When metals bond they share electrons very loosely, which means the electrons can move about from nucleus to nucleus very freely. This makes it easier for electricity to be conducted. It also means that the bonds are NOT rigid, so metals are more likely to bend than break.
it is shiny
The metallic bond is a delocalised bond with free electrons and also may include some covalent interaction This bonding is the cause of the luster, opacity, electrical conductivity, thermal conductivity, strength, malleability, ductility generally associated with the metals.
most metals are metallic in a way. the periodic table consists of 3 different types of elements metals, non metals and metalloids the most metallic are the metals because they posses the most metal like properties.
metallic character encompasses all the charateristics of metals, such as the melting point, conductivity, electromagnet properties, density etc. electropositivity is a measure of an element's ability to donate electrons, and therefore form positive ions. In general, the gretaer the metallic character of a metal, the more electropositive it is.
low first ionization energy and low electronegativity Someone suggested that this answer contained gibberish... But whoever answered it did so correctly. When you start a question with "Which" you should provide choices. If you are looking for "physical" characteristics of metals they might be that metals are lustrous, malleable, ductile, and conductive. But all of these properties stem from the molecular properties of the atoms such as low first ionization energy and low electronegativity. So... not gibberish.
It possesses metallic properties, and metals are conductors.
electrical conductivity, malleability, & ductility.
electrical conductivity, malleability, & ductility.
Three properties of metals that are caused by metallic bonding are electrical conductivity, malleability, and ductility.
Malleability, Ductile, Luster, Electrical Conductivity, and Thermal Conductivity.
Mallabillity, conductivity of electrons, conductivity of heat, shining 'silvery' glance
The metallic bond is a delocalised bond with free electrons and also may include some covalent interaction This bonding is the cause of the luster, opacity, electrical conductivity, thermal conductivity, strength, malleability, ductility generally associated with the metals.
Properties of metals as high boiling point, high melting point, malleability, ductility, electrical conductivity, thermal conductivity, lustre are explained by the theory of metallic bonds.
Properties of metals as high boiling point, high melting point, malleability, ductility, electrical conductivity, thermal conductivity, lustre are explained by the theory of metallic bonds.
Conduct electricity, and usually also heat, readily. Metallic bonding also contributes to malleability.
The main three properties of the metals are malleability (you can shape it easily), ductility (you can turn it into a wire) and conductivity (it will carry heat and electricity very well).
Metallic Bonds are sufficiently used. But in some cases of oddity Ionic Bonds may be involved.
Metallic ^^