Ionization energy is...

how much energy it takes to remove an electron from an atom

the energy required to add an electron to a specific atom

the energy required to shield the outer electrons from the nucleus

a measure of the ability of an atom to attract electrons

Metals have the largest -

atomic radius and electronegativity

electronegativity and ionization energy

ionization energy and atomic radius

Which statement correctly and completely identifies a trend?

Atomic radius decreases across a period and increases down a group.

Electronegativity decreases across a period and decreases down a group.

Ionization energy increases across a period and increases down a group.

Ionic radius increases across a period and increases down a group.

Atomic radius generally increases as we move __________.

down a group and from right to left across a period

up a group and from left to right across a period

down a group and from left to right across a period

up a group and from right to left across a period

Which statement correctly and completely identifies a trend?

Atomic radius decreases across a period and increases down a group.

Electronegativity decreases across a period and decreases down a group.

Ionization energy increases across a period and increases down a group.

Ionic radius increases across a period and increases down a group.

Atoms that have a high electronegativity, _______________.

hold on to their electrons more tightly.

give up their electrons more easily.

Ionization energy is...

how much energy it takes to remove an electron from an atom

the energy required to add an electron to a specific atom

the energy required to shield the outer electrons from the nucleus

a measure of the ability of an atom to attract electrons

Which statement correctly and completely identifies a trend?

Atomic radius decreases across a period and increases down a group.

Electronegativity decreases across a period and decreases down a group.

Ionization energy increases across a period and increases down a group.

Ionic radius increases across a period and increases down a group.

As you move across the periodic table from left to right, the atomic radius decreases. This is because -

the number of protons increases, so attraction to electrons increases

the number of energy levels increases

the number of electrons increases

Francium (Fr) has the lowest ionization energy in Group 1 because -

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

it has the smallest number of valence electrons

it has the greatest atomic mass

it has the greatest number of protons, so it attracts its electrons the strongest

the relative size of the atom's electron cloud

the relative size of the atom's nucleus

the energy required to shield the outer electrons from the nucleus

a measure of the ability of an atom to attract electrons

ionization energy, electronegativity and atomic radius

Authored by Richard Auka

Chemistry

9th - 12th Grade

NGSS covered

Used 573+ times

ionization energy, electronegativity and atomic radius

AI Actions

Add similar questions

Adjust reading levels

Convert to real-world scenario

Translate activity

More...

About

This quiz comprehensively covers periodic trends in chemistry, specifically focusing on three fundamental atomic properties: ionization energy, electronegativity, and atomic radius. Appropriate for grades 9-12, the questions assess students' understanding of how these properties change both across periods (left to right) and down groups (top to bottom) on the periodic table. Students need to master the underlying concepts of nuclear charge, electron shielding, and energy levels to successfully predict and explain these trends. The quiz requires students to apply knowledge of electron-nucleus interactions, understand how additional protons increase nuclear attraction while additional electron shells provide shielding, and recognize that electronegativity measures an atom's ability to attract electrons while ionization energy measures the energy required to remove them. Students must also demonstrate understanding of how atomic structure directly influences these measurable properties. Created by Richard Auka, a Chemistry teacher in the US who teaches grades 9-12. This quiz serves as an excellent tool for formative assessment, allowing teachers to gauge student mastery of periodic trends before moving to more complex bonding concepts. It works effectively as a review activity before unit exams, homework practice to reinforce classroom instruction, or a warm-up exercise to activate prior knowledge. Teachers can use this quiz to identify misconceptions about periodic trends and provide targeted feedback on areas where students struggle. The variety of question formats, from direct comparisons to trend explanations, supports differentiated instruction and helps students build confidence with these essential chemistry concepts. This assessment aligns with NGSS HS-PS1-1 and supports understanding of periodic properties that form the foundation for chemical bonding and molecular behavior.

Content View

Student View

55 questions

Show all answers

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Which of the following will have a larger radius than Zinc?

Gallium

Aluminum

Magnesium

Strontium

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Which of the following will have a higher electronegativity than arsenic (As)?

Carbon (C)

Neon (Ne)

Antimony (Sb)

Germanium (Ge)

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Which of the following will have a lower ionization energy than Scandium (Sc)?

Helium (He)

Titanium (Ti)

Calcium (Ca)

Magnesium (Mg)

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

decreases

increases

remains the same

none of the above

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

As you move down the periodic table atoms get bigger. This is because ____________.

The atoms have more mass.

The atoms have more protons.

The atoms have more energy levels

The atoms have more neutrons

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

As you move across the periodic table atoms tend to get smaller because, ______________.

the atoms have more mass.

the atoms have less mass

the atoms have more protons.

the atoms have less electrons.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Electronegativity is...

the ability of an atom to attract/ accept electrons

the ability of an atom to lose electrons

the energy required to remove an electron from a specific atom

how easy it is to make friends.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Access all questions and much more by creating a free account

Create resources

Host any resource

Get auto-graded reports

Continue with Google

Continue with Email

Continue with Classlink

Continue with Clever

or continue with

Microsoft

Apple

Others

Already have an account?

Similar Resources on Wayground

50 questions

Solutions & Solubility Questions

Quiz

•

9th Grade - University

50 questions

Chemistry Semester 1 Review & Exam

Quiz

•

10th Grade

55 questions

FINAL Physical Science FINAL Review

Quiz

•

9th - 12th Grade

60 questions

C5 C10 Metal Reactivity and Extraction

Quiz

•

9th - 12th Grade

50 questions

Chemistry Nomenclature

Quiz

•

11th - 12th Grade

59 questions

Electrons and Chemical Bonds

Quiz

•

9th - 12th Grade

52 questions

super honor

Quiz

•

9th - 12th Grade

57 questions

Chapter 5 Electrons

Quiz

•

10th - 12th Grade

Popular Resources on Wayground

15 questions

Fractions on a Number Line

Quiz

•

3rd Grade

20 questions

Equivalent Fractions

Quiz

•

3rd Grade

25 questions

Multiplication Facts

Quiz

•

5th Grade

29 questions

Alg. 1 Section 5.1 Coordinate Plane

Quiz

•

9th Grade

$fractions$

22 questions

fractions

Quiz

•

3rd Grade

11 questions

FOREST Effective communication

Lesson

•

20 questions

Main Idea and Details

Quiz

•

5th Grade

20 questions

Context Clues

Quiz

•

6th Grade

Discover more resources for Chemistry

22 questions

Unit 9 Gas Law Quiz

Quiz

•

10th Grade

10 questions

Exploring Types of Chemical Reactions

Interactive video

•

6th - 10th Grade

20 questions

Types of Chemical Reactions

Quiz

•

9th - 12th Grade

20 questions

Acids and Bases

Quiz

•

10th Grade

30 questions

Energy Review

Quiz

•

9th Grade

7 questions

GCSE Chemistry - Balancing Chemical Equations #4

Interactive video

•

9th - 10th Grade

20 questions

Chemistry: Classification of Matter

Quiz

•

10th Grade

40 questions

Unit 3 (Part 1) Chemical Equations & Reactions Review Game

Quiz

•

8th - 12th Grade

ionization energy, electronegativity and atomic radius

Which of the following will have a larger radius than Zinc?

Which of the following will have a higher electronegativity than arsenic (As)?

Which of the following will have a lower ionization energy than Scandium (Sc)?

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

As you move down the periodic table atoms get bigger. This is because ____________.

As you move across the periodic table atoms tend to get smaller because, ______________.

Electronegativity is...

Ionization energy is...

The atom with the largest atomic radius in Group 18 is -

Metals have the largest -

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry