CHEMISTRY(9-10)2010 1. What is the name of a naturally occurring unrefined petroleum product composed of hydrocarbon deposits and other organic materials? A. Kerosene B. Gasoline C. Crude oil D. Petroleum ether 2. What are the compositions of coal? It is mainly composed of A. Methane, ethane, propane, butane and small quantities of higher alkanes. B. Alkanes, cycloalkanes, and aromatic hydrocarbons. C. Element carbon, low percentage of solid, liquid and gaseous hydrocarbons. D. Low percentage of carbon, compounds of nitrogen and sulphur. 3. Industrially ethanol can be prepared by A. Dehydro halogenations of ethyl halide with KOH. B. Fermentation of carbohydrates such as sugar. C. The reaction between calcium carbide and water. D. The reaction between CH₃COONa and soda lime. 4. Which of the following is true about the homologous series? The homologous series is A. The existence of chemical compounds that have the same molecular formula but different structural formulas. B. A structure in which the isomers have different positions of groups with respect to the double bond. C. The property of an element to form chains with the repetition of the same atom. D. A group of molecules each differing from the next member by a certain group. 5. In which solvent will both alkenes and alknes dissolve? A. Alcohols B. Acetic acid C. Water D. Benzene 6. What is the molecular formula for butanal? A. C₄H₈O₂ B. C₄H₉O₂ C. C₄H₈O D. C₄H₁₀O 7. What are oxides? They are A. Base anhydrides that react with water to form bases. B. Binary compounds that contain oxygen in the -2 oxidation state. C. Acid anhydrides that react with water to from acids. D. Substances that have the link –O-O- 8. Which of the following is NOT true about the chemical property of acid anhydrides? They react with A. Both acids and bases to form salt and water. B. Basic oxides to give salts. C. Water to from acids. D. Bases to form salt and water. 9. Amphoteric oxides A. Can be represented by CuO, FeO, Fe2O, and Cr2O3 B. Are all non-metallic oxides. C. Have neither acidic nor basic properties. D. Have both acidic and basic properties. 10. Oxides that have neither acidic nor basic properties are____ A. Amphotheric B. Neutral C. Acidic D. Basic 11. The spatial arrangement of atoms or groups about a double bond is known as ___isomerism. A. Chain B. Functional C. Geometrical D. Position 12. What is the addition product formed when a mixture of benzene vapor and hydrogen is passed over finely divided nickel catalyst at 200 C? A. C₆H₁₄ B. C₆H₁₂ C. C₆H₁₀ D. C₆H₁₃ 13. A student took three different test tubes and added 5 ml of toluene (methylbenzene) to each test tube. Then, added 2 drops of Br2 in CC14 in the 1st test tuve, 2 drops of KMnO4 in the 2nd test tube and 2 drops of concentrated H2SO4 in the 3rd test tube. In which test tube does a reaction occur? In the_____ test tube(s). A. 1st and 3rd B. 1st, 2nd and 3rd C. 2nd D. 3rd 14. Natural gas is mainly composed of A. Gases such as oxygen and hydrogen disulphide. B. Methane gas. C. All hydrocarbons. D. Gases such as carbon dioxide and nitrogen. 15. Which of the following information can easily be obtained by just looking at the periodic table? A. Number of shells of an element. B. Number of valence electrons(s) of an element. C. Nature of the oxides of the elements. D. Names, and symbols of the elements. 16. Why atoms form a chemical bond? To A. Transfer one or more electrons. B. Share one or more electrons. C. Attains a state of higher potential energy. D. Achive noble gas electronic configuration. 17. Which of the following statement is true? A. Matals tend to gain electrons to form positively charged ions or cations. B. Non-metals tend to lose electrons to form negatively charged ions or anions. C. Group VIA elements form ions of the type X by losing 2 electrons. D. Group VA elements form ions of the type X by gaining 3 electrons. 18. What is an ionic bond? It is A. A bond whose formation is favored by high ionization energy and low electron affinity of the combining elements. B. A force of attraction between oppositely charged ions. C. A bond whose formation is favored by low ionization energy and low electron affinity of the combining elements. D. A force of attraction between positively charge nuclei of atoms and the shared electrons 19. Which of the following is NOT the postulate of modern atomic theory? Atoms A. of the same element have identical chemical properties. B. of different element have different chemical properties. C. are the smallest particles of elements D. are indivisible and indestructible. 