Basic Science Exam #21. The modern periodic law states that the properties of the elements are a periodic functionof their(1)(2)(3)(4)Atomic weightatomic mass;Atomic numberIsotope number2. Mendeleev’s periodic law stated that the properties of the elements are a periodic functionof their(1) atomic mass;(2) atomic weight(3) atomic number;(4) isotope number;(5) isotope mass number3. Which of the following elements would have the largest atoms(1) Os;(2) Fe;(3) Ni;(4) As.4. Elements in the same period generally have(1) similar chemical properties;(2) the same number of electrons in the outer major energy level;(3) similar physical properties;(4) both 1 and 2;(5) both 1 and 3;(6) all of the above;(7) none of the above.5. Elements in the same group generally show(1) decreasing size with increasing atomic number;(2) increasing size with increasing atomic number;(3) increasing ionization potential with increasing atomic number;(4) decreasing ionization potential with increasing atomic number;(5) both 1 and 3; (6) both 2 and 4;(7) none of the above.6. Which of the following would be most reactive toward fluorine?(1) K;(2) Ca;(3) Sc;(4) Co.7. Elements in the same period generally show(1) decreasing size with increasing atomic number;(2) increasing size with increasing atomic number;(3) increasing ionization potential with increasing atomic number;(4) decreasing ionization potential with increasing atomic number;(5) both 2 and 4; (1 2) both 1 and 3.8. Which of the following elements would have the lowest ionization potential?(1) Ir;(2) Pt;(3) Pb;(4) Ni;(5) Co.9. Which of the following elements would be the most reactive toward sodium?(1) O;(2) S;(3) Se;(4) Te.10. What type of element would you predict element 117 to be?(1) nonmetal;(2) metal;(3) noble gas;(4) alkali element;(5) metalloid. 11. Which of the following elements is an alkali metal?(1) fluorine;(2) oxygen;(3) nitrogen;(4) carbon;(5) boron;(6) beryllium;(7) lithium;(8) iron;(9) none of the above.12. Which of the elements in question 11 is a halogen?13. Which of the elements in question 11 is an alkaline earth element?14. Which of the following elements is most reactive toward chlorine?(1) Al;(2) Mg;(3) Ca;(4) Sr;(5) Y15. Which of the following elements are most reactive toward sodium?(1) Te;(2) I;(3) Br;(4) Cl;(5) S.16. Which of the following pairs of elements will not form ionic compounds?(1) sulfur and oxygen;(2) sodium and calcium;(3) sodium and sulfur;(4) barium and chlorine. 17. Which of the following bonds would be covalent but not polar covalent that is a non-polarcovalent bond?(1) Al–S;(2) Ge–As;(3) K–F;(4) N–O.18. Electronegativity is a measure of(1) an atom’s ability to pull protons to itself;(2) an atom’s ability to form ionic bonds;(3) an atom’s ability to form covalent bonds;(4) an atom’s ability to pull bonded electrons to itself.19. Which of the following compounds would most likely contain bonds formed by the sharingof electrons?(1) MgO;(2) NO220. The independent variable in an experiment is:a)b)c)d)The variable you hope to observe in an experiment.The variable you change in an experiment.The variable that isn’t changed in an experiment.none of these is correct21. “Qualitative results” refer to:a) Results that can be observed during an experiment.b) Results that are difficult to observe during an experiment.c) Results that require numerical data.d) none of these is correct.22. When drawing a graph that measures family average income over a period of 50 years the independent variable is:a) Incomeb) Averagec) Yearsd) It is impossible to say23. Accuracy is defined as:a) A measure of how often an experimental value can be repeated.b) The closeness of a measured value to the real value.c) The number of significant figures used in a measurement.d) None of these24. How many significant figures are present in the number 10 450?a) threeb) fourc) fived) none of these 25. What is the appropriate SI unit for distance?a) centimetersb) inchesc) metersd) kilometers26. How many decimeters are there in 15 centimeters?a) 150 dmb) 1.5 