Chem Jan 2011 Regents

49 Questions | Total Attempts: 71

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Chem Jan 2011 Regents

These multiple choice questions came from January 2011. Use your best judgment. . . Eliminate wrong choices and, in some cases, find the ODD MAN OUT. . . That's usually (I SAID USUALLY) the right answer.


Questions and Answers
  • 1. 
    An orbital is a region of space where there is a high probability of finding 
    • A. 

      A proton

    • B. 

      An electron

    • C. 

      A positron

    • D. 

      A neutron

  • 2. 
    Which statement matches a subatomic particle with its charge? 
    • A. 

      A neutron has a negative charge.

    • B. 

      A proton has a negative charge.

    • C. 

      A neutron has no charge.

    • D. 

      A proton has no charge.

  • 3. 
    An atom of any element must contain    
    • A. 

      An equal number of protons and neutrons

    • B. 

      An equal number of protons and electrons

    • C. 

      More electrons than neutrons

    • D. 

      More electrons than protons

  • 4. 
    Which statement compares the masses of two subatomic particles? 
    • A. 

      The mass of an electron is greater than the mass of a proton.

    • B. 

      The mass of an electron is greater than the mass of a neutron.

    • C. 

      The mass of a proton is greater than the mass of an electron.

    • D. 

      The mass of a proton is greater than the mass of a neutron.

  • 5. 
    The bright-line spectrum of sodium is produced when energy is 
    • A. 

      Absorbed as electrons move from higher to lower electron shells

    • B. 

      Absorbed as electrons move from lower to higher electron shells

    • C. 

      Released as electrons move from higher to lower electron shells

    • D. 

      Released as electrons move from lower to higher electron shells

  • 6. 
    The valence electrons of a germanium atom in the ground state are located in the 
    • A. 

      First shell

    • B. 

      Second shell

    • C. 

      Third shell

    • D. 

      Fourth shell

  • 7. 
    The elements on the Periodic Table are arranged in order of increasing 
    • A. 

      Atomic mass

    • B. 

      Atomic number

    • C. 

      First ionization energy

    • D. 

      Selected oxidation state

  • 8. 
    Which list of elements contains a metal, a metalloid, a nonmetal, and a noble gas? 
    • A. 

      Be, Si, Cl, Kr

    • B. 

      C,N,Ne,Ar

    • C. 

      K, Fe, B, F

    • D. 

      Na,Zn,As,Sb

  • 9. 
    The two forms of oxygen, O2(g) and O3(g), have   
    • A. 

      Different molecular structures and identical properties

    • B. 

      Different molecular structures and different properties

    • C. 

      Identical molecular structures and identical properties

    • D. 

      Identical molecular structures and different properties

  • 10. 
    The sum of the atomic masses of the atoms in one molecule of C3H6Br2 is called the 
    • A. 

      Formula mass

    • B. 

      Isotopic mass

    • C. 

      Percent abundance

    • D. 

      Percent composition

  • 11. 
    What is the total number of electron pairs shared between the two atoms in an O2 molecule? 
    • A. 

      1

    • B. 

      2

    • C. 

      6

    • D. 

      4

  • 12. 
    When an atom of lithium loses an electron, the atom becomes a 
    • A. 

      Negative ion with a radius smaller than the radius of the atom

    • B. 

      Negative ion with a radius larger than the radius of the atom

    • C. 

      Positive ion with a radius smaller than the radius of the atom

    • D. 

      Positive ion with a radius larger than the radius of the atom

  • 13. 
    Given the balanced equation representing a reaction: 2NaCl → 2Na + Cl2 To break the bonds in NaCl, the reactant must 
    • A. 

      Absorb energy

    • B. 

      Create energy

    • C. 

      Destroy energy

    • D. 

      Release energy

  • 14. 
    A molecular compound is formed when a chemical reaction occurs between atoms of 
    • A. 

      Chlorine and sodium

    • B. 

      Chlorine and yttrium

    • C. 

      Oxygen and hydrogen

    • D. 

      Oxygen and magnesium

  • 15. 
    Which substance can not be broken down by chemical means? 
    • A. 

      Ammonia

    • B. 

      Antimony

    • C. 

      Methane

    • D. 

      Water

  • 16. 
    Which two physical properties allow a mixture to be separated by chromatography? 
    • A. 

      Hardness and boiling point

    • B. 

      Density and specific heat capacity

    • C. 

      Malleability and thermal conductivity

    • D. 

      Solubility and molecular polarity

  • 17. 
    The solubility of KCl(s) in water depends on the    
    • A. 

      Pressure on the solution

    • B. 

      Rate of stirring

    • C. 

      Size of the KCl sample

    • D. 

      Temperature of the water

  • 18. 
    Which sample of water contains particles having the highest average kinetic energy? 
    • A. 

      25 mL of water at 95°C

    • B. 

      45 mL of water at 75°C

    • C. 

      75 mL of water at 75°C

    • D. 

      95 mL of water at 25°C

  • 19. 
    Under which conditions of temperature and pressure does carbon dioxide gas behave most like an ideal gas? 
    • A. 

      Low temperature and low pressure

    • B. 

      Low temperature and high pressure

    • C. 

      High temperature and low pressure

    • D. 

      High temperature and high pressure

  • 20. 
    Which process results in a chemical change?    
    • A. 

      Tearing tin foil

    • B. 

      Melting an iron bar

    • C. 

      Crushing an aluminum can

    • D. 

      Burning magnesium ribbon

  • 21. 
    For a chemical reaction, the heat of reaction is equal to the 
    • A. 

      Potential energy of the reactants, only

    • B. 

      Potential energy of the products, only

    • C. 

      Potential energy of the products plus the potential energy of the reactants

    • D. 

      Potential energy of the products minus the potential energy of the reactants

  • 22. 
    Given the equation representing a system at equilibrium: At equilibrium, the concentration of    
    • A. 

      SO2(g) must equal the concentration of SO3(g)

    • B. 

      SO2(g) must be constant

    • C. 

      O2(g) must equal the concentration of SO2(g)

    • D. 

      O2(g) must be decreasing

  • 23. 
    The two isomers of butane have different    
    • A. 

      Formula masses

    • B. 

      Empirical formulas

    • C. 

      Molecular formulas

    • D. 

      Structural formulas

  • 24. 
    An oxidation-reduction reaction involves the    
    • A. 

      Sharing of electrons

    • B. 

      Sharing of protons

    • C. 

      Transfer of electrons

    • D. 

      Transfer of protons

  • 25. 
    Which energy change occurs in an operating voltaic cell? 
    • A. 

      Chemical to electrical

    • B. 

      Electrical to chemical

    • C. 

      Chemical to nuclear

    • D. 

      Nuclear to chemical

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