20. One of the following statements is accepted by both Dalton’s and Modern atomic theories. Which one is it? A. All elements are made up of very small particles called atoms. B. Atoms of a given element are identical in mass. C. Atoms of the same element may not be exactly alike. D. An atom can be further subdivided into electrons, protons, and neutrons. 21. The existence of neutrons was discovered by A. Emest Rutherford. B. Robert Millikan. C. James Chadwick. D. Joseph John Thomson. 22. What is the relative electric charge of an electron? A. -1 B. +16 x 10⁻¹⁹C C. +1 D. -1.6 x 10⁻¹⁹C 23. Which of the following is true about the properties of ionic compounds? They A. Have crystalline nature. B. Are insoluble in polar solvents like water. C. Have low melting and boiling points. D. Conduct electricity in solid state. 24. A bond formed when atoms in a molecule share electron pairs is ____ A. Coordinate covalent B. Metallic C. Ionic D. Covalent 25. The inter – molecular attraction between a partially positive hydrogen atom in one molecule and the partially negative atom in another molecule is A. Van der waals force B. Hydrogen bonding C. London force. D. Dispersion force. 26. The statement ‘’Matter is neither created nor destroyed during a chemical reaction.’’ is the law of A. Conservation of mass. B. Definite proportion C. Multiple proportions. D. Constant composition. 27. The quantum mechanical description for the arrangement of electrons of an atom in atomic orbitals in order of increasing energy is known as _____ A. Valence shell B. Valence electron C. Electronic configuration D. Diagonal rule 28. The common name for group VIIA elements is A. Noble gases. B. Halogens C. Alkali metals. D. Alkaline earth metals. 29. What is the number of groups and periods in the modern periodic table respectively? A. 7, 18 B. 7, 16 C. 18, 7 D. 16, 7 30. Which of the following is NOT the industrial application of electrolysis? A. Production of non-metals. B. Purification of metals. C. Purification of non-metals. D. Production of metals. 31. Natural resources are A. Chemicals that are obtained from the industries. B. Organic chemicals that used to prepare a huge range of agricultural products. C. Minerals nutrients those are important in plant growth. D. Materials those are available on earth for people to use. 32. Which one of the following natural resources is renewable? A. Petroleum B. Water C. Coal D. Natural gas 33. Which of the following is NOT the general characteristic of industries? They A. Use large amounts of energy in their manufacturing process. B. Test their products during and after manufacturing in their quality control laboratories. C. Involve mostly chemical processes to transform the raw materials to the desired products. D. Use synthetic materials as raw materials for the production process 34. Which step in the manufacturing of pulp and paper is used to remove coloring matter from wood pulp? A. Kraft process B. Bleaching C. Pulping D. Sulphite process 35. What is the negative logarithm of hydrogen (hydronium) ion concentration? A. pH B. pKa C. pOH D. pKw 36. What is a strong base? It is a base that A. Contains relatively large amount of solute in a given volume of solution. B. Contains only a small amount of solute in a given volume of solution. C. Ionizes partially or slightly in aqueous solution. D. Ionizes completely or almost completely in aqueous solution 37. Of the following methods, which one is a traditional food preservation method? A. Vacuum packing B. Freeze drying C. Salting D. Freezing 38. Which of the following pollution is NOT common? A. Sound B. Air C. Water D. Land 39. Which of the following method can be used to reduce water pollution? A. Lowing temperature furnaces and engines that reduce the amount of nitrogen oxides produces. B. Banning of CFCs aerosol propellant gases to be replaced by less harmful alternatives. C. Using moderate amounts of agricultural non-degradable materials. D. Burning or recycling plastics and other non-degradable materials. 40. Converting potentially dangerous chemical wastes into harmless substances, by combustion or by other chemicals means is one the main methods used to reduce A. Air solution. B. Sound pollution. C. Water pollution. D. Land pollution. 41. Suppose that our teacher gave you a chance to visit a nearby cement industry. After the visit, you are expected to write a report about its environmental impact. What will be your main concern in your report? A. How the production efficiency could be enhanced B. How the environment is affected by the industry C. What raw materials are used D. What the industry does 42. What is the function of phosphorus in the growth of plants? It is used A. Fo active enzymes in photosynthesis. B. For the synthesis of chlorophyll. C. For the synthesis of amino acids. D. To form nucleic acids. 