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Quizzes > Science > Chemistry

Take the Periodic Table Quiz: Test Atomic Structure Skills

Dive into our Atomic Structure Quiz & Master the Periodic Table

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art periodic table atoms molecules and lab glassware on sky blue background for free chemistry quiz challenge

Calling all aspiring chemists and trivia buffs: it's time to put your skills to the test with our Ultimate Periodic Table Quiz: Atomic Structure Challenge. Dive into a periodic table quiz filled with periodic table questions on atomic numbers, group trends, and element properties. You'll tackle the elements quiz and explore subatomic mysteries via periodic table quiz or prove your mastery with the in-depth atomic structure quiz . Ideal for students prepping for exams or trivia fans, this challenge sharpens your knowledge through chemistry trivia questions in minutes. See your score instantly and share with peers - click Start Quiz and embrace the atomic adventure!

What is the atomic number of Hydrogen?
1
2
6
0
The atomic number equals the number of protons in an element; hydrogen has one proton in its nucleus, so its atomic number is 1. This places hydrogen at the top of the periodic table. The atomic number defines an element's identity. More on atomic numbers
Which element has the chemical symbol "O"?
Oxygen
Gold
Osmium
Oganesson
The symbol O designates oxygen, which is atomic number 8. Osmium uses Os, and Oganesson is Og. Gold is Au. Learn more about Oxygen
How many protons does carbon have?
6
8
4
12
Carbon has atomic number 6, which equals its number of protons. This defines its position in the periodic table. The atomic mass of carbon-12 is 12 amu, but that includes neutrons as well. Carbon details
What is the charge of an electron?
-1
+1
0
-2
An electron carries a fundamental charge of negative one elementary unit. Protons carry +1 and neutrons are neutral. This charge balance governs atomic structure. Electron charge info
Which of these is a noble gas?
Helium
Oxygen
Nitrogen
Fluorine
Helium is in group 18 of the periodic table, making it a noble gas with a full valence shell. Noble gases are inert due to their complete electron configuration. Others like oxygen and fluorine are highly reactive. Group 18 elements
Which element has atomic number 6?
Carbon
Nitrogen
Oxygen
Boron
Atomic number 6 corresponds to carbon. The atomic number increases by one for each element going across the table. Carbon is the backbone of organic chemistry. Carbon on Ptable
What term describes a horizontal row in the periodic table?
Period
Group
Series
Block
A horizontal row in the periodic table is called a period. Elements in the same period have the same number of electron shells. Vertical columns are known as groups. About periods
What is the smallest unit of an element that retains its chemical properties?
Atom
Molecule
Ion
Proton
An atom is the smallest unit of an element that maintains its chemical identity and properties. Molecules are combinations of atoms. Ions are charged atoms or groups of atoms. Atoms vs molecules
Which element is represented by the symbol "Na"?
Sodium
Nickel
Neon
Nitrogen
Na is the chemical symbol for sodium, derived from its Latin name 'natrium.' It is an alkali metal in group 1. Nickel is Ni and nitrogen is N. Sodium details
What is the electron configuration of Neon?
1s2 2s2 2p6
1s2 2s2 2p5
1s2 2s2 2p4
1s2 2s1 2p6
Neon has 10 electrons, which fill the 1s, 2s, and 2p orbitals: 1s˛ 2s˛ 2p?. This gives a noble gas configuration with a full valence shell. A full shell makes neon chemically inert. Electron configuration
Which element is the most electronegative?
Fluorine
Oxygen
Chlorine
Nitrogen
Fluorine has the highest electronegativity value (3.98 on the Pauling scale). It strongly attracts electrons in a bond. Oxygen and chlorine follow fluorine on the periodic table. Electronegativity trends
Magnesium belongs to which block of the periodic table?
s-block
p-block
d-block
f-block
Magnesium is in group 2 and has its valence electrons in an s orbital (3s˛), placing it in the s-block. The p-block starts at group 13. Transition metals occupy the d-block. Periodic table blocks
Which periodic trend generally increases across a period from left to right?
Electronegativity
Atomic radius
Metallic character
Atomic mass
Electronegativity increases across a period due to increasing nuclear charge attracting electrons more strongly. Atomic radius decreases instead. Metallic character diminishes, and atomic mass rises steadily. Periodic trends
What is the approximate atomic mass of the carbon-12 isotope?
12.01 amu
12.1 amu
12.5 amu
11.01 amu
The atomic mass of carbon-12 is defined as exactly 12 amu, but natural carbon's standard atomic weight is about 12.01 due to minor isotopic contributions. This value appears on the periodic table. NIST data
