Periodic Table Quiz

13 – 28 Questions 11 min

This periodic table quiz focuses on element symbols, atomic numbers, group and period classification, and periodic trends. You will apply concepts like valence electrons, electronegativity patterns, and block notation to realistic chemistry questions. Strong practice for high school and college chemistry students, lab assistants, and science teachers who build general chemistry skills.

Start Quiz Explore related quizzes

Part 1 — Questions

Answer each question on paper. Do not turn the page until you are ready to check your work.

In a basic periodic table quiz, you are asked for the chemical symbol of sodium. Which symbol should you select?

The symbol for potassium on the periodic table is K.

True
False

Your teacher reminds the class that the periodic table is arranged in order of increasing atomic number. What does the atomic number of an element represent?

Number of protons
Sum of protons and neutrons
Number of electrons
Number of neutrons

A student says that elements in the same horizontal row of the periodic table usually have the same number of electron shells. What is the name for a horizontal row?

Family
Group
Period
Block

During a general knowledge periodic table quiz, you are asked which group contains very unreactive gases commonly used in lighting and shielding atmospheres. Which group is the best answer?

Group 2
Group 1
Group 18
Group 17

All metalloids are located in a single vertical group on the periodic table.

True
False

Select all that apply. In a periodic table practice session, you review the halogens. Which statements correctly describe elements of the halogen group?

A.They are located in group 17.
B.They are typically nonmetals.
C.They are all noble gases.
D.They tend to form ions with a 1− charge.

Select all that apply. A teacher asks where elements from group 1, such as lithium and sodium, are commonly used in everyday life.

A.Sodium in table salt.
B.Cesium as a major component of the air we breathe.
C.Francium in household light bulbs.
D.Lithium in rechargeable batteries.

You are told an unknown element has 7 valence electrons in its outer shell in the ground state. In a periodic table of elements quiz, which group would you assign this element to?

Group 14
Group 17
Group 1
Group 2

10.

You compare three alkali metals, lithium, sodium, and potassium. If you arrange them by decreasing atomic radius, which order is correct?

Na > K > Li
K > Na > Li
Li > Na > K
Na > Li > K

11.

A lab needs a metal that can form ions with several possible positive charges, such as +2 and +3, for use as a variable catalyst. From the periodic table, which category is most likely to supply such a metal?

Alkali metals
Noble gases
Alkaline earth metals
Transition metals

12.

In a safety briefing, your instructor reminds you that reactivity with water increases down group 1. For lithium, sodium, and potassium, which metal will react most vigorously with water?

Lithium
All equally reactive
Potassium
Sodium

13.

While reviewing a periodic table quiz, you read the statement: "Within a group, the shielding effect increases as you move down, which helps explain why first ionization energy generally decreases."

True
False

14.

Select all that apply. You are checking answers on an elements quiz about periodic trends. Which of the following comparisons are correct?

A.Magnesium atoms are larger than aluminum atoms.
B.Potassium has a higher first ionization energy than sodium.
C.Chlorine has a higher electronegativity than sulfur.
D.Oxygen atoms are larger than sulfur atoms.

15.

Select all that apply. In a periodic table practice session, you check noble gas shorthand electron configurations for several main group elements. Which configurations are written correctly?

A.[Ne] 3s² 3p⁵ for chlorine
B.[Ne] 3s² for magnesium
C.[He] 2s² 2p⁶ 3s¹ for sodium
D.[Ar] 4s¹ for potassium
E.[He] 2s² 2p⁵ for oxygen

16.

You are arranging samples of four nonmetal elements by increasing atomic number for a classroom display. Put these elements in the correct order from lowest to highest atomic number.

Put these in the correct order (write 1–4 beside each):

____Ne
____C
____F
____O

17.

An element has valence electrons that occupy a 3d subshell while also having electrons in a 4s subshell. In a periodic table test, which block should you say this element belongs to?

p-block
f-block
d-block
s-block

18.

On a blank periodic table, you mark the position of an element in period 3 and group 2 (IUPAC numbering). Which element are you most likely marking?

Magnesium
Sodium
Aluminum
Silicon

19.

You are ranking several nonmetals for their ability to attract bonding electrons in a molecule. Given carbon, nitrogen, oxygen, and fluorine, which element should you predict has the highest electronegativity?

Fluorine
Oxygen
Carbon
Nitrogen

20.

