Electrical conductivity of SiCl4

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Discussion Overview

The discussion revolves around the electrical conductivity of silicon tetrachloride (SiCl4) in different states and its interaction with water. Participants explore the reasons for SiCl4's lack of conductivity in its molten state compared to when it is mixed with water, as well as the contrasting behavior of aluminum oxide (Al2O3).

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested

Main Points Raised

  • Some participants question why SiCl4 does not conduct electricity in its molten state, suggesting it may be due to its molecular structure compared to ionic compounds like Al2O3.
  • Others propose that Al2O3 is insoluble in water, which would not affect its conductivity, and emphasize the importance of ionic bonds in conductivity.
  • There is a suggestion that the behavior of SiCl4 in water is complex, with reactions leading to the formation of SiO2 and HCl, raising questions about the conductivity of these products.
  • One participant notes that SiCl4 does not have free electrons in its molten state, which contributes to its inability to conduct electricity.
  • Another participant highlights that while SiO2 is insoluble in water, HCl, which is produced from the reaction of SiCl4 with water, is ionic and can conduct electricity.

Areas of Agreement / Disagreement

Participants express differing views on the conductivity of SiCl4 and its reaction products, with no consensus reached on the underlying reasons for these behaviors.

Contextual Notes

Some assumptions about the nature of ionic versus molecular compounds and their solubility in water are present, but these are not fully explored or resolved in the discussion.

Janiceleong26
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Why doesn't SiCl4 conduct electricity when it's in its molten state and conducts electricity when water is added? The answer is C. I know very well what is X and Z, but unsure what is Y.. Why not Al2O3? What's the difference? Does it got to do with their structures? Al2O3 is ionic with a degree of covalent character whereas SiCl4 is a simple molecular? if so, what is the effect of it?
 
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What happens to each of those compounds when they are put into water? (Hint: "dissolve" and "doesn't dissolve" are not the only possible answers).
 
RUber said:
According to: https://en.wikipedia.org/wiki/Aluminium_oxide
Aluminum oxide is insoluble in water, so adding water would probably not affect its conductivity.
You are right to look for the ionic bond.
Thank you for the info. But SiCl4 is a simple molecular..it can react with water to form SiO2, but SiO2 is giant molecular! I'm really confused
 
Borek said:
What happens to each of those compounds when they are put into water? (Hint: "dissolve" and "doesn't dissolve" are not the only possible answers).
NaF will split and form Na+ and F-1 ions, SiCl4 reacts with water to form SiO2, and SiO2 has no reaction with water
 
Janiceleong26 said:
SiCl4 reacts with water to form SiO2
... and what else?
 
SiCl4 is not ionic, therefore it does not have free electrons to conduct electricity when in molten state.
However, when SiCl4 reacts with water, it form SiO2 and HCl. SiO2 is insoluble in water, but HCl conducts electricity since it's ionic.

Source from my school notes :D
 

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