dmc) 0.15 dmd) none of these27. How many kilograms are there in 4.21 pounds? There are 2.2 pounds in 1 kilogram.a) 9.26 kgb) 1.91 kgc) 0.523 kgd) none of these28. A homogenous material is defined as being:a) An elementb) Any material with uniform compositionc) Synonymous with “solution”d) More than one of these29. An example of a chemical property is:a) densityb) massc) acidityd) solubility30. “Exothermic” processes:a) Absorb energyb) Give off energyc) Have no energy changed) It is impossible to predict the energy change of an exothermic process.31. What is the density of an object with a volume of 15 mL and a mass of 42 grams?a) 0.352 g/mLb) 2.80 g/mLc) 630 g/mLd) None of the above is correct.32. Which of the following is not one of Dalton’s laws?a) Atoms are indestructible.b) Atoms of the same element have isotopes with different masses.c) Atoms of different elements have different chemical and physical properties.d) All of these are examples of Dalton’s laws.33. The “plum pudding” model of the atom was devised by:a) Daltonb) Democritusc) Rutherfordd) none of the above answers is correct34. Bohr’s model of the atom was able to accurately explain:a) Why spectral lines appear when atoms are heated.b) The energies of the spectral lines for each element. c) Why electrons travel in circular orbits around the nucleus.d) none of the above answers is correct.35. What subatomic particle has a mass of one atomic mass unit?a) protonb) neutronc) electrond) more than one of the above36. How many electrons does iron have?a) 26b) 30c) 56d) It depends on the isotope of iron37. Cations have:a) Positive chargeb) Negative chargec) No charged) It is impossible to predict the charge on a cation.38. Which pair of atoms would most likely form an ionic compound when bonded to eachother?a) calcium and fluorineb) silicon and nitrogenc) two oxygen atomsd) none of the above would probably form an ionic compound39. If the theoretical yield for a reaction was 156 grams and I actually made 122 grams of theproduct what is my percent yield?a) 78.2%b) 128%c) 19.0%d) none of these40. A beaker contains 600 cm3 of water at 50°C. If 200 cm3 of water at 10°C is added what will be thefinal temperature of the water after mixing?A) 30 degrees CelsiusB) 35 degrees CelsiusC) 40 degrees CelsiusD) 45 degrees celsius41. The temperature of water running from a tap is 10°C. 250 g of this water is poured into analuminum saucepan which is at room temperature 20°C. The mass of the saucepan is 520g and thespecific heat of aluminum is 0.92 J/g°C. 42. Disregarding any heat loss to the surroundings what will be the final temperature of the water andthe saucepan.?a) 17 degrees Celsiusb) 15 degrees Celsiusc) 14 degrees Celsiusd) 13 degrees Celsius43. A styrofoam cup contains some water at 22°C. When 420 g of water at 13°C is added to the cup thefinal temperature of the mixture is 16°C.44. If there is no heat loss what was the mass of the water in the styrofoam cup?a) 280gb) 210gc) 140gd) 84g45. A 150 g metal cube is heated to 100°C. The cube is then dropped into a beaker containing 200 mL ofwater at 25°C. The temperature of the mixture stabilizes at 30.6°C after 5 minutes. What is thespecific heat capacity of the metal?100°Cmetalcube200 mLof waterat 25°C 46. A 4.00 × 102 g piece of iron at 22.0°C is heated in a bomb calorimeter until the temperature is 250.0°C.If the iron absorbs 41.04 kJ of heat what is the specific heat capacity of the iron?A)4.5 × 10-4 J/(g•°C)B)4.5 × 10-1 J/(g•°C)C)4.5 J/(g•°C)D)4.5 × 101 J/(g•°C)47. A chemistry student found five unmarked oily liquids in a refrigerated cabinet in a lab. Using theconcept of characteristic properties the student decided to identify the liquid using calorimetry.The student took 100 mL of water at 27.1°C and then added 20.0 g of the oily substance whichwas at 4.2°C. The final temperature of the mixture was 24.7°C.Using the table of specific heat capacities identify the unknown liquid.LiquidSpecific HeatCapacity J/g°CAnilin2.18Castor Oil1.8Citron Oil1.84Ethylene glycol2.22Glycerine2.43
