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Physical Setting / Chemistry - New York Regents June 2012 Exam

   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.

Formats Worksheet / Test Paper Quiz Review
: Multiple choice

Your Performance  

1.

1 The mass of a proton is approximately equal to
  the mass of
  (1) an alpha particle   (3) a positron
  (2) a beta particle     (4) a neutron

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2.

2 An orbital of an atom is defined as the most
  probable location of
  (1) an electron        (3) a positron
  (2) a neutron          (4) a proton

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3.

3 What must occur when an electron in an atom
  returns from a higher energy state to a lower
  energy state?
  (1) A specific amount of energy is released.
  (2) A random amount of energy is released.
  (3) The atom undergoes transmutation.
  (4) The atom spontaneously decays.

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4.

4 Which element is a liquid at 305 K and
  1.0 atmosphere?
  (1) magnesium       (3) gallium
  (2) fluorine        (4) iodine

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5.

5 Which list of elements consists of a metal, a
  metalloid, and a nonmetal?
  (1) Li, Na, Rb          (3) Sn, Si, C
  (2) Cr, Mo, W           (4) O, S, Te

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6.

6 At STP, which physical property of aluminum
  always remains the same from sample to sample?
  (1) mass                 (3) length
  (2) density              (4) volume

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7.

7 Which statement describes a chemical property
  of silicon?
  (1) Silicon has a blue-gray color.
  (2) Silicon is a brittle solid at 20.°C.
  (3) Silicon melts at 1414°C.
  (4) Silicon reacts with fluorine.

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8.

8 Which diagram represents a mixture of two
  different molecular forms of the same element?

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9.

9 A compound is broken down by chemical means
  during
  (1) chromatography     (3) electrolysis
  (2) distillation       (4) filtration

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10.

10 Which quantities must be conserved in all
   chemical reactions?
   (1) mass, charge, density
   (2) mass, charge, energy
   (3) charge, volume, density
   (4) charge, volume, energy

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11.

11 Which phrase describes the distribution of
   charge and the polarity of a CH4 molecule?
   (1) symmetrical and polar
   (2) symmetrical and nonpolar
   (3) asymmetrical and polar
   (4) asymmetrical and nonpolar

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12.

12 What is the charge of the nucleus of an oxygen
   atom?
   (1) 0                    (3) +8
   (2) -2                   (4) +16

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13.

13 Which ion has no electrons?
   (1) H+                  (3) Na+
   (2) Li+                 (4) Rb+

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14.

14 To break a chemical bond, energy must be
   (1) absorbed           (3) produced
   (2) destroyed          (4) released

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15.

15 Which Lewis electron-dot diagram represents a
   nitrogen atom in the ground state?

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16.

16 What is the most likely electronegativity value
   for a metallic element?
   (1) 1.3                 (3) 3.4
   (2) 2.7                 (4) 4.0

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17.

17 Which polyatomic ion has a charge of 3-?
   (1) chromate ion       (3) phosphate ion
   (2) oxalate ion        (4) thiocyanate ion

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18.

18 Every chlorine atom has
   (1) 7 electrons
   (2) 17 neutrons
   (3) a mass number of 35
   (4) an atomic number of 17

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19.

19 Which substance can not be broken down by a
   chemical change?
   (1) ammonia            (3) propane
   (2) methanol           (4) phosphorus

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20.

20 At standard pressure, which substance becomes
   less soluble in water as temperature increases
   from 10.°C to 80.°C?
   (1) HCl                  (3) NaCl
   (2) KCl                  (4) NH4Cl

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21.

21 Which type of concentration is calculated when
   the grams of solute is divided by the grams of
   the solution, and the result is multiplied by
   1 000 000?
   (1) molarity             (3) percent by mass
   (2) parts per million    (4) percent by volume

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22.

22 Which type of energy is associated with the
   random motion of atoms and molecules in a
   sample of air?
   (1) chemical energy   (3) nuclear energy
   (2) electrical energy (4) thermal energy

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23.

23 The temperature of a sample of matter is a
   measure of the
   (1) total kinetic energy of the particles in the
       sample
   (2) total potential energy of the particles in the
       sample
   (3) average potential energy of the particles in
       the sample
   (4) average kinetic energy of the particles in the
       sample

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24.

24 Which unit is used to express the pressure of a
   gas?
   (1) mole                (3) kelvin
   (2) joule               (4) pascal

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25.

25 Which sample of matter sublimes at room
   temperature and standard pressure?
   (1) Br2(ℓ)             (3) CO2(s)
   (2) Cl2(g)             (4) SO2(aq)

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26.

26 Given the diagram representing a closed system
   at constant temperature:
Which statement describes this system at
equilibrium?
(1) The mass of H2O(ℓ) equals the mass of
    H2O(g).
(2) The volume of H2O(ℓ) equals the volume of
    H2O(g).
(3) The number of moles of H2O(ℓ) equals the
    number of moles of H2O(g).
(4) The rate of evaporation of H2O(ℓ) equals
    the rate of condensation of H2O(g).

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27.

27 Which reaction occurs at the cathode in an
   electrochemical cell?
   (1) combustion        (3) oxidation
   (2) neutralization    (4) reduction

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28.

28 Which substance yields H+(aq) as the only
   positive ion in an aqueous solution?
   (1) CH3CHO               (3) CH3COOH
   (2) CH3CH2OH             (4) CH3OCH3

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29.

29 Compared to the mass and the penetrating
   power of an alpha particle, a beta particle has
   (1) less mass and greater penetrating power
   (2) less mass and less penetrating power
   (3) more mass and greater penetrating power
   (4) more mass and less penetrating power

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30.

30 During a nuclear reaction, mass is converted
   into
   (1) charge             (3) isomers
   (2) energy             (4) volume

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