Transition Metal Complexes.  A covalent bond is a shared pair of electrons  Usually the two atoms involved in the covalent bond each contribute one.

Slides:

Advertisements

Similar presentations

Arrhenius Definition Acids produce hydrogen ions in aqueous solution.

Advertisements

COMPLEX IONS Compounds in which metal ion is surrounded by a group of anions or neutral molecules.

Complex Ions. Complex ions generally contain transition metals like iron, cobalt, nickel, copper, zinc, and silver. If you see these metals as a reactant,

Complex ions Transition metals can form complexes because their ions have a high charge density: o they have quite a large nuclear charge but are relatively.

Quick Equation review. Double displacement During a double replacement or metathesis reaction, two new combinations of ions are produced. We identify.

213 PHC 8 th lecture (1) Gary D. Christian, Analytical Chemistry, 6 th edition 1.

Thermodynamics and Further Inorganic Chemistry. Contents Thermodynamics Periodicity Redox Equilibria Transition Metals Reactions of Inorganic Compounds.

Title: Lesson 6 Complex Ions Learning Objectives: Explain and use the terms ligand/complex/complex ion and ligand substitutions. Describe the formation.

Coordination Chemistry ligands bonding to metals.

Coordination Chemistry ligands bonding to metals.

Transition Metal Complexes. Transition metal complexes consist of a central Transition metal ion surrounded by a number of ligands. As a result of their.

Advanced Higher Chemistry Unit 1 Transition metal complexes.

Transition Metal Chemistry The Chemistry of the d-block elements.

THE GENERAL FEATURES OF TRANSITION METAL CHEMISTRY.

Transition Metals.

Complex Ions A ligand is a species that can donate one or more lone pairs of electrons to form a coordinate bond with a central metal ion. A central metal.

Chemistry of Coordination Compounds Brown, LeMay Ch 24 AP Chemistry Monta Vista High School To properly view this presentation on the web, use the navigation.

COMPLEX IONS: PART 1 From left to right, aqueous solutions of: Co(NO 3 ) 2 (red); K 2 Cr 2 O 7 (orange); K 2 CrO 4 (yellow); NiCl 2 (green); CuSO 4 (blue);

Transition Metals & Complex ions

Starter Electronic configuration of: Sc3+ Fe2+ Cu+

Transition metal complexes

Chemsheets AS006 (Electron arrangement)

Bonding. This presentation shows two types of bonding. Ionic bonding Covalent bonding Click on the type of bonding you want to view.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Transition Metals...show great similarities within a given period as well as within.

Chemical Bonds. 2 Types of Chemical Bonds 1. Ionic 2. Covalent.

Complex Ions Naming and Formula Writing. Definitions Complex ion – A combination of a metal ion and a ligand Ligand – Group bonded to a metal ion Coordination.

Solubility Equilibria

Coordination Complex. AP Test These questions used to always be in the equation prediction section that has been removed. These questions used to always.

Coordination compounds Dr. Peter Warburton

Acidity or Hydrolysis Reactions.  Definition: A Lewis acid is an electron pair acceptor  Definition: A Lewis base is an electron pair donor  In a complex,

Drill: Determine the Ksp for Mn 2 S 3 when the solubility is 1 x

Complex ions Transition metals form at least one cation with vacant d orbitals.

Ag+(aq) + 2 H2O(l)  Ag(H2O)2+(aq)

ERT207 Analytical Chemistry Complexometric Titration

Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Acids and Bases TEXT REFERENCE Masterton and Hurley Chapter 4.2 (Review), 13, 14.1, 15.1 (page 427), 21.2 (page589)

TM I-Intro to Complexes

Title: Lesson 5: Lewis Acids and Bases Learning Objectives: – Understand that a Lewis acid is a lone pair acceptor and a Lewis base is a lone pair donor.

Definitions of Acids and Bases Green & Damjii – Chapter 8 – Section 1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction.

Chapter 15: Transition Metals 15.1 General Properties of Transition Metals 15.2 Complex Formation and the Shape of Complex Ions 15.3 Coloured Ions 15.4.

ERT207 Analytical Chemistry Complexometric Titration Pn Syazni Zainul Kamal PPK Bioproses.

 Complexes containing bidentate or multidentate ligands are called chelates  Chelation is the process of forming a complex with bidentate or multidentate.

Bidentate & Multidentate Ligands -Explain and use the term bidentate ligand - Describe stereoisomerism in transition element multidentate complexes (cis-trans.

COMPLEX FORMATION And THE SHAPE OF COMPLEX IONS L.O.:  Recall definition of ‘ligand’, ‘co-ordinative bond’, ‘co-ordination number’.  Identify unidentate,

Naming Complexes.

