Chemistry 27 January 2016

Chemistry 27 January 2016 Questions Answer Keys

The University Of The State Of New York
Regents High School Examination
Physical Setting
Chemistry
Wednesday, January 27, 2016 — 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. Which phrase describes the charge and mass of a neutron?

  • (1) a charge of +1 and no mass
  • (2) a charge of  +1 and an approximate mass of 1 u
  • (3) no charge and no mass
  • (4) no charge and an approximate mass of 1 u
Answer: (4) no charge and an approximate mass of 1 u 

2. What is the number of electrons in a potassium atom?

  • (1) 18
  • (2) 19
  • (3) 20
  • (4) 39
Answer: (2) 19 

3. The number of valence electrons in each atom of an element affects the element’s

  • (1) chemical properties
  • (2) number of isotopes
  • (3) decay mode
  • (4) half-life
Answer: (1) chemical properties 

4. The nuclides I-131 and I-133 are classified as

  • (1) isomers of the same element
  • (2) isomers of Xe-131 and Cs-133
  • (3) isotopes of the same element
  • (4) isotopes of Xe-131 and Cs-133
Answer: (3) isotopes of the same element

5. The elements on the Periodic Table are arranged in order of increasing

  • (1) mass number
  • (2) atomic number
  • (3) number of isotopes
  • (4) number of valence electrons
Answer: (2) atomic number

6. Compared to a 1.0-gram sample of chlorine gas at standard pressure, a 1.0-gram sample of solid aluminum at standard pressure has

  • (1) a lower melting point
  • (2) a higher boiling point
  • (3) a lower density
  • (4) a greater volume
Answer: (2) a higher boiling point

7. Which processes represent one chemical change and one physical change?

  • (1) freezing and melting
  • (2) freezing and vaporization
  • (3) decomposition and melting
  • (4) decomposition and combustion
Answer: (3) decomposition and melting

8. In the ground state, an atom of each of the elements in Group 2 has a different

  • (1) oxidation state
  • (2) first ionization energy
  • (3) number of valence electrons
  • (4) number of electrons in the first shell
Answer: (2) first ionization energy

9. Which statement explains why water is classified as a compound?

  • (1) Water can be broken down by chemical means.
  • (2) Water is a liquid at room temperature.
  • (3) Water has a heat of fusion of 334 J/g.
  • (4) Water is a poor conductor of electricity
Answer: (1) Water can be broken down by chemical means.

10. Which formula is an empirical formula?

  • (1) CH4
  • (2) C2H6
  • (3) C3H6
  • (4) C4H10
Answer: (1) CH4

11. Which compound contains both ionic and covalent bonds?

  • (1) KI
  • (2) CaCl2
  • (3) CH2Br2
  • (4) NaCN
Answer: (4) NaCN 

12. Given the balanced equation representing a reaction:

H2 → H  H

What occurs during this reaction?

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

13. Parts per million is used to express the

  • (1) atomic mass of an element
  • (2) concentration of a solution
  • (3) volume of a substance
  • (4) rate of heat transfer
Answer: (2) concentration of a solution.

14. According to Table F, which ions combine with chloride ions to form an insoluble compound?

  • (1) Fe2+ ions
  • (2) Ca2+ions
  • (3) Li+ ions
  • (4) Ag+ion
Answer: (4) Ag+ion

15. At 1 atm, equal masses of H2O(s), H2O(ℓ), and H2O(g) have

  • (1) the same density
  • (2) the same distance between molecules
  • (3) different volumes
  • (4) different percent compositions
Answer: (3) different volumes 

16. Which list includes three forms of energy?

  • (1) chemical, mechanical, electromagnetic
  • (2) chemical, mechanical, temperature
  • (3) thermal, pressure, electromagnetic
  • (4) thermal, pressure, temperature
Answer: (1) chemical, mechanical, electromagnetic

17. At STP, a 1-liter sample of Ne(g) and a 1-liter sample of Kr(g) have the same

  • (1) mass
  • (2) density
  • (3) number of atoms
  • (4) number of electrons
Answer: (3) number of atoms

18. A reaction will most likely occur if the colliding particles have the proper

  • (1) mass, only
  • (2) mass and volume
  • (3) orientation, only
  • (4) orientation and energy
Answer: (4) orientation and energy

19. Which factors have the greatest effect on the rate of a chemical reaction between AgNO3(aq) and Cu(s)?

  • (1) solution concentration and temperature
  • (2) solution concentration and pressure
  • (3) molar mass and temperature
  • (4) molar mass and pressure
Answer: (1) solution concentration and temperature

20. Which expression represents the heat of reaction for a chemical change in terms of potential energy, PE?

  • (1) (PEproducts) + (PEreactants)
  • (2) (PEproducts) –  (PEreactants)
  • (3) (PEproducts) × (PEreactants)
  • (4) (PEproducts) ÷ (PEreactants)
Answer: (2) (PEproducts) –  (PEreactants

21. When a chemical reaction is at equilibrium, the concentration of each reactant and the concentration of each product must be

  • (1) constant
  • (2) variable
  • (3) equal
  • (4) zero
Answer: (1) constant 

22. Which element is present in all organic compounds?

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

23. Two types of organic reactions are

  • (1) deposition and saponification
  • (2) deposition and transmutation
  • (3) polymerization and saponification
  • (4) polymerization and transmutation
Answer: (3) polymerization and saponification

24. Given the balanced equation representing a reaction:

2Al(s) + 3Cu2(aq) → 2Al3+ (aq)  3Cu(s)

Which particles are transferred in this reaction?

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

25. In an operating voltaic cell, reduction occurs

  • (1) at the anode
  • (2) at the cathode
  • (3) in the salt bridge
  • (4) in the wire
Answer: (2) at the cathode

26. Which type of substance yields hydrogen ions, H+, in an aqueous solution?

  • (1) an Arrhenius acid
  • (2) an Arrhenius base
  • (3) a saturated hydrocarbon
  • (4) an unsaturated hydrocarbon
Answer: (1) an Arrhenius acid

27. Phenolphthalein is pink in an aqueous solution having a pH of

  • (1) 5
  • (2) 2
  • (3) 7
  • (4) 12
Answer: (4) 12

28. According to one acid-base theory, NH3 acts as a base when an NH3 molecule

  • (1) accepts an H+ ion
  • (2) donates an H+ ion
  • (3) accepts an OH ion
  • (4) donates an OH ion
Answer: (1) accepts an H+ ion

29. Which reaction releases the greatest amount of energy per mole of reactant?

  • (1) decomposition
  • (2) esterification
  • (3) fermentation
  • (4) fission
Answer: (4) fission 

30. Which nuclear emission is negatively charged?

  • (1) an alpha particle
  • (2) a beta particle
  • (3) a neutron
  • (4) a positron
Answer: (2) a beta particle

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