Earth Science June 2005

Earth Science June 2005 Questions Answers Keys.

The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Wednesday, June 22, 2005 — 1:15 to 4:15 p.m., only

Directions : For each statement or question, write on the separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry.

1. In the modern wave-mechanical model of the atom, the orbitals are regions of the most probable location of

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

2. Compared to a proton, an electron has

  • (1) a greater quantity of charge and the same sign
  • (2) a greater quantity of charge and the opposite sign
  • (3) the same quantity of charge and the same sign
  • (4) the same quantity of charge and the opposite sign
Answer: (4) the same quantity of charge and the opposite sign 

3. Which two notations represent atoms that are isotopes of the same element?

Answer: (1)  

4. The elements in Period 5 on the Periodic Table are arranged from left to right in order of

  • (1) decreasing atomic mass
  • (2) decreasing atomic number
  • (3) increasing atomic mass
  • (4) increasing atomic number
Answer: (4) increasing atomic number 

5. Which list of elements contains a metal, a metalloid, and a nonmetal?

  • (1) Zn, Ga, Ge
  • (2) Si, Ge, Sn
  • (3) Cd, Sb, I
  • (4) F, Cl, Br
Answer: (3) Cd, Sb, I 

6. An example of a physical property of an element is the element’s ability to

  • (1) react with an acid
  • (2) react with oxygen
  • (3) form a compound with chlorine
  • (4) form an aqueous solution
Answer: (4) form an aqueous solution 

7. Which element is malleable and conducts electricity?

  • (1) iron
  • (2) iodine
  • (3) sulfur
  • (4) phosphorus
Answer: (1) iron 

8. At STP, solid carbon can exist as graphite or as diamond. These two forms of carbon have

  • (1) the same properties and the same crystal structures
  • (2) the same properties and different crystal structures
  • (3) different properties and the same crystal structures
  • (4) different properties and different crystal structures
Answer: (4) different properties and different crystal structures 

9. What is the formula of titanium(II) oxide?

  • (1) TiO
  • (2) TiO2
  • (3) Ti2O
  • (4) Ti2O3
Answer: (1) TiO 

10. Which substance can be decomposed by a chemical change?

  • (1) calcium
  • (2) potassium
  • (3) copper
  • (4) ammonia
Answer: (4) ammonia 

11. As a chlorine atom becomes a negative ion, the atom

  • (1) gains an electron and its radius increases
  • (2) gains an electron and its radius decreases
  • (3) loses an electron and its radius increases
  • (4) loses an electron and its radius decreases
Answer: (1) gains an electron and its radius increases 

12. Based on Reference Table S, the atoms of which of these elements have the strongest attraction for electrons in a chemical bond?

  • (1) N
  • (2) Na
  • (3) P
  • (4) Pt
Answer: (1) N 

13. Which terms are used to identify pure substances?

  • (1) an element and a mixture
  • (2) an element and a compound
  • (3) a solution and a mixture
  • (4) a solution and a compound
Answer: (2) an element and a compound 

14. The solubility of KClO3(s) in water increases as the

  • (1) temperature of the solution increases
  • (2) temperature of the solution decreases
  • (3) pressure on the solution increases
  • (4) pressure on the solution decreases
Answer: (1) temperature of the solution increases 

15. Compared to a 0.1 M aqueous solution of NaCl, a 0.8 M aqueous solution of NaCl has a

  • (1) higher boiling point and a higher freezingpoint
  • (2) higher boiling point and a lower freezingpoint
  • (3) lower boiling point and a higher freezingpoint
  • (4) lower boiling point and a lower freezing point
Answer: (2) higher boiling point and a lower freezingpoint 

16. The kinetic molecular theory assumes that the particles of an ideal gas

  • (1) are in random, constant, straight-line motion
  • (2) are arranged in a regular geometric pattern
  • (3) have strong attractive forces between them
  • (4) have collisions that result in the system losing energy
Answer: (1) are in random, constant, straight-line motion 

17. In which process does a solid change directly into a vapor?

  • (1) condensation
  • (2) sublimation
  • (3) deposition
  • (4) solidification
Answer: (2) sublimation 

18. Which statement must be true about a chemical system at equilibrium?

  • (1) The forward and reverse reactions stop.
  • (2) The concentration of reactants and products are equal.
  • (3) The rate of the forward reaction is equal to the rate of the reverse reaction.
  • (4) The number of moles of reactants is equal to the number of moles of product.
Answer: (3) The rate of the forward reaction is equal to the rate of the reverse reaction. 

19. Adding a catalyst to a chemical reaction results in

  • (1) a decrease in activation energy and a decrease in the reaction rate
  • (2) a decrease in activation energy and an increase in the reaction rate
  • (3) an increase in activation energy and a decrease in the reaction rate
  • (4) an increase in activation energy and an increase in the reaction rate
Answer: (2) a decrease in activation energy and an increase in the reaction rate 

20. Systems in nature tend to undergo changes toward

  • (1) lower energy and lower entropy
  • (2) lower energy and higher entropy
  • (3) higher energy and lower entropy
  • (4) higher energy and higher entropy
Answer: (2) lower energy and higher entropy 

21. Which element has atoms that can bond with each other to form long chains or rings?

  • (1) carbon
  • (2) nitrogen
  • (3) oxygen
  • (4) fluorine
Answer: (1) carbon  

22. Which formula represents an unsaturated hydrocarbon?

  • (1) C2H6
  • (2) C3H8
  • (3) C5H8
  • (4) C6H14
Answer: (3) C5H8 

23. Given the structural formula:

What is the IUPAC name of this compound?

  • (1) propane
  • (2) propene
  • (3) propanone
  • (4) propanal
Answer: (2) propene 

24. What is the oxidation state of nitrogen in NaNO2?

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

25. The three isomers of pentane have different

  • (1) formula masses
  • (2) molecular formulas
  • (3) empirical formulas
  • (4) structural formulas
Answer: (4) structural formulas 

26. Where does oxidation occur in an electrochemical cell?

  • (1) at the cathode in both an electrolytic cell and a voltaic cell
  • (2) at the cathode in an electrolytic cell and at the anode in a voltaic cell
  • (3) at the anode in both an electrolytic cell and a voltaic cell
  • (4) at the anode in an electrolytic cell and at the cathode in a voltaic cell
Answer: (3) at the anode in both an electrolytic cell and a voltaic cell 

27. Which formula represents an electrolyte?

  • (1) CH3OCH3
  • (2) CH3OH
  • (3) CH3COOH
  • (4) C2H5CHO
Answer: (3) CH3COOH 

28. When an Arrhenius acid dissolves in water, the only positive ion in the solution is

  • (1) H+
  • (2) Li+
  • (3) Na+
  • (4) K+
Answer: (1) H+  

29. What is the half-life and decay mode of Rn-222?

  • (1) 1.91 days and alpha decay
  • (2) 1.91 days and beta decay
  • (3) 3.82 days and alpha decay
  • (4) 3.82 days and beta decay
Answer: (3) 3.82 days and alpha decay 

30. Which equation represents a transmutation reaction?

Answer: (2)  

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