Aqa chemistry-bonding-structure-and-the-properties-of-matter-know it-gcse info

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PiXLKnowIT!
GCSE Chemistry
AQATopic– Bonding,structureand
the properties of matter

Overview
Bonding,Structureandthe properties of matterBonding
• Chemical bonds
• Ionic bonding
• Ionic compounds
• Covalent bonding
• Metallic bonding
Propertiesof substances
• Statesof matter
• State symbols
• Properties of ioniccompounds
• Properties of smallmolecules
• Polymers
• Giant covalent structures
• Properties of metals andalloys
Structureandbondingof carbon
• Diamond, graphite
• Graphene and fullerenes
Nanoparticles(ChemistryONLY)
• Sizeof particles
• Usesof nanoparticles

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Bondingpart 1
• Chemicalbonds
• Ionic bonding
• Ionic compounds

Chemical bonds
There are three types of strong chemicalbonds:
• Ionic
• Covalent
• Metallic
Ionic Covalent Metallic
Particles are
oppositely charged
ions
Particles are atoms
which share pairsof
electrons
Particles are atoms
which share
delocalised electrons
Between metalsand
non-metals
Most non-metallic
elements
Between non-metals
and non-metals
In metallic elements
and alloys
Youneed to be able toexplain chemical bonding in terms of electrostaticforces
and the transferofelectrons.

Ionic bonding
Ionic bonds form between metalsandnon-metals.Ionic bonding involvesthe
transfer of electrons in theouter shells.
Metals loseelectrons to become positivelychargedions
and non-metals gainelectrons to become negatively
charged ions.
Theelements in Group1
react with the elements
in Group7.
Groups1 elements can
eachlose oneelectron.
Thiselectron canbegiven
to an atom from Group7,
they both achieve the
stable electronic
structure of anoblegas.

Ionic bonding
Theelectrostatic attraction between the oppositely charged Na+ions and Cl-ions
is called ionicbonding.Theelectron transfer during the formation of an ionic
compound canbe represented by adot andcrossdiagram:
Thechargeon the ions produced by metals in group 1 and 2 and by non-metalsin
group 6 and 7 relates to the groupnumberof the element in the periodic table.
For example group1 form 1+ions,group3 form 3+ions,group6 form 2- ionsand
group7 form 1- ions.
When
completing
diagrams
alwaysinclude:
• Thecorrect
numberof
electronson
outershells
• Thecharge

Ionic bonding
Magnesiumoxide:
Sometimesthe atoms reacting need
to gain or lose two electronstogain a
stable noble gasstructure. Each
magnesium losestwo electrons and
eachoxygen gainstwo electrons.
Magnesium ions havethe formula
Mg2+, while oxide ions havethe
formula O2-.
Thismeansthat one magnesium
atom reacts with one oxygenatom,
giving the formulaMgO
CalciumChloride:
Eachcalcium atom (2, 8, 8, 2) needsto
lose two electrons but each chlorine
atom (2, 8, 7) needsto gain only one
electron.
Thismeansthat two chlorineatoms
react with every one calciumatom,
giving the formulaCaCl2

An ionic compound is agiantstructureof
ions.
Ionic compounds are held together by
strongelectrostaticforcesof attraction
between oppositelychargesions.These
forces act in all directions in the lattice –
this is called ionicbonding.
Empiricalformula
Themodels canindicate the chemical
formula of acompound by the simplest
ratio of atoms or ions in models of their
giant structure – this is called theempirical
formula.
e.g. there is a1:1 ratio of sodium to
chlorine in sodium chloride, sotheformula
is NaCl.
Thestructure of sodium chloride
canbe represented in the following
forms:
- Themodelsnever accurately
reflect the manymillionsof
atoms/ions bondedtogetherin
the giantlattices
Ioniccompounds

QuestionIT!
Bondingpart 1
• Chemicalbonds
• Ionic bonding
• Ioniccompounds

Bonding PART 1 – QuestionIT
1. What are the three types of strong chemical bond?
2. What particles are foundin:
a) Ionic bonding
b) Covalent bonding
c) Metallic bonding?
3. Which type of bonds occurs when metals combine with non-
metals?
4. What type ofbonding occurs in carbon dioxide? Why?
5. What type of bonding occurs inalloys?

6. What happens to the electrons in ionic bonding?
7. What electronic structure do theions produced by metals in
Groups 1 and 2 and the non-metals in Groups6 and 7have?
8. What is the link between the charge number on the ions in Groups
1, 2, 6 and 7 and their group?
9. What is an ionic compound?
10. How are ionic compounds heldtogether?

11. Why is the ball and stick model notan accurate representation of
the structure of an ioniccompound?
12. Draw adiagram to show how potassium and chlorineatoms
join together to formions.
13. Explain how you can use the following model to work out the
empirical formula of sodiumchloride.

