Module C5. What Types of Chemicals are there in the earth’s atmosphere?
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Transcript of Module C5. What Types of Chemicals are there in the earth’s atmosphere?
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Module C5
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What Types of Chemicals are there in the earth’s atmosphere?
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• The Earth is the
source of all our
materials.
• We can get things
from:
the atmosphere
the lithosphere
the
hydrosphere
Chemicals from the Earth’s spheres
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The Earth’s Spheres……..
• We can break down the part of the Earth where we live and move into 4 areas, we call them spheres.
• Lithosphere• Hydrosphere• Atmosphere
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Lithosphere• Made up of Crust & part of Mantle• About 80km in depth.• Broken into tectonic plates which are
moving.• Made up:
– Silicates (compounds of Silicon & Oxygen)
– Hydrocarbons (compounds of Hydrogen & Carbon)
– Carbonates (such as chalk, limestone and sea shells)
– Metal ores
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Hydrosphere• The hydrosphere contains all the
solid, liquid, and gaseous water of the planet.– 97% of water is salty
• It ranges from 10 to 20 kilometers in thickness.
• Made up of:– Water– Dissolved oxygen– Dissolved nitrogen– Dissolved salts – Sodium Chloride– Calcium Carbonates (sea shells)
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Atmosphere• It envelope all air that surrounds
the whole Earth.• It ranges up to 10,000km above
the Crust.• Protects us from UV radiation
from the Sun.• Made up of:
– Nitrogen– Oxygen– Carbon dioxide– Water vapour– Noble gases – Argon.
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What molecules are there in the atmosphere?
The atmosphere
OxygenFormula?
Nitrogen.Formula?
Water vapourFormula?
Carbon dioxideFormula?
Inert Gases.Formula?
Pollutants?
What do these substances have in common?
Bpt?State at room temp?
Structure?Type of chemical element?
Bonding?
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Covalent Bonds• When Non-metals combine they
share electrons.• i.e. H2• Hydrogen needs 1 electron (it has
one possible bond).• So 2 hydrogen atoms will share
there electrons with each other.• The Molecule is now held
together by electrostatic forces between nuclei & electrons.
• They can’t move any closer because there similar charged nuclei would repel.
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Strong & Weak BondingStrong Bonding• The forces inside the molecules holding the atoms
together are many times stronger than the weak interaction between molecules.
• So a very high temperature is needed to break apart an Oxygen molecule (O2).
• The bonds that hold the compounds and molecules in the atmosphere are called Covalent Bonds. In Greek:– “Co” means together– “Valentia” means strong
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Strong & Weak BondingWeak Bonding• There is an attractive force between all molecules and
compounds, but this is very weak.• We can think of the molecules moving in the atmosphere very
quickly, so quickly that when they collide this attractive force is still too small to let them join up.
• As we reduce the temperature there is more chance they will join together.
• Watch the animation below, but remember that the boiling point of water is 100oC and Carbon dioxide is -78oC)
• Animation
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Attractive forces between molecules are weak.
Small molecules are gases or liquids at room temperature.
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A line between element symbols to
show a covalent bond.
H—H
hydrogen, H2
O O
oxygen, O2
N N
nitrogen, N2
O C O
carbon dioxide,
CO2
H
H—C—H
H
methane, CH4
H H
H—C—C—O—H
H H
ethanol, C2H5OH
OH H
water, H2O
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Chemists have different ways of describing molecules.
molecular formula
2D displayed formulawith lines for covalent bonds
3D ball-and-stick model
3D space-filling model
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Is there a correlation between Bpt, Structure and rfm?
Formula Bpt degrees C
Structure rfm
CO2 -78 Molecular 44
CO -191 Molecular 28
O2 -183 Molecular 32
SO2 -10 Molecular 64
C - diamond
Giant 12
• What is the correlation between structure and boiling point?
• Why do molecular substances have a lower boiling point then giant structures?
• What is the correlation between rfm and boiling point for molecular structures?
• Would water fit this pattern? Explain.
• Explain why you think that water shows anomalous ( out of character )behaviour.
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Covalent bonding
• Hydrogen H2
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Covalent Bonding……………
• Fluorine – F2
• Chlorine – Cl2
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Summarising Covalent Bonds.
