Earth Science August 2000

Earth Science August 2000 Questions Answers Keys.

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

Answer: (3) 30. 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)

Answer: (1) CO₂(s) → CO₂(g)

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

Answer: (3) 5 g at 400 K

4. An example of a binary compound is

(1) He
(2) H₂O
(3) H₂
(4) H₂SO₄

Answer: (2) H₂O

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

Answer: (3) 19.8 mmHg

6. Which electron configuration represents an atom in the excited state?

(1) 1s²2s²2p⁵3s¹
(2) 1s²2s²2p⁶3s¹
(3) 1s ²2s²2p⁶ 3s²
(4) 1s²2s²2p⁶3s²3p¹

Answer: (1) 1s²2s²2p⁵3s¹

7. What is the charge and mass of a proton?

Answer: (1)

8. The orbital notation of an atom in the ground
state is

Which atom is represented by this notation?

(1) C
(2) N
(3) B
(4) Be

Answer: (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

Answer: (2) empty space and has a small, positively charged nucleus

10. In which two atoms do both nuclides contain the same number of neutrons?

Answer: (4)

11. What is the total number of sublevels in an atom’s fourth principal energy level?

(1) 8
(2) 16
(3) 3
(4) 4

Answer: (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

Answer: (3) release quanta and return to lower 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

Answer: (3) oxygen

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.

Answer: (2) A bond is formed 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

Answer: (2) (NH₄)₂SO₄

16. An example of an empirical formula is

(1) CH₄
(2) C₂H₄
(3) C₂H₄(OH)₂
(4) C₆H₁₂O₆

Answer: (1) CH₄

17. Which compound is a network solid at STP?

(1) CO₂
(2) H₂O
(3) SiC
(4) NaH

Answer: (3) SiC

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.

Answer: (2) Nitrogen provides a pair of electrons to be shared with 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

Answer: (3) NaCl

20. Which element exhibits both metallic and nonmetallic properties?

(1) bismuth
(2) helium
(3) silver
(4) tellurium

Answer: (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.

Answer: (2) The number of principal energy levels increases, and the number of valence electrons remains the same.

22. Which substance at STP exists in the form of a monatomic gas?

(1) neon
(2) oxygen
(3) chlorine
(4) nitrogen

Answer: (1) neon

23. Which noble gas has the highest first ionization energy?

(1) radon
(2) krypton
(3) neon
(4) helium

Answer: (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

Answer: (3) alkaline earth 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

Answer: (1) metallic elements in the same group

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

Answer: (2) 2.0 moles

27. What is the gram formula mass of Ca₃(PO₄)₂?

(1) 196 g
(2) 214 g
(3) 245 g
(4) 310. g

Answer: (4) 310. g

28. Which compound contains the greatest percentage of chlorine by mass?

(1) HCl
(2) NaCl
(3) FeCl₂
(4) ZnCl₂

Answer: (1) HCl

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

Answer: (3) 64.0 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

Answer: (4) 22.4 L

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