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Bondin
g PART
2
• Covalent bonding
• Metallic bonding

N
H
H H
NH3
Covalent bonding - PART 1
When atoms sharepairsof electrons,they form covalentbonds.
Theseare STRONGbonds.
Covalently bonded substancesmaybe: Smallmolecules,verylargemolecules or
giantcovalentstructures.
Youcandeducethe molecular
formula of a substancefrom a
givenmodelor diagram
showingthe atomsandbonds
in the moleculebycountingthe
numberof atoms.
H2O
H H
O
Polymersare examplesof very large covalent molecules, they canbe represented
in the form: where ‘n’ =averylarge number!
Examplesof covalently bonded substanceswith giantcovalentstructuresare
diamondand silicondioxide.

Covalently bonded substancesmayconsist of small molecules. Thecovalent bondin
molecules canbe represented in the following models. Likeall models, eachone is
useful but hassomelimitations.
AmmoniaNH3
Dot and crosswith outershells
ascircles:
2Dwith bonds:
- It showsthe H-N-Hbond
incorrectlyat 90°
+Showwhichatoms
are bondedtogether
3Dball and stick model:
+Attempts to showthe correct
H-N-H bondangleis 107.8°
+Showsthe impact of the lone
pair
+Showwhichatom the
electronsin the bondscome
from
- All electronsareidentical
Dot and crosswith
outer shellselectrons:

Theelectrons in the outer shellof metal atoms are delocalisedand are freeto
movethroughout the structure.
Thesharing of delocalised electrons leads to strongmetallicbonds.
Metallic bonding canbe represented in thefollowing form:
Theatoms in metals are built up layer uponlayer in aregular
pattern. Theyare another example of agiantstructure.
Metallic bonding

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Properties of
substancesPart 1
• Statesof matter
• State symbols

States of matter and state symbols
There are three states of matter – solid,liquid and gas.Toexplain the properties
of the states, the particle theoryis used. It is basedon the fact that all matter is
made up of tiny particles and describes the movementand distancebetween
particles.
In chemical equations, the three states are shown as(s), (l),(g)
and (aq) for aqueoussolutions.
Solid Liquid Gas
Closetogether, regular
pattern, vibrate onthe
spot.
Closetogether, random
arrangement, move
around eachother.
Farapart, random
arrangement,move
quickly.

Changes of state
Melting and freezingtake place at the melting point.
Boilingand condensingtake place at the boilingpoint.
The amount of energyrequired to change the state
depends on the strength of the forces between the
particles of thesubstance.
Thestrongerthe forcesbetween the particles the
higherthe melting andboiling point of thesubstance.
Thetype of bonding and the structure of the substance
depend on the particlesinvolved.
MeltingFreezing
Condensing Boiling
HTONLY- There are limitations of the particle model of matter:
• There are no forces
• All particles are shown asspheres
• Thespheres are solid

Changes of state
Thegraph showsaheatingcurveof a
solid, which showsthe temperature ofa
substance plotted against the amountof
energy it hasabsorbed:
Asubstancemust absorb
heat energy sothat it can
melt or boil. The
temperature of the
substance doesnot change
during melting,boilingor
freezing,even though energy
is still beingtransferred.

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Properties of
substancesPart 2
• Ioniccompounds
• Smallmolecules
• Polymers
• Giantcovalent structures
• Metals andalloys

Structure
Ionic compounds haveregularstructures
called giantioniclattices.
There is strongelectrostaticforcesof
attraction in all directions between
oppositelychangedions.
Properties
• Highmelting andboilingpoints– large
amounts of energy is needed to break
the many strongbondsand overcome
the electrostatic attraction.
• Conduct electricity when molten or
dissolved in water – ions are free to
moveand cancarry charge.
Propertiesof ioniccompounds

Structure
Theyhaveweakforcesbetween the
molecules.Theseweak forces are
overcome when they changestate notthe
strong covalent bonds.
Properties
• Lowmelting andboilingpoints– small
amounts of energy is needed to break
the intermolecular forces.Most are
gasesor liquids.
• Donot conductelectricity– Particles do
not havean overall electriccharge.
Propertiesof small molecules
Intermolecular forces
increase with the sizeofthe
molecules. Solarger
molecules havehigher
melting and boilingpoints.

Polymers
Somecovalently bonded substances
havevery largemolecules, suchas
polymers.
Structure
Polymers are made up from many
small reactive molecules that bond to
eachother to form longchains.The
atoms in the polymer molecules are
linked to other atoms by strong
covalentbonds.Theintermolecular
forcesbetween polymer moleculesare
relatively strong.
Properties
• Solidat room temperature –Strong
intermolecular forces.

