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Explain how does the sea of electrons model of metallic bonding explain the shared characteristics of metals?
Wiki User
∙ 11y ago
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.
Wiki User
∙ 11y ago
Wiki User
∙ 9y agoThe model shows a portion of the crystal structure of solid sodium. The atoms are arranged so that each sodium atom is surrounded by eight other sodium atoms. The atoms are relatively fixed in position, while the electrons are free to move throughout the crystal, forming an electron sea.
Wiki User
∙ 11y agothe positive ions and valance electrons in metals can move more freely allowing metals to conduct heat and electric current, to give off light(luster) and to undergo a change in shape easily.
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Does metallic bonding occur between atoms of copper or chlorine?
Metallic bonding occurs between copper atoms. Only copper is a metal and has the characteristics needed for metallic bonding. Metallic bonding occurs between atoms with low electronegativities (low tendency to attract electrons from other atoms) and low ionisation energies (little energy required to remove electrons from the atoms). The low tendency for the metallic atoms to keep their electrons allow their electrons to be shared between the atoms, which thus become cations. The cations tend to be very closely-packed; they are not repulsed by their similar positive charges, but attracted to the electrons flowing freely between the cations. Metallic bonding therefore occurs between copper atoms, which have low electronegativity and ionisation energy. Chlorine atoms have some of the highest electronegativity and ionisation energy of all elements, and thus do not exhibit metallic bonding.
In a metal lattice what are surrounded by a pool of electrons?
its called metallic bonding
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
Characteristics of metallic bonds?
The valence electrons of all the metal atoms go into delocalized bonds which cover the entire crystal lattice. These electrons are free to move around and give metals their special properties such as good electrical and thermal conduction. This situation is sometimes pictured as a regular array of metal ions floating in a 'sea' of electrons. Some of the characteristics of metallic bonding are that the substance will be very hard, made of some sort of metal, usually a gray or silver color, and most likely it will be somewhat shiny. Electrons move freely among many metal nuclei.
Elements whose atoms can combine to form compounds?
Reactive elements have atoms that can combine to form compounds. The atoms in a compound are combined through different types of bonds, such as ionic, covalent, hydrogen, and metallic bonding. With ionic bonding, there is an exchange of electrons between atoms. Covalent bonding occurs when electrons are shared by two atoms.
Does metallic bonding involve free-floating electrons?
Yes that is how metallic bonding is modeled - a sea of electrons.
What statement best describes metallic bonding?
electrons are free to move among many atoms
How does metallic bonding explain why metals are malleable and ductile?
Delocalized electrons. They are the ones that move around, causing the metal to be ductile and malleable.
Does metallic bonding occur between atoms of copper or chlorine?
Metallic bonding occurs between copper atoms. Only copper is a metal and has the characteristics needed for metallic bonding. Metallic bonding occurs between atoms with low electronegativities (low tendency to attract electrons from other atoms) and low ionisation energies (little energy required to remove electrons from the atoms). The low tendency for the metallic atoms to keep their electrons allow their electrons to be shared between the atoms, which thus become cations. The cations tend to be very closely-packed; they are not repulsed by their similar positive charges, but attracted to the electrons flowing freely between the cations. Metallic bonding therefore occurs between copper atoms, which have low electronegativity and ionisation energy. Chlorine atoms have some of the highest electronegativity and ionisation energy of all elements, and thus do not exhibit metallic bonding.
What atoms share electrons in their outer cell?
Any non-metallic atom can share electrons with another non-metallic atom, through covalent bonding. Metallic bonding is between metals. Covalent bonding is between non-metals. Ionic bonding is typically between a metal and a non-metal.
Can a bond be a covalent and ionic bond?
No. A bond cannot be both covalent and ionic. A bond can be covalent, ionic or metallic. In covalent bonding electrons are shared, electrons are transferred in ionic bonding and electrons move about in a sea of electrons in metallic bonds.
What role do valance electrons playing the formation of compounds and elements?
The valence electrons are the only electrons involved in chemical bonding. In covalent bonding sharing occurs In ionic bonding electrons are tranferrred In metallic bonding they are deloclaised across the lattice
How does metallic bonding explain the result at point c?
Sd
What are the mobile electrons surrounding the positive ions in metallic bonding?
They are just referred to as "delocalized" electrons
What type of bonding in which sea of electrons surrounds positvely charged ions?
I had the same question; the answer is Metallic Bonding.
Which part of metallic bonding theory helps the most to explain why metals are able to conduct electricity?
Electrons can move freely among all the atoms of the metal.
Is metallic bonding an attraction of positive and negative ions?
Metallic bonding is the attraction between positively charged metal ions and free (negatively charged) electrons.
