96516
C2
- atoms
- Nucleus
- neutron
- no charge
- same mass
as proton
- no charge
- proton
- number of protons
equals the number
of electrons
- positively
charged
- number of protons
equals the number
of electrons
- positively charged
because of the protons
in the nucleus
- neutron
- electron (around
the nucleus)
- negatively charged
- has no mass
- occupy shells around
the nucleus
- negatively charged
- electron and proton
charge cancel each
other out
- becomes an ion when electrons are
lost or gained making the ion charged
(number of protons no longer equals
the number of electrons)
- mass number= number of
protons+number of neutrons
- atomic number= number of protons
- Isotopes are different atomic
forms of the same element which
have the same number of protons
but a different number of neutrons
- Nucleus
- Bonding
- ionic
- atoms gain or
lose electrons
- form charged ions
- group one and two atoms do ionic
bonding most because they only
have one or two electrons in their
outer shell so are keen to lose
them (form +ve ions - cations)
- group six and seven atoms are
equally as keen to bond ionically as
group one and two as they only
need one or two electrons (gain
elecctrons, form -ve ions - anions
- the ions from then react with each other as
they will be oppositely charged and
oppositely charged ions attract - the cations
and the anions react to form ionic bonds
- ionic bonds produce
giant ionic structures
- closely packed regular lattice
- very strong chemical
bonds between all the ions
- high melting and boiling points
- high melting and boiling points
- When they are dissolved (or melted),
the ions separate, the electrons are then
free to move so can carry a current
- closely packed regular lattice
- only elements at opposite sides of
the periodic table can form ionic
bonds - group 1+7, group 2+6
- atoms gain or
lose electrons
- covalent
- atoms share electrons
with other atoms
- some covalent bonds form
giant covalent structures
- similar to giant ionic
but no charged ions
- all atoms are bonded
together with strong
covalent bonds
- very high melting
and boiling points
- they don't conduct electricity (even
when molten), and usually are
insoluble in water
- two examples are diamond
and graphite, both made
only from carbon atoms
- similar to giant ionic
but no charged ions
- some covalent bonds form
simple covalent structures
- atoms form very strong covalent
bonds forming small molecules
of two or more atoms
- inter-molecular forces (forces
of attraction) are very weak
- very low melting and boiling
points - atoms are easily parted
(weak inter-molecular forces)
- usually liquid or gas at room
temperature - most simple covalent
structures have a 'mushy' appearance
- liquid gas or an easily melted solid
- atoms form very strong covalent
bonds forming small molecules
of two or more atoms
- atoms share electrons
with other atoms
- ionic
- metallic structures
- metal properties are all due
to the sea of free electrons
- the free electrons come
from the outer shell of every
metal atom in the structure
- the electrons are free to move
so metals are good conductors
of heat and electricity
- the electrons hold the atoms
together in a regular structure
- the electrons allow the atoms to slide over
each other causing the metal to be malleable
- metal properties are all due
to the sea of free electrons
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