Lesson 4 The Halide Salts
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Transcript of Lesson 4 The Halide Salts
The Halide Salts.Aim: To identify and understand the general
properties of the halide salts.To understand that halide ions are reducing
agents and identify their reactions with concentrated sulphuric acid.
Properties of Halide Salts. Crystalline?
Water soluble?
Conductivity?
Mpt. Bpt?
Bonding?
Formation of Halide Salts. Reaction with group 1 metals. (Sodium
chloride)
Reaction with group 2 metals. (Magnesium chloride)
Reaction with d-block metals.( Copper (II) Chloride)
Halide Ions as Reducing agents. The reaction between (aq) sodium iodide and iron (III)
Chloride to make Iodine, Iron (II) chloride and Sodium chloride
NaI + FeCl3 I2 + FeCl2 + NaCl.
Ionic half equation for Iodine:
Ionic half equation for Iron:
Overall redox equation:
Reducing agent?
Halides as Reducing agents………… What is a reducing agent?
A substance that reduces another species by giving it one or more electrons. It undergoes oxidation as it loses electrons.
What is the trend in power of reducing power of halide ions as group 7 is descended?
I-1>Br-1>Cl-1>F-1 . I-1 loses electrons more
easily than F-1 Why?
Reaction of Halide Salts with Conc. Sulphuric Acid.
Acid + Halide salt can make
Hydrogen halides – HCl, HBr, HI.NaCl + H2SO4 HCl + NaHSO4
These products can go on to react with the sulphuric acid – and
reduce it.
How would we prove that
hydrogen halides are produced in the
reaction?
Hydrogen halides make dense white fumes when they react with conc
ammonia solution.
What is the equation for this type of reaction?
NH3+ HCl NH4Cl
Reaction of Hydrogen Halides with Conc Sulphuric acid.
Possible products when hydrogen halides react
with Conc sulphuric include sulphur dioxide, Hydrogen Sulphide and
the Halogen itself.
How do you test for Sulphur
dioxide?
Acidified potassium dichromate paper turns form orange to green
if sulphur dioxide is present.(Reaction type?)
How do you test for
Hydrogen Sulphide?
It smells of rotten eggs!
How do you identify the halogens?
Chlorine – Bleaches damp blue litmus
paper.Bromine – Slowly as above + distinctive
colour.Iodine – Distinctive
colour
Reaction of Halides with Sulphuric Acid.Halide Observation
with conc Sulphuric acid
Confirmatory test
Inference
KCl
KBr
KI.
Reaction of Halides with Sulphuric Acid.Halide Observation
with conc Sulphuric acid
Confirmatory test
Inference
KCl Steamy fumes in cold, no apparent effect when
heated
White smoke with ammonia - HCl, damp litmus paper turns red (not bleached) – no Cl2
HCl
KBr Steamy fumes in cold, brown gas on warming
(Br2)
White smoke with ammonia HBr.
acidified potassium dichromate(VI) goes from orange to green
– SO2 .
HBr & Br2, & SO2
KI. Steamy violet fumes in cold, more on warming (I2), bad egg smell (H2S)
White smoke with ammonia – HI
acidified potassium dichromate(VI) goes from orange to green – SO2
HI, I2 & H2S & SO2
Reaction with KCl KCl + H2SO4 HCl + KHSO4
What are the oxidation numbers of each element in each compound on the reactant side?
K = Cl= H= O= S=
Oxidation numbers on the product side? Is the Chloride ion acting as a reducing agent?
Reaction of KBr and Sulphuric Acid.
Reaction with KBr. Step 1 – Production of HBr. KBr + H2SO4 Step 2 – Reaction of HBr + H2SO4 HBr + H2SO4
What is the change in oxidation number of Bromide in the reaction?
Has the Bromide ion been oxidised or reduced? What is the change in oxidation number of
Sulphur during the reaction? Has Sulphur been oxidised or reduced? Is the Bromide ion a reducing or oxidising agent?
Br2 + SO2 + H2O
Reaction with KI 2KI(s) + H2SO4(l) KHSO4(s) + 2HI(g)
2HI(g) + H2SO4(l) SO2(g) + 2H2O(l) + I2(s)
AND 8HI(g) + H2SO4(l) H2S(g) + 4H2O(l) + 4I2(s)
Change in oxidation number of I-1? Change in oxidation number of S? Using these facts why is I-1 a stronger reducing
agent compared to Br-1?
Questions What halides have reduced the Sulphuric
acid? From your observations put the hydrogen
halides in order of reducing ability – most to the least.
How did you come to this conclusion? Explain why the hydrogen halide you have
chosen is the best reducing agent.
Homework Write up the halide ion tests in your lab
book from last week. See p.154 AS chemistry.
P156 AS chemistry Questions 1,2,3,4,6,7,10 –Only.
For Thursday.