Earth Science June 1998

Earth Science June 1998 Questions Answers Keys.

The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
CHEMISTRY
Tuesday,June 23, 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 diagrams below represent two solids and the temperature of each.

What occurs when the two solids are placed in contact with each other?

  • (1) Heat energy flows from solid A to solid B. Solid A decreases in temperature.
  • (2) Heat energy flows from solid A to solid B. Solid A increases in temperature.
  • (3) Heat energy flows from solid B to solid A. Solid B decreases in temperature.
  • (4) Heat energy flows from solid B to solid A. Solid B increases in temperature.
Answer: (3) Heat energy flows from solid B to solid A. Solid B decreases in temperature. 

2. The particles of a substance are arranged in a definite geometric pattern and are constantly vibrating. This substance can be in

  • (1) the solid phase, only
  • (2) the liquid phase, only
  • (3) either the liquid or the solid phase
  • (4) neither the liquid nor the solid phase
Answer: (1) The solid phase, only 

3. What is the pressure of a mixture of CO2. SO2, and H20 gases, if each gas has a partial pressure of 250 torr?

  • (1) 250 torr
  • (2) 500 torr
  • (3) 750 torr
  • (4) 1000 torr
Answer: (3) 750 torr 

4. Which substances can be decomposed chemically?

  • (1) CaO and Ca
  • (2) MgO and Mg
  • (3) CO and Co
  • (4) GaO and MgO
Answer: (4) GaO and MgO 

5. A gas sample has a volume of 25.0 milliliters at a pressure of 1.00 atmosphere. If the volume increases to 50.0 milliliters and the temperature remains constant, the new pressure will be

  • (1) 1.00 atm
  • (2) 2.00 atm
  • (3) 0.250 atm
  • (4) 0.500 atm
Answer: (4) 0.500 atm 

6. An atom with the electron configuration 1s22s22p63s23p63d54s2 has an incomplete

  • (1) 2p sublevel
  • (2) second principal energy level
  • (3) third principal energy level
  • (4) 4s sublevel
Answer: (3) third principal energy level 

7. Which orbital notation represents a boron atom in the ground state?

Answer: (2)  
Answer: (2)  

9. Which subatomic particle is found in the nucleus of all isotopes of hydrogen?

  • (1) proton
  • (2) neutron
  • (3) electron
  • (4) positron
Answer: (1) proton 

10. What is the highest principal quantum number (n) for an electron in an atom of sulfur in the ground state?

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

11. What is the total number of electrons in a comp letely filled fourth principal energy level?

  • (1) 8
  • (2) 10
  • (3) 16
  • (4) 32
Answer: (4) 32 

12. What is the total number of hydrogen atoms required to form 1 molecule of C3H5(OH)3?

  • (1) 1
  • (2) 5
  • (3) 3
  • (4) 8
Answer: (4) 8 

13. Which element is found in both potassium chlorate and zinc nitrate?

  • (1) hydrogen
  • (2) oxygen
  • (3) potassium
  • (4) zinc
Answer: (2) oxygen 

14. Which formula represents lead (II) phosphate?

  • (1) PbPO4
  • (2) Pb4PO4
  • (3) Pb3(P04)2
  • (4) Pb2(P04)3
Answer: (3) Pb3(P04)2 

15. Atoms of which element have the weakest attraction for electrons?

  • (1) Na
  • (2) P
  • (3) Si
  • (4) S
Answer: (1) Na 

16. The ability to conduct electricity in the solid state is a characteristic of metallic bonding. This characteristic is best explained by the presence of

  • (1) high ionization energies
  • (2) high electronegativities
  • (3) mobile electrons
  • (4) mobile protons
Answer: (3) mobile electrons 

17. When ionic bonds are formed, metallic atoms tend to

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

18. The bond between hydrogen and oxygen in a water molecule is classified as

  • (1) ionic and nonpolar
  • (2) ionic and polar
  • (3) covalent and nonpolar
  • (4) covalent and polar
Answer: (4) covalent and polar 

19. According to the Periodic Table, which element has more than one positive oxidation state?

  • (1) cadmium
  • (2) iron
  • (3) silver
  • (4) zinc
Answer: (2) iron 

20. Which group contains a liquid that is a nonmetal at STP?

  • (1) 14
  • (2) 15
  • (3) 16
  • (4) 17
Answer: (4) 17 

21. Which of these Group 14 elements has the most metallic properties?

  • (1) C
  • (2) Ge
  • (3) Si
  • (4) Sn
Answer: (4) Sn 

22. As the elements in Group 2 are considered in order of increasing atomic number, the atomic radius of each successive element increases. This increase is primarily due to an increase in the number of

  • (1) occupied principal energy levels
  • (2) electrons in the outermost shell
  • (3) neutrons in the nucleus
  • (4) unpaired electrons
Answer: (1) occupied principal energy levels 

23. Which element is classifIed as a metalloid (semimetal)?

  • (1) sulfur
  • (2) silicon
  • (3) barium
  • (4) bromine
Answer: (2) silicon 

24. Which element in Group 1 has the greatest tendency to lose an electron?

  • (1) cesium
  • (2) rubidium
  • (3) potassium
  • (4) sodium
Answer: (1) cesium 

25. The table below shows some properties of elements A, B, C, and D.

Which element is most likely a nonmetal?

  • (1) A
  • (2) B
  • (3) C
  • (4) D
Answer: (3) C 

26. What is the gram formula mass of Ca3(P04)2?

  • (1) 135 g/mol
  • (2) 215 g/mol
  • (3) 278 WmoI
  • (4) 310. g/mol
Answer: (4) 310. g/mol 

27. The gram atomic mass of oxygen is 16.0 grams per mole. How many atoms of oxygen does this mass represent?

  • (1) 16.0
  • (2) 32.0
  • (3) 6.02 x 1023
  • (4) 2(6.02 x 1023)
Answer: (3) 6.02 x 1023 

28. Given the unbatanced equation:

N2(g) + H2(g) → NH3(g)

When the equation is balanced using smallest whole-number coefficients, the ratio of moles of hydrogen consumed to moles of ammonia produced is

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

29. What is the concentration of a solution of 10. moles of copper (II) nitrate in 5.0 liters of solution?

  • (1) O.50M
  • (2) 2.0 M
  • (3) 5.OM
  • (4) 10. M
Answer: (2) 2.0 M 

30. Given the balanced equation:

Mg(s) + 2HCl(aq) → MgCl(aq) + H2(g)

At STP?, what is the total number of liters of hydrogen gas produced when 3.00 moles of hydrochloric acid solution is completely consumed?

  • (1) 11.2 L
  • (2) 22.4 L
  • (3) 33.6 L
  • (4) 44.8 L
Answer: (3) 33.6 L 

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