Electron Configurations for Ions Quiz

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Questions and Answers

What is ionic radius?

The measure used to describe the size of an ion.

Is the cation or parent atom smaller in size?

A cation is smaller than the atom from which it is derived.

Give an example of a cation and its parent atom.

The radius of a neutral aluminum atom is 118 pm, while that of Al3+ is 68 pm.

How does the removal of an electron affect Zeff?

Removing an electron increases Zeff for any remaining valence electrons. Signup and view all the answers

How does the charge of the cation affect the size?

Cations with larger charges are smaller than cations with smaller charges. Signup and view all the answers

What trend is observed for cations of successive elements in the periodic table?

They generally have larger radii. Signup and view all the answers

What is an anion formed by?

The addition of one or more electrons to the valence shell of an atom. Signup and view all the answers

What causes the radius of an anion to be larger than the neutral atom?

The increased number of electrons and decreased Zeff. Signup and view all the answers

What is the trend of principal quantum numbers and radii for consecutive elements in any group?

Anions have larger principal quantum numbers and larger radii. Signup and view all the answers

What are examples of isoelectronic species?

N3-, O2-, F-, Ne, Na+, Mg2+, and Al3+. Signup and view all the answers

What does isoelectronic mean?

Having the same number of electrons and the same electron configuration. Signup and view all the answers

What defines an isoelectronic series?

A series of atoms, ions, or molecules having the same number of electrons. Signup and view all the answers

In isoelectronic species, what determines the size?

The number of protons determines the size. Signup and view all the answers

What is the electron configuration of a N3- anion?

1s22s22p6. Signup and view all the answers

What is the electron configuration of a Mn2+ cation?

1s22s22p63s23p64s23d5. Signup and view all the answers

Would a nitrogen atom and a nitride anion (N3-) be paramagnetic or diamagnetic?

N atom would be paramagnetic, N3- anion would be diamagnetic. Signup and view all the answers

Would a manganese atom and a manganese(II) cation (Mn2+) be paramagnetic or diamagnetic?

Mn atom and Mn2+ cation would both be paramagnetic. Signup and view all the answers

What is paramagnetism?

The magnetic state of an atom with one or more unpaired electrons. Signup and view all the answers

What does Hund's Rule state?

Electrons must occupy every orbital singly before any orbital is doubly occupied. Signup and view all the answers

In what direction do unpaired electrons spin?

Unpaired electrons can spin in either direction. Signup and view all the answers

What are diamagnetic substances characterized by?

Paired electrons, i.e., no unpaired electrons. Signup and view all the answers

Why are atoms in diamagnetic substances not attracted into a magnetic field?

The electron spins are oriented in opposite directions, causing the magnetic fields to cancel out. Signup and view all the answers

How do you determine whether an atom is paramagnetic or diamagnetic?

You need to create and analyze the orbital box diagram to check for unpaired electrons. Signup and view all the answers

How can we determine whether a salt will be attracted to a magnet?

By analyzing the orbital box diagram for the ions, specifically the metal cations. Signup and view all the answers

Summarize the effects of ionic radii and electron configuration on paramagnetism and diamagnetism.

Anionic radii are larger due to more electrons but constant nuclear charge, while cationic radii are smaller due to decreased valence electrons and increased Zeff. Signup and view all the answers

Study Notes

Ionic Radius and Ions

Ionic radius refers to the size of an ion, essential for understanding ion behavior.
Cations (positively charged ions) are smaller than their parent atoms due to the removal of electrons.

Cations and Their Characteristics

Example: Neutral aluminum atom has a radius of 118 pm; Al3+ has an ionic radius of 68 pm.
Removal of electrons increases the effective nuclear charge (Zeff) for remaining valence electrons.
Cations with higher positive charges (e.g., V3+) are smaller than those with lower charges (e.g., V2+).

Trends in Ionic Sizes

In the periodic table, cations of successive elements typically exhibit larger radii down a group, corresponding to increased principal quantum number.
Anions (negatively charged ions) form by adding electrons, which leads to greater electron-electron repulsion and reduced Zeff.

Factors Affecting Anion Size

Anions are larger than neutral atoms due to an increased number of electrons and a decrease in Zeff.
Larger principal quantum numbers correlate with larger radii for anions as one moves down groups in the periodic table.

Isoelectronic Species

Isoelectronic species have the same electron configuration; examples include N3-, O2-, F-, Ne, Na+, Mg2+, and Al3+, all with electron configuration 1s22s22p6.
Nuclear charge impacts size within isoelectronic series; greater nuclear charge results in smaller ionic radii due to increased Zeff.

Electron Configuration and Ions

Cations form when valence electrons are removed; for main group elements, the last added electrons are lost first.
In transition metals, ns electrons are lost before (n-1)d or (n-2)f electrons.
Anions fill electrons following the Aufbau principle, adding electrons in order of increasing energy.

Magnetism and Electron Configuration

Paramagnetism arises from unpaired electrons, leading to attraction to magnetic fields.
Diamagnetic substances have all electrons paired and do not exhibit attraction to magnetic fields.
The Pauli Exclusion Principle explains the lack of attraction in diamagnetic substances: opposing electron spins cancel out magnetic fields.

Determining Magnetic Properties

To assess if an atom is paramagnetic or diamagnetic, analyze its orbital box diagram for unpaired electrons.
A salt's attraction to magnets can be deduced by examining the metal cation's electron configuration for unpaired electrons.

Summary of Key Points

Anionic radii are larger compared to neutral atoms; cationic radii are smaller due to reduced valence electrons and increased Zeff.
In cation and anion configurations, the most recently added electrons are generally the first to be removed.
Paramagnetic substances contain unpaired electrons; diamagnetic substances are characterized by completely paired electrons.

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Description

Test your knowledge on ionic radius and the differences between cations and parent atoms. This quiz will help you understand the concept of ionic size and its implications in chemistry. Perfect for students studying atomic structure and electron configurations.