Conductivity Prac
Aim: To investigate the electrical conductivities of metallic, ionic, covalent molecular and covalent network substances when in the solid, liquid, and solution phases.Substance Solid (Class) Molten SolutionLithium Chloride X Probably Ionic X
Therefore the separated substances can conduct electricity. On the other hand the covalent substance did not conduct in liquid or solid form or in H2O. A Covalent bond such as Ethanol, Glucose, Sucrose and Graphite generally do not conduct but in some cases they can. There is a cloud of elections moving freely so it enables metals to be good conductors. This could be overcome by using a thermometer to measure the amount of heat in the molten and check to see its melting point. An Ionic substance such as Potassium Chloride and Lithium Chloride do not conduct electricity in solid form but conducts when combined with H2O. This happens because of the free electron Graphite has. This could be overcome by heating the electrodes before sticking them into the experiment. Graphite is a non-metallic and is not an Ionic bond however it still conducts electricity. The Ionic Substances however did not conduct in a solid form but it did conduct in water and we can assume it happened because of flux. We can see that all the metallic substances conducted electricity quite well. However Diamond is also a covalent but does not have a free electron floating around like Graphite. Most metals are shiny and quite hard. The other possible error is that if the metal is not melted enough for the electrodes to conduct.
Common topics in this essay:
Graphite Diamond,
H2O Ionic,
Ionic Substances,
,
Bond N/A,
Metallic Bond,
Sucrose Graphite,
H2O Graphite,
Lithium Chloride,
bond n/a,
covalent bond,
metal bond n/a,
Tine Copper,
metal bond,
bond n/a n/a,
solid form,
n/a n/a,
strip metal bond,
ionic bond,
strip metal,
free electron,
bond x,
covalent bond x,
conduct electricity,
granules metal bond,
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