Completing the Model of the Atom

Practice Test
      
  1.The light emitted by the gas in a neon sign is _________________.  
  a.   an electron  
  b.   a filament  
  c.   an emission spectrum  
  d.   an incandescent light  
      
  2.


 
  a.   blue  
  b.   red  
  c.   violet  
  d.   green  
      
  3.The two rows beneath the main body of the periodic table contain the _________________.  
  a.   inner transition elements  
  b.   noble gases  
  c.   alkali metals  
  d.   halogens  
      
  4.These orbitals are aligned along the x, y, and z axes.  
  a.   p orbitals  
  b.   d orbitals  
  c.   s orbitals  
  d.   f orbitals  
      
  5.The elements in Groups 1, 2, and 13-17 are called the _____________.  
  a.   main group elements  
  b.   transition elements  
  c.   noble gases  
  d.   alkali metals  
      
  6.When an iron atom loses all its 4s electrons and one 3d electron, its oxidation number is ______.  
  a.   5+  
  b.   11+  
  c.   3+  
  d.   1+  
      
  7.Except for helium, noble gas atoms have _________.  
  a.   duets  
  b.   octets  
  c.   trios  
  d.   quartets  
      
  8.An electron in an atom emits energy in the form of light when it ________________.  
  a.   rises to a new energy level  
  b.   falls back to a lower energy level  
  c.   leaves the nucleus  
  d.   leaves the atom  
      
  9.1s22s22p1 is the electron configuration for _________.  
  a.   boron  
  b.   fluorine  
  c.   hydrogen  
  d.   lithium  
      
  10.What electron configuration describes the outermost energy level of a molybdenum atom?  
  a.   6p6  
  b.   5d4  
  c.   5s2  
  d.   4d4  
      
  11.The most stable arrangement of electrons in an atom's sublevels and orbitals is called its ________________.  
  a.   shape  
  b.   electronic arrangement  
  c.   electron orientation  
  d.   electron configuration  
      
  12.If an s sublevel could contain up to three electrons, which element would be the first noble gas?  
  a.   neon  
  b.   lithium  
  c.   helium  
  d.   carbon  
      
  13.What element has the electron configuration [Ar]4s23d3?  
  a.   scandium  
  b.   nitrogen  
  c.   vanadium  
  d.   arsenic  
      
  14.The space in which there is a 95% probability of finding an electron is called __________.  
  a.   an orbital  
  b.   an energy level  
  c.   an energy sublevel  
  d.   an electron sphere  
      
  15.The number of valence electrons in a sulfur atom is __________.  
  a.   four  
  b.   two  
  c.   six  
  d.   eight  
      
  16.Which of these is the electron configuration of an atom most likely to lose an electron?  
  a.   1s2 2s2 2p6 3s2 3p5  
  b.   [He]2s2 2p5  
  c.   1s2 2s2 2p6 3s2 3p6 4s1  
  d.   1s2 2s2 2p6  
      
  17.How many electrons may be contained in a p sublevel?  
  a.   three  
  b.   eight  
  c.   six  
  d.   ten  
      
  18.Energy sublevels are designated _____________.  
  a.   x, y, and z  
  b.   1, 2, 3, and 4  
  c.   s, p, d, and f  
  d.   a, b, c, and d  
      
  19.What electron configuration describes the outermost energy level of a selenium atom?  
  a.   4s23d10  
  b.   4s24p4  
  c.   4s24d104p4  
  d.   4s24d4  

 
   
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