Select all that apply. During a more advanced periodic table test, you are given electron configurations and asked which correspond to elements in the d-block of the periodic table.

A.[Xe] 6s² 4f¹⁴ 5d¹⁰
B.[Ar] 4s² 3d¹⁰
C.[Ne] 3s² 3p⁴
D.[Ar] 4s¹
E.[Ar] 4s² 3d⁶

21.

A chemist mentions a classic diagonal relationship in the periodic table, where a light alkali metal shares several properties with an alkaline earth metal one period down and one group to the right. Which pair is a standard example of this effect?

Rb and Sr
K and Mg
Na and Ca
Li and Mg

22.

A classmate claims that across a period from left to right, atomic radius usually increases because additional protons are added to the nucleus.

True
False

Part 2 — Answer key

Compare your answers after you have finished Part 1.

In a basic periodic table quiz, you are asked for the chemical symbol of sodium. Which symbol should you select?
Na
The symbol for potassium on the periodic table is K.
True
Your teacher reminds the class that the periodic table is arranged in order of increasing atomic number. What does the atomic number of an element represent?
Number of protons
A student says that elements in the same horizontal row of the periodic table usually have the same number of electron shells. What is the name for a horizontal row?
Period
During a general knowledge periodic table quiz, you are asked which group contains very unreactive gases commonly used in lighting and shielding atmospheres. Which group is the best answer?
Group 18
All metalloids are located in a single vertical group on the periodic table.
False
Select all that apply. In a periodic table practice session, you review the halogens. Which statements correctly describe elements of the halogen group?
They are located in group 17.; They are typically nonmetals.; They tend to form ions with a 1− charge.
Select all that apply. A teacher asks where elements from group 1, such as lithium and sodium, are commonly used in everyday life.
Sodium in table salt.; Lithium in rechargeable batteries.
You are told an unknown element has 7 valence electrons in its outer shell in the ground state. In a periodic table of elements quiz, which group would you assign this element to?
Group 17
You compare three alkali metals, lithium, sodium, and potassium. If you arrange them by decreasing atomic radius, which order is correct?
K > Na > Li
A lab needs a metal that can form ions with several possible positive charges, such as +2 and +3, for use as a variable catalyst. From the periodic table, which category is most likely to supply such a metal?
Transition metals
In a safety briefing, your instructor reminds you that reactivity with water increases down group 1. For lithium, sodium, and potassium, which metal will react most vigorously with water?
Potassium
While reviewing a periodic table quiz, you read the statement: "Within a group, the shielding effect increases as you move down, which helps explain why first ionization energy generally decreases."
True
Select all that apply. You are checking answers on an elements quiz about periodic trends. Which of the following comparisons are correct?
Magnesium atoms are larger than aluminum atoms.; Chlorine has a higher electronegativity than sulfur.
Select all that apply. In a periodic table practice session, you check noble gas shorthand electron configurations for several main group elements. Which configurations are written correctly?
[Ne] 3s² 3p⁵ for chlorine; [Ne] 3s² for magnesium; [Ar] 4s¹ for potassium
You are arranging samples of four nonmetal elements by increasing atomic number for a classroom display. Put these elements in the correct order from lowest to highest atomic number.
Correct order: C → O → F → Ne
An element has valence electrons that occupy a 3d subshell while also having electrons in a 4s subshell. In a periodic table test, which block should you say this element belongs to?
d-block
On a blank periodic table, you mark the position of an element in period 3 and group 2 (IUPAC numbering). Which element are you most likely marking?
Magnesium
You are ranking several nonmetals for their ability to attract bonding electrons in a molecule. Given carbon, nitrogen, oxygen, and fluorine, which element should you predict has the highest electronegativity?
Fluorine
Select all that apply. During a more advanced periodic table test, you are given electron configurations and asked which correspond to elements in the d-block of the periodic table.
[Xe] 6s² 4f¹⁴ 5d¹⁰; [Ar] 4s² 3d¹⁰; [Ar] 4s² 3d⁶
A chemist mentions a classic diagonal relationship in the periodic table, where a light alkali metal shares several properties with an alkaline earth metal one period down and one group to the right. Which pair is a standard example of this effect?
Li and Mg
A classmate claims that across a period from left to right, atomic radius usually increases because additional protons are added to the nucleus.
False

1In a basic periodic table quiz, you are asked for the chemical symbol of sodium. Which symbol should you select?

