Earth Science June 2003

Earth Science June 2003 Questions Answers Keys.

The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Tuesday, June 24, 2003 — 9:15 a.m. to 12:15 p.m., only

Directions : For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry.

1. The atomic number of an atom is always equal to the number of its

  • (1) protons, only
  • (2) neutrons, only
  • (3) protons plus neutrons
  • (4) protons plus electrons
Answer: (1) protons, only 

2. Which subatomic particle has no charge?

  • (1) alpha particle
  • (2) beta particle
  • (3) neutron
  • (4) electron
Answer: (3) neutron 

3. When the electrons of an excited atom return to a lower energy state, the energy emitted can result in the production of

  • (1) alpha particles
  • (2) isotopes
  • (3) protons
  • (4) spectra
Answer: (4) spectra 

4. The atomic mass of an element is calculated using the

  • (1) atomic number and the ratios of its naturally occurring isotopes
  • (2) atomic number and the half-lives of each of its isotopes
  • (3) masses and the ratios of its naturally occurring isotopes
  • (4) masses and the half-lives of each of its isotopes
Answer: (3) masses and the ratios of its naturally occurring isotopes 

5. The region that is the most probable location of an electron in an atom is

  • (1) the nucleus
  • (2) an orbital
  • (3) the excited state
  • (4) an ion
Answer: (2) an orbital 

6. Which is a property of most nonmetallic solids?

  • (1) high thermal conductivity
  • (2) high electrical conductivity
  • (3) brittleness
  • (4) malleability
Answer: (3) brittleness 

7. Alpha particles are emitted during the radioactive decay of

  • (1) carbon-14
  • (2) neon-19
  • (3) calcium-37
  • (4) radon-222
Answer: (4) radon-222 

8. Which is an empirical formula?

  • (1) P2O5
  • (2) P4O6
  • (3) C2H4
  • (4) C3H6
Answer: (1) P2O5 

9. Which substance can be decomposed by a chemical change?

  • (1) Co
  • (2) CO
  • (3) Cr
  • (4) Cu
Answer: (2) CO 

10. The percent by mass of calcium in the compound calcium sulfate (CaSO4) is approximately

  • (1) 15%
  • (2) 29%
  • (3) 34%
  • (4) 47%
Answer: (2) 29% 

11. What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table?

  • (1) the number of neutrons in the atom
  • (2) the number of protons in the atom
  • (3) the number of valence electrons in the atom
  • (4) the total number of electrons in the atom
Answer: (3) the number of valence electrons in the atom 

12. Which type of chemical bond is formed between two atoms of bromine?

  • (1) metallic
  • (2) hydrogen
  • (3) ionic
  • (4) covalent
Answer: (4) covalent 

13. Which of these formulas contains the most polar bond?

  • (1) H–Br
  • (2) H–Cl
  • (3) H–F
  • (4) H–I
Answer: (3) H–F 

14. According to Table F, which of these salts is least soluble in water?

  • (1) LiCl
  • (2) RbCl
  • (3) FeCl2
  • (4) PbCl2
Answer: (4) PbCl2 

15. Which of these terms refers to matter that could be heterogeneous?

  • (1) element
  • (2) mixture
  • (3) compound
  • (4) solution
Answer: (2) mixture 

16. In which material are the particles arranged in a regular geometric pattern?

  • (1) CO2(g)
  • (2) NaCl(aq)
  • (3) H2O()
  • (4) C12H22O11(s)
Answer: (4) C12H22O11(s) 

17. Which change is exothermic?

  • (1) freezing of water
  • (2) melting of iron
  • (3) vaporization of ethanol
  • (4) sublimation of iodine
Answer: (1) freezing of water 

18. Which type of change must occur to form a compound?

  • (1) chemical
  • (2) physical
  • (3) nuclear
  • (4) phase
Answer: (1) chemical  

19. Which formula correctly represents the composition of iron (III) oxide?

  • (1) FeO3
  • (2) Fe2O3
  • (3) Fe3O
  • (4) Fe3O2
Answer: (2) Fe2O3 

20. Given the reaction:

PbCl2(aq) + Na2CrO4(aq) → PbCrO4(s) + 2 NaCl(aq)

What is the total number of moles of NaCl formed when 2 moles of Na2CrO4 react completely?

  • (1) 1 mole
  • (2) 2 moles
  • (3) 3 moles
  • (4) 4 moles
Answer: (4) 4 moles 

21. Which hydrocarbon is saturated?

  • (1) propene
  • (2) ethyne
  • (3) butene
  • (4) heptane
Answer: (4) heptane 

22. Which statement correctly describes an endothermic chemical reaction?

  • (1) The products have higher potential energy than the reactants, and the ∆H is negative.
  • (2) The products have higher potential energy than the reactants, and the ∆H is positive.
  • (3) The products have lower potential energy than the reactants, and the ∆H is negative.
  • (4) The products have lower potential energy than the reactants, and the ∆H is positive.
Answer: (2) The products have higher potential energy than the reactants, and the ∆H is positive. 

23. At standard pressure when NaCl is added to water, the solution will have a

  • (1) higher freezing point and a lower boiling point than water
  • (2) higher freezing point and a higher boiling point than water
  • (3) lower freezing point and a higher boiling point than water
  • (4) lower freezing point and a lower boiling point than water
Answer: (3) lower freezing point and a higher boiling point than water 

24. Which element has atoms that can form single, double, and triple covalent bonds with other atoms of the same element?

  • (1) hydrogen
  • (2) oxygen
  • (3) fluorine
  • (4) carbon
Answer: (4) carbon 

25. Which compound is an isomer of pentane?

  • (1) butane
  • (2) propane
  • (3) methyl butane
  • (4) methyl propane
Answer: (3) methyl butane 

26. In which substance does chlorine have an oxidation number of +1?

  • (1) Cl2
  • (2) HCl
  • (3) HClO
  • (4) HClO2
Answer: (3) HClO 

27. Which statement is true for any electrochemical cell?

  • (1) Oxidation occurs at the anode, only.
  • (2) Reduction occurs at the anode, only.
  • (3) Oxidation occurs at both the anode and the cathode.
  • (4) Reduction occurs at both the anode and the cathode.
Answer: (1) Oxidation occurs at the anode, only. 

28. Given the equation:

2 Al + 3 Cu2+ → 2 Al3+ + 3 Cu

The reduction half-reaction is

  • (1) Al → Al3+ + 3e
  • (2) Cu2+ + 2e → Cu
  • (3) Al + 3e → Al3+
  • (4) Cu2+ → Cu + 2e
Answer: (2) Cu2+ + 2e → Cu 

29. Which 0.1 M solution contains an electrolyte?

  • (1) C6H12O6(aq)
  • (2) CH3COOH(aq)
  • (3) CH3OH(aq)
  • (4) CH3OCH3(aq)
Answer: (2) CH3COOH(aq) 

30. Which equation represents a neutralization reaction?

  • (1) Na2CO3 + CaCl2 → 2 NaCl + CaCO3
  • (2) Ni(NO3)2 + H2S → NiS + 2 HNO3
  • (3) NaCl + AgNO3 → AgCl + NaNO3
  • (4) H2SO4 + Mg(OH)2 → MgSO4 + 2 H2O
Answer: (4) H2SO4 + Mg(OH)2 → MgSO4 + 2 H2O 

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