Chemistry of Carbon
Chemistry of Carbon
Chemistry of Carbon
CHEMISTRY
FORM 3
Chemistry of
CARBON
Comprehensive tutorial notes
Julius G.Thungu
jgthungu@gmail.com
0711 354 885
A: CARBON
Carbon is an element in Group IV(Group 4)of the Periodic table .It has atomic
number 6 and electronic configuration 2:4 and thus has four valence
electrons(tetravalent).It does not easily ionize but forms strong covalent bonds with
other elements including itself.
(a)Occurrence
Carbon mainly naturally occurs as:
(i)allotropes of carbon i.e graphite, diamond and fullerenes.
(ii)amorphous carbon in coal, peat ,charcoal and coke.
(iii)carbon(IV)oxide gas accounting 0.03% by volume of normal air in the
atmosphere.
(b)Allotropes of Carbon
Carbon naturally occur in two main crystalline allotropic forms, carbon-graphite
and carbon-diamond
Carbon-diamond Carbon-graphite
Shiny crystalline solid Black/dull crystalline solid
Has a very high melting/boiling point Has a high melting/boiling point
because it has a very closely packed because it has a very closely packed
giant tetrahedral structure joined by giant hexagonal planar structure joined
strong covalent bonds by strong covalent bonds
Has very high density(Hardest known Soft
natural substance)
Abrassive Slippery
Poor electrical conductor because it has Good electrical conductor because it has
no free delocalized electrons free 4th valency delocalized electrons
Is used in making Jewels, drilling and Used in making Lead-pencils,electrodes
cutting metals in batteries and as a lubricant
Has giant tetrahedral structure Has giant hexagonal planar structure
c)Properties of Carbon
(i)Physical properties of carbon
Carbon occur widely and naturally as a black solid
It is insoluble in water but soluble in carbon disulphide and organic solvents.
It is a poor electrical and thermal conductor.
(ii)Chemical properties of carbon
I. Burning
Experiment
2
Introduce a small piece of charcoal on a Bunsen flame then lower it into a gas jar
containing Oxygen gas. Put three drops of water. Swirl. Test the solution with blue
and red litmus papers.
Observation
-Carbon chars then burns with a blue flame
-Colourless and odourless gas produced
-Solution formed turn blue litmus paper faint red. Red litmus paper remains
red.
Explanation
Carbon burns in air and faster in Oxygen with a blue non-sooty/non-smoky flame
forming Carbon (IV) oxide gas. Carbon burns in limited supply of air with a blue
non-sooty/non-smoky flame forming Carbon (IV) oxide gas. Carbon (IV) oxide
gas dissolve in water to form weak acidic solution of Carbonic (IV)acid.
Chemical Equation
C(s) + O2(g) -> CO2(g) (in excess air)
2C(s) + O2(g) -> 2CO(g) (in limited air)
CO2(g) + H2O (l) -> H2CO3 (aq) (very weak acid)
Chemical Equation
2CuO(s) + C(s) -> 2Cu(s) + CO2(g)
(black) (brown)
3
Fe2O3(s) + 3C(s) -> 2Fe(s) + 3CO2(g)
(brown when hot/cool (grey)
4
B: COMPOUNDS OF CARBON
The following are the main compounds of Carbon
(i)Carbon(IV)Oxide(CO2)
(ii)Carbon(II)Oxide(CO)
(iii)Carbonate(IV) (CO32-)and hydrogen carbonate(IV(HCO3-)
(iv)Sodium carbonate(Na2CO3)
(a)Occurrence
Carbon(IV)oxide is found:
-in the air /atmosphere as 0.03% by volume.
-a solid carbon(IV)oxide mineral in Esageri near Eldame Ravine and Kerita
near Limuru in Kenya.
(b)School Laboratory preparation
In the school laboratory carbon(IV)oxide can be prepared in the school laboratory
from the reaction of marble chips(CaCO3)or sodium hydrogen carbonate(NaHCO3)
with dilute hydrochloric acid.
5
1.Write the equation for the reaction for the school laboratory preparation of
carbon (IV)oxide gas.
Any carbonate reacted with dilute hydrochloric acid should be able to generate
carbon (IV)oxide gas.
