The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION

The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTINGCHEMISTRY June 2010

Table 1. The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space because most alpha particles directed at the foil • Passed through the foil • Remained trapped in the foil • Were deflected by the nuclei in gold atoms • Were deflected by electrons in gold atoms

Table 2. Which subatomic particles are located in thenucleus of a carbon atom? • Protons, only • Neutrons, only • Protons and neutrons • Protons and electrons

Table 3. Which part of a helium atom is positivelycharged? • Electron • Neutron • Nucleus • Orbital

Table 4. The mass of a proton is approximately equal tothe mass of • An alpha particle • An electron • A neutron • A positron

Table 5. At STP, solid carbon can exist as diamond andgraphite. Compared to the molecular structureand chemical properties of diamond, graphitehas • a different molecular structure and different properties • a different molecular structure and the same properties • the same molecular structure and different properties • the same molecular structure and the same properties

Table 6. Which Group 14 element is classified as a metal? • Carbon • Germanium • Silicon • Tin

Table 7. The light emitted from a flame is producedwhen electrons in an excited state • absorb energy as they move to lower energy states • absorb energy as they move to higher energy states • release energy as they move to lower energy states • release energy as they move to higher energy states

Table 8. An atom of which element has the greatestattraction for electrons in a chemical bond? • As • Ga • Ge • Se

Table 9. Which formula represents a polar molecule? • H2 • H2O • CO2 • CCl4

Table 10. Two categories of compounds are • covalent and molecular • covalent and metallic • ionic and molecular • ionic and metallic

Table 11. Which type of bond is found between atoms ofsolid cobalt? • Nonpolar covalent • Polar covalent • Metallic • Ionic

Table 12. Which equation represents sublimation? • I2(s) →I2(g) • I2 (s) →I2 (ℓ) • I2 (ℓ) →I2 (g) • I2 (ℓ) →I2 (s)

Table 13. Which sample of ethanol has particles with thehighest average kinetic energy? • 10.0 mL of ethanol at 25°C • 10.0 mL of ethanol at 55°C • 100.0 mL of ethanol at 35°C • 100.0 mL of ethanol at 45°C

Table 14. The molarity of an aqueous solution of NaCl isdefined as the • grams of NaCl per liter of water • grams of NaCl per liter of solution • moles of NaCl per liter of water • moles of NaCl per liter of solution

Table 15. A real gas behaves least like an ideal gas underthe conditions of • low temperature and low pressure • low temperature and high pressure • high temperature and low pressure • high temperature and high pressure

Table 16. Which sample of matter can be separated intodifferent substances by physical means? • LiCl(aq) • LiCl(s) • NH3(g) • NH3(ℓ)

Table 17. At STP, 1.0 liter of helium contains the sametotal number of atoms as • 1.0 L of Ne • 2.0 L of Kr • 0.5 L of Rn • 1.5 L of Ar

Table 18. Which statement describes the particles of anideal gas? • The particles move in well-defined, circular paths. • When the particles collide, energy is lost. • There are forces of attraction between the particles. • The volume of the particles is negligible.

Table 19. A chemical reaction between iron atoms andoxygen molecules can only occur if • the particles are heated • the atmospheric pressure decreases • there is a catalyst present • there are effective collisions between the particles

Table 20. Given the equation representing a phase changeat equilibrium: H2O(s) ⇌ H2O(l)Which statement describes this equilibrium? • The H2O(s) melts faster than the H2O(ℓ) freezes. • The H2O(ℓ) freezes faster than the H2O(s) melts. • The mass of H2O(s) must equal the mass of H2O(ℓ). • The mass of H2O(ℓ) and the mass of H2O(s) each remain constant.

Table 21. A molecule of an organic compound contains atleast one atom of • Carbon • Chlorine • Nitrogen • Oxygen

Table 22. In a chemical reaction, the difference betweenthe potential energy of the products and thepotential energy of the reactants is equal to the • activation energy • entropy of the system • heat of fusion • heat of reaction

Table 23. A carbon-carbon triple bond is found in amolecule of • Butane • Butanone • Butene • Butyne

Table 24. Which statement describes one characteristic ofan operating electrolytic cell? • It produces electrical energy. • It requires an external energy source. • It uses radioactive nuclides. • It undergoes a spontaneous redox reaction.

