5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons

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1 1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly and close together (C) regularly and far apart (D) regularly and close together 3. When a substance is dissolved in water, the temperature of the water increased. This process is described as (A) endothermic, with the release of energy (B) endothermic, with the absorption of energy (C) exothermic, with the release of energy (D) exothermic, with the absorption of energy 4. Compared to the entire atom, the nucleus of the atom is (A) smaller and contains most of the atom s mass (C) larger and contains most of the atom s mass (B) smaller and contains little of the atom s mass (D) larger and contains little of the atom s mass 5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons 6. Four valence electrons of an atom in the ground state would occupy the (A) s sublevel only (B) p sublevel only (C) s and p sublevels only (D) s, p, and d sublevels 7. An atom of carbon-14 contains (A) 8 protons, 6 neutrons, and 6 electrons (C) 6 protons, 8 neutrons, and 8 electrons (B) 6 protons, 6 neutrons, and 8 electrons (D) 6 protons, 8 neutrons, and 6 electrons 8. In an atom that has an electron configuration of 1s 2 2s 2 2p 3, what is the total number of electrons in its sublevel of highest energy? (A) 1 (B) 2 (C) 3 (D) 4 9. The correct electron dot formula for hydrogen chloride is (A) (B) (C) (D) 10. What is the total mass of oxygen in 1.00 mole of Al 2(CrO 4) 3? (A) 192 g (B) 112 g (C) 64.0 g (D) 48.0 g 11. Which molecule is nonpolar and has a symmetrical shape? (A) HCl (B) CH 4 (C) H 2O (D) NH 3

2 12. What is the correct formula for ammonium carbonate? (A) NH 4(CO 3) 2 (B) (NH 4) 2(CO 3) 2 (C) NH 4CO 3 (D) (NH 4) 2CO Which element is in Group 2 and Period 7 of the Periodic Table? (A) magnesium (B) radium (C) manganese (D) radon 14. Which ion has the largest radius? (A) I -1 (B) Br -1 (C) Cl -1 (D) F An atom in the ground state contains 8 valence electrons. This atom is classified as a (A) metal (B) noble gas (C) metalloid (D) halogen 16. Which tendencies favor a spontaneous reaction? (A) decreasing enthalpy and decreasing entropy (C) increasing enthalpy and decreasing entropy (B) decreasing enthalpy and increasing entropy (D) increasing enthalpy and increasing entropy 17. Which formula represents a salt? (A) KOH (B) CH 3OH (C) KCl (D) CH 3COOH 18. What is the H +1 ion concentration of a solution whose OH -1 ion concentration is 1 x 10-3 M? (A) 1 x 10-4 M (B) 1 x M (C) 1 x 10-7 M (D) 1 x M 19. Given the reaction: NH OH -1 H 2O + NH 3 Which species is the Bronsted-Lowry acid in the forward reaction? (A) NH 3 (B) OH -1 (C) H 2O (D) NH What is the conjugate base of NH 3? (A) NH 4 +1 (B) NO 3-1 (C) NH 2-1 (D) NO When a catalyst is added to a chemical reaction, there is a change in the (A) heat of reaction (B) rate of reaction (C) potential energy of the reactants (D) potential energy of the products 22. Nonmetals in the solid state are poor conductors of heat and tend to (A) be brittle (B) be malleable (C) have a shiny luster (D) have good electrical conductivity

3 23. Which group contains elements composed of diatomic molecules at STP? (A) 11 (B) 2 (C) 7 (D) Which metal s atoms can form ionic bonds by losing electrons from both the outermost and next to outermost energy levels? (A) Fe (B) Mg (C) Pb (D) Ca 25. Which species contains the greatest percent by mass of hydrogen? (A) OH -1 (B) H 3O +1 (C) H 2O (D) H 2O Given the reaction: CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2O (g) How many moles of oxygen are needed for the complete combustion of 3.0 moles of CH 4 (g)? (A) 6.0 moles (B) 3.0 moles (C) 2.0 moles (D) 4.0 moles 27. What mass contains 6.0 x atoms? (A) 6.0 g of carbon (B) 3.0 g of helium (C) 16 g of sulfur (D) 28 g of silicon 28. Which is a homogeneous mixture? (A) I 2 (s) (B) I 2 (l) (C) HCl (g) (D) HCl (aq) 29. Which element is so reactive that it occurs naturally only in compounds? (A) silver (B) potassium (C) sulfur (D) copper 30. Which change results in a release of energy? (A) the melting of H 2O (s) (B) the boiling of H 2O (l) (C) the evaporation of H 2O (l) (D) the condensation of H 2O (g) 31. A cylinder is filled with 2.00 moles of nitrogen, 3.00 moles of argon, and 5.00 moles of helium. If the gas mixture is at STP, what is the partial pressure of the argon? (A) 152 torr (B) 380. torr (C) 228 torr (D) 760. torr 32. Compared to the average kinetic energy of 1 mole of water at 0 o C, the average kinetic energy of 1 mole of water at 298 K is (A) the same, and the number of molecules is the same (B) the same, and the number of molecules is greater (C) greater, and the number of molecules is the same (D) greater, and the number of molecules is greater 33. Which formula represents a binary compound? (A) Ne (B) Br 2 (C) C 3H 8 (D) H 2SO 4

