Coordination Complexes of Cobalt Advanced Inorganic Chemistry Lab 02/27/2015 Abstract When the transition metal‚ cobalt‚ forms a complex involving a nitrate ion‚ the ligand has the ability to coordinate via N or O. The ability of the nitrate to attach via the N or O gives rise to the term‚ linkage isomers and can affect the functionality of the complex with other molecules. To explore structural differences between complexes‚ pentaaminechlorocobalt (III) chloride‚ pentaaminenitritocobalt (III)
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water ≥ 200 ppm 〖CaCo〗_3/L is labeled as “hard”. How: Ethylenediamminetetraacetic Acid (EDTA) is a complex versatile chelating agent. A chelating agent is a substance whose atoms can form several bonds (ligands) to a single metal ion. Chelating agents are multi-dentate ligands. Multidentate ligands are many clawed‚ holding onto the metal ion to form a very stable complex. EDTA can form four or six bonds with a metal ion. EDTA is used to capture and bind the metal ions. However‚ EDTA and the EDTA-complex
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The Complex Compounds [ Co (CN) 6 ] 3- and [Co (NH3)6 ]2+ have different colours explain 6. give an example of each of the following i. Neutral complex ii. Cationic Complex iii. Anionic Complex iv. Hexadentate ligand SECTION B 7. a) Giving reasons arrange the following isomeric alkanes in order of decreasing boiling points i. Pentane ii. 2‚ 2-dimethylpropane iii. 2-methylbutane a) How will you synthesize methane from
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COrdination compounds Question 9.1: Explain the bonding in coordination compounds in terms of Werner’s postulates. =Werner’s postulates explain the bonding in coordination compounds as follows: (i) A metal exhibits two types of valencies namely‚ primary and secondary valencies. Primary valencies are satisfied by negative ions while secondary valencies are satisfied by both negative and neutral ions. (In modern terminology‚ the primary valency corresponds to the oxidation number of the metal
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weakly bonded or more strongly as a ligand to form a complex ion‚ and these can also present in solid ’hydrated’ salts of crystallization. E.g Copper(II) nitrate (Cu(NO3) 2.3H2O). A complex ion has a metal ion at its centre with a number of other molecules or ions surrounding it. These can be considered to be attached to the central ion by co-ordinate (dative covalent) bonds. The molecules or ions surrounding the central metal ion are called ligands. Simple ligands include water‚ ammonia‚ acetyl acetone
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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
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molecules or ions called ligands • type of bond: Lewis acid -base • examples: metal: acid; base: ligand + 32 Ag(NH ) Cu(NH3)2+2 Fe(CN)6-4 Coordination Compounds • c ontains a complex ion [Co(NH3)6 ]Cl3 Fe4 [Fe(CN)6]3 [Co(H2 O)6 ][Co(CN)6 ] Ca[Cu(OH)3 (Br)(NH3 )2 ] 1 of 3 CHEM 301 LECTURE coordination number • number of atoms bonded to the central atom donor atom • a tom in the ligand that is directly bonded to the central atom t ype of ligands • monodentate • bidentate
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Oxidative Additions Oxidative addition reactions usually involve a coordinatively unsaturated 16-electron metal complex or five-coordinate 18-electron species‚ and take the general from: [pic] If the A and B ligands in the product are considered to be formally –1‚ then the metal center has increased its oxidation state by +2‚ and this is the origin of the name oxidative addition. Oxidative reaction can occur when a metal complex behaves as both a Lewis acid
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present investigation some new Schiff bases derived from Amoxicillin trihydrate with Cinnamaldehyde and p-Chlorobenzaldehyde and their complexes with bivalent transition metal ions viz. Co(II)‚ Zn(II)‚ Ni(II)‚ and Mn(II)‚ have been synthesized. The ligand and their metal complexes were characterized on the basis of elemental analysis and micro analytical datas. Shift in the characteristic spectral frequency of the metal complexes‚ confirms the coordination through metal ion with azomethine group. They
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Trial 4 0.00 0.17 0.21 0.25 0.14 0.12 0.13 0.12 Trial 5 0.00 0.14 0.18 0.23 0.11 0.09 0.08 0.08 Qualitative Analysis Table 2: Qualitative Observations and Descriptions Observation The solution’s color changes as metal to ligand ratio changes. Description I noticed that the solutions’ colors turned darker as the CuSO4 volume increased in the ratio with NH3‚ until a point was reached beyond which further increases in CuSO4 volume in proportion to NH3 volume made the
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