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AQA GCSE Chemistry
Structure and bonding
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Cards (72)
Structure of graphite
1. Each
carbon
atom forms
covalent
bonds to
three
other
carbon
atoms
2. Carbon atoms form
hexagonal
rings arranged into
layers
with
no covalent
bonds between the layers
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Properties of graphite
Soft
and
slippery
High melting
and
boiling
point
Good conductor
of both
electricity
and
heat
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Graphite is soft and slippery because
The
layers
can
slide
over each other due to no
covalent bonds
between them
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Graphite has a
high
melting and boiling point because
Breaking the
covalent bonds
in graphite requires a
great
deal of
energy
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Graphite is a good conductor of electricity and heat because
Carbon
atoms in graphite have
delocalized electrons
that can move, allowing for
conductivity
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Diamond
is a giant
covalent
molecule formed from
carbon
with each
carbon
atom forming
covalent
bonds to
four
other carbon atoms
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Diamond has a
high
melting and boiling point due to a large number of
strong covalent bonds
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Diamond cannot conduct electricity because all
outer electrons
are in
covalent bonds
with
no free electrons
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Graphite
is also a giant
covalent
molecule formed from
carbon
with each
carbon
atom forming
covalent
bonds to
three
other carbon atoms
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Graphite
is used as a
lubricant
in machines to reduce
friction
between moving parts
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Graphite contains
delocalized electrons
that allow it to conduct both
electricity
and
heat
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Structure of giant covalent molecules
Describe the
structure
of
diamond
and
silicon dioxide
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Properties of giant covalent molecules
Describe
the
properties
of
diamond
and
silicon dioxide
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Linking properties to structures
Link
the
properties
to the
structures
of the
molecules
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Small covalent molecules
have a small number of
covalent bonds
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Small
covalent substances
have weak
intermolecular forces
between the molecules
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When
melting
or
boiling
a small
covalent substance
, weak
intermolecular forces
need to be broken
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Breaking weak
intermolecular
forces in small
covalent
substances does not take a lot of
energy
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Small covalent substances have
low
melting and boiling points
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Most small covalent substances are
gases
at
room temperature
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Giant covalent substances
contain
millions
of
covalent bonds
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Giant covalent substances
Diamond
Silicon dioxide
or
silica
Graphite
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Giant covalent substances
are always
solids
at
room temperature
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All giant
covalent
substances have
high
melting and boiling points
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Melting
or
boiling
giant
covalent substances
requires breaking all covalent bonds, which takes a great deal of
energy
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Diamond
is formed from the
element carbon
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Carbon atom
Has
four
electrons in its
outer
energy level
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Diamond structure
Each
carbon
atom forms
covalent
bonds to
four
other
carbon
atoms
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Diamond
contains a huge number of
carbon
atoms joined by
covalent
bonds
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Diamond
is an
extremely hard substance
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Melting point of diamond is over
3,700
degrees Celsius
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Diamond
cannot
conduct electricity
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In diamond, all
outer electrons
are in
covalent bonds
, so there are
no free electrons
to carry
electrical charge
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Silicon dioxide or silica contains the elements
silicon
and
oxygen
covalently
bonded
together
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Silicon dioxide
has a very
high melting
and
boiling point
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Silicon dioxide
has a
huge
number of
strong covalent bonds
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In order to melt
silicon dioxide
, the
covalent bonds
must be
broken
, requiring a
great deal
of
energy
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What ratio do nanoparticles have?
Large surface area
to
volume
ratio
What size are nanoparticles?
Between
1nm- 100nm
Surface area to volume ratio?
surface area / volume
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