the halogens chapter 40. f cl br i at gp vii position in periodic table
TRANSCRIPT
The Halogens
Chapter 40
F
Cl
Br
I
At
Gp VII
Position in Periodic Table
General informationHalogen Atomic
radius (nm)Ionic radius (nm)
Melting Point (oC)
Boiling Point (oC)
Density (g cm-3)
Abundance on Earth (%)
Fluorine 0.072 0.133 -220 -188 1.11 0.062
Chlorine 0.099 0.181 -101 -34.7 1.56 0.013
Bromine 0.114 0.195 -7.2 58.8 3.12 0.0003
Iodine 0.133 0.216 114 184 4.93 0.00005
Astatine - - 302 380 - Trace
Characteristic properties
• Very reactive non-metals– High electronegativity– High electron affinity
• Bonding and Oxidation states
• Colour
Electronegativity
A measure of the attracting ability of bonding electrons.
Due to their large effective nuclear charge, halogens are the most electronegative element in the periodic table.
Element EN value
F 4.0
Cl 3.0
Br 2.8
I 2.5
Electron Affinity
Generally high electronaffinity. All are exothermic.
X(g) + e- X-(aq)
Element EA kJ/mol
F -348
Cl -364
Br -342
I -285
Bonding and Oxidation State
• ns2np5
• Ionic or covalent bond with oxidation state –1 or +1 (F shows –1 only)
• Except F, all other halogens can expand their octet by using the low-lying, vacant d-orbitals to form bonding. Their oxidation states range from –1 to +7.
Bonding and Oxidation State
ns
np
nd
(0, +1, -1 states)
Cl2, Cl-, OCl2
ns
np
nd
(+3 states)
HClO2, ClO2-
Bonding and Oxidation State
ns
np
nd
(+5 state)
HClO3, HBrO3, I2O5
ns
np
nd
(+7 state)
Cl2O7, HIO4
ColourElement Colour
In Standard State In Water In 1,1,1-trichloroethane
F Pale yellow Pale yellow Pale yellow
Cl Greenish yellow Pale yellow Yellow
Br Reddish brown Yellow Orange
I Violet black Brown Violet
Colour
White light
Iodine
Check point 40-1
E1
Iodine
E2
Fluorine
Variation in properties of Halogens
F Cl Br I At0
400
-300
(Temp. oC)
b.p.
m.p.
m.p./b.p. increase as Mr increasebecause Van der Waals’ Force increasewith Mr
Electronegativity
F Cl Br I
4
3
2
1
4.0
3.02.8
2.5
F form ionic compoundwith –1 oxidation state.
I shows highly positive oxidation states withmore electronegativeelement.e.g. KIO4
Electron affinity
F Cl Br I
280
320
340
EA decrease fromCl to I due to increasingatomic size which lowersthe nuclear attraction to the added electron.
F has exceptional lowerEA because its 2nd shellis already crowded with7 e-, the additional e-
will experienced a greatere-e repulsion than otherhalogens.
Variation in Chemical Properties of elements
All are good oxidizing agents. (F2>Cl2>Br2>I2)
½ X2(std.state) X-(aq)
X(g)
X-(g)
Hatom
H
HEA
Hhyd
H Hatom HEA Hhyd= + +
Oxidizing power
Element
F 79.1 -348 -506 -774.9
Cl 121 -364 -364 -607
Br 112 -342 -335 -565
I 107 -314 -293 -500
HHatom HEA Hhyd
Oxidizingstrength
Oxidizing properties
1. Oxidation of metalsa. F2 oxidizes all metals including Au and Ag.b. Cl2 oxidizes common metals such as Na and Cu.
2. Reactions with Fe2+(aq)2Fe2+ + Cl22Fe3+ + 2Cl-
2Fe2+ + Br22Fe3+ + 2Br-
2Fe3+ + 2I-2Fe2+ + I2
Standard electrode potential (V)
Cl2+e-
Cl-
1.36
Br2+e-
Br-
1.07
I2+e-I- 0.54
Fe3++e-
Fe2+
0.77
Oxidizing properties
3. Reaction with phosphorus 2P + 3X2 2PX3
2P + 5X2 2PX5
F2 and Cl2 form PX5 as they have high oxidizingStrength. They combine with P to exhibit its maximumoxidation state.
Br2 and I2 form PX3 only.
Reaction with water
Fluorine oxidizes water to form HF and O2
2F2 + 2H2O 2HF + O2
Chlorine undergoes disproportionation(self oxidationand reduction) to form HCl and HOCl.
Cl2 + H2O HCl + HOCl
Reaction with water
A mixture of Cl2(aq), HCl(aq) and HOCl(aq)is called chlorine water.
OCl- , chloric(I) ion
1. Strong oxidizing agent with bleaching property OCl- + dye (coloured) Cl- + dye (colourless)2. Unstable to heat and light 2OCl- O2 + 2Cl-
Reaction with water
Br2 is only slightly soluble in water.Br2 (aq) + H2O (l) HBr(aq) + HOBr(aq)
OBr-(aq) is unstable and with bleaching property:1. 2OBr- O2 + 2Br-
2. OBr- + dye(coloured) Br- + dye(colourless)
Reaction with water
I2 does not react with water and only veryslightly soluble in water.
I2 is more soluble in ethanol or in KI(aq). I2(aq) + I-(aq) I3
-(aq)
Reaction with alkalis
All halogens react with aqueous alkalis anddisproportionate in it. The products depend on temperature and concentration of the alkalis.
Reaction with alkalis
Cold dil.NaOH
2F2 + 2NaOH 2NaF + OF2 + H2O
Cl2 + 2NaOH NaCl + NaOCl + H2O
Br2 + 2NaOH NaBr + NaOBr + H2O3NaOBr 2NaBr + NaBrO3
(3Br2 + 6NaOH 5NaBr + NaBrO3 + 3H2O
I2 + 2NaOH NaI + NaOI + H2O3NaOI 2NaI+ NaIO3
(3I2 + 6NaOH 5NaI + NaIO3 + 3H2O
Reaction with alkalis
More concentrated NaOH
2F2 + 4NaOH 4NaF + O2 + 2H2O
Hot concentrated NaOH
Cl2 + 2NaOH NaCl + NaCl + H2O3NaOCl 2NaCl + NaClO3
(3Cl2 + 6NaOH 5NaCl + NaClO3 + 3H2O
Reaction with alkalis
The reverse reaction of I2 and KOH is usedto prepare standard iodine solution for iodometrictitration. Know amount of iodine is generated bydissolving known quantity of KIO3 in excess KIand H+.
5KI + KIO3 + 3H+ 3I2 + 6K+ + 3H2O
Halogen Displacement reactions
Oxidizing strength : F2 >Cl2 >Br2 >I2
Cl2 + 2Br- 2Cl- + Br2
Cl2 + 2I- 2Cl- + I2
Br2 + 2I- 2Br- + I2
Variation in properties of halides
Halide + c. H2SO4
NaCl + H2SO4 NaHSO4 + HCl2NaCl + H2SO4 Na2SO4 + HCl (500oC)
2NaBr + 2H2SO4 2HBr + Na2SO4
2HI + H2SO4 SO2 + Br2 + 2H2O
2NaI + 2H2SO4 2HI + Na2SO4
8HI + H2SO4 H2S + 4I2 + 4H2O
Relative reducing power: HCl < HBr < HI
Halide + c. H3PO4
3NaCl + H3PO4 Na3PO4 + 3HCl3NaBr + H3PO4 Na3PO4 + 3HBr3NaI + H3PO4 Na3PO4 + 3HI
H3PO4 is NOT a strong oxidizing agent.It reacts with halides to form HX.
Halides + Ag+(aq)
Ag+(aq) + Cl-(aq) AgCl(s) , white precipitate
Ag+(aq) + Br-(aq) AgBr(s) , pale yellow precipitate
Ag+(aq) + I-(aq) AgI(s) , yellow precipitate
Halides + Ag+(aq)
Ion Action of AgNO3=
Effect of Standing in
sunlight
Effect of adding excess aq. N
H3
Cl- White ppt. Turns grey White ppt. dissolves
Br- Pale yellow ppt. Turns yellowish grey
Pale yellow ppt. slightly dissol
ves
I- Yellow ppt. Remains yellow
Yellow ppt. does not dissolve
Relative acidity of HX
Hydrogen Halide Dissociation constant Degree of dissociation in 0.1M solution
HF 7x10-4 0.085
HCl 1x107 0.920
HBr 1x109 0.930
HI 1x1011 0.950
Relative Acidity of HX
HX(aq) H+(aq) + X-(aq)
HX(g)
H+(g) + X-(g)
H (g) + X (g)
H
H1
H5 H6
H3 H4H2
Relative Acidity of HX
HX
HF 48 566 1311 -333 -1091 -515 -14 -29 15
HCl 18 431 1311 -348 -1091 -381 -60 -13 -47
HBr 21 366 1311 -324 -1091 -347 -64 -4 -60
HI 23 299 1311 -295 -1091 -305 -58 4 -62
H1 H2 H3 H4 H5 H6 H TS G
Explanation of weak acid strength of HF:• HF has the greatest bond dissociation energy and exceptionally small electron affinity. It has the least exothermic H.2. Due to formation of strong hydrogen bond and greatest degree of hydration, HF has the smallest decrease of TS.
Anomalous behaviour of HF
According to La Chatelier’s Principle, the degreeof dissociation of a weak acid increases with dilution. HA H+ + X-
However, the acidity of conc. HF is greater thandilute HF. Why?
In conc. HF, HF molecules form dimers H2F2 by hydrogen bond. The acid strength of H2F2 isstronger than HF. H2F2 H+ + HF2
-
Uses of Halogens and Halides
• Teflon
• Na2SiF6 or NaF is used to fluoridate drinking water.
• Chlorine bleach, sterilization of water, PVC.• Anti-knocking agent (leaded petrol)• AgBr coating in film• Iodine tincture• AgI in coating film