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Atomic Structure
The Relative atomic mass of an
element (Ar) compares the mass
of atoms of the elements with the
C12 isotope. It's an average value
for the isotopes of the element
The Relative formula mass of a
compound (Mr) is the sum of the
relative atomic masses of the Atoms that have the same atomic
atoms in the number shown in the number but a different mass
formula. The relative formula number are called an isotope.
mass is 1 mole of that substance.…read more

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Ionic Bonding
Metal and non-metal electron
transfer.
Metals lose electrons and Metals in Group 1 form ions with
become positive ions. a 1+ charge.
Non-metals gain electrons and Metals in Group 2 form ions with
become negative ions. a 2+ charge.
Non metals in Group 6 form ions
Properties of an Ionic with a -2 charge
Compound
Non metals in Group 7 form ions
· Giant lattice structure with with a -1 charge.
strong electrostatic attractions
·High melting points, large
amounts of energy to break
·When melted or dissolved can
conduct electricity because ions
are free to move and carry
current.…read more

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Covalent Bonding - Molecules
Properties of covalent
compounds
·A covalent bond is a shared pair
of electrons.
·Substances that are simple
molecules have low melting and
boiling points.
·They have weak
intermolecular forces
·They don't conduct electricity
because they do not have an
overall electric charge. No free
electrons or ions.…read more

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Covalent Bonding- Giant
Diamond
All the atoms have 4 carbon-carbon
bonds. Very strong with a high
melting point.
Fullerenes
Carbon can form fullerenes with
different numbers of carbon atoms.
They are used for drug delivery into
the body, lubricants, catalysts
and in nanotubes.
Graphite
In graphite, each carbon atom bonds
to three others, forming layers. The
layers are able to slide over each
other because they aren't covalently
bonded. Graphite is soft and
slippery.…read more

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Metallic Bonding
Metals Alloys
·Regular pattern ·Two or more different metals.
Different sized atoms distort the
·The electrons in the outer shell are
delocalised and free to move structure making it harder to slide
through the structure and carry a over each other and generally stronger
charge. ·Conductions is dependent on ability
of electrons to move.
·Strong electrostatic attractions
due to a structure of positive ions.
·Conduct heat and electricity
·Layers of atoms are able to slide over
each other and the structure bends.
Shape Memory Alloys
Alloys that return to their original
shape after being deformed…read more

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