Chemistry 26 January 2012 Questions Answer Keys
The University Of The State Of New York
Regents High School Examination
Thursday, January 26, 2012 — 1:15 to 4:15 p.m., only
Directions (1–30): For each statement or question, write in your answer booklet 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. What is the number of electrons in a completely filled second shell of an atom?
- (1) 32
- (2) 2
- (3) 18
- (4) 8
2. What is the number of electrons in an atom that has 3 protons and 4 neutrons?
- (1) 1
- (2) 7
- (3) 3
- (4) 4
3. As a result of the gold foil experiment, it was concluded that an atom
- (1) contains protons, neutrons, and electrons
- (2) contains a small, dense nucleus
- (3) has positrons and orbitals
- (4) is a hard, indivisible sphere
4. Which statement describes the distribution of charge in an atom?
- (1) A neutral nucleus is surrounded by one or more negatively charged electrons.
- (2) A neutral nucleus is surrounded by one or more positively charged electrons.
- (3) A positively charged nucleus is surrounded by one or more negatively charged electrons.
- (4) A positively charged nucleus is surrounded by one or more positively charged electrons.
5. Which atom in the ground state has an outermost electron with the most energy?
- (1) Cs
- (2) K
- (3) Li
- (4) Na
6. Which particle has the least mass?
- (1) alpha particle
- (2) beta particle
- (3) neutron
- (4) proton
7. The elements in Group 2 are classified as
- (1) metals
- (2) metalloids
- (3) nonmetals
- (4) noble gases
8. Which list includes elements with the most similar chemical properties?
- (1) Br, Ga, Hg
- (2) Cr, Pb, Xe
- (3) O, S, Se
- (4) N, O, F
9. The notation for the nuclide 137 55Cs gives information about
- (1) mass number, only
- (2) atomic number, only
- (3) both mass number and atomic number
- (4) neither mass number nor atomic number
10. Which pair represents two forms of an element in the same phase at STP but with different structures and different properties?
- (1) I2(s) and I2(g)
- (2) O2(g) and O3(g)
- (3) H2(g) and Hg(g)
- (4) H2O(s) and H2O(ℓ)
11. The elements on the Periodic Table are arranged in order of increasing
- (1) atomic mass
- (2) atomic number
- (3) molar mass
- (4) oxidation number
12. What is the IUPAC name for the compound ZnO?
- (1) zinc oxide
- (2) zinc oxalate
- (3) zinc peroxide
- (4) zinc hydroxide
13. Which atom attains a stable valence electron configuration by bonding with another atom?
- (1) neon
- (2) radon
- (3) helium
- (4) hydrogen
14. An ionic bond can be formed when one or more electrons are
- (1) equally shared by two atoms
- (2) unequally shared by two atoms
- (3) transferred from the nucleus of one atom to the nucleus of another atom
- (4) transferred from the valence shell of one atom to the valence shell of another atom
15. Which sample of CO2 has a definite shape and a definite volume?
- (1) CO2(aq)
- (2) CO2(g)
- (3) CO2(ℓ)
- (4) CO2(s)
16. What occurs in order to break the bond in a Cl2 molecule?
- (1) Energy is absorbed.
- (2) Energy is released.
- (3) The molecule creates energy.
- (4) The molecule destroys energy.
17. A sealed, rigid 1.0-liter cylinder contains He gas at STP. An identical sealed cylinder contains Ne gas at STP. These two cylinders contain the same number of
- (1) atoms
- (2) electrons
- (3) ions
- (4) protons
18. Which statement describes a chemical change?
- (1) Alcohol evaporates.
- (2) Water vapor forms snowflakes.
- (3) Table salt (NaCl) is crushed into powder.
- (4) Glucose (C6H12O6) and oxygen produce CO2 and H2O.
19. Which statement describes the particles of an ideal gas according to the kinetic molecular theory?
- (1) The gas particles are arranged in a regular geometric pattern.
- (2) The gas particles are in random, constant, straight-line motion.
- (3) The gas particles are separated by very small distances, relative to their sizes.
- (4) The gas particles are strongly attracted to each other.
20. Which sample of matter is classified as a substance?
- (1) air
- (2) ammonia
- (3) milk
- (4) seawate
21. Which element has the lowest electronegativity value?
- (1) F
- (2) Fr
- (3) Cl
- (4) Cr
22. At standard pressure, CH4 boils at 112 K and H2O boils at 373 K. What accounts for the higher boiling point of H2O at standard pressure?
- (1) covalent bonding
- (2) ionic bonding
- (3) hydrogen bonding
- (4) metallic bonding
23. A mixture of sand and table salt can be separated by filtration because the substances in the mixture differ in
- (1) boiling point
- (2) density at STP
- (3) freezing point
- (4) solubility in water
24. 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
25. In the wave-mechanical model of the atom, an orbital is the most probable location of
- (1) a proton
- (2) a positron
- (3) a neutron
- (4) an electron
26. Functional groups are used to classify
- (1) organic compounds
- (2) inorganic compounds
- (3) heterogeneous mixtures
- (4) homogeneous mixtures
27. Which class of compounds contains at least one element from Group 17 of the Periodic Table?
- (1) aldehyde
- (2) amine
- (3) ester
- (4) halide
28. In a propanal molecule, an oxygen atom is bonded with a carbon atom. What is the total number of pairs of electrons shared between these atoms?
- (1) 1
- (2) 2
- (3) 3
- (4) 4
29. When a voltaic cell operates, ions move through the
- (1) anode
- (2) cathode
- (3) salt bridge
- (4) external circuit
30. When dissolved in water, an Arrhenius base yields
- (1) hydrogen ions
- (2) hydronium ions
- (3) hydroxide ions
- (4) oxide ions
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