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Quizzes > Science

Periodic Table Practice: Atoms and Elements Quiz

Quick atoms and elements quiz with instant results and clear feedback.

Editorial: Review CompletedCreated By: Edward BellUpdated Aug 27, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper-art depiction of colorful periodic table tiles and atom models on dark blue background promoting free practice quiz

This periodic table practice quiz helps you review atoms, elements, groups, and trends in minutes, with instant results. Check key facts like valence electrons, electron configurations, and atomic number vs. mass. Want more practice? Try our elements practice quiz, take a quick chemical symbol quiz, or build recall with a common elements quiz.

What does the atomic number of an element represent?
The total number of neutrons
The number of protons in the nucleus
The combined number of protons and neutrons
The total number of electrons only
The atomic number is defined as the number of protons in an atom's nucleus, which determines the element's identity. All atoms of a given element share the same atomic number. Neutrons and electrons can vary in isotopes and ions, but the atomic number remains fixed. .
Which symbol represents the element gold?
Go
Au
Ag
Gd
Gold's chemical symbol is Au, derived from its Latin name aurum. Silver is Ag (argentum), Gd is gadolinium, and Go is not an element symbol. These symbols are standardized by IUPAC. .
Which of the following elements is a noble gas at room temperature?
Oxygen
Chlorine
Helium
Nitrogen
Helium is a noble gas located in Group 18 and exists as a monatomic, inert gas at room temperature. Oxygen and nitrogen are diatomic gases but are not noble gases. Chlorine is a diatomic gas but is a halogen. .
In which period of the periodic table is the element calcium located?
Period 3
Period 5
Period 4
Period 2
Calcium (atomic number 20) sits in the fourth row (period) of the periodic table. Periods correspond to the highest occupied principal energy level. Elements 19 to 36 occupy period 4. .
Which group of the periodic table contains the alkali metals?
Group 18
Group 1
Group 17
Group 2
Alkali metals occupy Group 1 and include elements like lithium, sodium, and potassium. They have a single valence electron which makes them highly reactive. Group 2 are alkaline earth metals, Group 17 are halogens, and Group 18 are noble gases. .
How many valence electrons does carbon have?
4
8
2
6
Carbon is in Group 14 and has four electrons in its outermost shell (valence electrons). This tetravalency allows carbon to form up to four covalent bonds. Valence electrons are crucial in chemical bonding and reactivity. .
What is the standard state of bromine at room temperature?
Solid
Plasma
Gas
Liquid
Bromine is unique among nonmetal elements as it is a reddish-brown liquid at room temperature. Most nonmetals are gases or solids under standard conditions. Bromine's volatility contributes to its distinct vapor pressure. .
Which trend describes the change in atomic radius across a period from left to right?
It remains constant
It increases
It fluctuates randomly
It decreases
As you move from left to right across a period, protons are added to the nucleus, increasing effective nuclear charge. This pulls electrons closer and reduces atomic radius. Electron shielding does not increase enough to offset this effect. .
Which of the following has the highest electronegativity?
Fluorine
Nitrogen
Oxygen
Chlorine
Fluorine is the most electronegative element, with an electronegativity value of 3.98 on the Pauling scale. Its small atomic radius and high effective nuclear charge attract bonding electrons strongly. Oxygen and nitrogen follow, but are lower than fluorine. .
What is the general electron configuration for most transition metals?
ns¹ np?
(n-1)d¹ - ?? ns²
ns² np¹ - ?
(n-1)d¹? ns¹
Transition metals fill the (n-1)d orbitals after the ns subshell, giving a general configuration of (n-1)d¹ - ?? ns². This accounts for the variability in oxidation states and metallic behavior. p-block elements follow ns² np¹ - ? configurations. .
Which group is known for forming anions by gaining exactly one electron?
Group 2
Group 17
Group 18
Group 1
The halogens in Group 17 commonly gain one electron to achieve a full valence shell, forming monovalent anions (X - ). Group 1 elements lose one electron to form cations, Group 2 lose two, and Group 18 are already inert. .
The elements in the lanthanide series are found in which block of the periodic table?
d-block
f-block
p-block
s-block
Lanthanides occupy the f-block, filling the 4f orbitals between lanthanum and lutetium. They are often shown below the main body of the periodic table. d-block contains transition metals, p-block contains nonmetals and metalloids, s-block contains alkali and alkaline earth metals. .
Which of these elements is a halogen?
Calcium
Magnesium
Neon
Bromine
Bromine is one of the four common halogens (Group 17), along with fluorine, chlorine, and iodine. Magnesium is an alkaline earth metal, neon is a noble gas, and calcium is also an alkaline earth metal. Halogens are highly reactive nonmetals. .
