Chemistry 24 June 2014

Chemistry 24 June 2014 Questions Answer Keys

The University Of The State Of New York
Regents High School Examination
Physical Setting
Chemistry
Tuesday, June 24, 2014 — 9:15 a.m. to 12:15 p.m., only

Directions (1–30): For each statement or question, record on your 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 2011 Edition Reference Tables for Physical Setting/Chemistry.

1. Compared to the charge of a proton, the charge of an electron has

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

2. Which atom has the largest atomic radius?

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

3. In the wave-mechanical model of the atom, an orbital is defined as

  • (1) a region of the most probable proton location
  • (2) a region of the most probable electron location
  • (3) a circular path traveled by a proton around the nucleus
  • (4) a circular path traveled by an electron around the nucleus
Answer: (2) a region of the most probable electron location 

4. When an excited electron in an atom moves to the ground state, the electron

  • (1) absorbs energy as it moves to a higher energy state
  • (2) absorbs energy as it moves to a lower energy state
  • (3) emits energy as it moves to a higher energy state
  • (4) emits energy as it moves to a lower energy state
Answer: (4) emits energy as it moves to a lower energy state 

5. Which polyatomic ion is found in the compound represented by the formula NaHCO3?

  • (1) acetate
  • (2) hydrogen carbonate
  • (3) hydrogen sulfate
  • (4) oxalate
Answer: (2) hydrogen carbonate 

6. The atomic mass of magnesium is the weighted average of the atomic masses of

  • (1) all of the artificially produced isotopes of Mg
  • (2) all of the naturally occurring isotopes of Mg
  • (3) the two most abundant artificially produced isotopes of Mg
  • (4) the two most abundant naturally occurring isotopes of Mg
Answer: (2) all of the naturally occurring isotopes of Mg 

7. Which element has atoms that can form halide ions?

  • (1) iodine
  • (2) silver
  • (3) strontium
  • (4) xenon
Answer: (1) iodine 

8. Two forms of solid carbon, diamond and graphite, differ in their physical properties due to the differences in their

  • (1) atomic numbers
  • (2) crystal structures
  • (3) isotopic abundances
  • (4) percent compositions
Answer: (2) crystal structures 

9. Which quantity can be calculated for a solid compound, given only the formula of the compound and the Periodic Table of the Elements?

  • (1) the density of the compound
  • (2) the heat of fusion of the compound
  • (3) the melting point of each element in the compound
  • (4) the percent composition by mass of each element in the compound
Answer: (4) the percent composition by mass of each element in the compound 

10. Which terms identify types of chemical reactions?

  • (1) decomposition and sublimation
  • (2) decomposition and synthesis
  • (3) deposition and sublimation
  • (4) deposition and synthesis
Answer: (2) decomposition and synthesis 

11. The greatest amount of energy released per gram of reactants occurs during a

  • (1) redox reaction
  • (2) fission reaction
  • (3) substitution reaction
  • (4) neutralization reaction
Answer: (2) fission reaction 

12. Which element has atoms with the strongest attraction for electrons in a chemical bond?

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

13. Compared to the physical and chemical properties of the compound NO2, the compound N2O has

  • (1) different physical properties and different chemical properties
  • (2) different physical properties and the same chemical properties
  • (3) the same physical properties and different chemical properties
  • (4) the same physical properties and the same chemical properties
Answer: (1) different physical properties and different chemical properties 

14. Which phrase describes a molecule of CH4, in terms of molecular polarity and distribution of charge?

  • (1) polar with an asymmetrical distribution of charge
  • (2) polar with a symmetrical distribution of charge
  • (3) nonpolar with an asymmetrical distribution of charge
  • (4) nonpolar with a symmetrical distribution of charge
Answer: (4) nonpolar with a symmetrical distribution of charge 

15. Which sample of copper has atoms with the lowest average kinetic energy?

  • (1) 10. g at 45°C
  • (2) 20. g at 35°C
  • (3) 30. g at 25°C
  • (4) 40. g at 15°C
Answer: (4) 40. g at 15°C 

