Experiment
Experiment : 1
Tittle : Preparation of bis(acetylacetonato)copper(II) complex
Objective : To synthesis the bis(acetylacetonato)copper(II) complex
Introduction : A complex ion is usually form with high charge density metal ion as a central and formation of coordinate covalent bond (dative bond) with high electron molecules or ions. These molecules or ions are functioning as ligands (electrophile in organic compounds). They are easily attracted by electrophile (electron deficiency atoms or ions ). Ligands are species that have at least one lone pair of electrons that are readily donated to a metal or an ion to form a coordinate bond. According to lewis acid- base theory, all ligands are lewis base as they act as donor. In the contrary, the metal, central atom act as an lewis acid as it receives lone pair electrons from the ligands when forming the complex ions. The properties of lewis acid is to have high electron deficiency. For transition metals in this experiment, the high charge density, positive charge and their vacant bonding orbitals leads to tendency to attract lone pair electron by filling up their vacant orbitals. Metal acetylacetonates, formed by a metal and multiple acetylacetonate anions, are prime examples of coordination complexes. In this experiment, the metal use is copper (II) ion which is crystal blue in colour when it is copper(II)nitrate. All metal ions in solution can react well with water. The water molecules can also be weakly bonded or more strongly as a ligand to form a complex ion, and these can also present in solid ‘hydrated’ salts of crystallization. For example, copper (II) nitrate (Cu(NO3)2∙3H2O) The metal complexes that contain at least one ammonia (NH3) ligand are called metal ammine complexes. Metal acetylacetonates are coordination complexes derived from the acetylacetonate anion(acac) and metal ions.
The coordination number of a complex ion is the number of coordinate bonds being formed
Tittle : Preparation of bis(acetylacetonato)copper(II) complex
Objective : To synthesis the bis(acetylacetonato)copper(II) complex
Introduction : A complex ion is usually form with high charge density metal ion as a central and formation of coordinate covalent bond (dative bond) with high electron molecules or ions. These molecules or ions are functioning as ligands (electrophile in organic compounds). They are easily attracted by electrophile (electron deficiency atoms or ions ). Ligands are species that have at least one lone pair of electrons that are readily donated to a metal or an ion to form a coordinate bond. According to lewis acid- base theory, all ligands are lewis base as they act as donor. In the contrary, the metal, central atom act as an lewis acid as it receives lone pair electrons from the ligands when forming the complex ions. The properties of lewis acid is to have high electron deficiency. For transition metals in this experiment, the high charge density, positive charge and their vacant bonding orbitals leads to tendency to attract lone pair electron by filling up their vacant orbitals. Metal acetylacetonates, formed by a metal and multiple acetylacetonate anions, are prime examples of coordination complexes. In this experiment, the metal use is copper (II) ion which is crystal blue in colour when it is copper(II)nitrate. All metal ions in solution can react well with water. The water molecules can also be weakly bonded or more strongly as a ligand to form a complex ion, and these can also present in solid ‘hydrated’ salts of crystallization. For example, copper (II) nitrate (Cu(NO3)2∙3H2O) The metal complexes that contain at least one ammonia (NH3) ligand are called metal ammine complexes. Metal acetylacetonates are coordination complexes derived from the acetylacetonate anion(acac) and metal ions.
The coordination number of a complex ion is the number of coordinate bonds being formed