The Chemistry Examination of the College Entrance Examination Board

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The Chemistry Examination of the College Entrance Examination Board

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HE September, 1940, issue of the JOURNAL OF be more effectively taught if the instructor is given CHEMICAL EDUCATION contained the chemistry greater latitude in the selection of topics. svllabus urouosed bv the Colleee Entrance ExThe svllabus is divided into two sections: amination ~;ar;l's ~okmissionon Examinations in (1) a minimum syllabus, Part One and Part Two; Physics and Chemistry, and suggestions and criticisms (2) an extension syllabus, Part Three, which is subwere invited. The membership of the Commission divided into follows: (a) commercial chemistry, Dean John T. Tate, University of Minnesota (Chair(b) theoretical chemistry, and man) (c) . . orpanic chemistry. ~ o c t o rOtis E. Alley, Hixh - School, Winchester, Candidates will be examined on the minimum syllaMassachusetts bus only. Quantitative problems may be set upon Dean Janet H. Clark, University of Rochester those topics marked with an asterisk (*). Doctor Curtiss S. -Hitchcock. Lawrenceville School. In order that the objectives of the course of study Lawrenceville, New Jersey may be fully realized, it is essential that the study of Mr. John C. H o x ~Phillips , Exeter Academy, Exeter, chemistry be accompanied by individual laboratory ~ e ~wa m ~ s h i r ; work as well as by class demonstrations. The laboraProfessor Erwin B. Kelsey, Yale University tory work should occupy approximately one-third of Mr. Alfred R. Lincoln. Technical Hieh School. the time devoted to chemistry and it should continue Springfield, ~assachnsetts throughout the whole course. The need for accurate Professor Duane E. Roller, Hunter College observation and the relation between observation and Professor Francis W. Sears, Massachusetts Institute conclusion should be stressed. A list of experiments is of Technology not submitted as it is believed that the expe>ments will Professor Mary L. S h e d , Mount Holyoke College need to be varied according to the facilities of a particuMr. Howard A. Taber, Hotchkiss School, Lakeville, lar institution. The arrangement of the syllabus dws Connecticut not imulv a teachine sequence. The suggestions received were given careful conPART ONE-ENERAL CHEMISTRY sideration and many have been incorporated in the following syllabus which has been adopted as the basis for I. Chemical Changes. the chemistry examinations to be set by the College A. Element, compound, mixture. Entrance Examination Board in 1942 and thereafter. 1. Chemical change versus physical change. Teachers will note, however, that the main topics re2. Significance of t e r m s a t o m , molecule, main unaltered. This syllabus will be of special interradical. est to teachers whose pupils will take the Board's 3. Types of chemical reactions. examination in chemistry in June, 1942. 4. Electrochemical series of the common metalslimited to displacement reacREVISION OP C E E M I S ~ Y REQUIREMENT-JUNE 16, 1941 tions. The following suggested redefinition of the requireB. Balancing of equations. ment in chemistry indicates the nature and extent of the *C. Quantitative relationship in chemical reacbasic preparation considered necessary for college work. tions. 1. Signiiicance of symbol, formula, equaI t is estimated that from two-thirds to four-fifths of the school year will be required to cover the basic topics tion, atomic and molecular weights. suggested in the minimum syllabus given in Part One 2. Laws of combining proportion: and Part Two. Part Three is intended to show how (a) Conservation of Mass. the basic material of Parts One and Two can be ampli(b) Constant Proportions. fied. Additional spe&c material designed to meet the ( 6 ) Multiple Proportions. needs of the community and adapted to the level of the 3. Percentage composition. student body should also serve to enrich the basic 4. Problems based on chemical equations: course. Questions on topics beyond this suggested area (a) Wight relationships. will not be included since it is felt that the science will (b) Volume relationships of gases. 441

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Neutralization (quantitative). (a) Equivalent weights. (b) Molar solutions. (c) Normal solutions. 11. Physical Properties of Solids, Liquids, and Gases. A. 1. Kinetic molecular theorv-relation between temperature and speed of molecules. Differences between solids, liquids, and gases from kinetic molecular I viewpoint. 2. Factors which influence rate of reaction (concentration, temperature, catalyst. and state of division). 3. Equilibrium, mass action law, and principle of Le Chatelier as applied to gaseous reactions. *B. Gases. 1. The tempemhue, pressure, and volume relations. Explanation in terms of the kinetic theory. 2. Partial pressures of gases in a mixturerelated only to the vapor pressure of water. 3. Reduction to standard conditions (mcluding vapor pressure of water). 4. Avogadro's Principle. The relation of gram molecular volume, density, and molecular weight. 111. Periodic Law. Brief treatment giving variation in properties of the elements as illustrated in the halogen family and horizontally by argon through chlorine. Anomalies. IV. Theory of Atomic Structure. A. Dalton's Atomic Theory. B. Modem atomic theory. 1. units of structure. Proton, neutron, electron, characterization as to mass and charge. 2. Atomic number. Nuclear charge and arrangement of electrons (hydrogen through calcium). Isotope (hydrogen, chlorine). 3. Explanation of periodicity in properties of elements in terms of atomic struc5.

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4. Ionic valence and its relationship to inert gas structure.

