The Kinetic Theory of Matter

Practice Test
      
  1.The light emitted by the gas in a neon sign is _________________.  
  a.   an incandescent light  
  b.   an electron  
  c.   an emission spectrum  
  d.   a filament  
      
  2.This transition element is used in many barometers and thermometers.  
  a.   titanium  
  b.   iron  
  c.   copper  
  d.   mercury  
      
  3.In general, atomic size ___________ from top to bottom within a Group.  
  a.   increases  
  b.   increases, then decreases  
  c.   remains the same  
  d.   decreases  
      
  4.Why was Mendeleev's periodic table widely accepted?  
  a.   He organized the first 14 known elements.  
  b.   He predicted the existence and properties of undiscovered elements.  
  c.   He was the first to notice a pattern of similar properties among elements.  
  d.   His periodic table listed all of the elements in the correct order.  
      
  5.A chemical bond that results from a shared pool of valence electrons is called a ____________ bond.  
  a.   directional  
  b.   ionic  
  c.   metallic  
  d.   polar covalent  
      
  6.Plutonium and americium are ______________.  
  a.   Noble gases  
  b.   metalloids  
  c.   nonmetals  
  d.   synthetic elements  
      
  7.An electron in an atom emits energy in the form of light when it ________________.  
  a.   falls back to a lower energy level  
  b.   rises to a new energy level  
  c.   leaves the atom  
  d.   leaves the nucleus  
      
  8.The elements in Groups 1, 2, and 13-17 are called the _____________.  
  a.   noble gases  
  b.   alkali metals  
  c.   main group elements  
  d.   transition elements  
      
  9.Many transition elements have multiple positive oxidation states because their atoms can lose some of their _______________.  
  a.   nuclear protons  
  b.   s electrons  
  c.   d electrons  
  d.   p electrons  
      
  10.These two elements are liquids at room temperature and pressure.  
  a.   silver and nitrogen  
  b.   mercury and oxygen  
  c.   lithium and cesium  
  d.   mercury and bromine  
      
  11.________________ is the reverse of evaporation.  
  a.   Melting  
  b.   Condensation  
  c.   Freezing  
  d.   Boiling  
      
  12._____________ is the measure of an atom's ability to attract electrons in a bond.  
  a.   Ionic radius  
  b.   Electronegativity  
  c.   melting point  
  d.   Shielding  
      
  13.The boiling point of methane, CH4, is ___________ than that of water.  
  a.   much higher  
  b.   slightly higher  
  c.   much lower  
  d.   slightly higher  
      
  14. A transistor may be produced by placing a p-typesemiconductor between two _______________.  
  a.   electrons  
  b.   molecules  
  c.   n-type semiconductors  
  d.   p-type semiconductors  
      
  15.What element has the electron configuration [Ar]4s23d3?  
  a.   arsenic  
  b.   vanadium  
  c.   nitrogen  
  d.   scandium  
      
  16.Among the ions F-, Li+, Cs+, and At-, which would you expect to have the smallest ionic radius?  
  a.   Li+  
  b.   At-  
  c.   F-  
  d.   Cs+  
      
  17.A state of ___________ is reached in a sealed container that contains significant amounts of both a liquid substance and its vapor.  
  a.   elevation  
  b.   freezing  
  c.   Equilibruim  
  d.   reaction  
      
  18.Water molecules stick together to form droplets because of their ___________.  
  a.   volumes  
  b.   covalencies  
  c.   masses  
  d.   polarities  
      
  19.Gas particles _______________ kinetic energy when they collide with other particles or the walls of their container.  
  a.   gain some  
  b.   gain much  
  c.   lose some  
  d.   lose no  
      
  20.The _______________ states that the submicroscopic particles of all matter are in constant, random motion.  
  a.   Brownian law  
  b.   kinetic theory  
  c.   atomic theory  
  d.   molecular hypothesis  

 
   
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