4 34. What is the total number of occupied sublevels in an atom of chlorine in the ground state? (A) 1 (B) 3 (C) 5 (D) At standard pressure, which element at 25 o C could undergo a change of phase when the temperature is decreased? (A) aluminum (B) silicon (C) chlorine (D) sulfur 36. If the pressure on a given mass of gas is increased and the temperature remains constant, the volume of the gas will (A) decrease (B) increase (C) remain the same 37. A substance that has a melting point of 1074 K, conducts electricity when dissolved in water, but does not conduct electricity in the solid phase. The substance is most likely (A) an ionic solid (B) a metallic solid (C) a network solid (D) a molecular solid 38. A water molecule is best described as (A) polar with polar covalent bonds (C) nonpolar with polar covalent bonds (B) polar with nonpolar covalent bonds (D) nonpolar with nonpolar covalent bonds 39. When the equation: _ Al 2(SO 4) 3 +_ ZnCl 2 _ AlCl 3 + _ ZnSO 4 is correctly balanced using the smallest whole-number coefficients, the sum of the coefficients is (A) 9 (B) 5 (C) 8 (D) When ethylene glycol (an antifreeze) is added to water, the boiling point of the water (A) decreases, and the freezing point decreases (B) decreases, and the freezing point increases (C) increases, and the freezing point decreases (D) increases, and the freezing point increases 41. A sample of a compound contains 24 grams of carbon and 64 grams of oxygen. What is the empirical formula of this compound? (A) CO (B) CO 2 (C) C 2O 2 (D) C 2O Which gas has approximately the same density as C 2H 6 at STP? (A) NO (B) H 2S (C) NH 3 (D) SO At a temperature of 273 K, a 400. ml gas sample has a pressure of 760 mm Hg. If the pressure is changed to 380. mm Hg, at which temperature will this gas sample have a volume of 551 ml? (A) 100 K (B) 273 K (C) 188 K (D) 546 K 44. Which element is a solid at room temperature and standard pressure? (A) bromine (B) mercury (C) neon (D) iodine

5 45. As the atoms of the elements from atomic number 3 to atomic number 9 are considered in sequence from left to right on the Periodic Table, the atomic radius of each successive atom is (A) smaller, and the nuclear charge is less (B) smaller, and the nuclear charge is greater (C) larger, and the nuclear charge is less (D) larger, and the nuclear charge is greater 46. Which substance can act as an Arrhenius acid in aqueous solution? (A) NaI (B) LiH (C) NH 3 (D) HI 47. Which of the following metals will react most readily with HCl (aq) to release hydrogen gas? (A) aluminum (B) silver (C) gold (D) copper 48. The characteristic bright-line spectrum of sodium is produced when its electrons (A) return to lower energy levels (B) jump to higher energy levels (C) are lost by the neutral atoms (D) are gained by the neutral atoms 49. Given the reaction: 2 Na (s) + 2 H 2O (l) 2 Na +1 (aq) + 2 OH -1 (aq) + H 2 (g) This reaction goes to completion because one of the products formed is (A) an insoluble base (B) a precipitate (C) a soluble base (D) a gas 50. A student collected the data shown below to determine the density of distilled water experimentally. Mass of graduated cylinder + distilled H 2O sample 163 g Mass of empty cylinder 141 g Mass of distilled water sample g Volume of H 2O sample 25.3 ml Based on the experimental data collected, what is the density of the distilled water? (A) 1.0 g/ml (B) 0.87 g/ml (C) g/ml (D) 1.15 g/ml Get the answers to this practice test Back to the Review Materials Page Back to the Main Page

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