5. Chemical combination explained in terms of atomic structure. (a) Electrovslence - combmation and displacement;reactions in terms of electron transfer (oxidation and reduction). (b) Covalencesharing of electrons in the formation of unionized molecules. V. Electrolytes. A. 1. Physical evidence of dissociation in fused salts and bases and in water solution.

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2. Comparison of properties of electrolytes and non-electrolytes in water solution. Complete dissociation of salts and strong bases. Ionization. 1. Ionization of acids by reaction with water. 2. Degree of ionization of weak acids and weak bases--ionic equilibrium. 3. Common ion effect as applied to weak electrolytes. Completion of ionic reactions by: 1. Formation of a slightly ionized product. 2. Formation of an insoluble gaa or solid. Hydrolysis of salts (reaction of ions with water). Electrolysis of water solutions. PART TW-DESCRIPTIVE

CHEMISTRY

In general, the study of any element should be developed in the following sequence: history, occurrence, preparation (most important laboratory and commercial methods), properties (physical and chemical), uses, and identification. Historical treatment should be limited to cases where it offers a sound teaching approach and where it is of particular signi5cance in the study of an element; for example, as an introduction to oxygen and hydrogen. Similarly, the study of the important compounds of the elements should include preparation, properties (physical and chemical), uses, and identification. As illustrative of a typical study of an element and its important compounds, the topic Nitrogen is given in expanded form at the end of Part Two. I. Chemistry of Some Non-Metals and Their Common Compounds. A. Oxygen. B. Hydrogen. C. Water. 1. Composition by weight and volume. 2. Purification (atration and distillation). 3. Chemical reactions: (a) With o x i d e b a s i s of classification of metals and non-metals. (b) With salts to form hydrates. Efflorescence. (c) Test for presence of water. 4. Solutions: (a) Significance of termssaturated, unsaturated. (b) Interpretation of solubility curves. D. Carbou (allotropes). 1. Carbon dioxide and carbonic acid; types of carbonates; test for a carbonate. 2. Carbou monoxide. E. Halogen family. 1. Chlorine;, hydrogen chloride and hydrochloric acid; hypochlorous acid. 2. Bromine, iodine, fluorine, and the hydro-

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gen compounds as compared with chlorine and hydrogen chloride. 3. Tests for chloride, bromide, and iodide ions. 4. Displacement reactions. F. Sulfur. 1. Hydrogen sulfide, sulfides. 2. Sulfur dioxide--sulfurous acid, sulfites, bisulfites. 3. Sulfur trioxide (Contact process)sulfnric acid, sulfates, bisulfates. 4. Tests for sulfide, sulfite, and sulfate ions. G. The atmosphere. 1. Air as a mixture. 2. Nitrogen and the rare gases. H. Nitrogen compounds. 1. Ammonia-test for ammonium ion. 2. Oxides of nitrogen-nitric oxide and nitrogen dioxide. 3. Nitric acid. 4. Test for a nitrate ion. 11. Chemistry of a Metal and Its Typical Compounds. Sodium and its compounds. 1. Sodium hydroxide. 2. Sodium chloride. 3, sodium and sodium bicarbonate (Solvay process). 4. Sodium nitrate. 5. Sodium hypochlorite. 111. Nitrogen (Outlined in expanded form for illnstrative purposes). A. History. B. Occurrence. C. Preparation. 1. Atmospheric nitrogen 2. Pure nitrogen. D. Properties. 1. Physical. 2. Chemical. E. Uses. F. Compounds. 1. Ammonia. (a) Laboratory preparation. (b) Commercial preparation. (1) Synthetic (Haber). (2) Cyanamid. (3) Distillation of coal. (c) Ammonium compounds. (d) Test for ammonium ion. 2. Oxides of nitrogen. (a) Nitric oxide. (1) Preparation by: (a) oxidation of ammonia (Ostwald), (b) reduction of nitric acid. (2) Identification.

(b) Nitrogen dioxide. (1) Preparation by: (a) oxidation of nitric oxide, (b) reduction of nitric acid, (6) heating of nitrates. (2) Identification. 3. Nitric acid. (a) Preparation. (1) Laboratory. (2) Commercial: oxidation of ammonia (Ostwald); from sodium nitrate. (b) Properties. (1) Physical. (2) Chemical. (a) Reaction of concentrated and dilute acid on : (i) metals, (ii) non-metals, (iii) salts. (6) Test for nitrate ion. 4. Uses of nitrogen compounds. G. Nitrogen Cycle. PART THREE-EXTENSIONS

Parts One and Two give the basic material for preparation for college work. I t is recommended that the basic material be supplemented by topics from Part Three and also by various items of current and local interest. I. Commeraal Chemistry. A. Chemistry of four metals and their common compounds: aluminum, iron, zinc, and copPer. 1. Occurrence and extraction of these four elements from their ores. 2. Simple reactions of these elements and identification of their ions. B. Fuels. 1. Coal gas, producer gas, water gas. 2. Acetylene. 3. Petroleum and natural gas; distillation and cracking process. 11. Theoretical Chemistry. A. Distinction between a proton and the hydrated hydrogen ion (hydronium ion). B. Laboratory determination of: 1. Equivalent weight. 2. Molecular weight. 111. Organic Chemistry. A. Simple organic reactions. B. Foods. 1. Components, carbohydrates, fats, proteins, vitamins. 2. Hydrolysis. Uses of starch and sugar. 3. Fermentation.