Regents Chemistry Practice Test

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 Regents Chemistry Practice Test

  
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  • 1. 
    The modern model of the atom is based on the work of 
    • A. 

      One scientist over a short period of time

    • B. 

      One scientist over a long period of time

    • C. 

      Many scientists over a short period of time

    • D. 

      many scientists over a long period of time


  • 2. 
    Which statement is true about the charges assigned to an electron and a proton? 
    • A. 

      Both an electron and a proton are positive.

    • B. 

      An electron is positive and a proton is nega- tive.

    • C. 

      An electron is negative and a proton is posi- tive.

    • D. 

      Both an electron and a proton are negative.


  • 3. 
    In the wave-mechanical model, an orbital is a region of space in an atom where there is 
    • A. 

      A high probability of finding an electron

    • B. 

      A high probability of finding a neutron

    • C. 

      A circular path in which electrons are found

    • D. 

      A circular path in which neutrons are found


  • 4. 
    What is the charge of the nucleus in an atom of oxygen-17? 
    • A. 

      0

    • B. 

      -2

    • C. 

      +8

    • D. 

      +17


  • 5. 
    Which pair of symbols represents a metalloid and a noble gas? 
    • A. 

      Si and Bi

    • B. 

      As and Ar

    • C. 

      Ge and Te

    • D. 

      Ne and Xe


  • 6. 
    Which statement describes a chemical property of iron? 
    • A. 

      Iron can be flattened into sheets.

    • B. 

      Iron conducts electricity and heat.

    • C. 

      Iron combines with oxygen to form rust.

    • D. 

      Iron can be drawn into a wire.


  • 7. 

    Given the reaction: N2(g) + 3 H2(g) <-> 2 NH3(g) What is the mole-to-mole ratio between nitro- gen gas and hydrogen gas? 
    • A. 

      1:2

    • B. 

      1:3

    • C. 

      2:2

    • D. 

      2:3


  • 8. 
    What is the percent by mass of oxygen in propanal, CH3CH2CHO? 
    • A. 

      10.0%

    • B. 

      27.6%

    • C. 

      38.1%

    • D. 

      62.1%


  • 9. 
    Covalent bonds are formed when electrons are    
    • A. 

      Transferred from one atom to another

    • B. 

      Captured by the nucleus

    • C. 

      Mobile within a metal

    • D. 

      Shared between two atoms


  • 10. 
    Which type of molecule is CF4?    
    • A. 

      Polar, with a symmetrical distribution of charge

    • B. 

      Polar, with an asymmetrical distribution of charge

    • C. 

      Nonpolar, with a symmetrical distribution of charge

    • D. 

      Nonpolar, with an asymmetrical distribution of charge


  • 11. 
    Which change occurs when a barium atom loses two electrons? 
    • A. 

      It becomes a negative ion and its radius decreases.

    • B. 

      It becomes a negative ion and its radius increases.

    • C. 

      It becomes a positive ion and its radius decreases.

    • D. 

      It becomes a positive ion and its radius increases.


  • 12. 
    Which of these elements has the least attraction for electrons in a chemical bond? 
    • A. 

      Oxygen

    • B. 

      Fluorine

    • C. 

      Nitrogen

    • D. 

      Chlorine


  • 13. 
    Conductivity in a metal results from the metal atoms having 
    • A. 

      High electronegativity

    • B. 

      High ionization energy

    • C. 

      highly mobile protons in the nucleus

    • D. 

      highly mobile electrons in the valence shell


  • 14. 
    Recovering the salt from a mixture of salt and water could best be accomplished by
    • A. 

      Evaporation

    • B. 

      Filtration

    • C. 

      Paper chromatography

    • D. 

      Density determination


  • 15. 
    The average kinetic energy of water molecules is greatest in which of these samples? 
    • A. 

      10 g of water at 35°C

    • B. 

      10 g of water at 55°C

    • C. 

      100 g of water at 25°C

    • D. 

      100 g of water at 45°C


  • 16. 
    Helium is most likely to behave as an ideal gas when it is under 
    • A. 

