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What does the electron sea model of metallic bonds help you to explain?
Wiki User
∙ 6y ago
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.
Wiki User
∙ 6y ago
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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.
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.
A group of atoms united by ionic bonds?
In order to form an ionic bond, you need a metal and a non-metal. That would be one element to the right of the stairstep on the periodic table, and one from the left side. If they are both metals, it forms a metallic bond, and if they are both non-metals, it forms a covalent bond. Ionic bonds 'give and take' electrons compared to the 'sharing' of electrons in covalent bonds or the 'electron sea model' of metallic bonds. Ionic bonds are stronger than covalent bonds. They are also more brittle (less maleable) and don't have an odor. (Think gasoline compared to salt - 'NaCl')
What represents the way electrons exist in metals?
The electron sea model represents the way electrons exist in metals.
How are metallic bonds and ionic bonds similar and different?
The difference between ionic an metallic bonds is that the in ionic compounds the electrons are transferred and are "localised" to the anions and the cations. Ionic compounds contain a lattice of positive and negative ions which is held together by electrostatic attraction. Metallic bonds are sometimes described as ions in a sea of electrons. The presence of "ions" is sometimes taken as a similarity between ionic solids and metals. (Please remember this is a VERY simple model, and the reality is more complicated) The electrons in the "sea" are highly mobile, delocalised, and able to carry electricity.
What does the model of a sea of electrons help explain?
It helps explain metallic bonds.
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.
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.
A group of atoms united by ionic bonds?
In order to form an ionic bond, you need a metal and a non-metal. That would be one element to the right of the stairstep on the periodic table, and one from the left side. If they are both metals, it forms a metallic bond, and if they are both non-metals, it forms a covalent bond. Ionic bonds 'give and take' electrons compared to the 'sharing' of electrons in covalent bonds or the 'electron sea model' of metallic bonds. Ionic bonds are stronger than covalent bonds. They are also more brittle (less maleable) and don't have an odor. (Think gasoline compared to salt - 'NaCl')
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.
What represents the way electrons exist in metals?
The electron sea model represents the way electrons exist in metals.
The wave-mechanical model of the atom is required to explain the?
spectra of elements with multi-electron atoms
In which direction the electron revolve around the nucleus of hydrogen atom?
the way you look that direction is correct..it is only one model to explain..
What are similarities between ionic covalent and metallic bonds?
They are certainly not covalent in the sense of having localised 2 electron pair bonds. They have features in common with both ionic and delocalised covalent bonds.One very simple model describes metals as positive ions in a sea of electrons and while this rationalises the electrical conductivity of metals it does not explain why the metals generally have high melting points.The force that holds the lattice together is not a simple electrostatic force as in an ideal ionic lattice. In most metals some of the bonding derives from some covalent bonding between metal atoms allied with delocalised bonds occupied by free electrons. These delocalised bonds can be thought of as having superficial resemblance to the delocalised bonds in graphite.Read more: How_are_metallic_bonds_and_ionic_bonds_similar
What is a detailed explanation of the electron cloud model?
Scientist use the electron cloud model to represent an atom.In the electron cloud model, an atom has two distinct regions-the nucleus and the electron cloud.
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
How are metallic bonds and ionic bonds similar and different?
The difference between ionic an metallic bonds is that the in ionic compounds the electrons are transferred and are "localised" to the anions and the cations. Ionic compounds contain a lattice of positive and negative ions which is held together by electrostatic attraction. Metallic bonds are sometimes described as ions in a sea of electrons. The presence of "ions" is sometimes taken as a similarity between ionic solids and metals. (Please remember this is a VERY simple model, and the reality is more complicated) The electrons in the "sea" are highly mobile, delocalised, and able to carry electricity.
