klenk_edit_OSX_Chemistry2e_Ch06_PPT

Chapter 6: Electronic Structure and Periodic Properties of Elements

6.1 Electromagnetic Energy

• Basic Wave Behavior: Understand traveling and standing waves.

• Wave Nature of Light: Light exhibits wave-like properties.

• Calculating Properties: Use equations to determine frequency, wavelength, and energy.

• Emission Spectra: Differentiate between line spectra and continuous emission spectra.

• Particle Nature of Light: Recognize light's dual nature, as both wave and particle.

6.2 The Bohr Model

• Development of the Model: Niels Bohr's 1913 model revolutionized atomic theory.

• Assumptions: Electrons orbit the nucleus in quantized energy levels.

• Energy Absorption/Emission: Transitions between orbits involve specific energy changes corresponding to photons.

6.3 Development of Quantum Theory

• Wave-Particle Duality: Extends the concept of wave-particle duality to matter.

• Quantum Mechanical Description: Utilizes 3D wave functions/orbitals for electron distribution.

• Quantum Numbers: Four quantum numbers (n, l, m_l, ms) define electron states.

6.4 Electronic Structure of Atoms (Electron Configurations)

• Ground-state Configurations: Predicted via the Aufbau principle, detailing how electrons fill orbitals.

• Exceptions: Analyze atypical filling patterns in transition elements.

• Valence vs Core Electrons: Understand how electrons determine reactivity and properties of elements.

6.5 Periodic Variations in Element Properties

• Periodic Trends: Changes observed in atomic size, ionization energy, and electron affinities across the periodic table.

• Atomic Size Variations: Explained by effective nuclear charge and electronic repulsion.

• Ionization Energy: Amount of energy to remove an electron; trends increase across periods, decrease down groups.

• Electron Affinity: Measure of energy change upon adding an electron; typically becomes more negative across periods.