California Standards Test On Chemistry!

29 Questions | Total Attempts: 343

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Chemistry Practice Quizzes & Trivia

The following Chemistry questions are based on the California Standards Test which is conducted as part of the Standardized Testing and Reporting (STAR) Program under policies set by the State Board of Education. This quiz has been developed to test students knowledge about the fundamentals of chemistry and chemical reactions. Read the questions carefully and answer. So, let's try out the quiz. All the best!


Questions and Answers
  • 1. 
    Electrical fires cannot be safely put out by dousing them with water. However, fire extinguishers that spray solid carbon dioxide on the fire work very effectively. This method works because carbon dioxide
    • A. 

      Displaces the oxygen.

    • B. 

      Renders the fire’s fuel non-flammable.

    • C. 

      Forms water vapor.

    • D. 

      Blows the fire out with strong wind currents.

  • 2. 
    In order to advance to the level of a theory, a hypothesis should be
    • A. 

      Obviously accepted by most people.

    • B. 

      A fully functional experiment.

    • C. 

      In alignment with past theories.

    • D. 

      Repeatedly confirmed by experimentation.

  • 3. 
    When a metal is heated in a flame, the flame has a distinctive color. This information was eventually extended to the study of stars because
    • A. 

      The color spectra of stars indicate which elements are present.

    • B. 

      A red shift in star color indicates stars are moving away.

    • C. 

      Star color indicates absolute distance.

    • D. 

      It allows the observer to determine the size of stars.

  • 4. 
    Which of the following ordered pairs of elements shows an increase in atomic number but a decrease in average atomic mass?
    • A. 

      Ag to Pd

    • B. 

      Co to Ni

    • C. 

      Ge to Sn

    • D. 

      Cr to Mo

  • 5. 
    Iodine would have chemical properties most like
    • A. 

      Manganese (Mn)

    • B. 

      Tellurium (Te)

    • C. 

      Chlorine (Cl)

    • D. 

      Xenon (Xe)

  • 6. 
    The chart above shows the relationship between the first ionization energy and the increase in atomic number. The letter on the chart for the alkali family of elements is
    • A. 

      W

    • B. 

      X

    • C. 

      Y

    • D. 

      Z

  • 7. 
    Which of the following atoms has six valence electrons?
    • A. 

      Magnesium (Mg)

    • B. 

      Silicon (Si)

    • C. 

      Sulfur (S)

    • D. 

      Argon (Ar)

  • 8. 
    Which statement best describes the density of an atom’s nucleus?
    • A. 

      The nucleus occupies most of the atom’s volume but contains little of its mass.

    • B. 

      The nucleus occupies very little of the atom’s volume and contains little of its mass.

    • C. 

      The nucleus occupies most of the atom’s volume and contains most of its mass.

    • D. 

      The nucleus occupies very little of the atom’s volume but contains most of its mass.

  • 9. 
    • A. 

      Alpha

    • B. 

      Beta

    • C. 

      Gamma

    • D. 

      X-ray

  • 10. 
    The reason salt crystals, such as KCl, hold together so well is because the cations are strongly attracted to
    • A. 

      Neighboring cations.

    • B. 

      The protons in the neighboring nucleus.

    • C. 

      Free electrons in the crystals.

    • D. 

      Neighboring anions.

  • 11. 
    Which of the following elements has the same Lewis dot structure as silicon?
    • A. 

      Germanium (Ge)

    • B. 

      Aluminum (Al)

    • C. 

      Arsenic (As)

    • D. 

      Gallium (Ga)

  • 12. 
    Which substance is made up of many monomers joined together in long chains?
    • A. 

      Salt

    • B. 

      Protein

    • C. 

      Ethanol

    • D. 

      Propane

  • 13. 
    Proteins are large macromolecules composed of thousands of subunits. The structure of the protein depends on the sequence of
    • A. 

      Lipids

    • B. 

      Monosaccharides

    • C. 

      Amino acids

    • D. 

      Nucleosides

  • 14. 
    The volume of 400 mL of chlorine gas at 400 mm Hg is decreased to 200 mL at constant temperature. What is the new gas pressure?
    • A. 

      400mm Hg

    • B. 

      300mm Hg

    • C. 

      800mm Hg

    • D. 

      650mm Hg

  • 15. 
    Standard temperature and pressure (STP) are defined as
    • A. 

      0 ºC and 1.0 atm pressure.

    • B. 

      0 ºC and 273 mm Hg pressure.

    • C. 

      0 K and 1.0 atm pressure.

    • D. 

      0 K and 760 mm Hg pressure.

  • 16. 
    What is the equivalent of 423 kelvin in degrees Celsius?
    • A. 

      –223 ºC

    • B. 

      –23 ºC

    • C. 

      150 ºC

    • D. 

      696 ºC

  • 17. 
    If the attractive forces among solid particles are less than the attractive forces between the solid and a liquid, the solid will
    • A. 

      Probably form a new precipitate as its crystal lattice is broken and re-formed.

    • B. 

      Be unaffected because attractive forces within the crystal lattice are too strong for the dissolution to occur.

    • C. 

      Begin the process of melting to form a liquid.

    • D. 

      Dissolve as particles are pulled away from the crystal lattice by the liquid molecules.

  • 18. 
    If the solubility of NaCl at 25 ºC is 36.2 g/100 g H2O, what mass of NaCl can be dissolved in 50.0 g of H2O?
    • A. 

      18.1 g

    • B. 

      36.2 g

    • C. 

      72.4 g

    • D. 

      86.2 g

  • 19. 
    How many moles of HNO3 are needed to prepare 5.0 liters of a 2.0 M solution of HNO3?
    • A. 

      2.5

    • B. 

      5

    • C. 

      10

    • D. 

      20

  • 20. 
    The random molecular motion of a substance is greatest when the substance is
    • A. 

      Condensed

    • B. 

      A liquid

    • C. 

      Frozen

    • D. 

      A gas

  • 21. 
    The boiling point of liquid nitrogen is 77 kelvin. It is observed that ice forms at the opening of a container of liquid nitrogen. The best explanation for this observation is
    • A. 

      Water at zero degrees Celsius is colder than liquid nitrogen and freezes.

    • B. 

      The nitrogen boils and then cools to form a solid at the opening of the container.

    • C. 

      Water trapped in the liquid nitrogen escapes and freezes.

    • D. 

      The water vapor in the air over the opening of the liquid nitrogen freezes out.

  • 22. 
    • A. 

      1000 J

    • B. 

      720 J

    • C. 

      480 J

    • D. 

      240 J

  • 23. 
    Equal volumes of 1 molar hydrochloric acid (HCl) and 1 molar sodium hydroxide base (NaOH) are mixed. After mixing, the solution will be
    • A. 

      Strongly acidic

    • B. 

      Weakly acidic

    • C. 

      Nearly neutral

    • D. 

      Weakly basic

  • 24. 
    A catalyst can speed up the rate of a given chemical reaction by
    • A. 

      Increasing the equilibrium constant in favor of products.

    • B. 

      Lowering the activation energy required for the reaction to occur.

    • C. 

      Raising the temperature at which the reaction occurs.

    • D. 

      Increasing the pressure of reactants, thus favoring products.

  • 25. 
    When a reaction is at equilibrium and more reactant is added, which of the following changes is the immediate result?
    • A. 

      The reverse reaction rate remains the same.

    • B. 

      The forward reaction rate increases.

    • C. 

      The reverse reaction rate decreases.

    • D. 

      The forward reaction rate remains the same.