Earth Science January 2001

Earth Science January 2001 Questions Answers Keys.

The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
CHEMISTRY
Tuesday, January 23, 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. The heat absorbed when ice melts can be measured in a unit called a

  • (1) torr
  • (2) degree
  • (3) mole
  • (4) calorie
Answer: (4) calorie 

2. Which substance is a binary compound?

  • (1) ammonia
  • (2) argon
  • (3) glucose
  • (4) glycerol
Answer: (2) argon 

3. Which sample of matter is a mixture?

  • (1) H2O(s)
  • (2) H2O(g)
  • (3) NaCl(l)
  • (4) NaCl(aq)
Answer: (4) NaCl(aq) 

4. Which graph best represents the variation in the vapor pressure of water as temperature changes?

Answer: (4)  

5. Which atom in the ground state has five electrons in its outer level and ten electrons in its kernel?

  • (1) C
  • (2) Cl
  • (3) Si
  • (4) P
Answer: (4) P 

6. Which type of radiation continues in a straight line when passed through an electric field?

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

8. When an atom loses an electron, the atom becomes an ion that is

  • (1) positively charged and gains a small amount of mass
  • (2) positively charged and loses a small amount of mass
  • (3) negatively charged and gains a small amount of mass
  • (4) negatively charged and loses a small amount of mass
Answer: (2) positively charged and loses a small amount of mass 

9. The nucleus of which atom contains 48 neutrons?

Answer: (3)  

10. Experiments performed to reveal the structure of atoms led scientists to conclude that an atom’s

  • (1) positive charge is evenly distributed throughout its volume
  • (2) negative charge is mainly concentrated in its nucleus
  • (3) mass is evenly distributed throughout its volume
  • (4) volume is mainly unoccupied
Answer: (4) volume is mainly unoccupied 

11. Given the unbalanced equation:

Al(s) + O2(g) → Al2O3(s)

When this equation is correctly balanced using smallest whole numbers, what is the coefficient of O2(g)?

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

12. Which pair of atoms is held together by a covalent bond?

  • (1) HCl
  • (2) LiCl
  • (3) NaCl
  • (4) KCl
Answer: (1) HCl 

13. The formula H2O2 is an example of

  • (1) a molecular formula
  • (2) an empirical formula
  • (3) an ionic formula
  • (4) an organic formula
Answer: (1) a molecular formula 

14. What happens when NaCl(s) is dissolved in water?

  • (1) Cl ions are attracted to the oxygen atoms of water molecules.
  • (2) Na+  ions are attracted to the oxygen atoms of water molecules.
  • (3) Cl ions are repelled by the hydrogen atoms of water molecules.
  • (4) Na+  ions are repelled by the oxygen atoms of water molecules.
Answer: (2) Na+  ions are attracted to the oxygen atoms of water molecules. 

15. Which molecule has an asymmetrical shape?

  • (1) N2
  • (2) NH3
  • (3) Cl2
  • (4) CCl4
Answer: (2) NH3 

16. The forces between atoms that create chemical bonds are the result of interactions between

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

17. Which Group 16 element undergoes natural radioactive disintegration?

  • (1) Po
  • (2) S
  • (3) Se
  • (4) Te
Answer: (1) Po  

18. Pure silicon is chemically classified as a metalloid because silicon

  • (1) is malleable and ductile
  • (2) is an excellent conductor of heat and electricity
  • (3) exhibits hydrogen bonding
  • (4) exhibits metallic and nonmetallic properties
Answer: (4) exhibits metallic and nonmetallic properties 

19. In which group of elements do most atoms have completely filled s and p valence sublevels?

  • (1) halogens
  • (2) noble gases
  • (3) alkali metals
  • (4) alkaline earth metals
Answer: (2) noble gases 

20. Which ion has the largest radius?

  • (1) Na+
  • (2) Mg2+
  • (3) K+
  • (4) Ca2+
Answer: (3) K+ 

21. An aqueous solution of XCl2 contains colored ions. Element X could be

  • (1) Ba
  • (2) Ca
  • (3) Ni
  • (4) Bi
Answer: (3) Ni 

22. Which properties are most common in nonmetals?

  • (1) low ionization energy and low electronegativity
  • (2) low ionization energy and high electronegativity
  • (3) high ionization energy and low electronegativity
  • (4) high ionization energy and high electronegativity
Answer: (4) high ionization energy and high electronegativity 

23. One mole of O2 has approximately the same mass as one mole of

  • (1) CH4
  • (2) S
  • (3) LiH
  • (4) Cl2
Answer: (2) S 

24. Based on Reference Table E, which compound could form a concentrated solution?

  • (1) AgBr
  • (2) AgCl
  • (3) Ag2CO3
  • (4) AgNO3
Answer: (4) AgNO3 

25. A 2.00-liter sample of a gas has a mass of 1.80 grams at STP. What is the density, in grams per liter, of this gas at STP?

  • (1) 0.900
  • (2) 1.80
  • (3) 11.2
  • (4) 22.4
Answer: (1) 0.900  

26. What is the total number of neon atoms contained in 20.2 grams of neon gas?

  • (1) 1.01 × 1024
  • (2) 2.02 × 1024
  • (3) 3.01 × 1023
  • (4) 6.02 × 1023
Answer: (4) 6.02 × 1023 

27. What is the total number of moles of oxygen atoms in 1 mole of N2O3?

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

28. Which 1.0-mole sample at 1 atm has particles with the greatest entropy?

  • (1) CH4(g) at 25°C
  • (2) H2S(g) at 40°C
  • (3) CH4(g) at 300 K
  • (4) H2S(g) at 310 K
Answer: (2) H2S(g) at 40°C 

29. A 1.0-gram sample of powdered Zn reacts fasterwith HCl than a single 1.0-gram piece of Zn because the surface atoms in powdered Zn have

  • (1) higher average kinetic energy
  • (2) lower average kinetic energy
  • (3) more contact with the H+ ions in the acid
  • (4) less contact with the H+ ions in the acid
Answer: (3) more contact with the H+ ions in the acid 

30. In a reversible reaction, chemical equilibrium is attained when the

  • (1) rate of the forward reaction is greater than the rate of the reverse reaction
  • (2) rate of the reverse reaction is greater than the rate of the forward reaction
  • (3) concentration of the reactants reaches zero
  • (4) concentration of the products remains constant
Answer: (4) concentration of the products remains constant 

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