Chem Jan 2012 Regents

50 Questions  I  By Ionca
Please take the quiz to rate it.

 Chem Jan 2012 Regents
Use your Reference Table. As you go over this test, eliminate any wrong answers.

  
Changes are done, please start the quiz.


Questions and Answers

Removing question excerpt is a premium feature

Upgrade and get a lot more done!
  • 1. 
    What is the number of electrons in a completely filled second shell of an atom? 
    • A. 

      32

    • B. 

      2

    • C. 

      18

    • D. 

      8


  • 2. 
    What is the number of electrons in an atom that has 3 protons and 4 neutrons? 
    • A. 

      1

    • B. 

      7

    • C. 

      3

    • D. 

      4


  • 3. 
    As a result of the gold foil experiment, it was concluded that an atom 
    • A. 

      Contains protons, neutrons, and electrons

    • B. 

      Contains a small, dense nucleus

    • C. 

      Has positrons and orbitals

    • D. 

      Is a hard, indivisible sphere


  • 4. 
    Which statement describes the distribution of charge in an atom? 
    • A. 

      A neutral nucleus is surrounded by one or more negatively charged electrons.

    • B. 

      A neutral nucleus is surrounded by one or more positively charged electrons.

    • C. 

      A positively charged nucleus is surrounded by one or more negatively charged electrons.

    • D. 

      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? 
    • A. 

      Cs

    • B. 

      K

    • C. 

      Li

    • D. 

      Na


  • 6. 
    Which particle has the least mass?
    • A. 

      Alpha particle

    • B. 

      Beta particle

    • C. 

      Neutron

    • D. 

      Proton


  • 7. 
    The elements in Group 2 are classified as    
    • A. 

      Metals

    • B. 

      Metalloids

    • C. 

      Nonmetals

    • D. 

      Noble gases


  • 8. 
    Which list includes elements with the most similar chemical properties? 
    • A. 

      Br, Ga, Hg

    • B. 

      Cr, Pb, Xe

    • C. 

      O, S, Se

    • D. 

      N, O, F


  • 9. 

    • A. 

      Mass number, only

    • B. 

      Atomic number, only

    • C. 

      Both mass number and atomic number

    • D. 

      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? 
    • A. 

      I2(s) and I2(g)

    • B. 

      O2(g) and O3(g)

    • C. 

      H2(g) and Hg(g)

    • D. 

      H2O(s) and H2O(l)


  • 11. 
    The elements on the Periodic Table are arranged in order of increasing 
    • A. 

      Atomic mass

    • B. 

      Atomic number

    • C. 

      Molar mass

    • D. 

      Oxidation number


  • 12. 
    What is the IUPAC name for the compound ZnO? 
    • A. 

      Zinc oxide

    • B. 

      Zinc oxalate

    • C. 

      Zinc peroxide

    • D. 

      Zinc hydroxide


  • 13. 
    Which atom attains a stable valence electron configuration by bonding with another atom? 
    • A. 

      Neon

    • B. 

      Radon

    • C. 

      Hydrogen

    • D. 

      Helium


  • 14. 
    An ionic bond can be formed when one or more electrons are 
    • A. 

      Equally shared by two atoms

    • B. 

      Unequally shared by two atoms

    • C. 

      Transferred from the nucleus of one atom to the nucleus of another atom

    • D. 

      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? 
    • A. 

      CO2 (aq)

    • B. 

      CO2 (g)

    • C. 

      CO2 (l)

    • D. 

      CO2 (s)


  • 16. 
    What occurs in order to break the bond in a Cl2 molecule? 
    • A. 

      Energy is absorbed.

    • B. 

      Energy is released.

    • C. 

      The molecule creates energy.

    • D. 

      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 
    • A. 

      Atoms

    • B. 

      Electrons

    • C. 

      Ions

    • D. 

      Protons


  • 18. 
    Which statement describes a chemical change?    
    • A. 

      Alcohol evaporates.

    • B. 

      Water vapor forms snowflakes.

    • C. 

      Table salt (NaCl) is crushed into powder.

    • D. 

      Glucose (C6H12O6) and oxygen produce CO2 and H2O.


  • 19. 
    Which statement describes the particles of an ideal gas according to the kinetic molecular theory? 
    • A. 

      The gas particles are arranged in a regular geometric pattern.

    • B. 

      The gas particles are in random, constant, straight-line motion.

    • C. 

      The gas particles are separated by very small distances, relative to their sizes.

    • D. 

      The gas particles are strongly attracted to each other.


  • 20. 
    Which sample of matter is classified as a substance? 
    • A. 

      Air

    • B. 

      Ammonia

    • C. 

      Milk

    • D. 

      Seawater


  • 21. 
    Which element has the lowest electronegativity value? 
    • A. 

      F

    • B. 

      Fr

    • C. 

      Cl

    • D. 

      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? 
    • A. 

      Covalent bonding

    • B. 

      Ionic bonding

    • C. 

      Hydrogen bonding

    • D. 

      Metallic bonding


  • 23. 
    A mixture of sand and table salt can be separated by filtration because the substances in the mixture differ in 
    • A. 

      Boiling point

    • B. 

      Density at STP

    • C. 

      Freezing point

    • D. 

      Solubility in water


  • 24. 
    Systems in nature tend to undergo changes toward 
    • A. 

      Lower energy and lower entropy

    • B. 

      Lower energy and higher entropy

    • C. 

      Higher energy and lower entropy

    • D. 

      Higher entropy and higher entropy


  • 25. 
    In the wave-mechanical model of the atom, an orbital is the most probable location of 
    • A. 

      A proton

    • B. 

      A positron

    • C. 

