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AP Chemistry
Bonding Summary
Bonding Model
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Ionic
Bonding
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Covalent
Bonding
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Metallic
Bonding
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Properties
Results from the
attraction between
positive and negative
ions.
Electron transfer occurs
between atoms of large
EN difference (metals
and nonmetals)
Leads to crystalline
solids with ions packed
tightly in regular
arrays(no separate
molecules exist)
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Results from the
attraction between two
nuclei and a localized
electron pair.
Electron sharing occus
between atoms with a
small EN difference
(usually two nonmetals)
Leads to separate
molecules with specific
shapes or to extended
networks
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Results from the
attraction between the
cores of metal atoms
(metal cations) and
delocalized valence
electrons.
Arises through the
shared pooling of
valence electrons from
many atoms (Electron
Sea Model).
Leads to crystalline
solids
Metal ions not held in
place as ridigly as in an
ionic solid.
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Explanation of Properties
Hard
Rigid
Brittle
No conductivity in solid
state
Conductivity in melt and in
aqueous solution
High melting and boiling
temperatures
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Most compounds are gases
(methane or ammonia),
liquids (benzene or water),
or low-melting solids (sulfur
or wax).
Low melting and boiling
substances.
Most covalent substances
are poor electrical
conductors in all states.
If network solid (diamond)
exceeding hard
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Properties vary over a wide
range
Most have moderate to high
mp and much higher bp
Most are deformable
(malleable-sheets; ductilewire)
Conduct heat and electricity
in all states
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powerful attractive forces
hold ions in place
throughout the crystal
(resists boiling/melting)
Moving ions out of position
required overcoming the
forces (sample resists being
dented or cracked)
If enough pressure is
applied to overcome the
attractions, ion of like
charges are brought close
together; their repulsions
crack the sample
Weak intermolecular forces
between the molecules
(Vander Waals, dipole, Hbonds) lead to an ease of
separating the molecules
(low mp and bp, softness of
solids)
Electrons are localized, no
conductivity possible
For network covalent,
strong covalent bonds make
for a very strong substance
Properties are explained by
the regularity of metal-ion
array and the mobility of the
valence electron.
Melting – electrostatic
attractions not broken
(moderate mp)
Boiling – electrostatic
attraction must be broken
(very high bp)
More valance electrons,
higher mp/bp, better
conductors(mobile e-)
Malleablilty/ductilityElectron sea keeps bonding
structure intact. No
repulsions.