8.1investigating electrical conductivity of compounds all pure metals conduct an electric current....
TRANSCRIPT
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8.1 INVESTIGATING ELECTRICAL
CONDUCTIVITY OF COMPOUNDS
All pure metals conduct an electric current.
With the exception of carbon (in the form of graphite), all pure
non-metals do not conduct electricity.
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Figure 8.1 Investigating the electrical conductivity of compounds.
6 V battery+ _
light bulb
crocodile clipsolid piece
under test
(a) (b)
_+
crucible
liquid(molten)/aqueous under test
carbon (graphite) rods
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chlorine, carbon, hydrogen
1,1,1-trichloroethanesodium, hydrogen, oxygen
Sodium hydroxide
chlorine, carbonTetrachloromethanepotassium, manganese, oxygen
Potassium permanganate
carbon, hydrogenHexanecopper, sulphur, oxygen
Copper(II) sulphate
carbon, hydrogen, oxygen
Ethanol (an alcohol)magnesium, sulphur, oxygen
Magnesium sulphate
hydrogen, oxygenDistilled watercalcium, nitrogen, oxygen
Calcium nitrate
carbon, hydrogenPolythene (a plastic)potassium, iodinePotassium iodide
carbon, hydrogen, oxygen
Sugarlead, bromineLead(II) bromide
carbon, hydrogenWaxsodium, chlorineSodium chloride
Constituent elements
(Non-conductors whether solid, liquid or in aqueous solution)Constituent elements
(Non-conductors when solid, but conductors when molten or in aqueous solution)
Table 8.1 Electrical conductivity and constituent elements of some compounds.
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ELECTROLYTES are compounds which allow electricity to pass
through them only when molten or in aqueous solution.
Ionic compounds
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MetalsMetalsMetalsMetals
Non-Non-metalsmetals
Non-Non-metalsmetals
1 Compounds
solid state
molten or aqueoussolution
(conduct electricity)
(do not conduct electricity)
Electrolyte
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Compounds2
(do not conduct electricity)
solid, liquid or in aqueous solution
Non-Non-metalsmetals
Non-Non-metalsmetals
Non-Non-
metalsmetalsNon-Non-
metalsmetals
Non-Electrolyte
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• Why ionic compound is an electrolyte ?
• How do ionic compound conduct electricity in molten or aqueous state?
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Solid lead(II) bromide
Molten lead(II) bromide
does not conduct electricity
conducts electricity
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heat
molten lead(II) bromide
positive electrode (anode)
crocodile clip
clamp
boiling tube
negative electrode (cathode)
Glass tubing (connected to a rubber tubing which leads to the fume cupboard)
light bulb
6 V battery+ _
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Thus electric current is carried through molten lead(II) bromide by
mobile (freely moving) ions.
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Reddish brown brReddish brown bromine vapour is liomine vapour is li
beratedberated
At positive electrode At positive electrode (anode)(anode)
At positive electrode At positive electrode (anode)(anode)
At negative electrode At negative electrode (cathode)(cathode)
At negative electrode At negative electrode (cathode)(cathode)
A silvery grey substance (lead)
is deposited
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ELECTROLYTES AND IONS
Electrolytes
ELECTROLYTES are compounds which allow electricity to pass
through them only when molten or in aqueous solution. There is
chemical decomposition during the conduction.
ELECTROLYTES are compounds which allow electricity to pass
through them only when molten or in aqueous solution.
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Molten lead(II) bromide is thus decomposed to the two elements
lead and bromine.
The whole process is called electrolysis (meaning
'decomposition by electricity').
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Lead(II) bromide does not conduct electricity in solid state. This is
because ions in solids are not mobile (i.e. unable to move
freely).
Pb2+
Pb2+
Pb2+
Pb2+
Pb2+
Pb2+
Pb2+
Pb2+
Pb2+Br -
Br -
Br -
Br -
Br - Br -
Br -
Br - Br -
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Conclusions• Ionic compounds in molten or aqueous states can
conduct electricity. It is because there are mobile ions.
• Ionic compounds in solid state cannot conduct electricity. It is because ions are not mobile.
• Electrolytes are compounds which allow electricity to pass through them only when molten or in aqueous solution. There is chemical decomposition during the conduction.
• Electrolysis means 'decomposition by electricity'.
• You do not need to remember the observations in electrolysis.
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ELECTROLYSIS OF AQUEOUS COPPER(II)
CHLORIDE SOLUTION
Aqueous copper(II) chloride conducts electricity.
During electrolysis, copper(II) chloride is decomposed to form
copper (reddish brown solid) at cathode and chlorine gas (with
smell of swimming pool) at anode.
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Electrolysis of aqueous copper(II) chloride solution.
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Q8.2
(a) What charged particles does copper(II) chloride
consist of?
(b) Explain why solid copper(II) chloride does not
conduct electricity, but its aqueous solution does.
Q8.2
(a) What charged particles does copper(II) chloride
consist of?
(b) Explain why solid copper(II) chloride does not
conduct electricity, but its aqueous solution does.
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A8.2
(a) Positively charged copper(II) ions and negatively charged
chloride ions.
(b) Solid copper(II) chloride consists of ions which are not
mobile, therefore it does not conduct electricity. In aqueous
solution, the ions become mobile and thus the solution
conducts electricity.
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Q8.3
Which of the following are electrolytes?
Wax, sodium chloride, sodium, mercury, ethanol,
potassium iodide, sugar, carbon monoxide
Q8.3
Which of the following are electrolytes?
Wax, sodium chloride, sodium, mercury, ethanol,
potassium iodide, sugar, carbon monoxide
Sodium chloride and potassium iodide only.
A8.3
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An ION is an atom or a group of atoms having an overall electric
charge.
A simple (monoatomic) ion is derived from a single atom. A pol
yatomic ion is derived from a group of atoms.
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There are two kinds of ions: positively charged ions (cations) and
negatively charged ions (anions).
Cations and anions
cationscationscationscationsare attracted towards
anionsanionsanionsanionsare attracted towards
cathodecathode
anodeanode
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MIGRATION OF IONS
We can observe the migration (movement) of coloured ions durin
g electrolysis.
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Figure 8.7 To show the migration of coloured ions during electrolysis (using a U-tub
e).
carbon cathodecarbon anode
dilute hydrochloric acid
this region slowly becomes blue due to the migration of positive copper(II) ions towards the negative cathode
dilute hydrochloric acidthis region slowly becomes orange due to the migration of negative dichromate ions towards the positive anode
a gel containing copper(II) ions and dichromate ions
+ _
+ _
20V d.c. supply
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To show the migration of purple permanganate ions during under the influence of an
electric field(using a strip of filter paper on a microscope slide).
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Q8.6
Refer to again.
(a) Towards which electrode are potassium ions
migrating? Why?
(b) Can we see the movement of potassium ions?
Why?
(c) If a chromium(III) sulphate crystal was used
instead of a potassium permanganate crystal,
what would be observed? Why?
Q8.6
Refer to again.
(a) Towards which electrode are potassium ions
migrating? Why?
(b) Can we see the movement of potassium ions?
Why?
(c) If a chromium(III) sulphate crystal was used
instead of a potassium permanganate crystal,
what would be observed? Why?
Figure 8.8
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A8.6
(a) The cathode. Potassium ions are positively charged. They
are thus attracted towards the negative electrode
(cathode).
(b) No. Potassium ions are colourless.
(c) A green patch would move towards the negative electrode
(cathode). Chromium(III) ions are green in colour and
positively charged. They are attracted towards the negative
electrode.
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ObjectivesObjectives• To define what is chemical bondingTo define what is chemical bonding• To define what is ionic bondingTo define what is ionic bonding- Electrostatic attractions of opposite ionsElectrostatic attractions of opposite ions- Transfer of electron(s)Transfer of electron(s)- Non-directional forceNon-directional force- Obey the rule of stabilityObey the rule of stability
• To draw electron diagramsTo draw electron diagrams• To name and give chemical formula of the ionic compound To name and give chemical formula of the ionic compound
( both from mono or polyatomic ions)( both from mono or polyatomic ions)• To plan and describe experiments to realize what are electrTo plan and describe experiments to realize what are electr
olytes and non-electrolytes.olytes and non-electrolytes.• To realize the nature of ions of an ionic compound.To realize the nature of ions of an ionic compound.• To figure out the colour of an ionic compound in To figure out the colour of an ionic compound in aqueousaqueous s s
tate.tate.
