0
The characteristic that allows some metals to be better conductors of electricity is that they have 'free electrons'. Free Electrons simply means that there is a weaker bond between the electrons on the outer valence shell to the nucleus of the atom, than other atoms. This weak bond allows electrons in metals to become more easily excited (when mechanical means of generation occurs), where the electrons are able to transfer from one atom to another. I imagine this is what the question is asking. Basically, electricity is inherent in the material. Metals have weak bonds in their outer valence electron shell. A: In metals, the atoms move freely, allowing heat to travel faster. :)
What else can I help you with?
What property of metals contribute to their tendency to use electrical conductivity?
The electrons in metals are delocalized, they move freely.
What passes freely through metals?
Electricity passes freely through metals due to the presence of free electrons that can move easily within the metal structure. This property makes metals good conductors of electricity.
Do electrons free drift in metals?
Yes, electrons move freely in metals.
Why metals are goodconducter of electricity?
Metals have freely moving electrons as well as particles to conduct heat. The electrons move freely to pass thermal energy.
What type of compounds have freely moving electrons?
Compounds with freely moving electrons are typically metals. In metals, the outermost electrons are not strongly bound to any particular atom and can move freely throughout the material, leading to high electrical conductivity.
What characteristic of electrons do metals have in common?
Metals commonly have free or delocalized electrons that allow them to conduct electricity and heat efficiently. These electrons are not tightly bound to individual atoms, enabling them to move freely throughout the metallic lattice. This property contributes to the malleability and ductility of metals, as well as their shiny appearance. Additionally, the presence of these free electrons contributes to the formation of metallic bonds, which are fundamental to the structure and properties of metals.
How are metals distinguished from nonmetals?
The electrons in metals move freely. This means metals are metallic i.e. Shiny due to light reflecting off electrons and malleable i.e. Bendable due to free electrons
What explains the properties explains metals?
The electrons they contain, which have the ability to move freely
What specific property of metals accounts for their unusual conductivity?
Outermost orbital shell of a metal has very few electrons with corresponding values of energy. This specific property accounts for the unusual electrical conductivity of metals. Highest conductivity occurs in metals with only one valence electron.
How metals conduct electricity?
Metals conduct electricity easily because the electrons in a metal crystal can move freely among the atoms.They are know as free electrons.
Do freely moving valence electrons account for electrical conductivity in metals?
Yes, freely moving valence electrons account for electrical conductivity in metals. These electrons are not bound to specific atoms and can move throughout the metal lattice, creating a flow of electric charge when a voltage is applied. This mobility of electrons allows metals to conduct electricity efficiently.
What Electrons that are free to move in a metal are referred to as?
Electrons that are free to move in a metal are referred to as "conduction electrons." These electrons are not bound to any specific atom and can move freely throughout the metal lattice, allowing for the conduction of electricity. This property is essential for metals to conduct electric current efficiently.
