Earth Science June 2003 Questions Answers Keys.
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
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
2. Which subatomic particle has no charge?
- (1) alpha particle
- (2) beta particle
- (3) neutron
- (4) electron
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
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
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
6. Which is a property of most nonmetallic solids?
- (1) high thermal conductivity
- (2) high electrical conductivity
- (3) brittleness
- (4) malleability
7. Alpha particles are emitted during the radioactive decay of
- (1) carbon-14
- (2) neon-19
- (3) calcium-37
- (4) radon-222
8. Which is an empirical formula?
- (1) P2O5
- (2) P4O6
- (3) C2H4
- (4) C3H6
9. Which substance can be decomposed by a chemical change?
- (1) Co
- (2) CO
- (3) Cr
- (4) Cu
10. The percent by mass of calcium in the compound calcium sulfate (CaSO4) is approximately
- (1) 15%
- (2) 29%
- (3) 34%
- (4) 47%
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
12. Which type of chemical bond is formed between two atoms of bromine?
- (1) metallic
- (2) hydrogen
- (3) ionic
- (4) covalent
13. Which of these formulas contains the most polar bond?
- (1) H–Br
- (2) H–Cl
- (3) H–F
- (4) H–I
14. According to Table F, which of these salts is least soluble in water?
- (1) LiCl
- (2) RbCl
- (3) FeCl2
- (4) PbCl2
15. Which of these terms refers to matter that could be heterogeneous?
- (1) element
- (2) mixture
- (3) compound
- (4) solution
16. In which material are the particles arranged in a regular geometric pattern?
- (1) CO2(g)
- (2) NaCl(aq)
- (3) H2O()
- (4) C12H22O11(s)
17. Which change is exothermic?
- (1) freezing of water
- (2) melting of iron
- (3) vaporization of ethanol
- (4) sublimation of iodine
18. Which type of change must occur to form a compound?
- (1) chemical
- (2) physical
- (3) nuclear
- (4) phase
19. Which formula correctly represents the composition of iron (III) oxide?
- (1) FeO3
- (2) Fe2O3
- (3) Fe3O
- (4) Fe3O2
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
21. Which hydrocarbon is saturated?
- (1) propene
- (2) ethyne
- (3) butene
- (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.
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
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
25. Which compound is an isomer of pentane?
- (1) butane
- (2) propane
- (3) methyl butane
- (4) methyl propane
26. In which substance does chlorine have an oxidation number of +1?
- (1) Cl2
- (2) HCl
- (3) HClO
- (4) HClO2
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.
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–
29. Which 0.1 M solution contains an electrolyte?
- (1) C6H12O6(aq)
- (2) CH3COOH(aq)
- (3) CH3OH(aq)
- (4) CH3OCH3(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
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