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The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY

The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Wednesday , January 27, 2016. Table. 1. Which phrase describes the charge and mass of a neutron?. a charge of 1 and no mass a charge of 1 and an approximate mass of 1 u

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The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY

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  1. The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING CHEMISTRY Wednesday, January 27, 2016

  2. Table 1. Which phrase describes the charge and mass ofa neutron? • a charge of 1 and no mass • a charge of 1 and an approximate mass of 1 u • no charge and no mass • no charge and an approximate mass of 1 u

  3. Table 2. What is the number of electrons in a potassiumatom? • 18 • 19 • 20 • 39

  4. Table 3. The number of valence electrons in each atomof an element affects the element’s • Chemical properties • Number of isotopes • Decay mode • Half-life

  5. Table 4. The nuclides I-131 and I-133 are classified as • isomers of the same element • isomers of Xe-131 and Cs-133 • isotopes of the same element • isotopes of Xe-131 and Cs-133

  6. Table 5. The elements on the Periodic Table arearranged in order of increasing • mass number • atomic number • number of isotopes • number of valence electrons

  7. Table 6 Compared to a 1.0-gram sample of chlorine gasat standard pressure, a 1.0-gram sample of solidaluminum at standard pressure has • a lower melting point • a higher boiling point • a lower density • a greater volume

  8. Table 7. Which processes represent one chemical changeand one physical change? • freezing and melting • freezing and vaporization • decomposition and melting • decomposition and combustion

  9. Table 8. In the ground state, an atom of each of theelements in Group 2 has a different • oxidation state • first ionization energy • number of valence electrons • number of electrons in the first shell

  10. Table 9. Which statement explains why water is classifiedas a compound? • Water can be broken down by chemical means. • Water is a liquid at room temperature. • Water has a heat of fusion of 334 J/g. • Water is a poor conductor of electricity

  11. Table 10. Which formula is an empirical formula? • CH4 • C2H6 • C3H6 • C4H10

  12. Table 11. Which compound contains both ionic and covalentbonds? • KI • CaCl2 • CH2Br2 • NaCN

  13. Table 12. Given the balanced equation representing areaction: H2→ H HWhat occurs during this reaction? • Energy is absorbed as bonds are formed. • Energy is absorbed as bonds are broken. • Energy is released as bonds are formed. • Energy is released as bonds are broken.

  14. Table 13. Parts per million is used to express the • atomic mass of an element • concentration of a solution • volume of a substance • rate of heat transfer

  15. Table 14. According to Table F, which ions combine withchloride ions to form an insoluble compound? • Fe2+ ions • Ca2+ ions • Li+ ions • Ag+ ions

  16. Table 15. At 1 atm, equal masses of H2O(s), H2O(ℓ), andH2O(g) have • the same density • the same distance between molecules • different volumes • different percent compositions

  17. Table 16. Which list includes three forms of energy? • chemical, mechanical, electromagnetic • chemical, mechanical, temperature • thermal, pressure, electromagnetic • thermal, pressure, temperature

  18. Table 17. At STP, a 1-liter sample of Ne(g) and a 1-litersample of Kr(g) have the same • mass • density • number of atoms • number of electrons

  19. Table 18. A reaction will most likely occur if the collidingparticles have the proper • mass, only • mass and volume • orientation, only • orientation and energy

  20. Table 19. Which factors have the greatest effect on therate of a chemical reaction between AgNO3(aq)and Cu(s)? • solution concentration and temperature • solution concentration and pressure • molar mass and temperature • molar mass and pressure

  21. Table 20. Which expression represents the heat ofreaction for a chemical change in terms ofpotential energy, PE? • (PEproducts) +(PEreactants) • (PEproducts) - (PEreactants) • (PEproducts) x(PEreactants) • (PEproducts) ÷(PEreactants)

  22. Table 21. When a chemical reaction is at equilibrium,the concentration of each reactant and theconcentration of each product must be • constant • variable • equal • zero

  23. Table 22. Which element is present in all organiccompounds? • nitrogen • oxygen • carbon • sulfur

  24. Table 23. Two types of organic reactions are • deposition and saponification • deposition and transmutation • polymerization and saponification • polymerization and transmutation

  25. Table 24. Given the balanced equation representing areaction: 2Al(s) + 3Cu2+(aq) → 2Al3+ (aq) + 3Cu(s)Which particles are transferred in this reaction? • electrons • neutrons • positrons • protons

  26. Table 25. In an operating voltaic cell, reduction occurs • At the anode • At the cathode • In the salt bridge • In the wire

