Inorganic Chemistry

1. Inorganic Compounds
   1. Salts
      1. Ionic Compounds
         1. Formation
            1. Composed of cations and anions
            2. Lattice energy and its influence on stability
            3. Examples of common ionic compounds
         2. Structure
            1. Crystal lattice arrangement
            2. Coordination number in ionic crystals
         3. Properties
            1. Electrical conductivity in molten state or solution
            2. High melting and boiling points
      2. Solubility Rules
         1. General solubility trends
            1. Solubility of nitrates, sulfates, halides, etc.
            2. Exceptions to solubility rules
         2. Factors Affecting Solubility
            1. Temperature effects
            2. Common ion effect
            3. Ionic strength and its importance
      3. Precipitation Reactions
         1. Mechanisms
            1. Double displacement reactions
            2. Formation of an insoluble product
         2. Applications
            1. Water purification
            2. Qualitative analysis in laboratories
         3. Example Reactions
            1. Silver nitrate with sodium chloride
            2. Barium chloride with sulfuric acid
   2. Acids and Bases
      1. Definitions
         1. Arrhenius Concept
            1. Acids produce H+ in water
            2. Bases produce OH- in water
         2. Brønsted-Lowry Theory
            1. Proton donors and acceptors
         3. Lewis Theory
            1. Electron pair acceptors and donors
      2. Strong vs. Weak Acids/Bases
         1. Dissociation in Water
            1. Complete dissociation for strong acids/bases
            2. Partial dissociation and equilibrium for weak acids/bases
         2. Common Examples
            1. Strong acids like HCl, H2SO4
            2. Weak acids like acetic acid
            3. Strong bases such as NaOH
            4. Weak bases like ammonia
      3. pH and pKa
         1. pH Scale
            1. Measurement of acidity/basicity
            2. pH indicators
         2. pKa and Acid-Base Strength
            1. Relationship between pKa and strength of an acid
            2. Calculation of pH using pKa and concentration
         3. Buffer Solutions
            1. Definition and Composition
            2. Henderson-Hasselbalch equation
            3. Importance in biochemical processes
   3. Oxides
      1. Metal Oxides
         1. Basic Oxides
            1. Reaction with water to form bases
            2. Examples like Na2O, CaO
         2. Acid-Base Properties
            1. Formation of salts with acids
      2. Nonmetal Oxides
         1. Acidic Oxides
            1. Reaction with water to form acids
            2. Examples such as CO2, SO3
         2. Environmental Impact
            1. Role in acid rain formation
            2. Industrial emissions and control
      3. Amphoteric Oxides
         1. Definition and Behavior
            1. React with both acids and bases
            2. Examples such as Al2O3, ZnO
         2. Reactions and Examples
            1. Application in corrosion resistance
   4. Halides
      1. Ionic vs. Covalent Halides
         1. Comparison
            1. Ionic nature in metal halides
            2. Covalent characteristics in nonmetal halides
         2. Examples
            1. Sodium chloride vs. carbon tetrachloride
      2. Interhalogen Compounds
         1. Formation and Types
            1. Compounds formed between different halogens
            2. Variations in size and electronegativity
         2. Properties and Reactivity
            1. High reactivity due to bond polarity
            2. Use as reagents in synthesis
         3. Examples
            1. Iodine monochloride (ICl)
            2. Chlorine trifluoride (ClF3)