Ions: Representative and Transition Metals

Ion Configuration for Representative Elements

• Representative elements form definitive ions for stable, noble gas electron configurations.
• Metals typically form cations (positive ions) by losing electrons from their valence shell.
• Nonmetals typically form anions (negative ions) by gaining electrons in their valence shell.

Ion Configuration for Transition Metals

• Transition metals form ions and typically exhibit variable charges.
• When transition metals form ions, they lose electrons from the sublevel with the highest principal quantum number (n) first (often the s orbital), then from the (n-1)d orbitals if more electrons need to be removed.

Practice Problems and Examples

• The strontium ion (Sr²⁺) has the same electron configuration as xenon (Xe).
• The chlorine ion (Cl⁻) has the same electron configuration as the argon (Ar).
• The nitrogen ion (N³⁻) has the same electron configuration as the aluminum ion (Al³⁺).
• The nitrogen ion (N³⁻) has the same electron configuration as the magnesium ion (Mg²⁺).
• The nitrogen ion (N³⁻) has the same electron configuration as the sodium ion (Na⁺).
• The magnesium ion (Mg²⁺) has an electron configuration: 1s²2s²2p⁶.
• Manganese (Mn) can form a +2 ion with electron configuration: 1s²2s²2p⁶3s²3p⁶3d⁵.

Transition lons Lab

• Metal ions form when metal atoms lose valence electrons, with the number of electrons lost determining the ion's charge.

Analyzing Periodic Trends

• Atomic Radius is indicated on the periodic table using arrows, showing increasing trends.
• Ionization Energy is indicated on the periodic table using arrows, showing increasing trends.
• Electron Affinity is indicated on the periodic table using arrows, showing increasing trends.

Atomic Radius

• Atomic radius is half the distance between two nuclei in adjacent atoms.
• Atomic radius increases going down a group due to adding an energy level, reducing the force.
• Atomic radius decreases going left to right across a row because the effective nuclear charge increases.

Effective Nuclear Charge (Zeff)

• Effective nuclear charge is the net positive charge experienced by an electron in a polyelectronic atom, influenced by both the nuclear charge (Z) and the shielding effect of other electrons (σ).
• Zeff = Z - σ
• Across a period, because added electrons are valence electrons and do not shield each other well, the effective nuclear charge felt increases.

Ionic Radius

• The ionic radius is the radius of an atom's ion.
• If an atom forms an anion, its size increases due to increased repulsion between electrons.
• If an atom forms a cation, its size decreases due to decreased repulsion between electrons.

Ionization Energy

• Ionization Energy is the minimum energy required to remove an electron from a gaseous atom in its ground state.
• When an electron is removed, the repulsion among remaining electrons decreases.
• Because nuclear charge remains constant, more energy is needed to remove another electron.
• Ionization Energy increases: IE₁ < IE₂ < IE₃ < ...
• Metals have relatively low ionization energies compared to nonmetals.
• Ionization energy decreases going down a group because the electrons move further from the nucleus, causing less attraction.

Electron Affinity

• Electron Affinity measures the energy change when an electron is added to a gaseous atom.
• Elements closer to achieving a noble gas configuration are more likely to gain an electron.

Successive Ionization Energy

• Successive ionization energy is energy that is required to remove an additional electron from an atom.
• There exist irregularities but they will not be tested.
• Between Groups 2A & 3A elements in the same period (between Be & B, Mg & AI)
• Between Groups 5A & 6A elements in the same period (between N & O, P & S)

Coulombic Attraction

• Coulombic attraction refers to the attraction between oppositely charged particles, with strong or weak attractive forces.
• Distance and the magnitude of the charges of the particles impacts Coulombic Attraction.
• Force is dependent; distance is independent.
• The bigger # of distance; More the force.
• Each electron receives approximately the full attractive force of the nucleus (minus the repulsive effects).

Understand ion formation in representative and transition metals. Explore how metals lose electrons to form cations, while nonmetals gain electrons to form anions, achieving stable noble gas configurations. Includes practice problems.