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Word Count: 442
Aim To investigate the electrical conductivities of metallic ionic covalent molecular and covalent network substances when in the solid liquid and solution phases Results Ability to conduct SubstanceSolidClassMoltenSolution Zinc StripMetal BondNA NA Tin StripMetal BondNA NA GraphiteCovalent BondNA NA Copper StripMetal BondNA NA Zinc GranulesMetal Bond NA Tin GranulesMetal Bond NA Lithium ChlorideXProbably IonicX Potassium ChlorideXIonic BondX EthanolXCovalent BondXX GlucoseXCovalent BondXX SucroseXCovalent BondXX LiCl KCl H20NAIonic BondX NA test could not be done Tick shows conductivity more than one shows more conductivity Cross X no conductivity Discussion The Zinc Tine and Copper all conducted electricity and the bond is known as a Metallic Bond There is a cloud of elections moving freely so it enables metals to be good conductors Most metals are shiny and quite hard An Ionic substance such as Potassium Chloride and Lithium Chloride do not conduct electricity in solid form but conducts when combined with H2O When Ionic is in solid form most have a firm and secure bond but when combined with H2O the bond is worst Therefore the separated substances can conduct electricity A Covalent bond such as Ethanol Glucose Sucrose and Graphite generally do not conduct but in some cases they can For example Graphite can conduct electricity because it has a free electron We can see that all the metallic substances conducted electricity quite well 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 On the other hand the covalent substance did not conduct in liquid or solid form or in H2O Graphite is a non-metallic and is not an Ionic bond however it still conducts electricity This happens because of the free electron Graphite has However Diamond is also a covalent but does not have a free electron floating around like Graphite One of two possible errors
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