Which element has three valence electrons?
Aluminum
Magnesium
Silicon
Phosphorus
Aluminum is in group 13 and thus has three electrons in its outermost shell. Magnesium in group 2 has two, silicon in group 14 has four, and phosphorus in group 15 has five. Group numbers
What is the ground-state electron configuration of Iron (Fe)?
[Ar] 4s2 3d6
[Ar] 4s1 3d7
[Kr] 4d6 5s2
[Ar] 4s2 3d5
Iron has 26 electrons, filling up to argon core then 4s2 then 3d6. The 4s orbital fills before 3d in the ground state. Electron configurations
Which element has the electron configuration [Ne] 3s2?
Magnesium
Sodium
Aluminum
Silicon
After neon, which has 10 electrons, magnesium adds two electrons in the 3s orbital, giving [Ne]3s˛. Sodium is [Ne]3są, aluminum is [Ne]3s˛3pą, and silicon is [Ne]3s˛3p˛. Configurations
What is the common name for the elements in group 1 of the periodic table?
Alkali metals
Alkaline earth metals
Halogens
Noble gases
Group 1 elements are called alkali metals because they form alkaline hydroxides in water. The alkaline earth metals are group 2. Halogens are in group 17 and noble gases in group 18. Alkali metals info
Which element has the highest first ionization energy in period 2?
Neon
Fluorine
Oxygen
Nitrogen
Ionization energy generally increases across a period due to greater nuclear charge; neon, being a noble gas, has the highest first ionization energy in period 2. Fluorine is next but still lower than neon. Ionization energies
How does effective nuclear charge change across a period?
It increases
It decreases
It stays constant
It fluctuates irregularly
Effective nuclear charge increases across a period as protons are added to the nucleus without significant additional shielding. This draws electrons closer and affects trends like atomic radius. Zeff concept
Which isotope of hydrogen contains one proton and one neutron?
Deuterium
Protium
Tritium
Hydrogen-4
Deuterium is the hydrogen isotope with one proton and one neutron (mass number 2). Protium has no neutrons, and tritium has two neutrons. Hydrogen isotopes
How many unpaired electrons are in the ground state of an oxygen atom?
2
1
4
0
Oxygen (1s˛ 2s˛ 2p?) has two unpaired electrons in its 2p orbitals according to Hund’s rule. The other two 2p electrons pair up. Orbital filling
What is the approximate electron affinity of chlorine?
-349 kJ/mol
-125 kJ/mol
-75 kJ/mol
0 kJ/mol
Chlorine has one of the highest electron affinities, about -349 kJ/mol, indicating strong attraction for an added electron. Negative values show energy release. Electron affinity data
Which group of elements is known as the transition metals?
Groups 3-12
Groups 1-2
Groups 13-18
Groups 2-16
Transition metals occupy the d-block, which corresponds to groups 3 through 12. They often exhibit multiple oxidation states and form colored compounds. Group definitions
What is the oxidation state of manganese in KMnO4?
+7
+2
+4
+6
In KMnO?, oxygen is -2 (×4 = -8) and potassium is +1, so Mn must be +7 to balance the charges (+1 + Mn -8 = 0). Permanganate ion has manganese in its highest common oxidation state. Permanganate
Which element exhibits allotropy?
Carbon
Sodium
Chlorine
Argon
Carbon shows allotropy with multiple forms such as diamond, graphite, and graphene. Allotropy refers to the existence of an element in more than one structural form. Noble gases and alkali metals typically do not exhibit allotropy. Allotropy explained
Which quantum number indicates the shape of an orbital?
Angular momentum quantum number (l)
Principal quantum number (n)
Magnetic quantum number (m?)
Spin quantum number (m?)
The angular momentum quantum number, l, defines the shape of an orbital (s, p, d, f, etc.). The principal quantum number n indicates energy level, m? gives orientation, and m? describes electron spin. Quantum numbers
Which element violates the Aufbau principle in its ground-state electron configuration by having [Ar] 4s1 3d5?
Chromium (Cr)
Vanadium (V)
Iron (Fe)
Cobalt (Co)
Chromium is an exception to the Aufbau filling order: it promotes one 4s electron to the 3d subshell to achieve a half-filled d? configuration, which is more stable. Other nearby elements follow the expected order. Configuration exceptions
How many unique orbitals are present in the n = 4 shell?
16
10
18
32
For n=4, l can be 0 (1 orbital), 1 (3 orbitals), 2 (5 orbitals), and 3 (7 orbitals), for a total of 1+3+5+7 = 16 orbitals. Each orbital can hold up to two electrons. Orbital counts
Which oxide of vanadium is most stable under standard conditions?
V2O5
VO
V2O3
VO2
V2O5 (vanadium pentoxide) is the most stable and common oxide of vanadium, featuring vanadium in the +5 oxidation state. Other oxides are less stable in air and temperature conditions. Vanadium pentoxide
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Study Outcomes