      A neutron

    • D. 

      An electron


  • 26. 
    Functional groups are used to classify    
    • A. 

      Organic compounds

    • B. 

      Inorganic compounds

    • C. 

      Heterogeneous mixtures

    • D. 

      Homogeneous mixtures


  • 27. 
    Which class of compounds contains at least one element from Group 17 of the Periodic Table?
    • A. 

      Aldehyde

    • B. 

      Amine

    • C. 

      Ester

    • D. 

      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?
    • A. 

      1

    • B. 

      2

    • C. 

      3

    • D. 

      4


  • 29. 
    When a voltaic cell operates, ions move through the 
    • A. 

      Anode

    • B. 

      Cathode

    • C. 

      Salt bridge

    • D. 

      External circuit


  • 30. 
    When dissolved in water, an Arrhenius base yields
    • A. 

      Hydrogen ions

    • B. 

      Hydronium ions

    • C. 

      Hydroxide ions

    • D. 

      Oxide ions


  • 31. 
    What is the total number of valence electrons in a germanium atom in the ground state? 
    • A. 

      22

    • B. 

      2

    • C. 

      32

    • D. 

      4


  • 32. 
    Which element is paired with an excited-state electron configuration for an atom of the element? 
    • A. 

      Ca: 2-8-8-2

    • B. 

      Na: 2-8-2

    • C. 

      K: 2-6-8-3

    • D. 

      F: 2-8


  • 33. 
    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? 
    • A. 

      Single replacement and decomposition

    • B. 

      Single replacement and double replacement

    • C. 

      Synthesis and decomposition

    • D. 

      Synthesis and double replacement


  • 34. 
    An ion that consists of 7 protons, 6 neutrons, and 10 electrons has a net charge of 
    • A. 

      4−

    • B. 

      3−

    • C. 

      3+

    • D. 

      4+


  • 35. 
    Which Lewis electron-dot diagram represents a molecule having a nonpolar covalent bond? 
    • A. 
    • B. 
    • C. 
    • D. 

  • 36. 
    Which quantity is equal to 50 kilojoules?    
    • A. 

      0.05 J

    • B. 

      5000 J

    • C. 

      500 J

    • D. 

      50 000 J


  • 37. 
    Which compound is formed from its elements by an exothermic reaction at 298 K and 101.3 kPa? 
    • A. 

      C2H4 (g)

    • B. 

      HI (g)

    • C. 

      H2O (g)

    • D. 

      NO2 (g)


  • 38. 
    At which temperature is the vapor pressure of ethanol equal to 80. kPa? 
    • A. 

      48°C

    • B. 

      73°C

    • C. 

      80.°C

    • D. 

      101°C


  • 39. 
    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? 
    • A. 

      69 kPa

    • B. 

      93 kPa

    • C. 

      160 kPa

    • D. 

      230 kPa


  • 40. 
    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? 
    • A. 

      5.0 ppm

    • B. 

      15 ppm

    • C. 

      20. ppm

    • D. 

      50. ppm


  • 41. 
    Which equation represents a change that results in an increase in disorder? 
    • A. 

      I2 (s) → I2 (g)

    • B. 

      CO2 (g) → CO2 (s)

    • C. 

      2Na (s) + Cl2 (g) → 2NaCl (s)

    • D. 

      2H2 (g) + O2 (g) → 2H2O (l)


  • 42. 
    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 
    • A. 

      A lower boiling point and a lower freezing point

    • B. 

      A lower boiling point and a higher freezing point

    • C. 

      A higher boiling point and a lower freezing point

    • D. 

      A higher boiling point and a higher freezing point


  • 43. 

    Given the balanced ionic equation representing a reaction:  Which half-reaction represents the reduction that occurs? 
    • A. 
    • B. 
    • C. 
    • D. 

  • 44. 

    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? 
    • A. 

      +60. kJ/mol

    • B. 

      +20. kJ/mol

    • C. 

      +30. kJ/mol

    • D. 

      +40. kJ/mol


  • 45. 
    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? 
    • A. 

      The rate of dissolving is equal to the rate of crystallization.

    • B. 

      The rate of dissolving is greater than the rate of crystallization.

    • C. 

      The concentration of the solid is equal to the concentration of the solution.

    • D. 

      The concentration of the solid is greater than the concentration of the solution.


  • 46. 
    Which formula represents the product of the addition reaction between ethene and chlorine, Cl2? 
    • A. 
    • B. 
    • C. 
    • D. 

  • 47. 
    Based on Reference Table J, which two reactants react spontaneously? 
    • A. 

      Mg(s) + ZnCl2(aq)

    • B. 

      Cu(s) + FeSO4(aq)

    • C. 

      Pb(s) + ZnCl2(aq)

    • D. 

      Co(s) + NaCl(aq)


  • 48. 
    When the pH value of a solution is changed from 2 to 1, the concentration of hydronium ions 
    • A. 

      Decreases by a factor of 2

    • B. 

      Increases by a factor of 2

    • C. 

      Decreases by a factor of 10

    • D. 

      Increases by a factor of 10


  • 49. 

    Given the balanced equation representing a nuclear reaction:  Which phrase identifies and describes this reaction? 
    • A. 

      Fission, mass converted to energy

    • B. 

      Fission, energy converted to mass

    • C. 

      Fusion, mass converted to energy

    • D. 

      Fusion, energy converted to mass


  • 50. 

    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 
    • A. 

      NH3(g)

    • B. 

      H2O(l)

    • C. 

      NH4+(aq)

    • D. 

      OH (aq)


Back to top

Removing ad is a premium feature

Upgrade and get a lot more done!
Take Another Quiz
We have sent an email with your new password.