Chemistry 27 January 2016 Questions Answer Keys
The University Of The State Of New York
Regents High School Examination
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
2. What is the number of electrons in a potassium atom?
- (1) 18
- (2) 19
- (3) 20
- (4) 39
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
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
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
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
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
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
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
10. Which formula is an empirical formula?
- (1) CH4
- (2) C2H6
- (3) C3H6
- (4) C4H10
11. Which compound contains both ionic and covalent bonds?
- (1) KI
- (2) CaCl2
- (3) CH2Br2
- (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.
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
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
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
16. Which list includes three forms of energy?
- (1) chemical, mechanical, electromagnetic
- (2) chemical, mechanical, temperature
- (3) thermal, pressure, electromagnetic
- (4) thermal, pressure, temperature
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
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
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
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)
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
22. Which element is present in all organic compounds?
- (1) nitrogen
- (2) oxygen
- (3) carbon
- (4) sulfur
23. Two types of organic reactions are
- (1) deposition and saponification
- (2) deposition and transmutation
- (3) polymerization and saponification
- (4) polymerization and transmutation
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
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
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
27. Phenolphthalein is pink in an aqueous solution having a pH of
- (1) 5
- (2) 2
- (3) 7
- (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
29. Which reaction releases the greatest amount of energy per mole of reactant?
- (1) decomposition
- (2) esterification
- (3) fermentation
- (4) fission
30. Which nuclear emission is negatively charged?
- (1) an alpha particle
- (2) a beta particle
- (3) a neutron
- (4) a positron
Download Chemistry 27 January 2016 Questions Answers Keys
|Chemistry Examination Question|
|Scoring Key and Rating Guide|