1. An example of a chemical change is (A) freezing of water. (B) burning a match. (C) boiling carbon tetrachloride. (D) dissolving alcohol in water. (E) stretching a rubber band 2. Which involves a chemical change? (A) powdering sugar (B) condensing steam (C) magnetizing an iron bar (D) separating cream from milk (E) exposing photographic film to light 3. The law of multiple proportions is based upon the idea that atoms of some elements may (A) have several isotopes. (B) exist in several physical forms. (C) have more than one atomic mass. (D) have both metallic and non metallic properties. (E) have more than one valence number. 4. Rutherford s alpha particle bombardment of gold foil helped develop our current model of the atom by (A) finding the mass of the electron. (B) showing the existence of the neutron. (C) showing that the electron carries a negative charge. (D) showing that the atom has a concentrated central charge. 5. Which set consists only of compounds? (A) Na, Ca, He (C) NaCl, CH 4, Br 2 (B) H 3 O +, Cl, I 3 (D) H 2 S, CuCl 2, KI 6. Which property would be most helpful in identifying a substance? (A) mass (C) volume (B) state (D) melting point 7. An insoluble solid has a mass of 20.0 g. It is placed in a graduated cylinder containing 40.0 ml of water. The final volume is read as 46.0 ml. What is the density of the solid? (A) 0.300 g cm 3 (C) 2.30 g cm 3 (B) 0.500 g cm 3 (D) 3.33 g cm 3 8. A solid, pure, orange substance was heated yielding a colorless gas and a green solid. What kind of material was heated? (A) an element (C) a mixture (B) a compound (D) a solution 9. Which unit represents l x 10 3 mol? (A) decimole (C) millimole (B) kilomole (D) micromole 10. The volume of one milliliter most nearly equals (A) 454 g (B) 1000 L (C) 1 mg (D) 1 in (E) 1 cm 3
11. A barometer is used to measure the (A) pressure of the air at 0 C only. (B) mass of a column of mercury. (C) temperature of the air at standard pressure. (D) density of mercury. (E) pressure of the air. 12. Which apparatus delivers 50.00 ml of liquid most accurately? (A) 50 ml buret (B) 50 ml beaker (C) 50 ml test tube (D) 50 ml graduated cylinder 13. If atom A contains 18 protons and 22 neutrons, while atom B contains 20 protons and 20 neutrons, then atoms A and B are (A) isotopes. (B) both metallic. (C) both non metallic. (D) alike in number of'electrons. (E) different in number of electrons 14. The number of neutrons in an atom of the radioactive carbon isotope 14 6 C, is (A) 6 (B) 8 (C) 12 (D) 14 (E) 20 15. Which particle consists of 13 protons, 14 neutrons, and 10 electrons? (A) neon atom (D) silicon atom (B) sodium atom (E) phosphide ion (C) aluminum ion 16. A hypothetical element X has three isotopes: 40 X, 41 X, and 42 X. Their abundances are 72.0%, 9.00%, and 19.0% respectively. What is the atomic mass of X? (A) 40.5 u (B) 40.8 u (C) 41.0 u (D) 41.5 u 17. A chlorine atom (Cl) differs from a chloride ion (Cl ) in that a chlorine atom (A) has a positive nucleus while the ion s nucleus is negative. (B) has a neutral nucleus while the ion s nucleus is positive. (C) contains one electron less than the ion. (D) contains one electron more than the ion. (E) contains one proton more in the nucleus 18. All positive ions differ from their corresponding atoms by having (A) larger diameters. (B) fewer electrons. (C) a charge of +1. (D) greater atomic masses. (E) stronger metallic properties 19. The correct formula for iron(iii) sulfate is (A) FeSO 4 (D) Fe 2 (SO 4 ) 3 (B) Fe(SO 4 ) 2 (E) Fe 3 (SO 4 ) 2 (C) Fe 2 SO 4
