This mindmap is about metallic Bonding. It covers the following key topics:
- Metallic structure
- Physical properties of metals
- Alloys
The magnetic attraction between these free-moving (delocalized) electrons and the positive metal ions is known as the metallic bond. Metals often have high melting and boiling temperatures and can keep a consistent structure due to the strength of their metallic connections. Metals are efficient heat and electrical conductors.
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Structure and Bonding -
Metallic Bonding
metallic structure
subtances with metallic structure:
pure metals
aluminium
copper
potassium
sodium
Alloys -
mixtures of metals
steel
brass
structure of a metal
positive metals ions surrounded by a
'sea of mobile delocalised electrons'
delocalised valnece electrons move freely
like a cloud of negative charge
metallic bonding - strong electrostatic attraction
between positive metal ions and the 'sea of delocalised electrons
attraction between the delocalised electrons
and the metal cations is responsible for the
strength of the metal lattice
arrangement
close together in a regular manner
known as metal lattice
Physical metal properties
metals have high density
majority of metals have higher densities than non-metals
group 1 metals, also known as
light metals happen to be exceptions
to this generelization
this is because of the tightly packed crystal
lattice of the metallic structure
strength of metallic bonds for different metals
reaches a maximum around the centre of the
transition metal series as those elements have
large amiunts od delocalised electrons in the metallic bonds
metals have high melting and boiling points
metal atoms are held together by strong metallic bonds
a lot of energy is required to overcome
these bonds
explains the high melting
and boiling points
metals are good electrical conductors
when a potential difference is applied across the
ends of a metallic conductor,
delocalised electrons will be attracted and hence
move towards the positive end
movement of charge known as electric current
metals are good conductors of electricity because they
have delocalised mobile electrons that move towards the
positive terminal when connected to a circuit
metals are good heat conductors
metal atoms are closely packed
heat can be transferred from one atom to the next by
vibration as they are close together
the free electrons also suddenly
acquire more energy
they move faster and collide with the other
electrons, transferring part of the energy
thus heat is easily conducted from one
end to the other end of the metal
Metals are malleable and ductile
malleable (can be rolled into sheets)
when a metal is bent
layers of cations in the metal lattice slide
over one another easily and fit into new positions
the shape of the metal has changed
but it does not break apart
ductile (can be pulled into wires)
when force is applied to
1 layer of cations
this layer easily slides over the other layers
makes the metal longer and flatter without
breaking apart
this is possible because metallic
bonding reamin largely undisrupted
metal cations are shielded from each
other's repulsions by the 'sea of
delocalised electrons' in between them
shielding is present no matter how
much the lattice is distorted
bending and shearing forces can deform
metal lattices without shattering them
Alloys
a homogenous mixture of a metal and
another element
stronger and harder than pure metals
a metal can be made stronger and harder by the adding
other elements into its structure
The presence of atoms of a different size disrupts the
regular arrangement of the metal atoms
prevents the
metal atoms from sliding over one another easily
Structure and Bonding - Metallic Bonding Mind Map
181
Structure and Bonding -
Metallic Bonding
metallic structure
subtances with metallic structure:
pure metals
aluminium
copper
potassium
sodium
Alloys -
mixtures of metals
steel
brass
structure of a metal
positive metals ions surrounded by a
'sea of mobile delocalised electrons'
delocalised valnece electrons move freely
like a cloud of negative charge
metallic bonding - strong electrostatic attraction
between positive metal ions and the 'sea of delocalised electrons
attraction between the delocalised electrons
and the metal cations is responsible for the
strength of the metal lattice
arrangement
close together in a regular manner
known as metal lattice
Physical metal properties
metals have high density
majority of metals have higher densities than non-metals
group 1 metals, also known as
light metals happen to be exceptions
to this generelization
this is because of the tightly packed crystal
lattice of the metallic structure
strength of metallic bonds for different metals
reaches a maximum around the centre of the
transition metal series as those elements have
large amiunts od delocalised electrons in the metallic bonds
metals have high melting and boiling points
metal atoms are held together by strong metallic bonds
a lot of energy is required to overcome
these bonds
explains the high melting
and boiling points
metals are good electrical conductors
when a potential difference is applied across the
ends of a metallic conductor,
delocalised electrons will be attracted and hence
move towards the positive end
movement of charge known as electric current
metals are good conductors of electricity because they
have delocalised mobile electrons that move towards the
positive terminal when connected to a circuit
metals are good heat conductors
metal atoms are closely packed
heat can be transferred from one atom to the next by
vibration as they are close together
the free electrons also suddenly
acquire more energy
they move faster and collide with the other
electrons, transferring part of the energy
thus heat is easily conducted from one
end to the other end of the metal
Metals are malleable and ductile
malleable (can be rolled into sheets)
when a metal is bent
layers of cations in the metal lattice slide
over one another easily and fit into new positions
the shape of the metal has changed
but it does not break apart
ductile (can be pulled into wires)
when force is applied to
1 layer of cations
this layer easily slides over the other layers
makes the metal longer and flatter without
breaking apart
this is possible because metallic
bonding reamin largely undisrupted
metal cations are shielded from each
other's repulsions by the 'sea of
delocalised electrons' in between them
shielding is present no matter how
much the lattice is distorted
bending and shearing forces can deform
metal lattices without shattering them
Alloys
a homogenous mixture of a metal and
another element
stronger and harder than pure metals
a metal can be made stronger and harder by the adding
other elements into its structure
The presence of atoms of a different size disrupts the
regular arrangement of the metal atoms
prevents the
metal atoms from sliding over one another easily
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Structure and Bonding -
Metallic Bonding
metallic structure
thus heat is easily conducted from one
end to the other end of the metal
