Starter 2. Complete the electronic arrangement of the Co 2 + ion. (1 mark) [Ar] 3. Explain why complex ions with partially filled d sub-levels are usually.

Slides:

Advertisements

Similar presentations

INTRODUCTION TO THE TRANSITION ELEMENTS

Advertisements

Balancing Redox Equations in Acidic Conditions

Unit 20 Oxidation and reduction Activity 20.1 Investigating redox reactions Reference in textbook: Section S.

Oxidation-Reduction Dr. Ron Rusay Balancing Oxidation-Reduction Reactions.

6.9 Chemistry of Colour. Recapping from earlier Coloured substances absorb radiation in the visible region of the EM spectrum. Absorb energy - outermost.

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

Reactivity Series of Metals

AN INTRODUCTION TO TRANSITION METAL COMPLEXES KNOCKHARDY PUBLISHING 2008 SPECIFICATIONS.

Balancing Oxidation- Reduction Reactions Any reaction involving the transfer of electrons is an oxidation-reduction (or redox) reaction.

Oxidation-Reduction Dr. Ron Rusay Balancing Oxidation-Reduction Reactions.

Advanced Higher Chemistry Unit 1 Oxidation states of the transition metals.

Balance Redox Equations: Half Reaction concentrate on electrons, balance each ½ rx. separately Ex: Cr 2 O 7 2- (aq) + Cl - (aq)  Cr 3+ (aq) + Cl 2 (g)

Redox titrations. HIGHER GRADE CHEMISTRY CALCULATIONS Redox Titration. Redox titrations are used to find out information about one reactant, using known.

Transition metal ions. The elements in the middle ‘d’ block of the periodic table are collectively known as transition elements. Since these elements.

Transition Metals.

1 6FeSO 4 (aq) + K 2 Cr 2 O 7 (aq) +7H 2 SO 4 (aq)  3Fe 2 (SO 4 ) 3 (aq) + Cr 2 (SO 4 ) 3 (aq) +7H 2 O(l) + K 2 SO 4 (aq) What are we looking for? A.

Zn  Zn2+ + 2e- (oxidation) Cu e-  Cu (reduction)

1.5 Oxidation and Reduction. Learning Outcomes Introduction to oxidation and reduction: simple examples only, e.g. Na with Cl 2, Mg with O 2, Zn with.

Oxidation and reduction – oxygen transer A substance has been oxidised if it gains oxygen. Oxidation is gain of oxygen. A substance has been reduced if.

TOPIC B TYPES OF CHEMICAL REACTIONS. REDOX Oxidation is a loss of electrons Reduction is a gain of electrons OIL RIG or LEO GER An oxidizing agent --

INTRODUCTION OF D-BLOCK ELEMENTS. Why are they called d-block elements? Their last electron enters the d-orbital.

Q5 from 5.3 Identify all the species in the table which could convert I–aq) into I2(aq) but which could not convert Br–(aq) into Br2(l).

LEO SAYS GER Textbook ch 4.4 Oxidation-Reduction Reactions “Redox” Unit 1: Chemistry Basics 1.42 Oxidation-Reduction Reactions “Redox”

1. OXIDATION REDUCTION (a) Addition of oxygen Removal of oxygen (b) Removal of hydrogen Addition of hydrogen (c) Loss of electron Gain of electron (d)

CHAPTER 5 ANALYSING OXIDANTS AND REDUCTANTS. REDOX REACTIONS Redox reactions involve complementary processes of oxidation and reduction, and can be identified.

Objective: Determine the equivalence point. Equivalence point n OH - = n H + If 25.00mL of M NaOH is needed to react with mL of HCl. What is.

Precipitation Titrations Dr. Riham Ali Hazzaa Analytical chemistry Petrochemical Engineering.

REDOX REACTIONS. OXIDATION NUMBER  The oxidation state of an element in an elemental state is zero. (O 2, Fe, He)  The oxidation state of an element.

OILRIG Oxidation is loss of electrons. Reduction is gaining electrons. REDOX – oxidation and reduction happening together. Example Mg(s) —> Mg 2+ (aq)

Redox Titrations. Oxidation-reduction reactions involve a transfer of electrons. The oxidising agent accepts electrons and the reducing agent gives electrons.

Study Guide, for Wed tutorial

Applications of Redox Electrochemistry. Review Oxidation reduction reactions involve a transfer of electrons. OIL-RIG Oxidation Involves Loss Reduction.

Transition metals Transition Metals Coloured Compounds Diagram 1 Absorption of light energy Diagram 2 Example: a blue coloured compound arises because:

Chapter 5 – Analysing Oxidants & Reductants Week 3, Lesson 1.

14 Redox Equilibria 14.1 Redox Equations (Review) 14.2 Electrode Potentials and the Electrochemical Series 14.3 Predicting the Direction of Redox Reactions.

Oxidation and Reduction By the end of this lesson, you should be able to: 1.State that a metal element reacting to form a compound is an example of oxidation.

Redox Calculations.