Which element has the electron configuration [Ne] 3s¹?
Potassium
Lithium
Magnesium
Sodium
Sodium, with atomic number 11, has the ground-state electron configuration [Ne] 3s¹. Potassium is [Ar] 4s¹, lithium is [He] 2s¹, and magnesium is [Ne] 3s². Noble gas shorthand configurations simplify notation. .
Why is helium placed in group 18 despite having only two valence electrons?
It is monatomic under standard conditions
It has the highest ionization energy
It has a full first electron shell
It has one proton more than hydrogen
Helium's 1s² configuration fills its first shell, making it chemically inert like other noble gases. Group 18 elements share full valence shells and low reactivity. Its placement is based on electron configuration rather than group number patterns. .
What is the term for the net positive charge experienced by a valence electron in a multielectron atom, and how does it trend across a period?
Electron affinity; varies randomly
Shielding effect; decreases left to right
Ionization potential; remains constant
Effective nuclear charge; increases left to right
Effective nuclear charge (Zeff) is the net positive pull felt by an electron after accounting for shielding by inner electrons. Zeff increases across a period because protons are added while shielding remains similar. This trend influences atomic radius and ionization energy. .
Which ion has a larger ionic radius compared to its neutral atom?
Cl?
Ar
K?
Na?
When chlorine gains an electron to become Cl?, the added electron increases electron - electron repulsion, expanding its radius. In contrast, cations like Na? and K? lose electrons and shrink. Argon is neutral. .
According to Fajan's rules, which cation-anion pair is likely to exhibit the most covalent character?
NaCl
CaF?
BeS
MgO
Fajan's rules state that small, highly charged cations and large anions increase polarization and covalent character. Be²? is small and highly charged, and S²? is relatively large. NaCl, MgO, and CaF? are more ionic. .
Which explanation best describes the diagonal relationship in the periodic table?
Same valence electron configuration
Placement in the same block
Similar ionic sizes and charge densities among diagonal elements
Identical atomic numbers
Diagonal relationships arise because certain pairs (e.g., Li - Mg, Be - Al) have similar ionic sizes and polarizing power. They fall into adjacent groups and periods, balancing size increase with charge. This yields similar chemistry despite different group placements. .
Which scientist's work led to the modern definition of the atomic number?
Henry Moseley
J.J. Thomson
John Dalton
Dmitri Mendeleev
Henry Moseley used X-ray spectra to show that each element's characteristic X-ray frequency correlates with its nuclear charge, leading to atomic numbers. Mendeleev had ordered elements by atomic weight, while Dalton and Thomson proposed early atomic theories. Moseley's work firmly established atomic number. .
Which of the following describes the trend in first ionization energy down a group?
It remains constant
It decreases
It increases
It fluctuates randomly
Down a group, atomic radius increases and outer electrons are farther from the nucleus, reducing effective attraction. Increased shielding by inner shells further lowers ionization energy. Thus, first ionization energy decreases. .
Which element has a higher electron affinity: chlorine or bromine?
Bromine
Data is insufficient
Chlorine
They are the same
Chlorine has a higher electron affinity (about - 349 kJ/mol) than bromine (about - 325 kJ/mol) because its smaller size allows a stronger attraction for an added electron. Electron affinity generally decreases down a group. .
How many neutrons are in the most abundant isotope of oxygen (oxygen-16)?
6
8
10
16
Oxygen-16 has an atomic number of 8 (protons) and a mass number of 16, so the number of neutrons is 16 - 8 = 8. It is the most abundant oxygen isotope. Mass number equals protons plus neutrons. .
Given two isotopes of carbon, C-12 (98.9%) and C-14 (1.1%), what is the average atomic mass of carbon?
12.100
12.014
12.011
13.003
Average atomic mass = (0.989 × 12.000) + (0.011 × 14.000) = 11.868 + 0.154 = 12.022 (rounded to 12.011 by IUPAC standards). Isotopic weighting reflects natural abundances. Precise atomic masses account for binding energy differences. .
Why is there a drop in electron affinity from group 2 to group 13 elements?
Because of an unexpected increase in atomic radius only
Because shielding dramatically decreases
Due to a sudden decrease in ionization energy
Group 13 begins filling the p-orbital, causing extra electron - electron repulsion
Electron affinity drops from group 2 to 13 because group 13 adds the first p-electron into a new subshell (p-orbital), which experiences repulsion from its paired s-electrons. This repulsion lowers the energy release on adding an extra electron. Atomic radius and shielding changes are secondary. .
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Study Outcomes