Structure
All atoms within the structureare linked by
strongcovalentbonds.Thesebonds must
bebrokenfor asolid to melt orboil.
Properties
• Veryhighmelting andboiling points–
very large amounts of energy isneeded
to break the covalentbonds.
• Donot conductelectricity – Particles do
not havean overall electriccharge.
Giantcovalent structures

Thegiant structure of atoms with
strong metallic bonding givesmost
metals ahighmelting and boiling
point.
Metals are malleable(canbe
hammered into shape) and ductile
(can be drawn out into awire)because
the layersof atoms (or ions) in agiant
metallic structure canslideover each
other
Delocalisedelectrons in metals enable
electricityand heat to passthrough
the metaleasily.
Properties of metals and alloys
Ametal mixedwith other elementsis
called an alloy.Alloys are harder than
pure metals.Alloys are made fromtwo
or moredifferent metals.
Puremetal Alloy
Thedifferent sizedatoms of the metals
distort the layersin the structure,
making it more difficult for them to slide
over eachother, and somakethe alloys
harder than puremetals.
For example, goldis naturally softbut
adding copperto makejewellery
strongerand last longer.

Diamond
Diamond:
In diamond, each carbon atom formsfour
covalentbondswith other carbon atoms
in agiantcovalentstructure.
• Diamond is very hard– it is the
hardest natural substance, soit is
often usedto makejewelleryand
cutting tools.
• Diamond hasaveryhighmelting and
boilingpoint – alot of energy is
needed to break the covalentbonds.
• Diamond cannotconductelectricity –
there are no free electrons or ions to
carry acharge.

Graphite
Graphite:
In graphite, carbon atom forms three
covalent bonds with three other carbon
atoms, forming layers of hexagonalrings
which haveno covalent bonds between
the layers.
• Graphiteissoftandslippery– layers
caneasily slide over eachother
becausethe weak forces ofattraction
between the layers are easily broken.
Thisis why graphite is usedasa
lubricant.
• Graphiteconductselectricity– the
only non-metal to do so. Oneelectron
from eachcarbon atom isdelocalised.

Graphene
Graphene:
Thisis asinglelayer of graphite – alayer
of inter-locking hexagonal rings ofcarbon
atoms oneatom thick.
It is an excellent conductorof thermal
energy and electricity (even betterthan
graphite), hasavery low densityand is
incredibly strong.
It hasmany usesin theelectronics
industry.

Fullerenes
Fullerenes:
Fullerenesare molecules of carbon with hollowshapes.
Thestructure is basedon hexagonalrings of carbon
atoms, but mayhave5 or 7 carbon rings. Thefirst to be
discovered wasBuckminsterfullerene(C60)
which is spherical (like afootball).
This
Carbonnanotubesare cylindrical fullereneswith
very highlengthcomparedto their diameter.
makesthem useful for nanotechnology,
electronics and materials.

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Nanoparticles
(ChemistryONLY)
• Sizesof particlesand their
properties
• Usesofnanoparticles

CHEMISTRY ONLY
Nanoscience is the study of small
particles that are between 1 and100
nanometresin size.Particles consisting
of fewer than 100 atomsare often
called nanoclusters.
1 nanometre (1 nm) =1 x10-9 metres
(0.000 000 001m or abillionth of a
metre).
Nanoparticles are smaller than fine
particles(PM2.5) which havediameters
between
1 x10-7 metres and 2.5 x10-6.
Tocomprehend how small this is, coarse
particles,like dust, havediameters
between 1 x10-5 and 2.5 x10-6 .
Thesizeof a
typical
nanoparticle is…
… to a football as a
football is…
…to theEarth

CHEMISTRY ONLY
Nanoparticles show different properties to the samematerials in bulk asthey have ahigh
surfacearea to volume ratio.
Thediagram shows this idea:
Asparticle sizegets smaller, the
surface area to volume ratiogets
larger.
Asthe sideof cubedecreasesby
a factor of 10 the surfacearea to
volume ratio increasesbya
factor of 10.
Nanoparticles show different
properties to the samematerials
in bulk and have ahigh surface
area to volume ratio. It also
meansthat smaller quantities are
needed to be effective than the
materials with normal particle
sizes.
Surfacearea
(height xwidth xnumber ofsides)
3x3x6
=54
2x2x6
=24
1x1x6
=6
Volume
(height xwidth xlength)
3x3x3
=27
2x2x2
=8
1x1x1
=1
Surfaceto volumeratio
(surface area / volume)
54/27
=2
24/8
=3
6/1
=6

Nanoparticles havemany applications in
medicine,in electronics,in cosmetics
and sun creams,asdeodorants, and as
catalysts.
New developments in nanoscience are
very exciting but will need more
research into possible issuesthat might
arise from their increaseduse.
There are someconcerns that
nanoparticles maybe toxicto people.
Theymaybe able to enter the brain
from the bloodstream and causeharm.
Somepeople think more tests should
take place before nanoparticles of a
material are used on awider scale.
Usesof
nanoparticles
Healthcare
Clothing
Electronics
Sportsequipment
Cosmetics
Catalysts
Biomedical
Paints
Food
Industrial
Covalentbonding- PART3
CHEMISTRYONLY
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