C3 Flashcards
what are the states of matter
solid, liquid, gas and plasma
what is the structure of solids
molecules are packed together tightly
what is the structure of liquids
they are packed close together but can slip and slide over each other
what is the structure of gases
have lots of space between them
what is it called when a solid turns into a gas
sublimation
what is it called when a gas turns into a solid
deposition
where does ionic bonding take place
between non-metals and metals
what happen when sodium (has 1 electron in it’s outer shell) gives 1 electron to chlorine (has 7 electrons in it’s outer shell)
sodium loses 1 electron and Chlorine gains 1 electron so they both have a full outer shell. sodium becomes a +1 ion and Chlorine becomes a -1 ion. since they are positive and a negative ions they will attract each other forming a strong covalent bond
why do molecules ionically bonded together have high melting and boiling points
ionic bonds are really strong so they require a lot of energy to overcome
when can ionic compounds conduct electricity
when melted or are dissolved in water due to that causing the particle to move around freely
the formula for a hydroxide ion
OH -
the formula for a sulfate ion
SO4 2-
the formula for a nitrate ion
NO3 -
the formula for a carbonate ion
CO3 2-
the formula for a ammonium ion
NH4 +
the formula for a calcium hydroxide ion
CaOH
where does metalic bonding take place
in metals
what happens in a metal which causes electrons to be delocalised
the metal atoms give up their outer most electrons turning into ions and are therefore ‘sharing’ the electron which are now delocalised.
why can metals conduct electricity
due to the delocalised electrons
why does it require a lot of energy to break a metallic bond
the delocalised electrons acts like a glue, sticking the metal together due to the strong electrostatic forces which bond the metal ions together.
will ionic compounds conduct electricity
yh, it will
what happens in a covalent bond
electrons are shared
what are intermolecular forces
forces which hold covalently bonded compounds close to each other
how strong are intermolecular forces
easy to break
how strong are covalent bonds
they are very strong so they need a lot of energy to break
where does covalent bonding happen
in non-metals
what are simple molecules
a covalently bonded molecule with a low boiling and melting point which doesn’t have a continuous repetitive chain of molecules.
what are some examples of simple molecules
water and methane
why do simple molecules have low melting and boiling points
they have very weak intermolecular forces
do simple molecules conduct electricity and why
no they don’t as they have no overall charge
why do giant covalent structures have high melting and boiling points
because you need to break the covalent bonds themselves and not the intermolecular themselves.
how can you tell if something is a giant covalent structure
they have regular repeating lattices
do giant covalent structures conduct electricity
no they don’t
name me the properties of the allotrope diamond
each carbon atom is covalently bonded to 4 others
the bond in each molecule is very strong
don’t conduct electricity as they don’t have spare electrons
are hard substances
name me the properties of graphene
a single layer of graphite
do conduct electricity due to the free electron
one atom thick
low density
excellent conductor of heat and electricity]
name me the properties of quartz
strong covalent bonds = high melting and boiling point
are hard substances
don’t conduct electricity due to 1 molecule being bonded with 4 others
name the properties of graphite
each carbon atom is bonded to 4 others
strong covalent bonds
there are free electrons so they can conduct electricity
weak forces of attraction between each layer of graphite (graphene) so they can slide over each other
name the properties of fullerenes
molecules of carbon atoms with hollow shapes
based on hexagonal rings of carbon
rings may contain 4 or 5 carbon atoms
can be used for drug delivery
name me the properties of nanotubes
high tensile strength
high electric conductivity
high thermal conductivity
used for reinforcing materials
what is an alloy
a metal with 2 or more types of elements used to make the metal stronger
what are the properties of a pure metal
can be bent and shaped because the layer of atoms can slide over each other
delocalised electrons can allow electricity and thermal energy to pass through
why is an allow stronger than a pure metal
an alloy has different shaped atoms which means there won’t be straight rows of metal; it’ll be misshaped so layers will find it difficult to slide over each other
what are the size of nanoparticles
1nm- 100nm
what the surface area : volume ratio of nanoparticles
high
what are some uses of nanoparticles
catalysts
medicine
electrical circuits
and you are f-
-inally done
