Sections 7.4 – 7.5 Periodic Properties of Atoms and Ions

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Presentation transcript:

Sections 7.4 – 7.5 Periodic Properties of Atoms and Ions

Periodic Properties In these sections… Trends in Orbital Energies Atomic Size Ionization Energy Electron Affinity Ion Electron Configuration and Size

Periodic Properties of the Elements All atomic properties depend on energies of outermost orbitals. Relative energies of outermost orbitals depend on their size and their effective nuclear charge.

Trends in Orbital Energies

Across a period, orbital energies decrease.

Why do energies decrease moving left-to-right? Effective Nuclear Charge Z* = Z - S

General Periodic Trends Highest Occupied Orbital smaller, lower energy larger, high energy

Atomic Size What does that mean?

Atomic Size: Trends

Ionization Energy What does that mean? Atom(g)  Atom+(g) + e- E = ionization energy

Ionization Energy: Trends I

Ionization Energy: Trends II

Why the breaks in the line?

Electron Affinity What does that mean? Atom(g) + e-  Atom-(g) E = electron affinity Trends:

Why is EA sometimes zero?

Ion Formation: Why do ions have the charges they do?

Cations vs. Anions

Electron Configurations of Cations

Transition Metal Cations: Lose s electrons first

Ion Size In General: Anions are big. Cations are small.

Isoelectronic Species