      High pressure and high temperature

    • B. 

      High pressure and low temperature

    • C. 

      Low pressure and high temperature

    • D. 

      Low pressure and low temperature


  • 17. 
    At STP, the element oxygen can exist as either O2 or O3 gas molecules. These two forms of the element have 
    • A. 

      The same chemical and physical properties

    • B. 

      The same chemical properties and different physical properties

    • C. 

      Different chemical properties and the same physical properties

    • D. 

      Different chemical and physical properties


  • 18. 
    Which sample contains particles in a rigid, fixed, geometric pattern? 
    • A. 

      CO2 (aq)

    • B. 

      HCl (g)

    • C. 

      H2O (l)

    • D. 

      KCl (s)


  • 19. 
    Given the reaction at 25°C: Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) The rate of this reaction can be increased by using 5.0 grams of powdered zinc instead of a 5.0-gram strip of zinc because the powdered zinc has 
    • A. 

      Lower kinetic energy

    • B. 

      Lower concentration

    • C. 

      More surface area

    • D. 

      More zinc atoms


  • 20. 
    Which statement about a system at equilibrium is true? 
    • A. 

      The forward reaction rate is less than the reverse reaction rate.

    • B. 

      The forward reaction rate is greater than the reverse reaction rate.

    • C. 

      The forward reaction rate is equal to the reverse reaction rate.

    • D. 

      The forward reaction rate stops and the reverse reaction rate continues.


  • 21. 
    A catalyst increases the rate of a chemical reaction by 
    • A. 

      Lowering the activation energy of the reaction

    • B. 

      Lowering the potential energy of the products

    • C. 

      Raising the temperature of the reactants

    • D. 

      Raising the concentration of the reactants


  • 22. 
    Which element must be present in an organic compound? 
    • A. 

      Hydrogen

    • B. 

      Oxygen

    • C. 

      Carbon

    • D. 

      Nitrogen


  • 23. 
    Which compound is a saturated hydrocarbon?    
    • A. 

      Hexane

    • B. 

      Hexene

    • C. 

      Hexanol

    • D. 

      Hexanal


  • 24. 
    Which of these compounds has chemical prop- erties most similar to the chemical properties of ethanoic acid? 
    • A. 

      C3H7COOH

    • B. 

      C2H5OH

    • C. 

      C2H5COOC2H5

    • D. 

      C2H5OC2H5


  • 25. 
    Given the reaction that occurs in an electrochemical cell:  Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)     During this reaction, the oxidation number of Zn changes from
    • A. 

      0 to +2

    • B. 

      0 to -2

    • C. 

      +2 to 0

    • D. 

      -2 to 0


  • 26. 

    This reaction is an example of
    • A. 

      Fermentation

    • B. 

      Saponification

    • C. 

      Hydrogenation

    • D. 

      Esterification


  • 27. 
    A voltaic cell spontaneously converts    
    • A. 

      Electrical to chemical energy

    • B. 

      Chemical to electrical energy

    • C. 

      Electrical to nuclear energy

    • D. 

      Nuclear to electrical energy


  • 28. 
    Which pair of formulas represents two compounds that are electrolytes? 
    • A. 

      HCl and CH3OH

    • B. 

      HCl and NaOH

    • C. 

      C5H12 and CH3OH

    • D. 

      C5H12 and NaOH


  • 29. 
    Hydrogen chloride, HCl, is classified as an Arrhenius acid because it produces 
    • A. 

      H+ ions in aqueous solution

    • B. 

      Cl– ions in aqueous solution

    • C. 

      OH– ions in aqueous solution

    • D. 

      NH4+ ions in aqueous solution


  • 30. 
    Which compound could serve as a reactant in a neutralization reaction? 
    • A. 

      NaCl

    • B. 

      KOH

    • C. 

      CH3OH

    • D. 

      CH3CHO


  • 31. 
    Which of these particles has the greatest mass?    
    • A. 

      Alpha

    • B. 

      Beta

    • C. 

