Earth Science August 2000 Questions Answers Keys.
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
Wednesday, August 16, 2000 — 12:30 to 3:30 p.m., only
Directions : For each statement or question, select the word or expression that, of those given, best completes the statement or answers the question. Record your answer on the separate answer sheet in accordance with the directions on the front page of this booklet
1. If 60. liters of hydrogen gas at 546 K is cooled to 273 K at constant pressure, the new volume of the gas will be
- (1) 120 L
- (2) 20. L
- (3) 30. L
- (4) 40. L
2. Which phase change at STP represents sublimation?
- (1) CO2(s) → CO2(g)
- (2) H2O(s) → H2O()
- (3) CO2(L) → CO2(g)
- (4) H2O(L) → H2O(s)
3. Which sample of Fe contains particles having the highest average kinetic energy?
- (1) 5 g at 10°C
- (2) 10 g at 25°C
- (3) 5 g at 400 K
- (4) 10 g at 300 K
4. An example of a binary compound is
- (1) He
- (2) H2O
- (3) H2
- (4) H2SO4
5. Water will boil at 22°C if the pressure on the surface of the water is
- (1) 760.0 mmHg
- (2) 92.5 mmHg
- (3) 19.8 mmHg
- (4) 4.6 mmHg
6. Which electron configuration represents an atom in the excited state?
- (1) 1s22s22p53s1
- (2) 1s22s22p63s1
- (3) 1s 22s22p6 3s2
- (4) 1s22s22p63s23p1
7. What is the charge and mass of a proton?
8. The orbital notation of an atom in the ground
Which atom is represented by this notation?
- (1) C
- (2) N
- (3) B
- (4) Be
9. An experiment in which alpha particles were used to bombard thin sheets of gold foil led to the conclusion that an atom is composed mostly of
- (1) empty space and has a small, negatively charged nucleus
- (2) empty space and has a small, positively charged nucleus
- (3) a large, dense, positively charged nucleus
- (4) a large, dense, negatively charged nucleus
10. In which two atoms do both nuclides contain the same number of neutrons?
11. What is the total number of sublevels in an atom’s fourth principal energy level?
- (1) 8
- (2) 16
- (3) 3
- (4) 4
12. The characteristic bright-line spectrum of an element is produced when electrons
- (1) absorb quanta and return to lower energy levels
- (2) absorb quanta and move to higher energy levels
- (3) release quanta and return to lower energy levels
- (4) release quanta and move to higher energy levels
13. Which Group 16 element when combined with hydrogen forms a compound that would exhibit the strongest hydrogen bonding?
- (1) selenium
- (2) tellurium
- (3) oxygen
- (4) sulfur
14. Given the reaction:
Cl(g) + Cl(g) → Cl2(g) + energy
Which statement best describes the reaction?
- (1) A bond is formed and energy is absorbed.
- (2) A bond is formed and energy is released.
- (3) A bond is broken and energy is absorbed.
- (4) A bond is broken and energy is released.
15. Which formula is correct for ammonium sulfate?
- (1) NH4SO4
- (2) (NH4)2SO4
- (3) NH4(SO4)2
- (4) (NH4)2(SO4)2
16. An example of an empirical formula is
- (1) CH4
- (2) C2H4
- (3) C2H4(OH)2
- (4) C6H12O6
17. Which compound is a network solid at STP?
- (1) CO2
- (2) H2O
- (3) SiC
- (4) NaH
18. What occurs when a coordinate covalent bond is formed between nitrogen and hydrogen in the ammonium ion, NH4+?
- (1) Hydrogen provides a pair of electrons to be shared with nitrogen.
- (2) Nitrogen provides a pair of electrons to be shared with hydrogen.
- (3) Hydrogen transfers a pair of electrons to nitrogen.
- (4) Nitrogen transfers a pair of electrons to hydrogen.
19. A hard substance that has a high melting point and is a poor conductor of electricity in the solid phase could be
- (1) CO2
- (2) Mg
- (3) NaCl
- (4) CCl4
20. Which element exhibits both metallic and nonmetallic properties?
- (1) bismuth
- (2) helium
- (3) silver
- (4) tellurium
21. Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table?
- (1) The number of principal energy levels increases, and the number of valence electrons increases.
- (2) The number of principal energy levels increases, and the number of valence electrons remains the same.
- (3) The number of principal energy levels remains the same, and the number of valence electrons increases.
- (4) The number of principal energy levels remains the same, and the number of valence electrons decreases.
22. Which substance at STP exists in the form of a monatomic gas?
- (1) neon
- (2) oxygen
- (3) chlorine
- (4) nitrogen
23. Which noble gas has the highest first ionization energy?
- (1) radon
- (2) krypton
- (3) neon
- (4) helium
24. Atoms of which set of elements all exhibit the same oxidation state?
- (1) actinoid series
- (2) metalloids
- (3) alkaline earth metals
- (4) transition metals
25. Given the reactions:
2X(s) + 2H2O(L) → 2X+ (aq)+ 2OH– (aq) + H2(g)
2Y(s) + 2H2O(L) → 2Y+ (aq)+ 2OH– (aq) + H2(g)
The unknowns, X and Y, are most likely
- (1) metallic elements in the same group
- (2) metallic elements in the same period
- (3) nonmetallic elements in the same group
- (4) nonmetallic elements in the same period
26. Given the balanced equation:
2Na + S → Na2S
What is the total number of moles of S that reacted when 4.0 moles of Na were completely consumed?
- (1) 1.0 mole
- (2) 2.0 moles
- (3) 0.5 mole
- (4) 4.0 moles
27. What is the gram formula mass of Ca3(PO4)2?
- (1) 196 g
- (2) 214 g
- (3) 245 g
- (4) 310. g
28. Which compound contains the greatest percentage of chlorine by mass?
- (1) HCl
- (2) NaCl
- (3) FeCl2
- (4) ZnCl2
29. What is the total number of grams of HI in 0.500 liter of 1.00 M HI?
- (1) 1.00 g
- (2) 0.500 g
- (3) 64.0 g
- (4) 128 g
30. At STP, what is the total volume occupied by a 2.00-gram sample of H2(g)?
- (1) 1.00 L
- (2) 2.00 L
- (3) 11.2 L
- (4) 22.4 L
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