Electrical Conductivity Quiz

What is electrical conductivity a measure of?

• Ability of a material's charge carriers to move through the material

• Ability of a material to resist charge flow

• Ability of a material to store charge

• Ability of a material to generate charge

Why do gases have very low conductivity?

• Lack of free electrons

• Presence of excess electrons

• Strong metallic bonds

• High ionization potential

What makes most metals good electrical conductors?

• Tightly bound valence electrons

• Covalent bonding structure

• Presence of excess protons

• Lattice of metallic bonds with a sea of electrons

Why are nonmetals poor conductors of electricity?

• Strong metallic bonds

• High ionization potential

• Presence of excess free electrons

• Tightly bound valence electrons to atomic nuclei

What is the function of ions dissolved in water regarding its ability to conduct electricity?

• Has no effect on water's conductivity

• Reduces water's ability to conduct electricity

• Turns water into an insulator

• Enhances water's ability to conduct electricity

Why is air not a good conductor of electricity?

• Relatively high potential needed for charge carriers to travel

• Strong metallic bonds

• Low ionization potential

• Presence of excess free electrons

What are the charge carriers in solid materials?

• Electrons

• Neutrons

• Protons

• Valence electrons

What is the relationship between solid material's conductivity and valence electrons?

• Related to the number of electrons in the material

• Related to the number of neutrons in the nucleus

• Related to the number of protons in the nucleus

• Related to how loosely bound valence electrons are to a specific nucleus

Why does liquid metal conduct electricity very well?

• Lattice of metallic bonds with a sea of electrons

• Covalent bonding structure

• Tightly bound valence electrons

• Presence of excess protons

Why are covalent compounds usually good electrical insulators?

• Strong metallic bonds

• Presence of excess free electrons

• Tightly bound valence electrons to atomic nuclei

• High ionization potential