Periodicity Quiz: Test Your Knowledge of the Periodic Table

Periodic Table and Its Periodicity Quiz

Test your knowledge of the periodic table and its periodicity with this quiz. Explore the changes in atomic size and other properties of the elements, and learn the reasons behind these trends. Challenge yourself with questions that focus on the relationships between the elements and their positions on the table.

Created by

@FeistySkunk

Questions and Answers

What is the trend of atomic size in the periodic table and what are the reasons for this trend?

Atomic size decreases across a period and increases down a group due to the increase in effective nuclear charge and the increase in number of energy levels, respectively.

What are some other properties that exhibit periodicity in the periodic table?

Other properties that exhibit periodicity in the periodic table include ionization energy, electron affinity, and electronegativity.

How does the size of atoms affect the chemical reactivity of elements?

The size of atoms affects the chemical reactivity of elements because larger atoms have a weaker hold on their valence electrons, making them more likely to react with other elements to form compounds.

What is the relationship between atomic size and electronegativity in the periodic table?

As atomic size decreases across a period, electronegativity increases. As atomic size increases down a group, electronegativity decreases. Signup and view all the answers

Explain the trend of atomic radius in the periodic table.

Atomic radius decreases across a period from left to right due to increasing nuclear charge. Atomic radius increases down a group due to the increasing number of energy levels. Signup and view all the answers

How does the periodicity of ionization energy relate to the periodicity of atomic size?

Ionization energy increases across a period as atomic size decreases. Ionization energy decreases down a group as atomic size increases. Signup and view all the answers

Study Notes

Atomic Size Trend in the Periodic Table

Atomic size decreases from left to right across a period due to increasing nuclear charge, which pulls electrons closer to the nucleus.
Atomic size increases down a group due to the addition of energy levels, which increases the distance between the nucleus and outermost electrons.

Other Periodic Properties

Electronegativity increases from left to right across a period and decreases down a group, following a similar trend to atomic size.
Ionization energy increases from left to right across a period and decreases down a group, also following a similar trend to atomic size.

Atomic Size and Chemical Reactivity

Smaller atoms are more reactive due to their higher electronegativity and ability to gain or lose electrons more easily.
Larger atoms are less reactive due to their lower electronegativity and inability to gain or lose electrons easily.

Relationship Between Atomic Size and Electronegativity

There is an inverse relationship between atomic size and electronegativity, meaning smaller atoms have higher electronegativity and larger atoms have lower electronegativity.

Trend of Atomic Radius

Atomic radius decreases from left to right across a period due to increasing nuclear charge.
Atomic radius increases down a group due to the addition of energy levels.

Periodicity of Ionization Energy

Ionization energy increases from left to right across a period due to increasing nuclear charge.
Ionization energy decreases down a group due to the addition of energy levels.
There is a direct relationship between ionization energy and atomic size, with smaller atoms having higher ionization energies and larger atoms having lower ionization energies.