2The symbol for potassium on the periodic table is K.

True / False

3Your teacher reminds the class that the periodic table is arranged in order of increasing atomic number. What does the atomic number of an element represent?

4A student says that elements in the same horizontal row of the periodic table usually have the same number of electron shells. What is the name for a horizontal row?

5During a general knowledge periodic table quiz, you are asked which group contains very unreactive gases commonly used in lighting and shielding atmospheres. Which group is the best answer?

6All metalloids are located in a single vertical group on the periodic table.

True / False

7Select all that apply. In a periodic table practice session, you review the halogens. Which statements correctly describe elements of the halogen group?

Select all that apply

8Select all that apply. A teacher asks where elements from group 1, such as lithium and sodium, are commonly used in everyday life.

Select all that apply

9You are told an unknown element has 7 valence electrons in its outer shell in the ground state. In a periodic table of elements quiz, which group would you assign this element to?

10You compare three alkali metals, lithium, sodium, and potassium. If you arrange them by decreasing atomic radius, which order is correct?

11A lab needs a metal that can form ions with several possible positive charges, such as +2 and +3, for use as a variable catalyst. From the periodic table, which category is most likely to supply such a metal?

12In a safety briefing, your instructor reminds you that reactivity with water increases down group 1. For lithium, sodium, and potassium, which metal will react most vigorously with water?

13While reviewing a periodic table quiz, you read the statement: "Within a group, the shielding effect increases as you move down, which helps explain why first ionization energy generally decreases."

True / False

14Select all that apply. You are checking answers on an elements quiz about periodic trends. Which of the following comparisons are correct?

Select all that apply

15Select all that apply. In a periodic table practice session, you check noble gas shorthand electron configurations for several main group elements. Which configurations are written correctly?

Select all that apply

16You are arranging samples of four nonmetal elements by increasing atomic number for a classroom display. Put these elements in the correct order from lowest to highest atomic number.

Put in order

1Ne

17An element has valence electrons that occupy a 3d subshell while also having electrons in a 4s subshell. In a periodic table test, which block should you say this element belongs to?

18On a blank periodic table, you mark the position of an element in period 3 and group 2 (IUPAC numbering). Which element are you most likely marking?

19You are ranking several nonmetals for their ability to attract bonding electrons in a molecule. Given carbon, nitrogen, oxygen, and fluorine, which element should you predict has the highest electronegativity?

20Select all that apply. During a more advanced periodic table test, you are given electron configurations and asked which correspond to elements in the d-block of the periodic table.

Select all that apply

21A chemist mentions a classic diagonal relationship in the periodic table, where a light alkali metal shares several properties with an alkaline earth metal one period down and one group to the right. Which pair is a standard example of this effect?

22A classmate claims that across a period from left to right, atomic radius usually increases because additional protons are added to the nucleus.

True / False

Frequent Errors on Periodic Table Quiz Questions

Confusing Groups and Periods

Many learners mix up vertical groups with horizontal periods. This leads to wrong answers about valence electrons or reactivity. Remember that groups run top to bottom and contain elements with similar outer electron configurations. Periods run left to right and reflect increasing principal energy level.

Ignoring Atomic Number Ordering

Some students still think the periodic table is arranged by atomic mass. Modern tables are ordered by atomic number. If you forget this, you may miss questions about why argon comes before potassium or why isotopes do not change an element's position.

Misreading Element Symbols

Common trap questions use similar symbols, such as Co versus C or Mg versus Mn. A quick but unfocused scan of the table can cause mistakes. Train yourself to read every symbol completely and connect it to both name and atomic number.

Overgeneralizing Periodic Trends

Students often memorize that atomic radius decreases across a period or that ionization energy increases, then forget the small exceptions. Transition metals and noble gases can behave differently from simple patterns. Always think about nuclear charge and shielding, not just a memorized rule.

Forgetting Charge and Group Relationships

Questions about common ion charges catch many test takers. Group 1 metals typically form +1 ions and group 17 nonmetals typically form -1 ions. Learners who do not connect group number to valence electrons struggle with formula prediction and bonding questions that reference the periodic table.

Periodic Table of Elements Quick Reference Sheet

Using This Periodic Table Practice Sheet

Use this sheet while you prepare for periodic table quiz questions on symbols, atomic numbers, and trends. You can print this page or save it as a PDF for quick revision before chemistry tests or lab work.

Table Layout Essentials

Periods: 7 horizontal rows. Period number equals the highest occupied main energy level in the ground state.
Groups: 18 vertical columns. Elements in the same group share similar valence electron patterns and chemical behavior.
Blocks: s-block (groups 1, 2 and He), p-block (groups 13, 18), d-block (transition metals), f-block (lanthanides and actinides).

Key Element Families

Alkali metals (group 1, except H): very reactive, 1 valence electron, form +1 ions.
Alkaline earth metals (group 2): 2 valence electrons, form +2 ions, fairly reactive.
Halogens (group 17): 7 valence electrons, highly reactive nonmetals, form -1 ions.
Noble gases (group 18): full valence shells, very low reactivity, gases at room temperature.

Core Periodic Trends

Atomic radius: decreases across a period from left to right. Increases down a group.
Ionization energy: increases across a period. Decreases down a group.
Electronegativity: generally increases across a period and decreases down a group. Fluorine is the most electronegative element.
Metallic character: strongest at the bottom left of the table. Weakest at the top right.

High-Yield Element Facts

H: atomic number 1, nonmetal, often grouped with alkali metals for convenience.
C: forms four bonds, central to organic chemistry.
O: strongly electronegative, essential for combustion and respiration.
Fe, Cu, Zn: common transition metals with multiple oxidation states.
U, Pu: actinides, radioactive, important in nuclear chemistry contexts.

Worked Periodic Table Quiz Style Examples

Example 1: Identifying an Element from Clues

Question: An element is in period 3 and group 16. It has 6 valence electrons and forms a -2 ion. Which element is it, and is it a metal or nonmetal?

Find period 3 on the table. The row starts at Na and ends at Ar.
Locate group 16 within that period. Reading left to right, group 16 in period 3 is S.
Confirm valence electrons. Group 16 elements have 6 valence electrons, so sulfur matches.
Check typical ion charge. Group 16 nonmetals often form -2 ions, again consistent with sulfur.
Answer: Sulfur, a nonmetal in the p-block.

Example 2: Predicting Relative Atomic Radius

Question: Which atom has the largest atomic radius, Li, C, or F?

All three elements lie in period 2. This means same principal energy level but different nuclear charge.
Across a period from left to right, nuclear charge increases while shielding stays similar.
Stronger nuclear attraction pulls electrons closer, so radius decreases across the period.
Li is leftmost, then C, then F on the right.
Answer: Li has the largest atomic radius. F has the smallest.

Example 3: Determining Metal, Metalloid, or Nonmetal

Question: An element has atomic number 14. Classify it as metal, metalloid, or nonmetal.

Atomic number 14 corresponds to silicon.
Silicon lies along the staircase dividing metals and nonmetals in the p-block.
Elements along this line often show intermediate properties.
Answer: Silicon is a metalloid with both metallic and nonmetallic behavior.

Periodic Table Quiz Study FAQ

What prior knowledge helps most on this periodic table quiz?

You should already know basic atomic structure, including protons, neutrons, electrons, and the idea of atomic number. Familiarity with common families such as alkali metals, halogens, and noble gases helps. You should also recognize the general layout of groups, periods, and the s, p, d, and f blocks.

How does this quiz differ from a simple elements name test?

This quiz goes beyond matching names and symbols. Questions ask you to infer properties from positions on the table, compare periodic trends, and predict ion charges or bonding patterns. You practice reasoning with the table as a problem solving tool instead of treating it as a static chart to memorize.

Which periodic trends are most likely to appear?

You will often see questions on atomic radius, ionization energy, electronegativity, and metallic character. Expect comparisons such as which element has the higher ionization energy or which atom forms a larger ion. Many items test your ability to apply up down and left right reasoning across the table.

How should I use the periodic table during practice?

Keep a printed or digital periodic table beside you. For each question, actively point to the relevant group and period instead of guessing from memory. Mark families, blocks, and common ion charges as you go. This builds a mental map that transfers well to exams where a standard table is provided.

What topics should I review if my quiz score is low?

Identify which items you missed. If they cluster around symbols, review the first twenty elements. If you miss trend questions, focus on atomic radius, ionization energy, and electronegativity patterns. If charges and formulas are weak, study how group number connects to typical ion charge for main group elements.