Chemical equations
CaCO3(s) + 2HCl(aq) -> CaCO3 (aq) + H2O(l) + CO2 (g)
ZnCO3(s) + 2HCl(aq) -> ZnCO3 (aq) + H2O(l) + CO2 (g)
MgCO3(s) + 2HCl(aq) -> MgCO3 (aq) + H2O(l) + CO2 (g)
CuCO3(s) + 2HCl(aq) -> CuCO3 (aq) + H2O(l) + CO2 (g)
NaHCO3(s) + HCl(aq) -> Na2CO3 (aq) + H2O(l) + CO2 (g)
KHCO3(s) + HCl(aq) -> K2CO3 (aq) + H2O(l) + CO2 (g)
2.What method of gas collection is used in preparation of Carbon(IV)oxide
gas. Explain.
Downward delivery /upward displacement of air/over mercury
Carbon(IV)oxide gas is about 1½ times denser than air.
3.What is the purpose of :
(a)water?
To absorb the more volatile hydrogen chloride fumes produced during the
vigorous reaction.
(b)sodium hydrogen carbonate?
To absorb the more volatile hydrogen chloride fumes produced during the vigorous
reaction and by reacting with the acid to produce more carbon (IV)oxide gas .
Chemical equation
NaHCO3(s) + HCl(aq) -> Na2CO3 (aq) + H2O(l) + CO2 (g)
(c)concentrated sulphuric(VI)acid?
To dry the gas/as a drying agent
6
Carbon(IV)oxide gas reacts with lime water(Ca(OH)2) to form an insoluble white
precipitate of calcium carbonate. Calcium carbonate reacts with more Carbon(IV)
oxide gas to form soluble Calcium hydrogen carbonate.
Chemical equation
Ca(OH)2(aq) + CO2 (g) -> CaCO3 (s) + H2O(l)
CaCO3 (aq) + H2O(l) + CO2 (g) -> Ca(HCO3) 2 (aq)
7. Dry and wet litmus papers were separately put in a gas jar containing dry
carbon (IV)oxide gas. State and explain the observations made.
Observation
Blue dry litmus paper remain blue
Red dry litmus paper remain Red
Blue wet/damp/moist litmus paper turn red
Red wet/damp/moist litmus paper remain red
Explanation
Dry Carbon (IV) oxide gas is a molecular compound that does not dissociate/ionize
to release H+ and thus has no effect on litmus papers.
Wet/damp/moist litmus papers contains water that dissolves/react with dry carbon
(IV) oxide gas to form the weak solution of carbonic (IV) acid(H2CO3).
Carbonic (IV) acid dissociate/ionizes to a few /little free H+ and CO32-.
The few H+ (aq) ions are responsible for turning blue litmus paper to faint red
showing the gas is very weakly acidic.
7
Chemical equation
H2CO3(aq) -> 2H+ (aq) + CO32-(aq)
8. Explain why Carbon (IV)oxide cannot be prepared from the reaction of:
(i) marble chips with dilute sulphuric(VI)acid.
Explanation
Reaction forms insoluble calcium sulphate(VI)that cover/coat unreacted marble
chips stopping further reaction
Chemical equation
CaCO3(s) + H2SO4 (aq) -> CaSO4 (s) + H2O(l) + CO2 (g)
PbCO3(s) + H2SO4 (aq) -> PbSO4 (s) + H2O(l) + CO2 (g)
BaCO3(s) + H2SO4 (aq) -> BaSO4 (s) + H2O(l) + CO2 (g)
(ii) Lead(II)carbonate with dilute Hydrochloric acid.
Reaction forms insoluble Lead(II)Chloride that cover/coat unreacted Lead(II)
carbonate stopping further reaction unless the reaction mixture is heated.
Lead(II)Chloride is soluble in hot water.
Chemical equation
PbCO3(s) + 2HCl (aq) -> PbCl2 (s) + H2O(l) + CO2 (g)
9
(c)Properties of Carbon (II)Oxide(Questions)
1.Write the equation for the reaction for the preparation of carbon(II)oxide
using;
(i)Method 1;
Chemical equation
HOOCCOOH(s) –Conc.H2SO4--> CO(g) + CO2 (g) + H2O(l)
H2C2O4(s) –Conc.H2SO4--> CO(g) + CO2 (g) + H2O(l)
(ii)Method 2;
Chemical equation
HCOOH(s) –Conc.H2SO4--> CO(g) + H2O(l)
H2CO2(s) –Conc.H2SO4--> CO(g) + H2O(l)
2.What method of gas collection is used during the preparation of carbon (II)
oxide.
Over water because the gas is insoluble in water.
Downward delivery because the gas is 1 ½ times denser than air .
3.What is the purpose of :
(i) Potassium hydroxide/sodium hydroxide in Method 1
To absorb/ remove carbon (II) oxide produced during the reaction.
2KOH (aq) + CO2 (g) -> K2CO3 (s) + H2O(l)
2NaOH (aq) + CO2 (g) -> Na2CO3 (s) + H2O(l)
6. Dry and wet/moist/damp litmus papers were separately put in a gas jar
containing dry carbon(IV)oxide gas. State and explain the observations made.
Observation
-blue dry litmus paper remains blue
-red dry litmus paper remains red
- wet/moist/damp blue litmus paper remains blue
- wet/moist/damp red litmus paper remains red
10
Explanation
Carbon(II)oxide gas is a molecular compound that does not dissociate /ionize to
release H+ ions and thus has no effect on litmus papers. Carbon(II)oxide gas is
therefore a neutral gas.
7. Carbon (II)oxide gas was ignited at the end of a generator as below.
Flame K
Dry carbon(II)oxide
(i)State the observations made in flame K.
Gas burns with a blue flame
(ii)Write the equation for the reaction taking place at flame K.
2CO(g) + O2 (g) -> 2CO2 (g)
Experiment
Pass carbon(II)oxide through glass tube containing copper (II)oxide. Ignite any
excess poisonous carbon(II)oxide.
Observation
Colour change from black to brown. Excess carbon (II)oxide burn with a blue
flame.
Explanation
Carbon is a reducing agent. It is used to reduce metal oxide ores to metal, itself
oxidized to carbon(IV)oxide gas. Carbon(II)Oxide reduces black copper(II)oxide
to brown copper metal
Chemical Equation
CuO(s) + CO(g) -> Cu(s) + CO2(g)
(black) (brown)
PbO(s) + CO(g) -> Pb(s) + CO2(g)
(brown when hot/ (grey)
yellow when cool)
ZnO(s) + CO(g) -> Zn(s) + CO2(g)
(yellow when hot/ (grey)
white when cool)
Fe2O3(s) + 3CO(s) -> 2Fe(s) + 3CO2(g)
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(brown when hot/cool (grey)
Observation inference
White precipitate/ppt CO32- ,SO32- ,SO42- ,Cl-
-
II. To the preserved solution ,add six drops of dilutte nitric(V)acid. Preserve.
15
Observation inference
White precipitate/ppt persists SO42- ,Cl-
II. To the preserved sample( that do not form a precipitate ),add three drops of
acidified potassium manganate(VII)/lime water
Observation inference
Effervescence/bubbles/fizzing SO32-
colourless gas produced
Acidified KMnO4 decolorized/no white
precipitate on lime water
Effervescence/bubbles/fizzing CO32-
colourless gas produced
Acidified KMnO4 not decolorized/
white precipitate on lime water
Experiments/Observations:
(b)Using Barium(II)nitrate(V)/ Barium(II)chloride
I. To about 5cm3 of a salt solution in a test tube add four drops of Barium(II)
nitrate (V) / Barium(II)chloride. Preserve.
Observation Inference
White precipitate/ppt SO42- , SO32- , CO32- ions
II. To the preserved sample in (I) above, add six drops of 2M nitric(V) acid .
Preserve.
Observation 1
Observation Inference
White precipitate/ppt persists SO42- , ions
Observation 2
Observation Inference
16
White precipitate/ppt dissolves SO32- , CO32- , ions
III.To the preserved sample observation 2 in (II) above, add 4 drops of acidified
potassium manganate(VII) /dichromate(VI).
Observation 1
Observation Inference
(i)acidified potassium manganate(VII)decolorized SO32- ions
(ii)Orange colour of acidified potassium
dichromate(VI) turns to green
Observation 2
Observation Inference
(i)acidified potassium manganate(VII) not CO32- ions
decolorized
(ii)Orange colour of acidified potassium
dichromate(VI) does not turns to green
Explanations
Using Lead(II)nitrate(V)
(i)Lead(II)nitrate(V) solution reacts with chlorides(Cl-), Sulphate (VI) salts
(SO42- ), Sulphate (IV)salts (SO32-) and carbonates(CO32-) to form the insoluble
white precipitate of Lead(II)chloride, Lead(II)sulphate(VI), Lead(II) sulphate (IV)
and Lead(II)carbonate(IV).