43. What is the difference between metallic and electrolytic conductivity? A. In metallic conduction new substance is produced. B. Conductivity of electricity by electrolytic conductivity is a simple physical change. C. In metallic conduction there is net movement of the metal atoms. D. In electrolytic conduction the charge carriers are positive and negative ions. 44. Electrolysis is a A. Process in which electrical energy is used to produce chemical changes. B. Process which consists of two electrodes inside the cell. C. Process in which there is a selection of the electrodes for one kind of ion. D. System consisting of electrodes that dips into an electrolyte and in which chemical reaction generates electrical energy. 45. The strips of metals or graphite that allow electrons to leave or enter the electrolyte are known as ._____ A. anions B. electodes C. charge carriers D. cations 46. Which one of the following statements is rue about electrolytic and galvanic cells? A. In electrolytic cells, elections flow anode to cathode where as in voltaic cells from cathode to anode. B. In electrolytic cells, chemical reaction generate electricity where as in voltaic cells electricity brings about chemical reactions C. In both electrochemical cells, anode is positive and cathode is negative. D. In both electrochemical cells, oxidation takes place at anode and reduction takes place at cathode. 47. Which one of the following statements is true about electrolytic and galvanic cells? A. In electrolytic cells, electrons flow anode to cathode where as in voltaic cells from cathode to anode. B. In electrolytic cells, chemical reactions generate electricity where as in voltaic cell electricity brings about chemical reactions C. In both electrochemical cells, anode is positive and cathode is negative. D. In both electrochemical cells, oxidation takes place at anode and reaction takes place at cathode. 48. Why does an increase in temperature affect the rate of a reaction? Because, reactant molecules collide A. More frequently with greater energy. B. Less frequently with greater energy. C. More frequently with less energy. D. Less frequently with less energy. 49. Consider the following reaction that takes place inside a sealed reaction chamber. 2KC1O3(s) →2KC1(s) + O2(g) A. Which of the following will NOT increase the rate of reaction? B. Decreasing the pressure. C. Increasing the amount of KCIO3 D. Increasing the temperature. 50. Reactions which can take place in both forward and backward directions are called ___ A. One – way B. Reversible C. Irreversible D. Equilibrium 51. According to the kinetic molecular theory, A. Gases do not diffuse spontaneously into each other. B. It is assumed that there is a strong attractive force between the gas molecules, because gas molecules are very close to each other. C. Molecules in a gas have different velocity with different kinetic energies. D. Gases are denser than solids and liquids. 52. The following equation represents the oxidation of a ammonia. NH3 + O2 →NO + H2O A. 4, 5, 4, and 6 B. 4, 6, 4, and 5 C. 2, 2, 2 and 6 D. 6, 2, 2 and 2 53. In an endothermic reaction A. The value of H is negative. B. Heat is released to the surroundings. C. Heat is absorbed from the surroundings. D. The internal energy of the reactants is more than the internal energy of the products. 54. Charles’ law states that A. The volume of a fixed mass of a gas at a constant pressure is directly proportional to the temperature measured on the Kelvin scale. B. Equal volumes of all gases, measured at the same temperature and pressure contain equal number of molecules. C. The volume of a fixed mass of a gas is inversely proportional to its pressure when temperature is kept constant. D. At constant volume, the pressure of a given mass of gas is directly proportional to the Kelvin temperature 55. The migration or intermingling of molecules of different gases as a result of random molecular motion is known as ______ A. Convection B. Diffusion C. Evaporation D. Osmosis 56. The evaporation of a liquid depends on A. Surface area. B. Catalysts. C. Concentration. D. Volume. 57. How do you define oxidation in terms of electron transfer? It is the A. Process whereby electrons are removed from atoms or ions. B. Process were by electrons are added to atoms or ions. C. Combining of oxygen with other substances or the addition of oxygen to substances. D. Process in which there is a decrease in the oxidation number of an element 58. Which one of the following statements is true about oxidizing and reducing agents? A. An oxidizing agent causes reduction to occur. B. A reducing agent gains electrons(s). C. A reducing agent is reduced. D. An oxidizing agent gains electron(s). Loading … Question 1 of 58
