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Some reactions involving iodine/iodide
Potassium iodide solution (right) is colourless. Here we are about to oxidise the iodide using orange bromine water. Oxidation of iodide
The orange colour of the bromine changes to the darker brown colour of iodine, I 2.
The brown colour of iodine in iodide is clearly seen in this beaker. Br 2 + 2e - → 2Br - 2I - → I 2 + 2e - Br 2 + 2I - → 2Br - + I 2 I 2 + I - → I 3 -
Reduction of iodine Iodine is a mild oxidising agent.
Colourless sodium thiosulfate solution will be used to reduce iodine to iodide.
As the thiosulfate solution is added, the brown colour begins to fade.
Almost all the iodine (I 2 ) has been reduced to iodide (I - ).
The final solution is completely colourless. I 2 + 2e - → 2I - 2S 2 O 3 2- → S 4 O 6 2- + 2e - I 2 + 2S 2 O 3 2- → 2I - + S 4 O 6 2-
SO 2 gas and BrO 3 -. Sulfur dioxide gas is generated by reacting dilute hydrochloric acid with solid sodium sulfite. 2HCl(aq) + Na 2 SO 3 (s) → SO 2.
Permanganate reactions. Manganese exists in many different oxidation states, each with a characteristic colour including: Mn VII: MnO 4 – purple Mn VI:
Iodimetry using iodate-thiosulfate
Unit 20 Oxidation and reduction Activity 20.1 Investigating redox reactions Reference in textbook: Section S.
Displacement of halogens
Lead dioxide and conc HCl. Lead dioxide, PbO 2, contains lead(IV). It is a strong oxidising agent. PbO 2 is very dark brown. “Red lead”, Pb 3 O 4, contains.
Alkaline permanganate and hydrogen sulfite
Reactivities of the group 7 elements (the halogens)
Balancing Redox Equations in Acidic Conditions
Unit 20 Oxidation and reduction Activity 20.2 Investigating redox reactions of aqueous chlorine Reference in textbook: Section S.
Group 7 – the halogens The elements in group 7 of the periodic table, on the right, are called the halogens. I Br Cl F At fluorine chlorine bromine iodine.
Redox reactions of the halogens
Chemistry Revision 3. Electronic configurations State which block in the periodic table you find the following elements: Sulphur Vanadium Strontium.
Copper sulfate solution and potassium iodide solution
R edox by ycs. Why Redox? Combination of two processes Reduction Oxidation.
Experiment 39: Analysis of Commercial Bleach Purpose Introduction: Many commercial products are effective because they contain oxidizing agents. Some products.
Oxidised state MnO 4 - Purple (aq) Permanganate Oxidised state Cr 2 O 7 2- Orange (aq) Dichromate Reduced state Cr 3+ Green (aq) Chromium ion Oxidised.
Oxidation of alcohols.
The effect of concentration on reaction rate
TOPIC 10 Making Electricity Making Electricity. A cell is an apparatus which generates electricity from a chemical reaction. A Battery is when two or.
LO: I understand which alkanols can be oxidised.
Determination of blood glucose Done by: Sahar Al-Subaie.
Qualitative organic analysis
All toxic All form Diatomic molecules All form ionic salts
2.7 Inorganic chemistry of group 7 (limited to chlorine, bromine and iodine) Cro2012.
Chemical tests for redox species. Test for SO 4 2–, the sulfate ion The sulfate ion is colourless.
Reactions of alcohols.
Manganate(V11) and Dichromate(V1) as oxidizing agents
What’s this? Gp2 NO3-& CO32- are more stable down group. MCO3->MO+CO2; 2M(NO3)2- >2MO+O2+4NO2. Gp1 CO32- stable, NO3-: 2MNO3->2MNO2+O2. Li like gp 2.
Permanganate and hydrogen peroxide. Hydrogen peroxide solution is colourless. Permanganate in neutral conditions.
This PowerPoint Will highlight the main chemical tests you MUST be familiar with before the observation exercise and then give you some examples to work.
Experiment 39: Analysis of Commercial Bleach
Chemistry NCEA L2 2.7 Redox 2013.
Experiment Questions Alcohol from Yeast.
Physical Properties colourless crystalline solid. soluble in water and is stable in cold but reacts with water when warmed. It decomposes easily in the.
Background The halogens, the group VII elements, are all oxidising agents as they tend to gain electrons to form halide ions. For example, chlorine tends.
Periodicity is a regular periodic variation of properties of elements with atomic number and positions in the periodic table.
A group of non metal elements
Oxidation of alcohols, aldehydes and ketones
9.2 Redox reactions.
Chemistry 2.7 (AS 90306) Describe oxidation-reduction reactions Questions may involve any of the following: the properties of common oxidants and reductants,
Study Guide, for Wed tutorial
Halogens AS. F Cl Br I (At) Generally: Oxidising agents Germicides Note: Atoms are halogens Ions are halides Ions have 8 electrons by borrowing one, so.
AG Oxidation Reduction Revision. AG Definitions Oxidation is addition of loss of increase in oxygen electrons oxidation number Exam Q (Hons) ‘13/Q10(b)
Telling a story…. We are going to take a written description about a chemical reaction and transfer it into a balanced chemical equation !
12 Chemistry 2.2 quantitative chemistry CR 07 Halogens: F 2, Cl 2, Br 2, I 2 Halogens as oxidants: Halogens attract electrons from other substances – they.
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