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Atomic structure and Periodicity

Quiz by Natalie Wieland

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12 questions
Show answers
  • Q1
    The formation of an aluminum ion occurs when 3 electrons are removed. Which electron would require the most energy to remove?
    3p because it is farther from the nucleus
    3s because it experiences higher attractive forces
    3s because it is filled before 3p
    3p because it only has 1 electron in the orbital
  • Q2
    The concentration of a red-colored solution of cobalt(II) ions needs to be determined. What spectroscopic technique would be the best choice?
    infrared spectrometry because the solution is red
    photoelectron spectroscopy because the electron arrangement is responsible for the color
    mass spectrometry because knowing the mass can allow for calculation of concentration
    UV-Vis spectrometry because the solution has a color
  • Q3
    The quantum mechanical atomic model replaced the Bohr atomic model because
    the quantum mechanical model was based on mathematics
    Bohr's model could not predict the spectra for elements other than hydrogen
    Bohr's model did not account for neutrons
    electrons act as waves as well as particles
  • Q4
    What is the average atomic mass of element X based on the data above?
    Question Image
    49.5 amu
    49.0 amu
    49.8 amu
    50 amu
  • Q5
    Why does chlorine gain an electron to become a chloride ion?
    Atoms become stable when they achieve a full octet
    Less shielding means there is room for another electron
    An electron is attracted to the large effective nuclear charge
    Adding an electron completely fills the s and p orbitals of energy level 3
  • Q6
    The mass spectrum for an unknown element is shown above. According to the information in the spectrum, the atomic mass of the unknown element is closest to
    Question Image
    94 amu
    90 amu
    91 amu
    93 amu
  • Q7
    How many unpaired electrons are in the atom represented by the electron configuration above?
    Question Image
  • Q8
    The complete photoelectron spectrum of an element is given above. Which labeled peak corresponds to the 1s electrons and why?
    Question Image
    Peak Y, because electrons in the 1s sublevel are the farthest from the nucleus.
    Peak Y, because there are fewer electrons in an s sublevel than in a p sublevel.
    Peak X, because 1s electrons are the easiest to remove from the atom.
    Peak X , because 1s electrons have the strongest attractions to the nucleus.
  • Q9
    The atomic radii of the elements in the nitrogen group in the periodic table are given in the table above. Which of the following best helps explain the trend of increasing atomic radius from N to Bi ?
    Question Image
    The attractive force between the valence electrons and the nuclei of the atoms decreases.
    The number of electrons in the outermost shell of the atom increases.
    The repulsive force between the valence electrons and the electrons in the inner shells decreases.
    The number of particles in the nucleus of the atom increases.
  • Q10
    Which of the following best helps to explain why the atomic radius of K is greater than that of Br?
    The first ionization energy of K is higher than that of Br .
    In the ground state, an atom of K has fewer unpaired electrons than an atom of Br has.
    The effective nuclear charge experienced by valence electrons is smaller K for than for Br .
    The valence electrons in K are in a higher principal energy level than those of Br .
  • Q11
    Which of the following best helps explain why an atom of Rb gas more easily loses an electron in a chemical reaction than an atom of Li gas?
    The atom Rb has a greater number of valence electrons than the atom Li has.
    The nucleus of the Rb atom has a greater number of protons and neutrons than the nucleus of the Li atom has.
    In the Rb atom the valence electron is farther from its nucleus than the valence electron of Li is from its nucleus
    Rb has a higher electronegativity than Li has
  • Q12
    Rb reacts with O in a mole ratio of 2 to 1 , forming the ionic Rb2C compound . Which of the following elements will react with O in a mole ratio of 2 to 1 , forming an ionic compound, and why?
    Br, because the atomic mass of Br is similar to that of Rb .
    Cs, because it is in the same group as Rb .
    Sr, because it is in the same period as Rb .
    S, because it is in the same group as O .

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