CHEMISTRY.docx

1、CHEMISTRYCHEMISTRY-For 2010 SAM Chapter 1 How to name the compounds 1.1 How to classify the matters 1.2 How to name the compounds 1.2.1 Nomenclature of the ions 1.2.2 Nomenclature of the ionic compounds 1.2.3 Nomenclature of the oxides 1.2.4 Nomenclature of the acids and bases1.1 How to classify the

2、 matters1.2 How to name the compounds 4.2.1 How to name the ions I Cations (positively charged particles) For a metal cation, the name is simply the name of the metal from which it is derived. Example: Na+ sodium Mg2+ magnesium Al3+ aluminium K+ potassium There are some situations, especially with t

3、he transition elements, where a metal can form more than one positive ion. To distinguish between the different cations, the charge on the ion is designated with a Roman numeral in brackets immediately following the name of the name of the ion. Example: Cu2+ copper (II) Fe3+ iron (III) Cu+ copper (I

4、) Fe 2+ iron (II) Pb2+ lead (II) Hg+ mercury (I) Pb4+ lead (IV) Hg2+mercury(II) Ni2+ nickel (II) Sn2+ tin (II) Ni3+ nickel (III) Sn4+ tin (IV)Exceptions: There are some exceptions, the positively charged particles are not formed from metal atoms. They have their own names as follows: NH4+ ammonium N

5、H3 ammonia H3O+ hydronium H2O hydrogen oxide (water)II Anions (negatively charged particles)1. Monatomic anions A monatomic anion exists as a single-atom ion which is derived from a non-metal atom by gaining electrons. Monatomic ions are named by adding -ide to the stem of the name of the non-metal

6、element from which it is derived. Example: F- fluoride fluorine Cl- chloride chlorine Br- bromide bromine I- iodide iodine N3- nitride nitrogen O2- oxide oxygen S2- sulfide sulfur2.Polyatomic anions Polyatomic anions are made from two or more non-metal atoms, especially ones containing oxygen (oxyan

7、ions).a. The ion with general No. of oxygen atoms is given the suffix -ate. NO3- nitrate SO42- sulfate CO32- carbonate PO43- phosphateb. The ion with the smaller No. of oxygen atoms is given the suffix -ite. NO2- nitrite SO32- sulfite c. The ion with the smallest No. of oxygen atoms has the prefix h

8、ypo- and the suffix -ite. ClO- hypochlorite ClO2- chlorite ClO3- chlorated. The ion with the largest No. of oxygen atoms has the prefix per- and the suffix -ate. ClO4- perchloratee. Oxyanions that contain hydrogen are named by using the word hydrogen as a prefix. The No. of hydrogen atoms is also in

9、dicated by di- for two, tri- for three, and so on. Example:HCO3- hydrogen carbonate /bicarbonateHSO4- hydrogen sulfateHSO3- hydrogen sulfiteHPO42- hydrogen phosphateH2PO4- dihydrogen phosphateExceptions:Cr2O72- dichromateMnO4- permanganateAlO2- aluminateZnO22- zincateName of the cations +name of the

10、 anionsExample:NaCl sodium chlorideCuSO4 copper (II) sulfateNote: Never forget the valence in the brackets for the cations have more than one oxidation states.I.Name the following compounds:CaSO4 ZnSLiFKIAl2O3(NH4)2SO4Ca(HCO3)2Fe2O3CuS2.Write formulae for the following compounds. a. calcium oxide b.

11、 iron (II) sulfide c. sodium bicarbonate d. aluminium chloride e. lithium hydride f. hydrogen chloride g. sulfur trioxide h. ammonia Na2O sodium oxide CuO copper (II) oxideNa2O2 sodium peroxideKO2 potassium superoxideP2O5 diphosphorus pentoxideNO nitrogen monoxide or nitric oxideCO carbon monoxide C

12、O2 carbon dioxideSiO2 silicon dioxide or silicaAl2O3 aluminium oxide or alumina I. Bases or Alkalis OH- hydroxide NaOH sodium hydroxide Fe(OH)2 iron(II) hydroxide II. Acids HCl(aq) hydrochloric acid H2SO4 sulfuric acid H2CO3 carbonic acid H2SO3 sulfurous acid HNO3 nitric acid HNO2 nitrous acid H3PO4

13、 phosphoric acid HClO4 perchloric acid II. Acids HCl(aq) hydrochloric acid H2SO4 sulfuric acid H2CO3 carbonic acid H2SO3 sulfurous acid HNO3 nitric acid HNO2 nitrous acid H3PO4 phosphoric acid HClO4 perchloric acidChapter 2 Experiment in the Lab2.1 Safety precautions2.2 Important instrument/apparatu

