as proteins and polysaccharides(starch) that have dimensions significantly greater than the pore diameter of the dialysis tubing can pass through the tubings and they are retained inside the tubings.Smaller molecules such as water molecules and iodide ions are small enough to pass through the pores. The left-handed dialysis tubing contains 20%sucrose and iodine solution .The right-handed dialysis tubing contained 5% starch solution . The two entire dialysis tubings are submerged in distilled water
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and water .................. (e) zinc sulfate crystals from aqueous zinc sulfate .................. (f) hexane from a mixture of the liquids‚ hexane and octane .................. [1] [1] [1] [1] [1] [1] [Total: 6] 2 Selenium and sulfur are in Group VI. They have similar properties. (a) One of the main uses of selenium is in photoelectric cells. These cells can change light into electrical energy. (i) Name a process which can change light into chemical energy.
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Edexel IGCSE Chemistry Revision Notes IGCSE Chemistry Triple Award Revision Guide Topic Introduction to chemistry Atomic Structure Structure and Bonding – Ionic Bonding Structure and Bonding – Covalent and Metallic Bonding Organic Chemistry - Alkanes Organic Chemistry – Alkenes / Addition Polymerisation Organic Chemistry – Alcohols / Condensation Polymerisation Calculations Periodic Table Reactivity Series and Metal Extraction Electrolysis Energetics Acids‚ Bases‚ Salts and Neutralisation Preparing
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Applications of Le Châtelier’s Principle (September 11 - 15‚ 2014) **The purpose of this experiment was to visually observe the effects of how changing certain aspects of the reaction affected the observed equilibrium. PROCEDURE: Introductory activity Part A: Effect of Concentration: Two different temperature water baths were created‚ one at 65-70oC‚ the other ice‚ and set aside for Part B. 20 mL of potassium thiocyanate solution were poured into a petri dish. The initial color and all subsequent
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Purpose: • To study some of the physical properties of two types of solids – ionic and molecular solids. • To classify three unknown substances as ionic compounds‚ polar covalent compounds or non-polar covalent compounds. • To identify the three unknowns. Observations: A B C Solubility in: • H2O • 2-Propanol Soluble Insoluble Soluble Insoluble Insoluble Soluble Conductivity None High None Melting Point 100 – 525 ℃ > 525 ℃ < 100 ℃ Odour Subtle None Very Strong Concluding
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Periodic Table Trends: Atomic Radius - half of the distance between the centers of two atoms that are touching each other decreases moving left to right increases moving top to bottom Ionization Energy - energy required to remove an electron increases moving left to right decreases moving top to bottom Electron Affinity - ability to accept an electron alkaline earth elements have low electron affinities halogens have high electron affinities noble gases have electron affinities near zero
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Salts 1. Salts A salt is an ionic compound. The anion part comes from the acid while the cation part comes from a base. Example: KCl‚ KOH(aq) + HCl(aq) KCl(aq) + H2O(l) A salt is a compound formed when the hydrogen ion. H+ from an acid is replaced by a metal ion or an ammonium ion‚ NH4+. Salts Nitrate salts Carbonate salts Chloride salts Soluble All nitrate salts Potassium carbonate‚ K2CO3 Ammonium carbonate‚ (NH4)2CO3 Sodium carbonate‚ Na2CO3 All chloride salts Except Sulphate salts All sulphate
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Through an oxidation reaction of synthesizing pentaaminechloridocobalt (III) chloride with cobalt (II) hexahydrate and hydrogen peroxide‚ and then reacting the product with ammonium chloride and ammonia‚ complexes are formed with the chloride and ammonia ions. The balanced
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Hwa Chong Institution (High School) Secondary 4 End of Year Examinations Chemistry Revision Notes List of topics: 1. Atomic Structure 2. Separation Techniques 3. Chemical Bonds and Bonding (Ionic‚ Covalent) 4. Metals 5. Properties and structures of compounds 6. Qualitative Analysis 7. Acids‚ Bases and Salts 8. Chemical Periodicity 9. Chemical Calculations 10. Air and Environment 11. Electrochemistry (Including Redox reactions) 12. Thermochemistry 13. Rates of Reaction 14. Chemical
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Writing ionic equations for redox reactions You can split the ionic equation into two parts‚ and look at it from the point of view of the magnesium and of the copper(II) ions separately. This shows clearly that the magnesium has lost two electrons‚ and the copper(II) ions have gained them. These two equations are described as "electron-half-equations" or "half-equations" or "ionic-half-equations" or "half-reactions" - lots of variations all meaning exactly the same thing! Any redox reaction
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