Atomic structure and Periodicity
Quiz by Natalie Wieland
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12 questions
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- Q1The 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 nucleus3s because it experiences higher attractive forces3s because it is filled before 3p3p because it only has 1 electron in the orbital120s
- Q2The 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 redphotoelectron spectroscopy because the electron arrangement is responsible for the colormass spectrometry because knowing the mass can allow for calculation of concentrationUV-Vis spectrometry because the solution has a color30s
- Q3The quantum mechanical atomic model replaced the Bohr atomic model becausethe quantum mechanical model was based on mathematicsBohr's model could not predict the spectra for elements other than hydrogenBohr's model did not account for neutronselectrons act as waves as well as particles120s
- Q4What is the average atomic mass of element X based on the data above?49.5 amu49.0 amu49.8 amu50 amu120s
- Q5Why does chlorine gain an electron to become a chloride ion?Atoms become stable when they achieve a full octetLess shielding means there is room for another electronAn electron is attracted to the large effective nuclear chargeAdding an electron completely fills the s and p orbitals of energy level 3120s
- Q6The 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 to94 amu90 amu91 amu93 amu120s
- Q7How many unpaired electrons are in the atom represented by the electron configuration above?0132120s
- Q8The complete photoelectron spectrum of an element is given above. Which labeled peak corresponds to the 1s electrons and why?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.120s
- Q9The 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 ?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.120s
- Q10Which 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 .120s
- Q11Which 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 nucleusRb has a higher electronegativity than Li has120s
- Q12Rb 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 .120s