0
Metals are described as malleable because of the ability of the atoms to roll over each other into new positons.
Wiki User
∙ 12y ago
Add your answer:
Earn +20 pts
What happens to a valence electron in a metallic bond?
Valence electrons in a metallic bond are delocalized and can move freely within the metal atoms. This gives metals their malleability and luster.
What are three reasons why atoms bond?
they give an electron or two to the other atom, share an electron or two with another atom of (if they're both metals) lose all their outer shell electrons and form a load of 'positive ions in a sea of electrons'
How do the electron's in a metallic bond affect the metal?
Because of the common sea of electrons, these electrons can move readily, creating electricity.
What type of bonding has electron moving freely in the electron sea?
Ionic bonds
What does the model sea of electrons help explain?
Mobile electrons are shared by all the atoms in an electron-sea model of a metallic bond. The electrons are delocalized, which means that they do not belong to any one atom but move freely about the metal's network of empty atomic orbitals.
The electron sea model for metlas suggests that?
the valence electrons drift freely around the metal cations.
What represents the way electrons exist in metals?
The electron sea model represents the way electrons exist in metals.
What type of atom involved with metallic bonds?
At the risk of stating the obvious, metals are the kind of atoms that form metallic bonds.
What does the phrase sea of electrons mean?
A sea of electrons can be found in metals. The positive ions are arranged in fixed positions, while the electrons 'float' or 'wander' among the the positive ions. This makes metals good conductors of electricity. ----------------- Electrons of metals flow freely
The electron sea model of the metallic bond helps to explain why metals are what?
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.
Explain how does the sea of electrons model of metallic bonding explain the shared characteristics of metals?
Basically, electricity is a force caused by electrons hitting each other. The electron sea model explains the conductivity of transition metals by showing that they hang onto their many electrons loosely and are practically floating in them. With so many free electrons, it's a lot easier to conduct electricity.
What does the electron sea model of metallic bonds help you to explain?
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.
What type of ion will metals always form?
Positive. Metals 'lose' an electron during metallic bonding, this causes a sea of negative electrons throughout the metal molecules, leaving posotive metal ions
What happens to a valence electron in a metallic bond?
Valence electrons in a metallic bond are delocalized and can move freely within the metal atoms. This gives metals their malleability and luster.
What best describes the arrangement of electrons in a metallic bond?
A sea of electrons. This is a very good description of the bonding in group 1 group 2 metals. A more advanced view for transition metals calls the sea of electrons an "sp electron gas" alongside covalent bonding involving d electrons. This accounts for the melting point trends in transition metals
What is the electron behavior for metallic bond?
electron sea
What are three reasons why atoms bond?
they give an electron or two to the other atom, share an electron or two with another atom of (if they're both metals) lose all their outer shell electrons and form a load of 'positive ions in a sea of electrons'
