metallic bond ib. formation of metallic bond the metal atoms "lose" one or more of their...
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Metallic BondIB
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Formation of metallic bond
• the metal atoms "lose" one or more of
their outer electrons
• These electrons become delocalized, and
free to move throughout the entire metal.
• These negative delocalized
electrons hold the metal cations together
strongly.
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Metallic bonding in sodium
• Each positive centre in the diagram represents all the rest of the atom apart from the outer electron,
• but that electron hasn't been lost - it may no longer have an attachment to a particular atom, but it's still there in the structure.
• Sodium metal is therefore written as Na - not Na+ or potassium metal is written as K but not K+.
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Metallic bond definition
• It is the attraction force between
positive metal ions and the
delocalized electrons.
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Metallic bond properties• Unlike ionic bonding, distorting the atoms does not cause
repulsion so metallic substances are:
• ductile (can be stretched into wires)
• malleable (can be formed into shapes).
• Heat and electricity conductivity.
• The free moving electrons also allow for high thermal conductivity, and the electrons can carry the heat energy rather than it being transferred slowly through atoms vibrating.
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Electrical conductivity of metals
•Electric current is the flow of electrons in a wire.
•In metals, the outer electrons of the atoms belong to a
‘cloud’ of delocalised electrons.
• They are no longer firmly held by a specific atom, but
instead they can move freely through the lattice of
positive metal ions. Normally they move randomly.
•when the wire is connected to a cell, they are pushed
away from the negative terminal and drawn to the
positive one. The cloud of electrons drifts through the
wire