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Chemical bonding (attractionChemical bonding (attraction))
Ionic bondingCovalent bonding
Forms between Forms between
metals and nonmetals nonmetals and nonmetals
Metallic bonding
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Ionic bonding• The reaction of sodium and chlorine .
Sodium Chloride
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Na
loses 1 e-
+
Na
unstable and unstable and reactivereactive
unstable and unstable and reactivereactive
sodium atom (Na) 2, 8, 1sodium atom (Na) 2, 8, 1 Na ionNa ion+
stablestablestablestable
CATIONCATIONCATIONCATION
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Clgains 1 e-
_
unstable and unstable and reactivereactive
unstable and unstable and reactivereactive
chlorine atom (Cl) 2, 8, 7chlorine atom (Cl) 2, 8, 7 Cl ionCl ion-
stablestablestablestable
xx
xx
x
x
x
xx
xx
xx
xx
xx
Cl
xx
xx
x
x
x
xx
xx
xx
xx
xx
ANIONANIONANIONANION
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When a sodium atom and a chlorine atom react, the sodium atom
loses one electron to the chlorine atom. As a result of this
transfer of electron, two ions are formed.
FORMATION OF IONIC BOND
IONIC BONDING AND IONIC SUBSTANCES
Sodium Chloride (Salt)
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NaNa+ ClCl_attracted by ionic bond
Nature of ionic bond
•The attraction force is non-directional
ClCl_
In sodium chloride
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Figure 8.15 Crystal of an ionic compound, sodium chloride.
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Sodium chloride has a giant ionic structure. It consists of Na+ and Cl– ions held
together by ionic bonds.
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Sodium chloride has a giant ionic structure. It consists of Na+ and Cl– ions held
together by ionic bonds.
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IONIC BOND is the strong non-directional electrostatic force of
attraction between oppositely charged ions.
An ionic bond is formed by the transfer of one or more electrons
from one atom (or group of atoms) to another.
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Monoatomic ion (consists of 1 atom only)
Polyatomic ion (consists of 2 or more atoms )
Na+ OH-
K+ NO3-
Ag+ SO42-
Hg+
I-
Cl-
Br-
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1) All simple (single) metal ions are cations.
2a) All simple (single) non-metal ions are anions (except H+).
2b) All polyatomic ions are anions (except NH4+)
3) There is only one common polyatomic cation - NH4+.
4) Polyatomic ions usually consist of non-metals only, but some consist of a metal and a non-metal.
5) When a metal forms only one cation, the ion has the same name as the metal.
6) Transition metals are rather unusual- the same metal can form more than one simple cation with different charges. To name each ion, a Roman numeral indicating the charge is written in brackets after the name of the metal.
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7) Simple (single) anion names ending in –ide
8) Polyatomic anions containing oxygen ofter have names ending in –ate or –ite. The polyatomic anion with more oxygen is named as –ate, and that with less oxygen as –ite.
9)Ions with 4+ or 4- are uncommon. (unstable)
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Questions
• Lead(II) dichromate• Iron(III) oxide• Potassium permanganate• Zinc hydroxide• KNO3
• CaCO3
• Ca(HCO3)2
• Fe2(SO4)3
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ObjectivesObjectives• To define what is chemical bondingTo define what is chemical bonding• To define what is ionic bondingTo define what is ionic bonding- Electrostatic attractions of opposite ionsElectrostatic attractions of opposite ions- Transfer of electron(s)Transfer of electron(s)- Non-directional forceNon-directional force- Obey the rule of stabilityObey the rule of stability
• To draw electron diagramsTo draw electron diagrams• To name and give chemical formula of the ionic To name and give chemical formula of the ionic
compound ( both from mono or polyatomic ions)compound ( both from mono or polyatomic ions)
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ENDENDENDEND