  1. Analyze Atomic Structure -

    Break down the roles of protons, neutrons, and electrons to understand how atomic structure defines each element's identity.

  2. Compare Group Characteristics -

    Examine why atoms of elements in the same group have the same characteristics by exploring their valence electron configurations and periodic trends.

  3. Identify True Statements about Elements -

    Evaluate multiple-choice scenarios to determine which of the following is true about elements and solidify your conceptual understanding.

  4. Differentiate Atoms and Elements -

    Clarify whether atoms and elements are the same by comparing their definitions, structures, and roles in chemical behavior.

  5. Interpret Periodic Trends -

    Investigate how properties like atomic radius, ionization energy, and electronegativity vary across periods and down groups.

  6. Apply Knowledge in a Periodic Table Practice -

    Engage in a targeted test on atoms and elements to reinforce learning and boost confidence through hands-on periodic table practice.

Cheat Sheet

  1. Element vs Atom Distinction -

    In periodic table practice, an element is a pure substance composed of one type of atom, but an atom is the smallest unit that retains chemical properties. Understanding this answers which of the following is true about elements versus atoms: they are related but not identical. The element's identity is defined by its atomic number, while atoms are the building blocks of all matter.

  2. Atomic Number and Mass Number -

    The atomic number (Z) equals the number of protons and defines each element's unique identity, so two atoms with the same Z are the same element. The mass number (A) is the sum of protons and neutrons, given by A = Z + N, which you'll use to compare isotopes. This formula is foundational in any test on atoms and isotopic calculations.

  3. Electron Configuration & Periodic Position -

    Electron configurations show how electrons fill shells and dictate an element's spot in the table - for example, sodium is [Ne] 3s¹. Using the Aufbau mnemonic "1s² 2s² 2p❶ 3s²…" helps you predict configurations quickly. Mastering this makes periodic table practice both efficient and satisfying.

  4. Key Periodic Trends -

    Across a period, atomic radius decreases while ionization energy and electronegativity (Pauling scale) increase; for instance, fluorine (4.0) is more electronegative than lithium (0.98). These trends help you predict reactivity and bonding types in any test on atoms or compounds. Remember: "Big Atoms Lose Electrons Easily" can help recall radius vs. ionization energy changes.

  5. Group Similarity Trick -

    Atoms of elements in the same group have the same number of valence electrons, which drives similar chemical behavior - for example, all alkali metals (Li, Na, K) have one valence electron. Use the mnemonic "Love Nasty Kittens" to remember Li, Na, K for Group 1. Recognizing that atoms of elements in the same group have the same valence count boosts your confidence in predicting reactivity.

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