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Metallic Bonds & Properties of Metals (7.4)
Metallic Bonds - Electron Sea Model; Delocalized Electrons Properties of Metals Metal Alloys - Properties & Types
Terms in this set (20)
the attraction of a metallic cation for "delocalized" electrons in a metallic solid
How is metallic bonding similar to ionic bonding?
1.there is an attraction between particles of unlike charges.
2. a lattice structure is formed in the solid state: from 8 to 12 atoms/ions surround each atom/ion.
How is metallic bonding different from ionic bonding?
1. In an ionic bond the valence electrons are transferred from the metal only to the neighboring nonmetal, but in metallic bonding the valence electrons of each atom/ion are free to move or float around within the entire metal solid.
2. in an ionic bond there are positive and negative ions being formed, but in metallic bonding there are only positive ions being formed
Electron Sea Model
all of the metal atoms in a metallic solid contribute electrons into a vast "seaof electrons". These electrons are free to move around within the entire metallic solid. This "sea of electrons" surrounds each of the metal atoms in the solid.
Because the electrons of each metal atom do not remain around the atom from which they came - they are free to move or roam about within the metallic solid - they are called "delocalized" electrons.
attraction between the positively charged metal ions and the "sea of delocalized electrons"
Properties of Metals
explained by metallic bonding (the attraction between the positive metal ions and the "sea of delocalized electrons".
Metals have high...
melting & boiling points
Delocalized electrons allow metal ions to easily shift when struck by an outside force, this is why metals are...
malleable, ductile and durable
Delocalized electrons are able to transfer heat and electrical current quickly and easily throughout a metallic solid, that is why metals ar good''...
conductors of heat and electricity
Metals that have three or more valence electrons provide a larger "sea of delocalized electrons" which makes those metals...
strong and hard.
early in the history of human civilizations there was a recognition that by mixing and melting different metals together, the mixture of those metals (alloy) had different properties than the individual metals.
Copper + Zinc =
(plumbing, musical instruments, hardware)
Copper + Zinc + Tin =
(statues, ancient tools and weapons)
Iron + Chromium + Nickel =
(instruments for varoius industries)
Uses of Aluminium Alloys
Used in the production of automotive engine parts; applications like transport, packaging, electrical application, medicine, and construction of homes and furniture; strong aluminium alloys allow jets to fly at high altitudes with huge pressures and stresses
Uses of Titanium Alloys
Due to high strength, toughness and stiffness, titanium alloys are used for different spacecraft parts, jet engines and airframe to save weight and improve aircraft efficiency. Corrosion resistance allow its uses in chemical, petrochemical and biomaterial applications.
Uses of Nickel Alloys
Nickel alloys have good corrosion resistance and heat resistance and are used for a wide variety of applications like aircraft gas turbines, nuclear power systems and chemical and petrochemical industries.
Uses of Copper Alloys
Copper alloys have excellent electrical and thermal performance, good corrosion resistance, high ductility and relatively low cost. Copper alloys are less expensive than gold or platinum. Due to high strength, electrical and thermal conductivity copper alloys are used in the manufacture of all types of electrical equipment.
Common alloys in your everyday life...
sterling silver, gold jewelry, silver amalgam (used by dentists to fill cavities), solder (used in welding), brass musical instruments, titanium alloy sporting equipment (golf clubs, bicycles, baseball bats, and tennis rackets)
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