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Questions and Answers
What is ionic radius?
What is ionic radius?
The measure used to describe the size of an ion.
Is the cation or parent atom smaller in size?
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.
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?
How does the removal of an electron affect Zeff?
How does the charge of the cation affect the size?
How does the charge of the cation affect the size?
What trend is observed for cations of successive elements in the periodic table?
What trend is observed for cations of successive elements in the periodic table?
What is an anion formed by?
What is an anion formed by?
What causes the radius of an anion to be larger than the neutral atom?
What causes the radius of an anion to be larger than the neutral atom?
What is the trend of principal quantum numbers and radii for consecutive elements in any group?
What is the trend of principal quantum numbers and radii for consecutive elements in any group?
What are examples of isoelectronic species?
What are examples of isoelectronic species?
What does isoelectronic mean?
What does isoelectronic mean?
What defines an isoelectronic series?
What defines an isoelectronic series?
In isoelectronic species, what determines the size?
In isoelectronic species, what determines the size?
What is the electron configuration of a N3- anion?
What is the electron configuration of a N3- anion?
What is the electron configuration of a Mn2+ cation?
What is the electron configuration of a Mn2+ cation?
Would a nitrogen atom and a nitride anion (N3-) be paramagnetic or diamagnetic?
Would a nitrogen atom and a nitride anion (N3-) be paramagnetic or diamagnetic?
Would a manganese atom and a manganese(II) cation (Mn2+) be paramagnetic or diamagnetic?
Would a manganese atom and a manganese(II) cation (Mn2+) be paramagnetic or diamagnetic?
What is paramagnetism?
What is paramagnetism?
What does Hund's Rule state?
What does Hund's Rule state?
In what direction do unpaired electrons spin?
In what direction do unpaired electrons spin?
What are diamagnetic substances characterized by?
What are diamagnetic substances characterized by?
Why are atoms in diamagnetic substances not attracted into a magnetic field?
Why are atoms in diamagnetic substances not attracted into a magnetic field?
How do you determine whether an atom is paramagnetic or diamagnetic?
How do you determine whether an atom is paramagnetic or diamagnetic?
How can we determine whether a salt will be attracted to a magnet?
How can we determine whether a salt will be attracted to a magnet?
Summarize the effects of ionic radii and electron configuration on paramagnetism and diamagnetism.
Summarize the effects of ionic radii and electron configuration on paramagnetism and diamagnetism.
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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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