Answer the following questions in your own words, using complete sentences. Based on your observations in the lab, categorize each unidentified compound as ionic or covalent. Explain in one or two sentences why you categorized the compounds the way that you did. (5 points)
Based on my observations in the lab I categorized Substance A and Substance C as an ionic bonds because the solids don‘t conduct electricity but when in liquid state and aqueous solutions, electricity was conducted. I categorized substances B and D as covalent bonds because the solids conduct electricity but the liquid state and aqueous solution do not.
Explain, in your own words, the differences between ionic and covalent bonding that account for the differences in their melting points. (4 points) Ionic bonds typically have much higher melting points than covalent bonds because of their crystal-like structures. The bondage is much more complex and requires higher heat to break than a covalent whose bonds are broken relatively easy.
In order to conduct an electrical current, a substance must have charged particles (ions or electrons) that are free-moving (able to move about throughout the sample).
Why do you think ionic compounds are not able to conduct electricity as solids, even though they can as liquids and in solution? (2 points) I think ionic compounds can’t conduct electricity as solids because the particle are all packed together and have no room to move freely as opposed to the particle when in liquid state or solutions.
Based on your research and observations, why do you think pure (distilled) water does not conduct electricity but tap water usually does? (2 points)
I think this is because tap water contains more ions than distilled water allowing it to conduct electricity. I also think the minerals that dissolve in the water have a lot to do with the conductivity.