Oxidation states and half-equations

KNOCKHARDY PUBLISHING

Redox Reactions in Solution. Predicting Redox Rxns (The normal way) 1.Identify all the entities present in the solution 2.Decide which are oxidizing agents.

Chemistry NCEA L2 2.7 Redox 2013.

Lecture 19. The d-Block Elements. IV-VI B groups PhD. Halina Falfushynska.

R edox by ycs. Why Redox? Combination of two processes Reduction Oxidation.

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.

Analysing Oxidants and Reductants. What is a redox reaction? The reactant that loses electrons is oxidised Mnemonic devices OIL RIG O(xidation) I(s) L(oss.

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

OCR: Energetics, Equilibrium and Elements. Physical Properties  A transition metal is a d block element that has a partially filled d-subshell of electrons.

Acid Base Character of period 3

Chemistry 2.7 (AS 90306) Describe oxidation-reduction reactions Questions may involve any of the following: the properties of common oxidants and reductants,

Transition elements Introduction

2.7: Demonstrate understanding of oxidation-reduction

HC CHEMISTRY HC CHEMISTRY CHEMISTRY IN SOCIETY (E) CHEMICAL ANALYSIS.

Complexes and Coloured Ions

AH Chemistry – Unit 1 Transition Metals.

Chapter 6 OXIDATION & REDUCTION.

NCEA Chemistry 2.7 Redox AS

Do Now Knowing what you already know… write out the reaction between hexaaquachromium(III) ion and aqueous sodium hydroxide. Knowing what you already.

Ar 1s2 2s2 2p6 3s2 3p6 Energy 4p 3d 4s 3p 3s 2p 2s 1s

2Fe2O3 + 3C → 4Fe + 3CO2 The reactivity series

Transition elements Introduction

Chapter 5 – Analysing Oxidants & Reductants

LO: I know how to write redox equations.

Oxidation-Reduction Reactions “Redox”

Zinc and Scandium are not transition elements!

KNOCKHARDY PUBLISHING

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

Presentation transcript:

Starter 2. Complete the electronic arrangement of the Co 2 + ion. (1 mark) [Ar] 3. Explain why complex ions with partially filled d sub-levels are usually coloured. ( 2 marks) 4.What is meant by the term co-ordinate bond?

Starter 2. Complete the electronic arrangement of the Co2+ ion. (1 mark) [Ar]3d7 3. Explain why complex ions with partially filled d sub-levels are usually coloured. ( 2 marks) Electrons excited / transition from ground state to excited state (1) Energy absorbed from visible / light (spectrum) (1)

4.What is meant by the term co-ordinate bond? Shared or pair of electrons Come from one atom (1)

Variable oxidation states of transition metals. L.O.:  Determine the concentration of iron (II) ions in aqueous solutions.  Explain the conditions required to obtain Cr 2+. Homework: Q6 &7 from wiki

PSA10 part 1

TiScVCrMnFeCoNiCuZn

Fe(II) Iron exists in two common oxidation states, +2 (Fe 2+ ) and +3 (Fe 3+ ). In aqueous solution, the Fe is readily oxidized from Fe 2+ to Fe 3+ : Fe 2+ (aq)  Fe 3+ (aq) + e How could you determine the concentration of iron(II) in solution? Redox titration using Cr 2 O 7 2- Redox titration using MnO 4 -

Task: Write a balance equation for the reaction of acidified potassium dichromate(VI) with Fe(II)

Oxidation state ColourorangeGreenblue IonCr 2 O 7 2- Cr 3+ Cr 2+ Oxidation state +6+3 ColouryellowGreen IonCrO 4 2- Cr(OH) CrO 4 2- (aq) + 2H + (aq)  Cr 2 O 7 2- (aq) + H 2 O(l) Which Cr(VI) compound is more stable in acid?

Redox Chemistry of Cr Cr(III) is more stable than Cr(II) How could you oxidise Cr(II) to Cr(III)? By oxygen Which conditions are need for Zn to reduce Cr(III) to Cr(II)?

Describe what you would see, and explain the changes which occur when each of the following solutions is treated with an excess of zinc and hydrochloric acid in an apparatus which excludes air. a)Potassium Dichromate (VI) (5 marks) the Cr(VI) is reduced to +3 which is green and then +2 which is blue (5)

Variable oxidation states of transition metals. L.O.:  Determine the concentration of iron (II) ions in aqueous solutions.  Explain the conditions required to obtain Cr 2+. Homework: Q6 &7 from wiki

Why do oxidations of transition metals tend to happen in alkaline solutions?

In ammoniacal solution, Co2+ ions can be oxidised by oxygen in the air. Oxidation state +3+2 Colouryellowbrown IonCo(NH 3 ) 6 3+ Co(NH 3 ) 6 2+

5.4 EXERCISE 3 – Variable oxidation states and catalysis

Variable oxidation states of transition metals. L.O.:  How can the concentration of iron(II) ions in aqueous be found?  How can chromium (II) ions be oxidised?  How can cobalt(II) ions be oxidised?