Ionic Nomenclature

nothing Ionic Nomenclature

D.1 Intro:Elements, Compounds and Nomenclature • Chemical nomenclature:the organized system used to name substances and write their chemical formulas. • Chemical formula:represents the number of each kind of atom bonded together in a substance. • Subscript:indicates the number of atoms or ions present in the formula.

D.1 Intro:Elements, Compounds and Nomenclature Example(formula for water):

D.2 The History of Chemical Nomenclature • Lavoisier’s system of nomenclature is sometimes called theClassical System. • This system of naming is used to the present day.

Example:carbon dioxide Dalton formula: Berzelius formula:CO2 D.2 The History of Chemical Nomenclature • Chemical formulas of compounds… • are written using two or more symbols side by side. • use subscripts to make the formulas more compact.

D.2 The History of Chemical Nomenclature • Many elements form several compounds with another given element. • Lavoisier’s Classical System was modified to include suffixes to name these compounds: Examples: ferric oxideFe2O3 ferrous oxideFeO (More will be said on this in Section D.6.)

D.2 The History of Chemical Nomenclature Examples:

D.3 Classification of Compounds • Ionic compoundsare formed when oppositely charged ions are attracted to each other. • Strong electrostatic attractions. • High melting point and boiling point solids. • Capable of dissolving in water.

D.3 Classification of Compounds • Cationsare positively-chargedions. Examples: Na+, K+, Ca2+, Al3+, Fe3+ • Anionsare negatively-chargedions. Examples: Cl–, F–, S2–, Se2–, P3–

D.3 Classification of Compounds • Molecular compoundsare pure substances composed of atom groupings called molecules. • strong covalent bonds between atoms • atoms share electrons • each atom has a noble-gas electron arrangement • possess weak bonds between molecules • low melting point and boiling point gases, liquids and solids

D.4 Binary Ionic Compounds • Molecular Formula: • Chemical formula for molecular substances. • The actual number of each kind of atom present in the molecule. • Empirical Formula: • Indicates the simplest whole number ratio of atoms or ions in the compound.

D.4 Binary Ionic Compounds • Naming Binary Ionic Compounds • When naming any ionic compounds, simply write the name of the positive ion followed by the name of the negative ion. • The rules for naming simple ions were given in Unit B.

D.4 Binary Ionic Compounds • Name the cation by writing the full name of the metallic element. • Na+ is a sodium ion • Zn2+ is a zinc ion • Al3+ is an aluminum ion. • Name the anion by abbreviating the full name of the nonmetallic element and adding –ide. • Cl– is a chloride ion • S2– is a sulfide ion • P3– is a phosphide ion

D.4 Binary Ionic Compounds Examples: • NaCl{from Na+Cl–} sodiumchloride Sodium chloride is table salt. • CaCl2{from Ca2+(Cl–)2} calciumchloride Calcium chloride is a drying agent also used to melt ice.

D.4 Binary Ionic Compounds • Writing Chemical Formulas for Binary Ionic Compounds • When given the name of the ionic compound, first write the symbols for the ions involved. • Next, determine the lowest whole number ratio of ions that will provide an overall net charge of zero. (Criss-Cross)

D.4 Binary Ionic Compounds Examples:

Ionic Nomenclature