      Neutron

    • D. 

      Positron


  • 32. 
    In a nuclear fusion reaction, the mass of the products is 
    • A. 

      Less than the mass of the reactants because some of the mass has been converted to energy

    • B. 

      Less than the mass of the reactants because some of the energy has been converted to mass

    • C. 

      More than the mass of the reactants because some of the mass has been converted to energy

    • D. 

      More than the mass of the reactants because some of the energy has been converted to mass


  • 33. 
    Which of these types of radiation has the greatest penetrating power? 
    • A. 

      Alpha

    • B. 

      Beta

    • C. 

      Gamma

    • D. 

      Positron


  • 34. 
    How many electrons are contained in an Au3+ ion?
    • A. 

      76

    • B. 

      79

    • C. 

      82

    • D. 

      197


  • 35. 
    Which electron configuration represents the electrons of an atom in an excited state? 
    • A. 

      2-4

    • B. 

      2-6

    • C. 

      2-7-2

    • D. 

      2-8-2


  • 36. 

    • A. 

      Three fewer neutrons

    • B. 

      Three fewer valence electrons

    • C. 

      Three more neutrons

    • D. 

      Three more valence electrons


  • 37. 
    Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element X be found? 
    • A. 

      1

    • B. 

      2

    • C. 

      15

    • D. 

      16


  • 38. 
    What is the empirical formula for the compound C6H12O6? 
    • A. 

      CH2O

    • B. 

      C2H4O2

    • C. 

      C3H6O3

    • D. 

      C6H12O6


  • 39. 
    The bonds between hydrogen and oxygen in a water molecule are classified as 
    • A. 

      Polar covalent

    • B. 

      Nonpolar covalent

    • C. 

      Ionic

    • D. 

      Metallic


  • 40. 

    • A. 

      AB

    • B. 

      BC

    • C. 

      CD

    • D. 

      EF


  • 41. 
    Using your knowledge of chemistry and the information in Reference Table H, which statement concerning propanone and water at 50°C is true? 
    • A. 

      Propanone has a higher vapor pressure and stronger intermolecular forces than water.

    • B. 

      Propanone has a higher vapor pressure and weaker intermolecular forces than water.

    • C. 

      Propanone has a lower vapor pressure and stronger intermolecular forces than water.

    • D. 

      Propanone has a lower vapor pressure and weaker intermolecular forces than water.


  • 42. 
    A solution that is at equilibrium must be    
    • A. 

      Concentrated

    • B. 

      Dilute

    • C. 

      Saturated

    • D. 

      Unsaturated


  • 43. 

    • A. 

      Increasing the concentration of NO (g)

    • B. 

      Increasing the concentration of N2 (g)

    • C. 

      Decreasing the reaction temperature

    • D. 

      Decreasing the reaction pressure


  • 44. 
    Which 10-milliliter sample of water has the greatest degree of disorder? 
    • A. 

      H2O (g) at 120°C

    • B. 

      H2O (l) at 80°C

    • C. 

      H2O (l) at 20°C

    • D. 

      H2O (s) at 0°C


  • 45. 
    Which pH indicates a basic solution?    
    • A. 

      1

    • B. 

      5

    • C. 

      7

    • D. 

      12


  • 46. 
    Which structural formula represents 2-pentyne?
    • A. 
    • B. 
    • C. 
    • D. 

  • 47. 
    Which structural formula represents an ether?
    • A. 
    • B. 
    • C. 
    • D. 

  • 48. 

    • A. 

      Al + 3e– → Al3+

    • B. 

      Al → Al3+ + 3e–

    • C. 

      O2 +4e– →2O2–

    • D. 

      O2 →2O2– +4e–


  • 49. 
    Based on Reference Table N, what fraction of a sample of gold-198 remains radioactive after 2.69 days? 
    • A. 

      1/4

    • B. 

      1/2

    • C. 

      3/4

    • D. 

      7/8


  • 50. 
    As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally 
    • A. 

      Decreases

    • B. 

      Increases

    • C. 

      Remains the same


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