Inorganic and Physical Chemistry Definitions Lecture

Introduction

• Purpose: Video providing definitions for Inorganic and Physical Chemistry
• Definitions: Though not asked as frequently, they remain important.
• Usage: Watch through or listen casually.
• Slides: 51 slides total

Key Definitions

Basic Chemistry Terms

• Activation Energy: Minimum energy needed to start a reaction by breaking bonds.
• Alkali: A soluble base releasing hydroxide ions (OH⁻).
• Atomic Orbital: Region around nucleus holding up to two electrons with opposite spins.

Bonding

• Bond Enthalpy: Energy needed to break one mole of a specific bond in the gas state.
• Covalent Bond: Electrostatic attraction between a shared pair of electrons and nuclei.
• Dative Covalent Bond: Shared pair of electrons provided by one bonding atom.
• Ionic Bond: Electrostatic attraction between oppositely charged ions.
• Metallic Bond: Attraction between metal cations and delocalized electrons.
• Hydrogen Bond: Strong dipole-dipole attraction involving N-H, O-H, or H-F.

Acids and Bases

• Bronsted-Lowry Acid: Proton donor.
• Bronsted-Lowry Base: Proton acceptor.
• Buffer Solution: Minimizes pH changes upon addition of small amounts of acid/base.
• Conjugate Acid-Base Pair: Species transforming by gain/loss of a proton.
• Strong Acid: Acid that fully dissociates in solution.
• Weak Acid: Acid that partially dissociates in solution.
• Reducing Agent: Species which donates electrons.
• Oxidizing Agent: Species which accepts electrons.

Chemical Equilibria

• Dynamic Equilibrium: Continuous reaction in a closed system with no net concentration change.
• Homogeneous Equilibrium: All species in the same physical state.
• Heterogeneous Equilibrium: Species in different physical states.

Thermodynamics

• Enthalpy Change of Combustion: Enthalpy change when one mole of substance reacts completely with O₂ under standard conditions.
• Enthalpy Change of Formation: Enthalpy change when one mole of compound forms from its elements.
• Enthalpy Change of Hydration: Enthalpy change when gaseous ions dissolve to become aqueous under standard conditions.
• Enthalpy Change of Neutralization: Enthalpy change when an acid reacts with a base to form one mole of H₂O.
• Enthalpy Change of Solution: Enthalpy change when one mole of compound dissolves in water.
• Lattice Enthalpy: Enthalpy change for forming one mole of an ionic compound from its gaseous ions.
• Entropy: Measure of disorder or energy dispersal in a system.

Other Key Terms

• Empirical Formula: Simplest ratio of atoms within a compound.
• First Electron Affinity: Enthalpy change when one mole of electrons is added to gaseous atoms.
• First Ionization Energy: Energy needed to remove one mole of electrons from gaseous atoms.
• Half-Life: Time for the concentration of a reactant to halve.
• Ligand: Molecular ion donating a pair of electrons in a coordinate bond.
• Mole: Amount containing 6.02 × 10²³ particles.
• Order of Reaction: Power to which reactant concentration is raised in the rate equation.
• Rate of Reaction: Change in concentration of a reactant/product per unit time.
• Simple Molecular Lattice: Molecular structure held by intermolecular forces.
• Standard Solution: Solution of known concentration.
• Transition Element: d-block element forming ions with incomplete d subshells.
• Isotope: Atoms of the same element, with different neutron counts.
• Relative Atomic Mass: Weighted average mass compared to 1/12 of carbon-12.
• Relative Isotopic Mass: Isotope mass compared to 1/12 of carbon-12.

Conclusion

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