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Structure & Bonding
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Ionic bonding -
metals
+
non
metals
Electrostatic
attraction between
oppositely
charged
ions
What are cations?
Positively
charged ions
What are anions?
Negatively
charged ions
Covalent bonding -
non
metal
+
non
metal
Electrostatic
attraction between a shared
pair
of
electrons
+ two
nuclei
Metallic bonding - two
metals
Ionic compound structure
Giant
ionic
lattice
Mp + Bp of giant ionic lattices
High
Electric conductivity of giant ionic lattices
Only when
molten
or
aqueous
as ions are able to move around and carry a
charge.
Ions are
fixed
in place during solid form.
Solubility of giant ionic lattices
Often
soluble
Higher
charge
= higher mp and bp in giant ionic lattices
Most covalent bonds are
simple
molecular
structures
Are covalent bones strong or weak?
Strong
Are intermolecular forces in covalent bonds strong or weak?
Weak
Where are intermolecular forces found? (covalent bonding)
Between
adjacent
molecules
Melting and boiling points of simple covalent substances
Low
- intermolecular forces are
weak
and
little
energy is needed to overcome them
Electricity conductivity of simple molecular substances
Insulator
- can't
conduct
- no
ions
or
delocalised
electrons
Solubility of simple covalent substances
Insoluble
-molecules are
neutral
so water molecules aren't attracted to them
Giant covalent exceptions:
Diamond
Graphite
Silicon
dioxide
Structure of metallic bonding
Giant metallic lattices
Metallic bonding
Electrostatic
attraction
between the
metal
cations
and the
delocalised
electrons
Metallic bonding:
A)
delocalised electrons
B)
metal ions
2
Covalent
bonding:
Ionic
bonding:
Density of metallic bonds
High
- particles are closely packed together in a
regular
arrangement
Mp + Bp of metals
High
- a
lot
of energy is required to break the
strong
electrostatic
attractions between the
cations
and
delocalised
electrons.
What is an alloy?
A mixture of
two
or
more
elements
, at least
one
of which is a
metal.
Metal conductivity
Good
conductor
- lots of
delocalised
electrons
to move around and carry a charge
Why are metals malleable?
Layers of
cations
can
slide
over each other
What happens to substances when they are heated?
They
expand
(gases can also increase
pressure
)
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