14、s2.3 Skills in the laboratory2.4 Present a lab report2.1.1 Safety precautions Follow teachers instructions Wear safety glasses Use protective clothing Do not attempt any unauthorised experiment Never point the test tube at your classmates faces Ask, if in doubt. It is common sense to check on a poin

15、t, not an admission of weakness. This rule must not be forgotten, no matter what the situation.2.1.2 General rules for school laboratory Wearing goggles & Lab coats Read the instructions Unauthorised experiments are forbidden Be safety conscious Plan your time carefully Be clean and tidy in your wor

16、k habits2.2 Important instrument/apparatus2.3 Skills in the laboratory :1. Keep the tip well below the surface of the solution in order to prevent entry of air. 2. Fill to a little above the calibration mark, and then close the end with the forefinger. Rotate the pipette gently against the forfinger

17、. 3. Stop when the bottom of the meniscus comes level with the mark, at eye level.Rinse the burette with correct liquidClamped in a vertical positionFilled using a funnel (not filled to zero each time)Appropriate manipulation of tapRemoving funnel from buretteNo splashingAppropriate amount of indica

18、tor in the conical flaskQ: How to rinse the pipette, burette How to rinse the conical flask, volumetric flask How to choose the indicators Exercise two: A solution of 0.10 mol L-1 potassium iodide with a volume of 10 mL is available. What volume of distilled water is required to obtain 0.0050 mol L-

19、1 of KI? A solution of calcium chloride, CaCl2, is made by dissolving 2.20 g of solid in a total solution volume of 250 mL. (a) calculate the concentration(浓度) of the solution (mol L-1 ) (b) how many mole of Cl- are present in 2.20 g of CaCl2?3. Look at the piece of glassware sketched below.(a) Name

20、 it(b) With what would you wash this item immediately before use?2.4 Present a lab report1.The report must have a well-planned structure: a title the aims Safety precautions the main body of procedures results discussion improvement conclusion 2. Use short sentences-got to the point.3. Make statemen

21、ts and conclusions are supported by data.4. Do not use the first person. (I and me)5. Use your own words. 6. Use tables, figures and graphs.7. Keep a written record of sources used in order that they can be acknowledged in the main body of the presentation or in the bibliography.Procedures: The mixt

22、ure was then distilled. The ester was collecting in three separate beakers from temperature 0 - 120C, 120 - 125C, and 125 - 130C. The first solution collected would have contained some butanol, while the ester in the last two beakers should have been pure. So this was done to guarantee the purest po

23、ssible ester. Uncertainty Systematic error Random errorSystematic error are recurrent errors inherent in the apparatus or experimental method used.Resources of systematic errorThey arise when:1. a measuring instrument is not calibrated is incorrectly calibrated;2. a piece of apparatus has an inheren

24、t fault. For example a polystyrene foam cup used for calorimetry experiments loses heat to the surroundings;3. contaminated standards are used in quantitative analysisFor a particular experiment, systematic errors are biased in one direction and cant be eliminated or reduced by repeating the procedu

25、re.Systematic errors are linked to the accuracy of measurement.A measurement is accurate to the extent that systematic errors have been minimized.Accuracy The accuracy of a measurement (or a series of measurements) indicates its relation to the true value.Random error are chance variations between s

26、uccessive measurements over which the experimenter has little or no control.Random errors are linked to the precision of the measurements. A measurement is precise to the extent that random errors have been minimized.Precision One measurement Resolution of the measuring instrument Several measuremen

27、ts Scatter of the data points Exercise three:The mass of an object was determined using a very precise balance to be 6.235 grams (the accepted value). Four students, each using a different balance, weighed the same object four times.The results (in grams) obtained by each student were follows, rate

28、the precision and accuracy of each students results as high or low:Exercise Four: An experiment was carried out in which 2.0 molL-1 HNO3 (nitric acid) was added to marble chips (CaCO3) in five separate flask. The temperature of the nitric acid and the volume of carbon dioxide (CO2) gas produced in 2

29、 minutes for each flask was recorded. The results of the experiment are given in the following table: b. (i) Name the glassware/apparatus used to measure the temperature change. (ii) Identify two variables that should be held constant in all five flasks.c. Graph the results of this experiment on the grid.Chapter 3 Organic Compounds3.1 General Instructions3.2 Systematic names of Hydrocarbons3.3 Nomenclature for Derivatives of hydrocarbons3.4 Type of reactions