Table 25. Which compound when dissolved in water is anArrhenius acid? • CH3OH • HCl • NaCl • NaOH

Table 26. An acid can be defined as an • H+acceptor • H+ donor • OH- acceptor • OH- donor

Table 27. Which nuclear emission has no charge and nomass? • Alpha particle • Beta particle • Gamma ray • Positron

Table 28. During which process can 10.0 milliliters of a0.05 M HCl(aq) solution be used to determinethe unknown concentration of a given volume ofNaOH(aq) solution? • Evaporation • Distillation • Filtration • Titration

Table 29. Which radioisotope is matched with its decaymode? • (1) H-3 and γ • (2) K-42 and β+ • (3) N-16 and α • (4) P-32 and β−

Table 30. Which reaction is accompanied by the release ofthe greatest amount of energy? • combustion of 10. g of propane • electrolysis of 10. g of water • nuclear fission of 10. g of uranium • oxidation of 10. g of iron

Table 31. The total number of protons, electrons, and neutrons in each of four different atoms are shown in the table below. Which two atoms are isotopes of the same element? • A and D • A and Z • X and D • X and Z

Table 32. Which Lewis electron-dot diagram represents anatom in the ground state for a Group 13 element? • Diagram (1) • Diagram (2) • Diagram (3) • Diagram (4)

Table 33. Which element forms a compound with chlorinewith the general formula MCl? • Rb • Ra • Re • Rn

Table 34. A sample of an element has a mass of 34.261 grams and a volume of 3.8 cubic centimeters. To which number of significant figures should the calculated density of thesample be expressed? • 5 • 2 • 3 • 4

Table 35. Which characteristics both generally decreasewhen the elements in Period 3 on the PeriodicTable are considered in order from left to right? • nonmetallic properties and atomic radius • nonmetallic properties and ionization energy • metallic properties and atomic radius • metallic properties and ionization energy

Table 36. Which formula is both a molecular and anempirical formula? • C6H12O6 • C2H4O2 • C3H8O • C4H8

Table 37. An atom of argon in the ground state tends notto bond with an atom of a different elementbecause the argon atom has • more protons than neutrons • more neutrons than protons • a total of two valence electrons • a total of eight valence electrons

Table 38. Which formula represents a molecule having anonpolar covalent bond? • Diagram (1) • Diagram (2) • Diagram (3) • Diagram (4)

Table 39. Which compound has the lowestvapor pressureat 50°C? • Ethanoic acid • Ethanol • Propanone • Water

Table 40. Given the potential energy diagram and equationrepresenting the reaction between substancesA and D:According to Table I, substance G could be • HI(g) • H2O(g) • CO2(g) • C2H6(g)

Table 41. A sample of gas confined in a cylinder with amovable piston is kept at constant pressure. Thevolume of the gas doubles when the temperatureof the gas is changed from • 400. K to 200. K • 200. K to 400. K • 400.°C to 200.°C • 200.°C to 400.°C

Table 42. According to Table F, which compound is solublein water? • barium phosphate • calcium sulfate • silver iodide • sodium perchlorate

Table 43. Given the equation representing a system at equilibrium: N2(g) +3H2(g) ⇌ 2NH3(g) +energy Which changes occur when the temperature ofthis system is decreased? • The concentration of H2(g) increases andthe concentration of N2 (g) increases. • The concentration of H2 (g) decreases andthe concentration of N2 (g) increases. • The concentration of H2(g) decreases andthe concentration of NH3 (g) decreases. • The concentration of H2 (g) decreases andthe concentration of NH3(g) increases.

Table 44. Which formula represents an unsaturatedhydrocarbon? • Diagram (1) • Diagram (2) • Diagram (3) • Diagram (4)

Table 45. Which half-reaction equation represents thereduction of an iron(II) ion? • Fe2+→ Fe3++ e− • Fe2+ + 2e−→ Fe • Fe3+ + e−→ Fe2+ • Fe → Fe2+ + 2e−

Table 46. Which metal is more active than H2? • Ag • Au • Cu • Pb

Table 47. Given the balanced ionic equation representingthe reaction in an operating voltaic cell: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)The flow of electrons through the external circuit in this cell is from the • Cu anode to the Zn cathode • Cu cathode to the Zn anode • Zn anode to the Cu cathode • Zn cathode to the Cu anode

Table 48. Which laboratory test result can be used todetermine if KCl(s) is an electrolyte? • pH of KCl(aq) • pH of KCl(s) • electrical conductivity of KCl(aq) • electrical conductivity of KCl(s)

Table 49. Which compound is produced when HCl(aq) isneutralized by Ca(OH)2(aq)? • (1) CaCl2 • (2) CaH2 • (3) HClO • (4) HClO2

The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION