Atomic Radius Ionic Radius

Atomic and Ionic Radii

Exploring the sizes of atoms and ions

Atomic and Ionic Radii

To determine atomic radius, remember that it increases as we move to the left on the periodic table. This is because there are fewer protons, resulting in less electromagnetic attraction between the nucleus and electrons. For ionic radius, consider the following order of increasing size: O^2-, F^-, Ne, Na⁺, and Mg²⁺.

Multiple Choice

Why does atomic radius increase as we move to the left on the periodic table?

• Because there are more protons, resulting in more electromagnetic attraction between the nucleus and electrons.

• Because there are fewer protons, resulting in less electromagnetic attraction between the nucleus and electrons.

• Because there are more electrons, resulting in more electromagnetic attraction between the nucleus and electrons.

• Because there are fewer electrons, resulting in less electromagnetic attraction between the nucleus and electrons.

Atomic Radius

Trivia: As we move to the left on the periodic table, the atomic radius increases. This is because there are fewer protons, resulting in less electromagnetic attraction between the nucleus and electrons. This allows the electrons to be further away from the nucleus, leading to a larger atomic radius.

Atomic and Ionic Radii

Atomic radius increases going left and down the periodic table, while ionic radius is influenced by the number of electrons. The correct order of increasing atomic radius is Krypton, Bromine, Germanium, Lead, Flerovium. Understanding these trends helps in predicting the size of atoms and ions.

Atomic and Ionic Radii

Atoms and ions with the same number of electrons are called isoelectronic species. They experience the same amount of electron repulsion, resulting in similar atomic radii. For example, O^2-, Mg²⁺, F^-, Na⁺, and Ne all have 10 electrons and exhibit the same electron configuration as neon.

Multiple Choice

What is the term used to describe atoms and ions with the same number of electrons?

• Isotonic species

• Isoelectronic species

• Isobaric species

• Isomeric species

Isoelectronic Species

Isoelectronic species are atoms and ions that have the same number of electrons. This means they have similar electron configurations, resulting in similar chemical properties. Examples include Neon and Oxygen. Isotonic, isobaric, and isomeric species refer to different concepts and are not related to electron numbers.

Exploring Atomic and Ionic Radii

• Electrons are not a factor in determining the trend of atomic and ionic radii.
• The number of protons in the nucleus determines the ionic radii.
• More protons in the nucleus result in stronger attraction and contraction of the ionic radius.
• For iso-electronic species, the ionic radius decreases as the number of protons increases.
• The correct order of increasing ionic radius is: Mg²⁺, Na⁺, Ne, F^-, O^2-.

Multiple Choice

What determines the trend of atomic and ionic radii?

• Electrons

• Protons

• Neutrons

• Isotopes

Protons Determine Radii Trend

Interesting Trivia: The number of protons in an atom's nucleus determines its atomic and ionic radii. As the number of protons increases, the radii decrease. This is because the increased positive charge attracts the negatively charged electrons closer to the nucleus, resulting in a smaller radius. Protons play a crucial role in determining the size of atoms and ions.