Nomenklatura Związków Nieorganicznych

Nomenclature of Inorganic Compounds

• Inorganic compounds are named according to rules and conventions for unambiguous identification.
• The naming system depends on the oxidation state of elements.
• The cation (positive ion) name precedes the anion (negative ion) name.

Binary Ionic Compounds

• Binary ionic compounds contain a metal cation and a nonmetal anion.
• The metal cation's name comes first, followed by the nonmetal anion name ending in "-ide".
  • Example: Sodium chloride (NaCl)

Polyatomic Ions

• Polyatomic ions are charged groups of atoms acting as a single unit; names must be memorized.
  • Examples: Sulfate (SO₄²⁻), Nitrate (NO₃⁻), Phosphate (PO₄³⁻)
• The compound name combines cation and polyatomic anion names.
  • Example: Potassium sulfate (K₂SO₄)

Transition Metal Cations

• Transition metals have multiple oxidation states.
• The oxidation state is indicated by a Roman numeral in parentheses after the metal name.
  • Example: Iron(II) oxide (FeO), Iron(III) oxide (Fe₂O₃).

Acids

• Acid names depend on the anion.
  • Anion ending in "-ide" -> "hydro-" prefix + "-ic acid" suffix.
    • Example: Hydrogen chloride (HCl) is hydrochloric acid.
  • Anion ending in "-ate" -> "-ic acid" suffix.
    • Example: Sulfuric acid (H₂SO₄).
  • Anion ending in "-ite" -> "-ous acid" suffix.
    • Example: Sulfurous acid (H₂SO₃).

Hydrates

• Hydrates are ionic compounds with water molecules in their crystal structure.
• Greek prefixes indicate the number of water molecules per formula unit.
  • Example: Copper(II) sulfate pentahydrate (CuSO₄⋅5H₂O).
    • Mono (1), di (2), tri (3), tetra (4), penta (5), hexa (6), etc. for water molecules.

Molecular Compounds - Non-metal compounds

• Molecular compounds contain only nonmetal atoms.
• Naming uses prefixes for the number of atoms of each element:
  • The element farther left and lower on the periodic table is named first.
  • The prefixes indicate the number of atoms (mono - 1, di - 2, tri - 3, tetra - 4, penta - 5, hexa - 6 etc.).
  • The second element name ends in "-ide".
  • Example: Carbon dioxide (CO₂), Nitrogen trioxide(N₂O₃)

Stock System

• Alternative method for naming ionic compounds, mainly for transition metals.
• Oxidation state of the metal is shown in parentheses as a Roman numeral.

Oxyanions

• Oxyanions are polyatomic anions containing oxygen.
• Oxyanion names often follow patterns, like changing "-ite" to "-ate" to reflect different oxygen numbers.

Nomenclature of Coordination Compounds

• Coordination compounds have central metal ions linked to surrounding ligands.
• Naming is complex, including ligands, central metal, and its oxidation state.

Conclusion

• Understanding inorganic compound nomenclature is crucial for effective chemical communication and comprehension.
• Standardized naming rules ensure consistent compound identification and formula clarity. Practice helps master these rules.

Oxides: Classification and Properties

• Oxides are chemical compounds where a chemical element (often a metal) combines with oxygen.
• General formula for oxides: Metal/Nonmetal + O₂ → Oxide
• Classification of oxides is based on the chemical nature of the element combining with oxygen, and on the properties of the resulting oxide.

Classification by Chemical Nature

• Basic Oxides (Basic):

  • Formed by the reaction of a metal (except group 18 metals) with oxygen.
  • React with water, forming hydroxides.
  • Examples: Na₂O, CaO, MgO.
  • These oxides are basic, often decomposing into corresponding hydroxides in water (e.g., Na₂O + H₂O → 2NaOH)

• Acidic Oxides (Acidic):

  • Formed by the reaction of a nonmetal with oxygen, or some transition metals in high oxidation states.
  • React with water, forming acids.
  • Examples: SO₃, CO₂, P₂O₅.
  • These oxides are acidic, soluble in water, and decompose into acids (e.g., SO₃ + H₂O → H₂SO₄)

• Neutral Oxides:

  • Do not exhibit either acidic or basic properties.
  • Reaction with water practically does not occur.
  • Examples: CO, NO.
  • These oxides do not react with water and do not form salts with acids and bases.

Division by Oxygen Nature

• Metallic Oxides: Formed from metals (often in a higher oxidation state).

  • Examples of different oxidation states of the same metal: MnO, MnO₂, Mn₂O₇.

• Nonmetallic Oxides: Formed from nonmetals (often in a higher oxidation state but not exclusively).

  • Examples: SiO₂, CO₂

• Amphoteric Oxides:

  • Exhibit both basic and acidic properties depending on the reactant.
  • Examples: Al₂O₃, ZnO. Can react with both bases and acids.

Additional Notes

• The oxidation state of oxygen in oxides is always -2, except for peroxides and ozonides.
• Oxide names are named according to IUPAC nomenclature, based on the oxidation state of the element forming the oxide.
• Besides the above classification, there is also a classification according to the redox behavior of oxides and other applications.