Coordinate Covalent Bond Ammonia NH 3 to Ammonium Ion [NH 4 ] + One atom contributes both electrons in a bond.

16 Reactions of inorganic compounds in aqueous solution 16.1 Lewis acids and bases 16.2 Ligand substitution reactions 16.3 Summary: Acid-Base and substitution.

Topic 13 - Periodicity. Ionic properties High melting and boiling point Conduct electricity in molten and aqueous states Crystalline solids Soluble.

Acid Base Character of period 3

Yr 10 Chemistry Lewis Structures.  Questions of Doom Starter.

Solubilities. pH and Solubility   This is primarily LeCh â telier’s principle   If a compound contains the conjugate base of a weak acid, addition.

1 Lewis acid = a substance that accepts an electron pair Lewis Acids & Bases Lewis base = a substance that donates an electron pair.

TRANSITION METAL COMPLEXES.

Analysis of a Mixture of Cations

Access to Science - Chemistry

ERT207 Analytical Chemistry Complexometric Titration

Do Now – Complete the table

Complex Formation Do Now: What is a coordinate bond?

Coordination Compounds: AP Material

Metal Complexes -- Chapter 24

Drill: Determine the Ksp for Mn2S3 when the solubility is 1 x

Lewis acids and bases.

Assign.#17.7– Complex Ion Formation, Equilibrium Constants, and ΔG

Predicting Reaction Products - Question 4

What can you see in this picture? CO-ORDINATION NUMBER and LIGAND

The Chemistry of the Transition Elements

Presentation transcript:

Transition Metal Complexes

 A covalent bond is a shared pair of electrons  Usually the two atoms involved in the covalent bond each contribute one electron  Definition: In a co-ordinate bond, one atom donates both of the electrons in the shared pair of electrons  In order for a co-ordinate bond to form there must be a lone pair of electrons on one of the atoms  A co-ordinate bond is represented by an arrow, →

 Definition: A complex is a central metal ion surrounded by ligands  Definition: A ligand is an ion or molecule that can donate a lone pair of electrons to the central metal ion  The ligand donates its lone pair of electrons to the metal ion forming a co-ordinate bond  The ligand must have a lone pair of electrons

 Ligands can be negative ions such as:  Halide ions - Chloride ions, :Cl -, Bromide ions, :Br -  Hydroxide ion, :OH -  Cyanide ion, :CN -  Ligands can also be neutral molecules which contain more than one lone pair of electrons such as:  Ammonia, :NH 3  Water, H 2 O: The oxygen atom in water has two lone pairs of electrons

 A ligand that can donate one lone pair of electrons is a unidentate ligand  A ligand that can donate two lone pairs of electrons is a bidentate ligand  A ligand that can donate more than two lone pairs of electrons is a multidentate ligand  Even although water has two lone pairs of electrons, it can only donate one pair of electrons  Therefore water is a unidentate ligand O HH : :

 Definition: The co-ordination number is the number of pairs of electrons donated to the central metal ion  Co-ordination numbers are 2, 4 or 6 ComplexCo-ordination number [Ag(NH 3 ) 2 ] + [CuCl 4 ] 2- [Cu(H 2 O) 6 ] 2+ [FeCl 4 ] 2- [Cu(H 2 O) 4 (OH) 2 ] [Ag(H 2 O) 2 ]

 The central metal ion has a positive charge  The overall charge on the complex depends on the charge of the metal ion and the charge on the ligands  Example: [Cu(H 2 O) 6 ] 2+  Overall charge = 2+  Oxidation state of copper = +2  Remember water is a neutral ligand

ComplexOverall chargeOxidation state of metal ion [Ag(NH 3 ) 2 ] + [Cu(H 2 O) 6 ] 2+ [CuCl 4 ] 2- [V(H 2 O) 6 ] 3+ [Cu(H 2 O) 4 (OH)] [Ag(CN) 2 ] - [NiCl 4 ] 2- [CrCl 2 (H 2 O) 4 ]

 Silver forms complexes with a co-ordination number of 2  The shape of the complex is linear  Example: Tollens’ reagent (Test for aldehydes)  Tollen’s reagent contains the complex, [Ag(NH 3 ) 2 ] +  There are two ammonia ligands each donating one lone pair of electrons to the Ag + ion [H 3 N: → Ag + ← :NH 3 ] +

 When Tollen’s reagent is warmed with an aldehyde, the silver(I) ion (Ag + ) is reduced to silver atoms (Ag) producing a silver mirror  Ketones do not reduce the silver(I) ion and no silver mirror is formed