solvolysis reaction using ethanol. The concerted bimolecular reaction has no intermediate. The reaction is promoted by the use of a polar aprotic solvent and requires the presence of a strong nucleophile. For this experiment‚ you will use sodium iodide (NaI) in acetone. You will test nine substrates (Figure 1) under each of these two reaction conditions to see which compounds will do SN1‚ SN2‚ neither reaction or both. You will observe the formation of a precipitate upon reaction. For the SN2
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1. (a)Correct the following statements. (i) The melting points of crystalline and amorphous solids are not definite. The melting point of an amorphous solid is not definite. OR The melting point of a crystalline solid is definite. P Ps X solute . Ps P Ps The equation for relative lowering of vapour pressure when solute remains normal is X solute P (iii)The degree of ionization decreases with dilution. The degree of ionisation increases with dilution. (iv) Tertiary butyl halide
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due to their loosely packed metallic lattices. 6. Alkali metals‚ except lithium‚ show photoelectric effect. Due to small size and high ionization enthalpy‚ the electrons of lithium cannot be emitted. 7. Alkali metals do not form dipositive ions because of their very high second ionization enthalpies. 8. All alkali metals are paramagnetic but their salts are diamagnetic. 9. Alkali metals impart characteristic colors to the flame‚ i.e.‚ lithium imparts crimson red‚ sodium imparts golden
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Experiment #9 – Identification of Aldehydes and Ketones Introduction Aldehydes and ketones share the carbonyl functional group which features carbon doubly bonded to oxygen. In the case of ketones there are two carbon atoms bonded to the carbonyl carbon and no hydrogens. In the case of aldehydes there is at least one hydrogen bonded to the carbonyl carbon; the other attachment may be to a carbon or a hydrogen. In all cases the carbon(s) that are attached to the carbonyl group may be aliphatic (not
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oxides of nitrogen on reacting with metals while other acids react with metals to evolve hydrogen. xxii) Burning magnesium continues to burn in nitric oxide while burning Sulphur extinguishes. xxiii) Phosphorous does not form phosphorous penta-iodide. xxiv) Phosphorous acid is a dibasic acid. xxv) (SiH3)3N is a weaker base than (CH3)3N. xxvi) Mg3N2 when reacted with water gives off NH3 but HCl is not obtained from MgCl2 on reaction
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Kinetics of a Reaction I. List of reagents & products 1. 1.0 M Copper(II) nitrate (Cu(NO3)2‚ 0.10 M Hydrochloric Acid (HCl)‚ 0.010 M Potassium Iodide (KI)‚ 0.040 M Potassium Bromate (KBrO3)‚ 0.0010 M Sodium Thiosulfate (N2S2O3)‚ 2% Starch solution‚ Water (H2O) II. Summary of Procedure. Part 1: Find the Volume of One Drop of Solution 2. Fill pipet with 3ml of distilled water 3. Mass a beaker and record 4. Put 5 drops of water into beaker and record
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zinc and iodine‚ and comparing their total to the mass of the zinc iodide product plus the excess zinc. The total mass of the reactants was determined by subtracting the mass of the empty beaker from the mass of the beaker with initial amounts of zinc and iodine in it. The mass of the reactants was 5.266g. The mass of the products was obtained by adding the mass of zinc iodide with the mass of the excess zinc. The mass of zinc iodide was 2.412g. The mass of excess zinc was 2.695g. 2.142g was then added
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other (groups of twos) in test tubes to test which reaction will result in an insoluble solid. See method for more detail. It is expected that the following compounds will form precipitates Silver Sulphate‚ Copper Hydroxide‚ Copper Iodide‚ Silver Hydroxide‚ Silver Iodide‚ Cobalt Hydroxide and two Silver Chlorides. This was worked out by completing the double displacement reactions and using a table of solubilities. (See appendix one & two) In any experiment involving chemicals a hard wearing plastic
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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
Free Atom Electron Chemical bond
with the sample under controlled conditions. The quantity of oxidant consumed is expressed in terms of its oxygen equivalence. Because of its unique chemical properties‚ the dichromate ion (Cr2O72–) is the specified oxidant in Methods Section 5220B‚ Section 5220C‚ and Section 5220D; it is reduced to the chromic ion (Cr3+) in these tests. Both organic and inorganic components of a sample are subject to oxidation‚ but in most cases the organic component predominates and is of the greater interest. If
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