• Covalent bonds share a pair of electrons that holds two atoms together.
• Covalent bonds are strong. • They also have a definite direction so
that molecules have a specific shape.
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Summary1) Our atmosphere is a relatively thin layer of air that
surrounds the Earth 2) Dry air is a mixture of chemicals such as N2, O2, and Ar,
which are elements and CO2, which is a compound3) These chemicals have low boiling points which means they
are gases over the range of temperatures found on the Earth.
4) Harmful gases that are added to the atmosphere by human activity are called pollutants
5) All the chemicals that make up our atmosphere are gases because they are made up of small molecules.
6) Small molecules are made up of atoms of one or more non-metal elements.
7) The atoms in the molecules are held together by strong covalent bonding.
8) The attractive forces between molecules are weak so they have low boiling points and are gases at normal temperatures.
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Physical properties of chemicals in the spheres……
• Describe the physical properties of the chemicals found in the:
• Lithosphere.• Atmosphere.• Hydrosphere. Describe solubility, melting points – high or low, and physical
state at room temperature.• Explain why these properties link to the presence of the
chemicals in each sphere.
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What Reactions Happen in the Hydrosphere?
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Salt harvesters in Thailand raking salt into piles
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• A sodium chloride crystal is made up of millions of
Na+ and Cl– ions arranged in a regular pattern.
• The regular pattern is responsible for the cubic
range of all sodium chloride crystals.
Crystals of sodium chloride
Ionic Salt crystals - NaCl
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+
• The ions can move independently, so a
solution of NaCl in water conducts electricity.
What happens when water dissolves an ionic salt?
Polar ( Charged) water molecules pull individual ions from the ionic crystal
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• A sodium chloride crystal is made up of millions of Na+ and Cl– ions arranged
in a regular pattern called a crystal lattice.
• The lattice is responsible for the cubic shape of all sodium chloride crystals.
Crystals of sodium chloride
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• Oppositely charged ions attract each other.
• Each ion will attract oppositely charged
ions from all directions.
• Each of these ions will in turn attract more
ions.
• A giant ionic lattice, made up of millions of
ions, is built up and forms a sodium
chloride crystal.
Physical properties:High Mpt/Bpt...Why?
Electrical Conductivity Solid?Electrical Conductivity in aqueous
solution?
Physical Properties of Sodium Chloride
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Are all Ionic Salts Soluble?
What Happens when Lead Nitrate reacts with Potassium Iodide?
Pb( NO3)2 (aq) + K I(aq)
Pb(I)2(ppt) + KNO3(aq)
Soluble
Insoluble - ppt
SolubleSoluble
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Precipitates and Predicting if one will form!
Precipitates form when an insoluble salt in formed during a reaction.
Ion Soluble? Insoluble ppts
Nitrate ( NO3) All NoneChloride ( Cl-1) Mostly Ag and Pb ChloridesSulphate ( SO4
-2) Mostly Ba and Pb sulphatesCarbonates ( CO3
-2) Only Na and Potassium Carbonates
Mainly
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Predict and Apply!!!!Reactant 1 Reactant 2 Products PPt?
Lead Nitrate Barium Chloride
Sodium Nitrate Barium Chloride
Copper Sulphate Barium Chloride
Copper Sulphate Lead Nitrate
Copper Sulphate Sodium Nitrate
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Predict!!!! AnswersReactant 1 Reactant 2 Products PPt?
Lead Nitrate Barium Chloride Yes – Lead Chloride
Sodium Nitrate Barium Chloride No
Copper Sulphate Barium Chloride Yes – Barium Sulphate
Copper Sulphate Lead Nitrate Yes – Lead Sulphate
Copper Sulphate Sodium Nitrate No
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Testing for Positive and Negctive Ions in Ionic Salts
Ions such as chlorine, fluorine,
calcium and sulfate are tested for to
check they are within allowed limits.
Metal and non metal ions give characteristic reactions with reagents so
that they can be identified.
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Testing for
positive ions
hydroxide ions in sodium hydroxide test solutionOH-(aq)
calcium ions in water sampleCa2+(aq)
Foe example,Calcium ions
have a positive charge. They
form a precipitate when mixed
with sodium hydroxide.
The amount of precipitate
indicates the amount of
calcium in the water sample. calcium hydroxide precipitateCa(OH)2(s)
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Positive Ions Test Reaction with NaOH
Name of Ion Observed colour : Product?
Iron(II), Fe2+ green precipitate
Iron(III), Fe3+ red-brown precipitate
Copper(II),Cu2+ light blue precipitate
Calcium, Ca2+ white precipitate
Zinc , Zn2+ white precipitate dissolves in excess sodium hydroxide solution
These positive metal ions form insoluble metal hydroxides with a characteristic colour
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Testing for
negative ions
barium ions in barium chloride test solutionBa2+(aq)
sulfate ions in water sampleSO4
2-(aq)
For example, sulphate ions
have a negative charge. They
form a precipitate when mixed
with barium chloride.
The amount of precipitate
indicates the amount of
Sulphate in the water sample. barium sulfate precipitateBaSO4(s)
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Negative Non Metal Ion TestsName of Ion and formulae Observed colour : Product?
Negative ion solution Result of test for ion
chloride, Clwhite precipitate with silver nitrate
bromide, Br
cream precipitate with silver nitrate
iodide, Iyellow precipitate with silver nitrate
sulfate, SO42
white precipitate with barium Sulphate
carbonate, CO32 Bubbles of CO2 gas;
limewater turns cloudy with HCl and limewater
These negative non metal ions form insoluble solids when reacted with another chemical reagent such as silver nitrate
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What types of chemicals make up the Earth’s
Lithosphere?
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Giant Covalent Structures…….
• Diamond – C.
• Graphite – C.
• Quartz – SiO2
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Structure of diamond and Graphite.
Explain why diamond has a high melting point
Explain why diamond does not conduct electricity
Explain why diamond does not dissolve in water
Explain why diamond is one of the hardest known materials.
Why do you think Graphite is a softer material than both SiO2 and diamond?
How many bonds does each Carbon atom make in Diamond? ……. In Graphite?
Why does Graphite conduct electricity?
In terms of structure what does SiO2resemble………. How does this explain its properties?
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Bonding in SiO2 ……………………
• How many bonds does each silicon atom make ?
• How many bonds does each Oxygen atom make?
• What group is Silicon in? Use this information to explain why Si makes four bonds.
• Why does Oxygen only make 2 bonds?
Si
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Silicon dioxide (SiO2) – explaining the observations……………..
• Why does SiO2 have a high mpt?
• Why Is SiO2 crystalline?
• Why is SiO2 a non conductor of electricity?
• Why is SiO2 a hard substance?
• Why is SiO2 not soluble in water?
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How can we extract Useful Metals From
Minerals?
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Iron
GoldAluminium
CopperSilver
Examples of common andimportant metals.
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What is an ore?
• An ore is a volume of rock containing components or minerals in a mode of occurrence that renders it valuable for mining.
• The impurities are removed so that the real metal can be seen or used.
• Examples of metal ores are Haematite and Bauxite
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Extraction processes
The ReactivitySeries
potassium
sodiumcalciummagnesium
aluminium
zinciron
copper
gold
(carbon)
Incr
easi
ng r
eact
ivity
Metals above carbon must be extracted using electrolysis.
Metals below carboncan be extracted from the ore by reduction using carbon, coke, or charcoal.
Gold and silver often do not need to be extracted. They occur native.
The reactivity of a metal determines the method of extraction.
lead
silver
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Apply.• The metal ores that can react with the carbon are: Copper Oxide Iron Oxide Zinc Oxide
• This is because Carbon is more reactive than these metals therefore can REDUCE the metal oxide
Explain the terms OXIDATION and REDUCTION.
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Oxidation and Reduction reactions – how do they work?
• CuO + C
• FeO + C
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The Electrolysis of Molten Lead Bromide
• Electrolysis is the decomposition of an ELECTROLYTE with an electric current.
• N:\C5 EAM\IC5_9.swf ( use this file to explain the process of electrolysis)
• Metals form at the Negative electrode
• Non Metals form at the positive electrode
• Reaction at the negative electrode:
• Pb+2
• Reaction at the positive electrode:
• 2Br-1
+
Lead Bromide
PbBr2
Heat
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Electrolysis of Lead Bromide.