  27. Table 26. Which type of substance yields hydrogen ions,H+, in an aqueous solution? • an Arrhenius acid • an Arrhenius base • a saturated hydrocarbon • an unsaturated hydrocarbon

  28. Table 27. Phenolphthalein is pink in an aqueous solutionhaving a pH of • 5 • 2 • 7 • 12

  29. Table 28. According to one acid-base theory, NH3 acts asa base when an NH3 molecule • accepts an H+ ion • donates an H+ion • accepts an OH-ion • donates an OH- ion

  30. Table 29. Which reaction releases the greatest amount ofenergy per mole of reactant? • decomposition • esterification • fermentation • fission

  31. Table 30. Which nuclear emission is negatively charged? • An alpha particle • A beta particle • A neutron • A positron

  32. Table 31. Which electron configuration represents anatom of chlorine in an excited state? • 2-7-7 • 2-7-8 • 2-8-7 • 2-8-8

  33. Table 32. Given the balanced equation representing areaction occurring at 101.3 kilopascals and 298 K: 2H2(g) + O2(g) → 2H2O(ℓ) + energyWhat is the net amount of energy released whenone mole of H2O(ℓ) is produced? • 241.8 kJ • 285.8 kJ • 483.6 kJ • 571.6 kJ

  34. Table 33. Element X reacts with copper to form thecompounds CuX and CuX2. In which group onthe Periodic Table is element X found? • Group 1 • Group 2 • Group 13 • Group 17

  35. Table 34. What is the mass of 1.5 moles of CO2? • 66 g • 44 g • 33 g • 29 g

  36. Table 35 Given the balanced equation representing a reaction: K2CO3(aq) + BaCl2(aq) → 2KCl(aq) + BaCO3(s)Which type of reaction is represented by this equation? • synthesis • decomposition • single replacement • double replacement

  37. Table 36. Which sample, when dissolved in 1.0 liter of water,produces a solution with the highest boiling point? • 0.1 mole KI • 0.2 mole KI • 0.1 mole MgCl2 • 0.2 mole MgCl2

  38. Table 37. Given the balanced equation representing areaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)What is the number of moles of H2O(g) formedwhen 2.0 moles of NH3(g) react completely? • 6.0 mol • 2.0 mol • 3.0 mol • 4.0 mol

  39. Table 38 A rigid cylinder with a movable piston contains asample of gas. At 300. K, this sample has apressure of 240. kilopascals and a volume of70.0 milliliters. What is the volume of this samplewhen the temperature is changed to 150. K andthe pressure is changed to 160. kilopascals? • 35.0 mL • 52.5 mL • 70.0 mL • 105 mL

  40. Table 39. A 100.-gram sample of H2O(ℓ) at 22.0°Cabsorbs 8360 joules of heat. What will be thefinal temperature of the water • 18.3◦C • 20.0◦C • 25.7◦C • 42.0◦C

  41. Table 40. Which compound has the strongest hydrogenbonding at STP? • H2Te

  42. Table 41. Which formula represents an unsaturatedhydrocarbon? • C2H4 • C3H8 • C4H10 • C5H12

  43. Table 42 Which radioisotope is used in dating geologicalformations? • I-131 • U-238 • Ca-37 • Fr-220

  44. Table 43. The heating curve below represents a sample ofa substance starting as a solid below its meltingpoint and being heated over a period of time. Which statement describes the energy of theparticles in this sample during interval DE? • Both potential energy and average kinetic energy increase. • Both potential energy and average kinetic energy decrease. • Potential energy increases and average kinetic energy remains the same. • Potential energy remains the same and average kinetic energy increases.

  45. Table 44. Given the potential energy diagram for areaction: Which intervals are affected by the addition of acatalyst? • 1 and 2 • 1 and 3 • 2 and 4 • 3 and 4

  46. Table 45 Which balanced equation represents a redoxreaction? • Mg + Cl2 → MgCl2 • CaO + H2O → Ca(OH)2 • HNO3 + NaOH → NaNO3+ H2O • NaCl + AgNO3 → AgCl + NaNO3

  47. Table 46. The pH of a solution is 7. When acid is added tothe solution, the hydronium ion concentrationbecomes 100 times greater. What is the pH ofthe new solution? • 1 • 5 • 9 • 14

  48. Table 47. Given the formula for a compound:A chemical name for this compound is • butanal • butanol • butanone • butanoic acid

  49. Table 48. What occurs in both fusion and fission reactions? • Small amounts of energy are converted into large amounts of matter. • Small amounts of matter are converted into large amounts of energy. • Heavy nuclei are split into lighter nuclei. • Light nuclei are combined into heavier nuclei.

  50. Table 49 Given the reaction:Which particle is represented by X?

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