  1. Understand Atomic Structure Principles -

    Gain a clear grasp of protons, neutrons, and electrons and how they form the foundation of all periodic table questions.

  2. Identify Element Properties -

    Learn to recognize key element attributes like atomic number, mass and chemical behavior across the periodic table quiz.

  3. Apply Electron Configuration Rules -

    Master the order of electron filling and orbital notation to solve atomic structure quiz challenges accurately.

  4. Analyze Periodic Trends -

    Explore patterns in electronegativity, atomic radius and ionization energy to predict element behavior.

  5. Recall Element Symbols and Numbers -

    Enhance your memory of chemical symbols and atomic numbers to answer elements quiz questions swiftly.

  6. Evaluate Quiz Performance -

    Use your scores to identify strengths and pinpoint areas for further chemistry study and improvement.

Cheat Sheet

  1. Atomic Number vs. Mass Number -

    Atomic number (Z) represents the number of protons and defines each element's identity, while mass number (A) equals protons plus neutrons. For example, carbon-12 has Z=6 and A=12, meaning six neutrons (A - Z=6). Mastering these basics from NIST's database helps you quickly interpret periodic table entries.

  2. Electron Configuration & Aufbau Principle -

    Electrons fill orbitals in order of increasing energy following the Aufbau principle, Hund's rule, and the Pauli exclusion principle (e.g., 1s² 2s² 2p❶). A mnemonic like "1s, 2s, 2p, 3s, 3p…" can keep you on track. Resources like MIT OCW highlight how these rules predict chemical behavior and reactivity.

  3. Periodic Trends -

    Key trends across periods and down groups include atomic radius (decreases left to right, increases top to bottom), ionization energy (increases left to right), and electronegativity (Pauling scale). Remember the phrase "FINE: From left Increased, Nuclear pull Encourages electrons" to recall F (ionization energy) and EN trends. Data from ACS publications underpin these predictable patterns.

  4. Quantum Numbers & Orbital Shapes -

    Each electron's state is defined by four quantum numbers (n, â„“, mâ„“, ms), describing shell, subshell, orbital orientation, and spin. Visualizing s (spherical), p (dumbbell), and d (cloverleaf) orbitals in an online NIST chart helps cement their shapes. This framework is crucial for understanding bonding and molecular geometry.

  5. Isotopes & Nuclear Stability -

    Isotopes are atoms of the same element with different neutron counts, affecting mass and stability (e.g., carbon-14 for radiocarbon dating). The neutron-to-proton ratio chart from IAEA shows why heavy nuclei require more neutrons to remain stable. Recognizing common isotopes deepens your grasp of radioactivity and atomic mass calculations.

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