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Reaction at the anode and cathode
The reactions are as follows:at the anode:• 2Br –
(l) → Br2(g) + 2e– Oxidation
at the cathode:• Pb2+
(l) + 2e– → Pb(l) Reduction
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Extraction of Al from it’s ore by Electrolysis
• http://www.rsc.org/learn-chemistry/resource/res00001027/industrial-process-videos?cmpid=CMP00001681
• ( 7 minute video of the extraction )
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A bauxite / cryolite mixture is melted in a steel container containing a carbon lining.
Graphite (carbon) anodes
Tanklinedwith
carboncathode
Molten electrolytebauxite + cryolite
Steelcase
Graphite anodes are inserted into the molten electrolyte ready for electrolysis.
Electrolytic extraction
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Aluminium formationOxygen formation
Anode (+ electrode)2O2-
(l) O2 (g) + 4e-
Cathode (- electrode)Al3+(l) + 3e- Al(l)
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Carbon dioxide formation at anode
• Carbon dioxide is formed at the anode rapidly .
• Explain why this is an added cost to the Al extraction industry.
• Write a chemical equation for this reaction.
• Why is there formation of carbon dioxide at the anode, explain in terms of ions, electrons and charge
.
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Extraction of aluminium using electrolysis – half reactions
Anode (+ve electrode)2O2-
(l) O2 (g) + 4e-
Cathode (-ve electrode)Al3+ (l) + 3e- Al (l)
Overall2Al2O3 (l) 4Al (l) + 3O2 (g)
The anode reacts to form carbon dioxide
C + O2 CO2
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Why are metals so Important?
• Uses related to strength, malleability, high melting point and electrical conductivity
Metals are bonded so that the positive nuclei are surrounded by a sea of electrons that are free to move –
this explain conductivity. Malleability the atoms have the ability to slip over the top of
one another High melting point – strong forces of attraction between the
electrons and the +ve nuclei
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How much metal can be extracted form it’s ore?
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Quantitative Chemistry………
• What does ram stand for?• Relative atomic mass• What does rfm stand for?• Relative formula mass.• Calculate the rfm of H2SO4. (H=1,S=32,O=16)• 98g.• Calculate the rfm of Al2(SO4)3(Al=27,S=32,O=16)• 342g
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Calculating the % of an element in a compound.
• Calculate the % of Nitrogen in NH4NO3.N=14; H=1;O=16)
• 35%• Calculate the % the metal in each of these
compounds.• Copper chloride• Sodium Oxide• Iron (III) Oxide.
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How much metal using %s
• Calculate the mass of Copper that would be extracted from 75kg of the ore – Copper oxide.
• Stage 1 – Calculate the % of copper in the compound.
• Stage 2 – Using this % calculate the mass of Cu in 75kg.
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Your turn…………………..
• The formula of red lead oxide is Pb3O4. Work out:
• The rfm of the red lead oxide• The % of lead in red lead oxide• The mass of Pb that would be extracted from
150kg of the ore.
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Question 2
• Work out the % of copper in these minerals:• Cuprite Cu2O
• Chalcopyrite CuFeS2
• Malachite Cu2CO3(OH)2
• Calculate the mass of Cu that would be extracted from 3000kg of each mineral.
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Using balanced Equations……..
• Calculate the mass of MgO that forms when 10.5g of Mg is burned in excess air?
• Write the equation for the reaction.• Identify chemicals in question.• Convert formulae to grammes using RFMs.• Calculate for 1g.• Calculate for quantity in question.
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Questions……………………
• What mass of copper oxide would form from the thermal decomposition of 1 tonne of copper carbonate?
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Questions……………………
• What mass of copper would form from the reaction of carbon with 0.75 tonnes of copper oxide?
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Identify from the list those you can do and explain how they are done….
• I can calculate rfms…….• I can calculate %s of element in a compound…..• I can calculate the mass of a metal that would be formed from
a kg quantity of ore…………• I can balance and use chemical equations to calculate reacting
masses using gramme quantities………• I can balance and use chemical equations to calculate reacting
masses using gramme quantities using Kg quantities…..• I can balance and use chemical equations to calculate reacting
masses using metric tonne quantities………