20. Which formula is incorrect? (A) BaHCO 3 (B) Ca(OH) 2 (C) Al 2 O 3 (D) K 2 SO 4 (E) ZnCO 3 21. The compound not properly named is (A) Fe 2 O 3, iron(iii) oxide. (B) Pb 3 O 4, trilead tetraoxide. (C) CuCl 2, copper(ii) chloride. (D) Pb 3 (PO 4 ) 2, lead(iii) phosphate 22. What is the total number of oxygen atoms represented by the formula KAl(SO 4 ) 2 12H 2 O? (A) 9 (B) 16 (C) 20 (D) 48 (E) 96 23. Using only these formulas, XY 2 X 2 Z QZ what formula would you expect for a compound of elements Q and Y? (A) QY (B) QY 2 (C) Q 2 Y (D) QY 4 24. In the reaction 4Al + 3O 2 2Al 2 O 3 how many moles of aluminum oxide, Al 2 O 3, are produced from one mole of aluminum, Al? (A) 0.5 (B) 2 (C) 3 (D) 4 25. Which expression is correctly balanced? (A) Na 2 O 2 + 2H 2 O 2NaOH + O 2 (B) 2Na 2 O 2 + 2H 2 O 4NaOH + 2O 2 (C) 4Na 2 O 2 + 3H 2 O 4NaOH + 2O 2 (D) 2Na 2 O 2 + 2H 2 O 4NaOH + O 2 (E) 3Na 2 O 2 + 2H 2 O 6NaOH + O 2 26. Consider the unbalanced expression:? CH 3 CH 2 CHO(l) +? O 2 (g)? CO 2 (g) +? H 2 O(g) Which set of coefficients balances the equation? (A) 2, 8, 3, 6 (D) 1, 8, 3, 3 (B) 3, 8, 6, 6 (E) 1, 4, 3, 3 (C) 1, 4, 3, 2
27. Given the equation N 2 + 3H 2 2NH 3 Theoretically, the number of moles of ammonia produced from 2 mol of nitrogen is (A) 1 (B) 2 (C) 3 (D) 4 (E) 5 28. One mole of substance X reacts with one mole of water and produces one mole of oxygen and two moles of hydrogen fluoride. What is the formula of substance X? X + H 2 O O 2 + 2HF (A) F 2 (B) OF 2 (C) O 2 F (D) HOF 2 29. When basic copper(ii) carbonate, CuCO 3 Cu(OH) 2, is heated, it decomposes. What is the missing product in this equation? CuCO 3 Cu(OH) 2 2CuO + CO 2 +? (A) H 2 CO 3 (B) H 2 O (C) CuH 2 (D) H 2 30. What is the net ionic equation for the reaction between solutions of sodium chloride, NaCl, and silver nitrate, AgNO 3? (A) Na + (aq) + NO 3 (aq) Na(s) + 1/2N 2 (g) + 3/2O 2 (g) (B) Ag + (aq) + Cl (aq) Ag(s) + 1/2Cl 2 (g) (C) Ag + (aq) + Cl (aq) Ag + (aq) + Cl (aq) (D) Ag + (aq) + Cl (aq) AgCl(s) 31. Which two ions do not participate in the reaction between solutions of silver nitrate, AgNO 3, and potassium chloride, KCl? (A) K + and Ag + (C) K + and Cl (B) K + and NO 3 (D) Ag + and Cl 32. A compound whose empirical formula is CH 2 has a molar mass of 28 g mol 1. What is the molecular formula? H 1.0 g mol 1 (A) CH 2 (B) C 2 H 4 (C) C 2 H 2 (D) CH 4
33. A substance with a molar mass of 92 g mol 1 consists of equal numbers of S and N atoms. What is the formula of the substance? N 14.0 g mol 1 S 32.1 g mol 1 (A) SN (B) S 2 N 2 (C) S 3 N 3 (D) S 4 N 4 34. What is the mass of one mole of calcium nitrate, Ca(NO 3 ) 2? Ca 40. g mol 1 N 14. g mol 1 O 16. g mol 1 (A) 82 g (B) 102 g (C) 164 g (D) 204 g 35. What is the percentage by mass of carbon in oxalic acid, H 2 C 2 O 4? H 1.0 g mol 1 O 16.0 g mol 1 (A) 2.22% (B) 3.75% (C) 25.0% (D) 26.7% 36. How many molecules are in 11.0 g of carbon dioxide, CO 2? O 16.0 g mol 1 (A) 1.50 x 10 23 (C) 4.40 x 10 23 (B) 2.24 x 10 23 (D) 5.60 x 10 23 37. Calculate the mass of 12.0 x 10 23 molecules of chlorine gas, Cl 2. Atomic Molar Mass Cl 35.5 g mol 1 (A) 35.5 g (B) 71.0 g (C) 142 g (D) 284 g
38. At STP, 4.48 L of hydrogen was prepared using the reaction: Approximately what mass of zinc was required? Zn + 2HCl ZnCl 2 + H 2 Zn 65 g mol 1 Atomic Molar Mass (A) 1.5 g (B) 2.0 g (C) 13.0 g (D) 36.5 g (E) 65.0 g 39. This potential energy diagram shows that the reaction A + B C is Energy! A + B x C Reaction Coordinate! (A) slow. (B) rapid. (D) endothermic. (E) at equilibrium. (C) exothermic. 40. Note the equation: 2Fe(s) + 3/2O 2 (g) Fe 2 O 3 (s) ΔH = 840 kj mol 1 Fe 2 O 3 If 0.100 mol of iron reacts, how much heat is liberated? (A) 42.0 kj (B) 84.0 kj (D) 420 kj (E) 840 kj (C) 210 kj
41. The gaseous molecules that have the greatest average velocity at 150 C are represented by F 19.0 g mol 1 H 1.0 g mol 1 N 14.0 g mol 1 O 16.0 g mol 1 (A) O 2 (B) F 2 (C) H 2 (D) N 2 (E) H 2 O 42. The approximate number of molecules of hydrogen in 1.00 L of H 2 gas at STP is (A) 1.35 x 10 22 (D) 2.69 x 10 22 (B) 3.01 x 10 23 (E) 5.38 x 10 22 (C) 6.02 x 10 23 43. A cylinder equipped with a movable piston contains 50.0 cm 3 of a gas. What is the new volume when the pressure is doubled at constant temperature? (A) 25.0 cm 3 (C) 75.0 cm 3 (B) 50.0 cm 3 (D) 100 cm 3