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Chem Jan 2012 Regents

50 Questions  I  By Ionca
CHEM JAN 2012 REGENTS
Use your Reference Table.  As you go over this test, eliminate any wrong answers.

  
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1.  The elements on the Periodic Table are arranged in order of increasing 
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B.
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D.
2.  What is the number of electrons in an atom that has 3 protons and 4 neutrons? 
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B.
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D.
3. 
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D.
4.  As a result of the gold foil experiment, it was concluded that an atom 
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5.  Given the balanced equation representing a nuclear reaction:  Which phrase identifies and describes this reaction? 
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D.
6.  Which element has the lowest electronegativity value? 
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7.  Which quantity is equal to 50 kilojoules?    
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8.  Which element is paired with an excited-state electron configuration for an atom of the element? 
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9.  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 
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D.
10.  Which particle has the least mass?
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11.  Given the balanced ionic equation representing a reaction:  Which half-reaction represents the reduction that occurs? 
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12.  Given the equation and potential energy diagram representing a reaction:  If each interval on the axis labeled “Potential Energy (kJ/mol)” represents 10. kJ/mol, what is the heat of reaction? 
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13.  What is the number of electrons in a completely filled second shell of an atom? 
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14.  When a voltaic cell operates, ions move through the 
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15.  A solution consists of 0.50 mole of CaCl2 dissolved in 100. grams of H2O at 25°C. Compared to the boiling point and freezing point of 100. grams of H2O at standard pressure, the solution at standard pressure has 
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16.  When the pH value of a solution is changed from 2 to 1, the concentration of hydronium ions 
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17.  What is the total number of valence electrons in a germanium atom in the ground state? 
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D.
18.  A mixture of sand and table salt can be separated by filtration because the substances in the mixture differ in 
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D.
19.  An ion that consists of 7 protons, 6 neutrons, and 10 electrons has a net charge of 
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20.  Given the equation representing a reversible reaction:  According to one acid-base theory, the reactant that donates an H+ ion in the forward reaction is 
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21.  The elements in Group 2 are classified as    
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22.  Which statement describes the distribution of charge in an atom? 
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23.  Which list includes elements with the most similar chemical properties? 
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24.  Some solid KNO3 remains at the bottom of a stoppered flask containing a saturated KNO3(aq) solution at 22°C. Which statement explains why the contents of the flask are at equilibrium? 
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25.  What is the IUPAC name for the compound ZnO? 
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26.  Based on Reference Table J, which two reactants react spontaneously? 
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D.
27.  Which sample of CO2 has a definite shape and a definite volume? 
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28.  Which sample of matter is classified as a substance? 
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29.  At 25°C, gas in a rigid cylinder with a movable piston has a volume of 145 mL and a pressure of 125 kPa. Then the gas is compressed to a volume of 80. mL. What is the new pressure of the gas if the temperature is held at 25°C? 
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30.  Which compound is formed from its elements by an exothermic reaction at 298 K and 101.3 kPa? 
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31.  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?
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32.  In the wave-mechanical model of the atom, an orbital is the most probable location of 
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33.  Which atom attains a stable valence electron configuration by bonding with another atom? 
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34.  Which Lewis electron-dot diagram represents a molecule having a nonpolar covalent bond? 
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35.  At which temperature is the vapor pressure of ethanol equal to 80. kPa? 
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D.
36.  An ionic bond can be formed when one or more electrons are 
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37.  Which statement describes a chemical change?    
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38.  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? 
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39.  Systems in nature tend to undergo changes toward 
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40.  Given the balanced equations representing two chemical reactions:      Cl2 + 2NaBr → 2NaCl + Br2      2NaCl → 2Na + Cl2 Which types of chemical reactions are represented by these equations? 
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41.  What occurs in order to break the bond in a Cl2 molecule? 
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42.  Which equation represents a change that results in an increase in disorder? 
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43.  Which formula represents the product of the addition reaction between ethene and chlorine, Cl2? 
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44.  Which pair represents two forms of an element in the same phase at STP but with different structures and different properties? 
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D.
45.  When dissolved in water, an Arrhenius base yields
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46.  Which class of compounds contains at least one element from Group 17 of the Periodic Table?
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47.  Which atom in the ground state has an outermost electron with the most energy? 
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48.  A 2400.-gram sample of an aqueous solution contains 0.012 gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million? 
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49.  Which statement describes the particles of an ideal gas according to the kinetic molecular theory? 
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50.  Functional groups are used to classify    
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