Earth Science June 2000

Earth Science June 2000 Questions Answers Keys.

The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
CHEMISTRY
Thursday, June 22, 2000 — 9:15 a.m. to 12:15 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. The formula Al2S3 represents

  • (1) an element
  • (2) a binary compound
  • (3) a ternary compound
  • (4) a mixture
Answer: (2) a binary compound 

2. As the temperature of a gas is increased from 0°C to 10°C at constant pressure, the volume of the gas will

Answer: (2)  

3. Water boils at 90°C when the pressure exerted on the liquid is equal to

  • (1) 50.0 torr
  • (2) 100.0 torr
  • (3) 525.8 torr
  • (4) 760.0 torr
Answer: (3) 525.8 torr 

4. Which species readily sublimes at room temperature?

  • (1) CO2(s)
  • (2) CO2(L)
  • (3) CO2(g)
  • (4) CO2(aq)
Answer: (1) CO2(s) 

5. Which statement best describes all compounds?

  • (1) They can be decomposed by chemical change.
  • (2) They can be decomposed by physical means.
  • (3) They contain at least three elements.
  • (4) They contain ionic bonds.
Answer: (1) They can be decomposed by chemical change. 

6. What is the electron configuration of a Mn atom in the ground state?

  • (1) 1s22s22p63s2
  • (2) 1s22s22p63s23p63d54s2
  • (3) 1s22s22p63s23p63d54s14p1
  • (4) 1s22s22p63s23p63d7
Answer: (2) 1s22s22p63s23p63d54s2 

7. Which orbital notation correctly represents a noble gas in the ground state?

Answer: (3)  

8. Which type of radiation has zero mass and zero charge?

  • (1) alpha
  • (2) beta
  • (3) neutron
  • (4) gamma
Answer: (4) gamma 
  • (1) 37
  • (2) 49
  • (3) 86
  • (4) 123
Answer: (3) 86 

10. What is the total number of valence electrons in an atom of boron in the ground state?

  • (1) 1
  • (2) 7
  • (3) 3
  • (4) 5
Answer: (3) 3 

11. What causes the emission of radiant energy that produces characteristic spectral lines?

  • (1) neutron absorption by the nucleus
  • (2) gamma ray emission from the nucleus
  • (3) movement of electrons to higher energy levels
  • (4) return of electrons to lower energy levels
Answer: (4) return of electrons to lower energy levels 

12. Which atom in the ground state has three halffilled orbitals?

  • (1) P
  • (2) Si
  • (3) Al
  • (4) Li
Answer: (1) P 

13. Which particles may be gained, lost, or shared by an atom when it forms a chemical bond?

  • (1) protons
  • (2) electrons
  • (3) neutrons
  • (4) nucleons
Answer: (2) electrons 

14. Which molecular formula is correctly paired with its corresponding empirical formula?

  • (1) CO2 and CO
  • (2) C2H2 and CH2
  • (3) C6H6 and C2H2
  • (4) P4O10 and P2O5
Answer: (4) P4O10 and P2O5 

15. Which of the following elements has the strongest attraction for electrons?

  • (1) boron
  • (2) aluminum
  • (3) oxygen
  • (4) sulfur
Answer: (3) oxygen 

16. The table below shows four compounds and the boiling point of each.

Which type of molecular attraction accounts for the high boiling point of H2O?

  • (1) molecule–ion
  • (2) ion–ion
  • (3) hydrogen bonding
  • (4) van der Waals forces
Answer: (3) hydrogen bonding 

17. Which elements are both classified as metalloids?

  • (1) Ge and As
  • (2) Bi and Po
  • (3) B and C
  • (4) Si and P
Answer: (1) Ge and As 

18. Which electron dot diagram represents a molecule that has a polar covalent bond?

Answer: (1)  

19. What is the total number of moles of atoms present in 1 gram formula mass of Pb(C2H3O2)2?

  • (1) 9
  • (2) 14
  • (3) 3
  • (4) 15
Answer: (4) 15 

20. Elements in the Periodic Table are arranged according to their

  • (1) atomic number
  • (2) atomic mass
  • (3) relative activity
  • (4) relative size
Answer: (1) atomic number  

21. Which Group 15 element exists as a diatomic molecule at STP?

  • (1) phosphorus
  • (2) nitrogen
  • (3) bismuth
  • (4) arsenic
Answer: (2) nitrogen 

22. Which element reacts vigorously with water?

  • (1) Zn
  • (2) Cu
  • (3) Fe
  • (4) Li
Answer: (4) Li 

23. Atoms of metals tend to

  • (1) lose electrons and form negative ions
  • (2) lose electrons and form positive ions
  • (3) gain electrons and form negative ions
  • (4) gain electrons and form positive ions
Answer: (2) lose electrons and form positive ions 

24. Which halogen is a solid at STP?

  • (1) Br2
  • (2) F2
  • (3) Cl2
  • (4) I2
Answer: (4) I2 

25. What is the total number of molecules in a 0.5-mole sample of He gas?

  • (1) 6 x 1023
  • (2) 2 x 1023
  • (3) 3 x 1023
  • (4) 4 x 1023
Answer: (3) 3 x 1023 

26. What occurs as the atomic number of the elements in Period 2 increases?

  • (1) The nuclear charge of each successive atom decreases, and the covalent radius decreases.
  • (2) The nuclear charge of each successive atom decreases, and the covalent radius increases.
  • (3) The nuclear charge of each successive atom increases, and the covalent radius decreases.
  • (4) The nuclear charge of each successive atom increases, and the covalent radius increases.
Answer: (3) The nuclear charge of each successive atom increases, and the covalent radius decreases. 

27. Given the balanced equation:

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

What is the total number of liters of CO2(g) produced when 20.0 liters of O2(g) are completely consumed?

  • (1) 12.0 L
  • (2) 22.4 L
  • (3) 3.00 L
  • (4) 5.00 L
Answer: (1) 12.0 L  

28. Given the balanced equation:

Fe(s) + CuSO4(aq) → FeSO4(aq)+ Cu(s)

What total mass of iron is necessary to produce 1.00 mole of copper?

  • (1) 26.0 g
  • (2) 55.8 g
  • (3) 112 g
  • (4) 192 g
Answer: (2) 55.8 g 

29. The percent by mass of nitrogen in NH4NO3 is closest to

  • (1) 15%
  • (2) 20.%
  • (3) 35%
  • (4) 60.%
Answer: (3) 35% 

30. What is the molarity of a solution that contains 40. grams of NaOH in 0.50 liter of solution?

  • (1) 1.0 M
  • (2) 2.0 M
  • (3) 0.50 M
  • (4) 0.25 M
Answer: (2) 2.0 M 

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