What is a metallic bond?
Q: What is a metallic bond?
A: A metallic bond is the sharing of many detached electrons between many positive ions, where the electrons act as a "glue" giving the substance a definite structure. It is unlike covalent or ionic bonding.
Q: Why do metals have low ionization energy?
A: Metals have low ionization energy because their valence electrons can be delocalized throughout the metals, meaning they are not associated with a particular nucleus of metal and are free to move throughout the whole crystalline structure forming a "sea" of electrons.
Q: How does metallic bonding cause certain traits in metals?
A: Metallic bonds causes many of the traits of metals, such as strength, malleability, ductility, luster, conduction of heat and electricity. This is because the electrons move freely which allows for electrical conductivity and quick transferral of energy through them generating an electric current.
Q: What type of bonds do not all metals exhibit?
A: Not all metals exhibit metallic bonding; for example mercury ions (Hg2+2) form covalent metal-metal bonds.
Q: What is an alloy?
A: An alloy is a solution of metals that often has similar properties to pure metals such as being shiny.
Q: How does graphite conduct electricity even though it's not a metal?
A: Graphite conducts electricity even though it's not a metal because like some other non-metals it also has free electrons that allow for electrical conductivity.
Q: Are there any other non-metals that can conduct electricity besides graphite?
A: Yes, some ionic compounds that are molten or dissolved in water also have free moving ions which allow them to conduct electricity too.