16. Which change results in the formation of different substances?

  • (1) burning of propane
  • (2) melting of NaCl(s)
  • (3) deposition of CO2(g)
  • (4) solidification of water
Answer: (1) burning of propane 

17. Which substance can not be broken down by a chemical change?

  • (1) ammonia
  • (2) ethanol
  • (3) propanal
  • (4) zirconium
Answer: (4) zirconium 

18. According to Table I, which equation represents a change resulting in the greatest quantity of energy released?

  • (1) 2C(s)  3H2(g) → C2H6(g)
  • (2) 2C(s)  2H2 (g) → C2H4(g)
  • (3) N2(g)  3H2 (g) → 2NH3(g)
  • (4) N2(g)  O2 (g) → 2NO(g)
Answer: (3) N2(g)  3H2 (g) → 2NH3(g) 

19. Which element is a liquid at STP?

  • (1) bromine
  • (2) cesium
  • (3) francium
  • (4) iodine
Answer: (1) bromine 

20. Which statement describes a reversible reaction at equilibrium?

  • (1) The activation energy of the forward reaction must equal the activation energy of the reverse reaction.
  • (2) The rate of the forward reaction must equal the rate of the reverse reaction.
  • (3) The concentration of the reactants must equal the concentration of the products.
  • (4) The potential energy of the reactants must equal the potential energy of the products.
Answer: (2) The rate of the forward reaction must equal the rate of the reverse reaction. 

21. Given the balanced equation representing a reaction:

O2 → O + O

What occurs during this reaction?

  • (1) Energy is absorbed as bonds are broken.
  • (2) Energy is absorbed as bonds are formed.
  • (3) Energy is released as bonds are broken.
  • (4) Energy is released as bonds are formed.
Answer: (2) Energy is absorbed as bonds are formed. 

22. In terms of entropy and energy, systems in nature tend to undergo changes toward

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

23. Which term is defined as the difference between the potential energy of the products and the potential energy of the reactants in a chemical reaction?

  • (1) activation energy
  • (2) thermal energy
  • (3) heat of fusion
  • (4) heat of reaction
Answer: (4) heat of reaction 

24. What is the atomic number of the element whose atoms bond to each other in chains, rings, and networks?

  • (1) 10
  • (2) 8
  • (3) 6
  • (4) 4
Answer: (3) 6 

25. How many pairs of electrons are shared between two adjacent carbon atoms in a saturated hydrocarbon?

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

26. Given the balanced equation representing a reaction:

4Al(s) 3O2(g) → 2Al2O3(s)

As the aluminum loses 12 moles of electrons, the oxygen

  • (1) gains 4 moles of electrons
  • (2) gains 12 moles of electrons
  • (3) loses 4 moles of electrons
  • (4) loses 12 moles of electrons
Answer: (2) gains 12 moles of electrons  

27. Which compound is an electrolyte?

  • (1) CH3CHO
  • (2) CH3OCH3
  • (3) CH3COOH
  • (4) CH3CH2CH3
Answer: (3) CH3COOH  

28. Which statement describes one acid-base theory?

  • (1) An acid is an H+ acceptor, and a base is an H+ donor.
  • (2) An acid is an H+ donor, and a base is an H+ acceptor.
  • (3) An acid is an H acceptor, and a base is an H donor.
  • (4) An acid is an H donor, and a base is an H acceptor.
Answer: (2) An acid is an H+ donor, and a base is an H+ acceptor.  

29 Which compounds are classified as Arrhenius acids?

  • (1) HCl and NaOH
  • (2) HNO3 and NaCl
  • (3) NH3 and H2CO3
  • (4) HBr and H2SO4
Answer: (4) HBr and H2SO4  

30. Which statement describes the stability of the nuclei of potassium atoms?

  • (1) All potassium atoms have stable nuclei that spontaneously decay.
  • (2) All potassium atoms have unstable nuclei that do not spontaneously decay.
  • (3) Some potassium atoms have unstable nuclei that spontaneously decay.
  • (4) Some potassium atoms have unstable nuclei that do not spontaneously decay
Answer: (3) Some potassium atoms have unstable nuclei that spontaneously decay.  

 

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