Compare the electrical conductivity of a metal with that of an ionic compound. How is it the same?How is it different?
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2007-02-19 10:23:46 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Other - Science
Metals generally have good conductivity relative to other substances, because the lattice of atoms is sharing the valence electrons, so it is easy for an electrical charge (a voltage) to cause the electrons to move through the lattice as an electrical current.
Ionic compounds, by contrast, have exchanged electrons in the act of forming a compound, and each atom has a complete shell of valence electrons (no excess electrons, and no incomplete shells). Consequently, it is not easy for an electrical charge to break an electron free to move it through the compound.
Conclusion: Metals are good conductors. Ionic compounds are not.
2007-02-19 10:48:35 · answer #1 · answered by actuator 5 · 1⤊ 0⤋
They are generally higher because the electronegativity difference between the constituents of an ionic compound are much greater than those in a molecular compound. Since these forces pull the atoms harder, it takes more energy to excite them and get them to change state.
2016-05-24 17:48:33 · answer #2 · answered by ? 4 · 0⤊ 0⤋