Earth Science June 2001

Earth Science June 2001 Questions Answers Keys.

The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
CHEMISTRY
Thursday, June 21, 2001 — 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. Which graph best shows the relationship between Kelvin temperature and average kinetic energy?

Answer: (1)  

2. At 1 atmosphere of pressure, water and ice can exist in equilibrium at a temperature of

  • (1) 212°C
  • (2) 100°C
  • (3) 32°C
  • (4) 0°C
Answer: (4) 0°C 

3. Which unit is used to express the energy absorbed or released during a chemical reaction?

  • (1) kelvin
  • (2) calorie
  • (3) volt
  • (4) torr
Answer: (2) calorie 

4. When the vapor pressure of water is 149.4 torr, the temperature of the water is

  • (1) 20°C
  • (2) 40°C
  • (3) 60°C
  • (4) 80°C
Answer: (3) 60°C 

5. Which substance will readily sublime at STP?

  • (1) Fe(s)
  • (2) C6H12O6(s)
  • (3) NaCl(s)
  • (4) CO2(s)
Answer: (4) CO2(s) 

6. Standard temperature and a pressure of 0.5 atmosphere are equal to

  • (1) 0°C and 380 torr
  • (2) 32°C and 380 torr
  • (3) 0°C and 760 torr
  • (4) 32°C and 760 torr
Answer: (1) 0°C and 380 torr 

7. An atom of fluorine has a mass of 19 atomic mass units. The total number of protons and neutrons in its nucleus is

  • (1) 9
  • (2) 10
  • (3) 19
  • (4) 28
Answer: (3) 19 

Which type of emanation is represented by X?

  • (1) alpha particle
  • (2) beta particle
  • (3) proton
  • (4) positron
Answer: (1) alpha particle  

9. What is the atomic number of an element that has six protons and eight neutrons?

  • (1) 6
  • (2) 2
  • (3) 8
  • (4) 14
Answer: (1) 6 

10. Which statement about the mass of an electron is correct?

  • (1) The mass of an electron is equal to the mass of a proton.
  • (2) The mass of an electron is less than the mass of a proton.
  • (3) The mass of an electron is equal to the mass of a neutron.
  • (4) The mass of an electron is greater than the mass of a neutron.
Answer: (2) The mass of an electron is less than the mass of a proton. 

11. How many electrons are in the outermost principal energy level of an atom of carbon in the ground state?

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

12. In which group do the particles contain only nucleons?

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

13. Given the electron dot diagram:

The electrons in the bond between hydrogen and flourine are more strongly attracted to the atom of

  • (1) hydrogen, which has the higher electronegativity
  • (2) fluorine, which has the higher electronegativity
  • (3) hydrogen, which has the lower electronegativity
  • (4) fluorine, which has the lower electronegativity
Answer: (2) fluorine, which has the higher electronegativity 

14. In which system do molecule-ion attractions exist?

  • (1) KCl(s)
  • (2) KCl(aq)
  • (3) KCl(l)
  • (4) KCl(g)
Answer: (2) KCl(aq) 

15. In which compound do atoms form bonds by sharing electrons?

  • (1) H2O
  • (2) Na2O
  • (3) CaO
  • (4) MgO
Answer: (1) H2 

16. Which type of attraction results from the formation of weak momentary dipoles?

  • (1) ionic
  • (2) metallic
  • (3) molecule-ion
  • (4) van der Waals forces
Answer: (4) van der Waals forces 

17. Which substance contains nonpolar covalent bonds?

  • (1) H2
  • (2) H2O
  • (3) Ca(OH)2
  • (4) CaO
Answer: (1) H2 

18. Silicon dioxide (SiO2) and diamonds are best described as

  • (1) molecular substances with coordinate covalent bonding
  • (2) molecular substances with ionic bonding
  • (3) network solids with covalent bonding
  • (4) network solids with ionic bonding
Answer: (3) network solids with covalent bonding 

19. When a reaction occurs between atoms with ground-state electron configurations of 1s22s1 and 1s22s2 2p5 , the bond formed is mainly

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

20. According to Reference Table K, which sequence correctly places the elements in order of increasing ionization energy?

  • (1) H → Li → Na → K
  • (2) I → Br → Cl → F
  • (3) O → S → Se → Te
  • (4) H → Be → Al → Ga
Answer: (2) I → Br → Cl → F 

21. Which of the following Period 4 elements has the most metallic characteristics?

  • (1) Ca
  • (2) Ge
  • (3) As
  • (4) Br
Answer: (1) Ca  

22. Which element is an alkali metal?

  • (1) Na
  • (2) Mg
  • (3) Al
  • (4) Cl
Answer: (1) Na  

23. In general, atoms of transition elements in Period 5 are characterized by an incomplete

  • (1) 3p subshell
  • (2) 4p subshell
  • (3) 3d subshell
  • (4) 4d subshell
Answer: (4) 4d subshell 

24. Most of the groups in the Periodic Table of the Elements contain

  • (1) nonmetals, only
  • (2) metals, only
  • (3) nonmetals and metals
  • (4) metals and metalloids
Answer: (2) metals, only 

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

Answer: (1)  

26. The empirical formula of a compound is CH3. The molecular formula of this compound could be

  • (1) CH4
  • (2) C2H4
  • (3) C2H6
  • (4) C3H6
Answer: (3) C2H6 

27. Given the equation:

H2(g) + Cl2(g) → 2HCl(g)

What is the total number of moles of HCl(g) produced when 3 moles of H2(g) is completely consumed?

  • (1) 5 moles
  • (2) 2 moles
  • (3) 3 moles
  • (4) 6 moles
Answer: (4) 6 moles 

28. The number of moles of molecules in a 12.0-gram sample of Cl2 is

Answer: (2)  

29. The percent by mass of water in the hydrate Na2SO4•10H2O is closest to

  • (1) 18%
  • (2) 44%
  • (3) 56%
  • (4) 76%
Answer: (3) 56% 

30. Which compound is least soluble in 100 grams of water at 40°C?

  • (1) SO2
  • (2) NaCl
  • (3) KClO3
  • (4) NH4Cl
Answer: (1) SO2 

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