers and reinforces learning as you progress.

  4. Analyze incorrect responses -

    Use feedback to identify misconceptions about atom components and their functions. This reflection enhances retention and improves accuracy on subsequent quiz items.

  5. Evaluate your atom knowledge -

    Measure your proficiency in atom terminology and concepts through a structured quiz format. Track your progress to gain confidence in identifying subatomic particles or regions of the atom.

Cheat Sheet

  1. Fundamental Particle Properties -

    Protons carry a +1 charge and have a mass of ~1.0073 u, neutrons are neutral with ~1.0087 u, and electrons have a −1 charge and a negligible mass (~0.00055 u). Remember "PEN" (Proton, Electron, Neutron) to recall the three key particles. These definitions come straight from standard chemistry texts like those at MIT OpenCourseWare.

  2. Atomic and Mass Numbers -

    The atomic number (Z) equals the number of protons, while the mass number (A) equals protons plus neutrons (A = Z + N). For example, carbon-14 has Z = 6 and N = 8, giving A = 14. This formula is a staple in IUPAC recommendations and university general chemistry courses.

  3. Isotopes and Ions -

    Isotopes share Z but differ in N, affecting stability and mass; ions result when electrons are gained (anion) or lost (cation). For instance, Na❺ has 11 protons and 10 electrons, whereas Cl❻ has 17 protons and 18 electrons. Understanding these definitions is essential for nuclear chemistry, as covered in journals like the Journal of Chemical Education.

  4. Electron Configuration & Energy Levels -

    Electrons occupy quantized shells and subshells following the Aufbau principle, Pauli exclusion, and Hund's rule. A handy mnemonic is "1s², 2s², 2p❶, 3s²…" to build up configurations. These rules are detailed in quantum chemistry modules at institutions like Stanford University.

  5. Regions of the Atom -

    The atom consists mostly of empty space: a tiny, dense nucleus at the center surrounded by an electron cloud. The nucleus (radius ~10❻¹❵ m) houses protons/neutrons, while the electron cloud (up to ~10❻¹❰ m) defines chemical behavior. Modern physics sources such as CERN explain how this spatial separation shapes atomic interactions.

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