Chemical/ionic equation:
Pb2+(aq) + Cl- (aq) -> PbCl2(s)
2+
Pb (aq) + SO42+ (aq) -> PbSO4 (s)
2+
Pb (aq) + SO32+ (aq) -> PbSO3 (s)
2+
Pb (aq) + CO32+ (aq) -> PbCO3 (s)
(Orange) (green)
- Carbon(IV)oxide forms an insoluble white precipitate of calcium
carbonate if three drops of lime water are added into the reaction test tube when
effervescence is taking place. Sulphur(IV)oxide will not.
Chemical equation:
Ca(OH)2(aq) + CO2 (g) -> CaCO3(s) + H2O(l)
These tests should be done immediately after acidifying to ensure the gases
produced react with the oxidizing agents/lime water.
Chemical equation:
Ca(OH)2(aq) + CO2 (g) -> CaCO3(s) + H2O(l)
These tests should be done immediately after acidifying to ensure the gases
produced react with the oxidizing agents/lime water.
(iii) Sodium carbonate(IV) (Na2CO3)
(a)Extraction of sodium carbonate from soda ash
Sodium carbonate naturally occurs in Lake Magadi in Kenya as Trona.trona is the
double salt ; sodium sesquicarbonate. NaHCO3 .Na2CO3 .H2O.It is formed from the
volcanic activity that takes place in Lake Naivasha, Nakuru ,Bogoria and
Elementeita .All these lakes drain into Lake Magadi through underground rivers.
Lake Magadi has no outlet.
Solubility of Trona decrease with increase in temperature.High temperature during
the day causes trona to naturally crystallize .It is mechanically
scooped/dredged/dug and put in a furnace.
Inside the furnace, trona decompose into soda ash/sodium carbonate.
Chemical equation
2NaHCO3 .Na2CO3 .H2O (s) -> 3Na2CO3 (s) + 5H2O(l) + CO2 (g)
(trona) (soda ash)
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Soda ash is then bagged and sold as Magadi soda.It is mainly used:
(i)in making glass to lower the melting point of raw materials (sand/SiO 2
from 1650oC and CaO from 2500oC to around 1500oC)
(ii)in softening hard water
(iii)in the manufacture of soapless detergents.
(iv)Swimming pool “pH increaser”
Sodium chloride is also found dissolved in the lake. Solubility of sodium chloride
decrease with decreases in temperature/ sodium chloride has lower solubility at
lower temperatures. When temperatures decrease at night it crystallize out .The
crystals are then mechanically dug/dredged /scooped then packed for sale as
animal/cattle feeds and seasoning food.
Summary flow diagram showing the extraction of Soda ash from Trona
Carbon(IV) oxide
Crystals of sodium
Soda ash
chloride(At night)
Bagging Bagging
Na2CO3 (s)
NaCl(s)
(ii)Chemical processes
Ammonia gas is passed up to meet a downward flow of sodium chloride solution /
brine to form ammoniated brine/ammoniacal brine mixture in the ammoniated
brine chamber
The ammoniated brine mixture is then pumped up, atop the carbonator/ solvay
tower.
In the carbonator/ solvay tower, ammoniated brine/ammoniacal brine mixture
slowly trickle down to meet an upward flow of carbon(IV)oxide gas.
The carbonator is shelved /packed with quartz/broken glass to
(i) reduce the rate of flow of ammoniated brine/ammoniacal brine mixture.
(ii)increase surface area of the liquid mixture to ensure a lot of ammoniated
brine/ammoniacal brine mixture react with carbon(IV)oxide gas.
Insoluble sodium hydrogen carbonate and soluble ammonium chloride are formed
from the reaction.
Chemical equation
CO2(g) + H2O(l) + NaCl (aq) + NH3(g) -> NaHCO3(s) + NH4Cl(aq)
The products are then filtered. Insoluble sodium hydrogen carbonate forms the
residue while soluble ammonium chloride forms the filtrate.
Sodium hydrogen carbonate itself can be used:
(i) as baking powder and preservation of some soft drinks.
(ii) as a buffer agent and antacid in animal feeds to improve fibre digestion.
(iii) making dry chemical fire extinguishers.
In the Solvay process Sodium hydrogen carbonate is then heated to form Sodium
carbonate/soda ash, water and carbon (IV) oxide gas.
Chemical equation
2NaHCO3 (s) -> Na2CO3(s) + CO2(g) + H2O(l)
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Water and carbon(IV)oxide gas are recycled back to the ammoniated
brine/ammoniacal brine chamber.
More carbon(IV)oxide is produced in the kiln/furnace. Limestone is heated to
decompose into Calcium oxide and carbon(IV)oxide.
Chemical equation
CaCO3 (s) -> CaO(s) + CO2(g)
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Brine Brine saturated with ammonia Coke & Limestone
Practice
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1. The diagram below shows part of the Solvay process used in manufacturing
sodium carbonate. Use it to answer the questions that follow.
Carbon (IV)oxide
Ammonium chloride
(a)Explain how Sodium Chloride required for this process is obtained from
the sea.
Sea water is pumped /scooped into shallow pods. Evaporation of most of the water
takes Saturated
place leaving
Ammonia a very concentrated solution.
Process I Sodium hydrogen carbonate
sodium
(b)(i) Name chloride
process:
I. solution
Filtration
II. Decomposition
(ii) Write the equation forSodium
the reaction in process: Process II
carbonate
Process I
Chemical equation
CO2(g) + H2O(l) + NaCl (aq) + NH3(g) -> NaHCO3(s) + NH4Cl(aq)
Process II
Chemical equation
2NaHCO3 (s) -> Na2CO3(s) + CO2(g) + H2O(l)
(c)(i) Name two substances recycled in the solvay process
Ammonia gas , Carbon(IV)Oxide and Water.
(ii)Which is the by-product of this process?
Calcium(II)Chloride /CaCl2
(iii)State two uses that the by-product can be used for:
1. As a drying agent in the school laboratory preparation of gases.
2. In the Downs cell/process for extraction of Sodium to lower the
melting point of rock salt.
(iv)Write the chemical equation for the formation of the by-
products in the Solvay process.
Chemical equation
Ca(OH)2 (aq) +2NH4Cl (aq) -> CaCl2(s) + 2NH3(g) + H2O(l)
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(d)In an experiment to determine the % purity of Sodium carbonate
produced in the Solvay process ,2.15g of the sample reacted with exactly
40.0cm3 of 0.5M Sulphuric(VI)acid.
(i)Calculate the number of moles of sodium carbonate that reacted.
Chemical equation
Na2CO3 (aq) +H2SO4 (aq) -> Na2SO4 (aq)+ CO2(g) + H2O(l)
Mole ratio Na2CO3 :H2SO4 => 1:1
Moles H2SO4 = Molarity x Volume => 0.5 x 40.0 = 0.02 Moles
1000 1000
Moles of Na2CO3 = 0.02 Moles
(ii)Determine the % of sodium carbonate in the sample.
Molar mass of Na2CO3 = 106g
Mass of Na2CO3 = moles x Molar mass => 0.02 x 106 = 2.12 g
% of Na2CO3 = ( 2.12 g x 100) = 98.6047%
2.15
(e) State two uses of soda ash.
(i) during making glass/lowering the melting point of mixture of sand/SiO 2
from 1650oC and CaO from 2500oC to around 1500oC
(ii) in softening hard water
(iii) in the manufacture of soapless detergents.
(iv) swimming pool “pH increaser”.
Raw
Excess Carbon(IV)oxide
material
Metal plates
Substance
A
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Sodium hydrogen carbonate
(i)Name the raw materials needed in the above process
-Ammonia
-Water
-Carbon(IV)oxide
-Limestone
-Brine/ Concentrated sodium chloride
(ii)Identify substance A
Ammonium chloride /NH4Cl
(iii) Write the equation for the reaction taking place in:
I.Tower.
Chemical equation
CO2(g) + NaCl (aq) + H2O(l) + NH3(g) -> NaHCO3(s) + NH4Cl(aq)
II. Production of excess carbon (IV)oxide.
Chemical equation
CaCO3 (s) -> CaO(s) + CO2(g)
III. The regeneration of ammonia
Chemical equation
Ca(OH)2 (aq) +2NH4Cl (aq) -> CaCl2(s) + 2NH3(g) + H2O(l)
(iv)Give a reason for having the circular metal plates in the tower.
-To slow the downward flow of brine.
-To increase the rate of dissolving of ammonia.
-To increase the surface area for dissolution
(v)Name the gases recycled in the process illustrated above.
Ammonia gas , Carbon(IV)Oxide and Water.
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2. Describe how you would differentiate between carbon (IV)oxide and
carbon(II)oxide using chemical method.
Method I
-Bubble both gases in lime water/Ca(OH)2
-white precipitate is formed if the gas is carbon (IV) oxide
- No white precipitate is formed if the gas is carbon (II) oxide
Method II
-ignite both gases
- Carbon (IV) oxide does not burn/ignite
- Carbon (II) oxide burn with a blue non-sooty flame.
Method III
-Lower a burning splint into a gas containing each gas separately.
-burning splint is extinguished if the gas is carbon (IV) oxide
-burning splint is not extinguished if the gas is carbon (II) oxide.
3.Using Magnesium sulphate(VI)solution ,describe how you can differentiate
between a solution of sodium carbonate from a solution of sodium hydrogen
carbonate
-Add Magnesium sulphate(VI) solution to separate portions of a solution of sodium
carbonate and sodium hydrogen carbonate in separate test tubes
-White precipitate is formed in test tube containing sodium carbonate
-No white precipitate is formed in test tube containing sodium hydrogen carbonate.
Chemical equation
Na2CO3 (aq) +MgSO4 (aq) -> Na2SO4 (aq)+ MgCO3(s)
(white ppt)
Ionic equation
CO32- (aq) + Mg2+ (aq) -> MgCO3(s)
(white ppt)
Chemical equation
2NaHCO3 (aq) +MgSO4 (aq) -> Na2SO4 (aq) + Mg(HCO3)2 (aq)
(colourless solution)
4. The diagram below shows a common charcoal burner .Assume the burning
take place in a room with sufficient supply of air.
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(a)Explain what happens around:
(i)Layer A
Sufficient/excess air /oxygen enter through the air holes into the burner .It reacts
with/oxidizes Carbon to carbon(IV)oxide
Chemical equation
C(s) + O2(g) -> CO2 (g)
(ii)Layer B
Hot carbon(IV)oxide rises up and is reduced by more carbon/charcoal to carbon
(II)oxide.
Chemical equation
C(s) + CO2(g) -> 2CO (g)
(ii)Layer C
Hot carbon(II)oxide rises up and burns with a blue flame to be oxidized by the
excess air to form carbon(IV)oxide.
2CO (g) + O2(g) -> 2CO2(g)
(b)State and explain what would happen if the burner is put in an enclosed
room.
The hot poisonous /toxic carbon(II)oxide rising up will not be oxidized to
Carbon(IV)oxide.
(c)Using a chemical test , describe how you would differentiate two unlabelled
black solids suspected to be charcoal and copper(II)oxide.
Method I
-Burn/Ignite the two substances separately.
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-Charcoal burns with a blue flame
- Copper(II)oxide does not burn
Method II
-Add dilute sulphuric(VI)acid/Nitric(V)acid/Hydrochloric acid separately.
-Charcoal does not dissolve.
- Copper(II)oxide dissolves to form a colourless solution.
5. Excess Carbon(II)oxide was passed over heated copper(II)oxide as in the set
up shown below for five minutes.
Copper(II)oxide
Blue flame A
Dry
carbon
(IV)oxide
HEAT
(d) Using dot () and cross(x) to represent electrons show the bonding in a
molecule of :
(i) Carbon(II)oxide
lone pairs of electrons in carbon and oxygen
atoms
●●
C x ●
x●
xx
O xx
6 bonded pairs of
electrons
2covalent bonds
1 dative bond
56 jgthungu@gmail.com
(ii) Carbon(IV)Oxide.
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lone pairs of electrons in oxygen atom
●●
●●
O ●x
●x C ●x
●x O
●● ●●
4 bonded pairs of
electrons
6.Study the flow chart below and use it to answer the questions that follow.
(a)Name:
(i)the white precipitate A
Calcium carbonate
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(ii) solution B
Calcium hydrogen carbonate
(iii) gas C
Carbon(IV)oxide
(iv) white residue B
Calcium oxide
(v) solution D
Calcium hydroxide/lime water
(b)Write a balanced chemical equation for the reaction for the formation of:
(i) the white precipitate A from solution D
Chemical equation
Ca(OH)2(aq) + CO2 (g) -> CaCO3 (s) + H2O(l)
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