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Chapter 23: Problem 4

Considering that electricity is the flow of electrons from one place to another, propose an explanation for why metals are generally good conductors of electricity, whereas covalently bonded compounds are not.

Short Answer

Expert verified
Metals are good conductors of electricity due to their free moving valence electrons which allow for easy flow of electric current. Covalently bonded compounds, on the other hand, do not conduct electricity well because they do not have these free-moving electrons; their electrons are shared between atoms and are not free to move.

Step by step solution

01

Understand the electron configuration in metals

Metals have free moving electrons in their outermost shell called 'valence electrons'. They are organised in a type of structure known as metallic bonding. This is a structure where positive metal ions are surrounded by a 'sea' of delocalised electrons, making the electrons able to move freely throughout the entire structure. This electron mobility is responsible for the good electrical conductivity in metals.
02

Understand electron configuration in covalently bonded compounds

Covalent compounds, often non-metals, form bonds by sharing their valence electrons with other atoms to form a covalent bond. Unlike metals, the electrons in a covalent compound are not free to move around. Therefore, covalently bonded compounds typically do not conduct electricity well because they lack the free-moving electrons.

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Most popular questions from this chapter

A student suggests that the reason the dividing line goes down and to the right has to do with how electronegativies vary in the periodic table. She says that in order to correspond to a roughly constant electronegativity, the line must be oriented the way that it is (as opposed to being, for example, horizontal or vertical). Indicate whether you agree or disagree with this student, and explain your reasoning.
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