ch23
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Livro Prentice-Hall 2002TRANSCRIPT
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Philip DuttonUniversity of Windsor, Canada
N9B 3P4
Prentice-Hall © 2002
General ChemistryPrinciples and Modern Applications
Petrucci • Harwood • Herring
8th Edition
Chapter 23: Main-Group Elements II: Nonmetals
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Prentice-Hall © 2002 General Chemistry: Chapter 23 Slide 2 of 51
Contents
23-1 Group 18: The Noble Gases
23-2 Group 17: The Halogens
23-3 Group 16: The Oxygen Family
23-4 Group 15: The Nitrogen Family
23-5 Group 14 Nonmetals: Carbon and Silicon
23-6 The Group 13 Nonmetal: Boron
Focus On Glassmaking
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23-1 The Noble Gases
• Initially thought to be chemically inert.• Pauling predicted reactivity of xenon.
– XeF2, XeF4, XeOF2, XeF6, XeO3, XeO4 and H4XeO6.
XeF2(aq) + 2 H+(aq) + 2 e- → Xe(g) + 2 HF(aq) E° = +2.64 V
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Xenon and Fluorine
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23-2 Group 17: The Halogens
• Diatomic molecules symbolized by X2.
• mp and bp increase down the period.• Reactivity decreases down the period.• Fluorine
– Most electronegative element.
– Forms strong bonds (ionic and covalent)
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Table 23.1 Group 17 Elements: The Halogens
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Electrode Potential Diagrams
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Production and Uses of Halogens
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Production and Uses of Halogens
• Chlorine and fluorine – by electrolysis, for example:
• Bromine– Seawater is 70 ppm Br-, acidify and oxidize with Cl2
2 HF → H2(g) + F2(g)
Cl2(g) + 2 Br-(aq) → 2 Cl- + Br2(l) E°cell = 0.293 V
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Prentice-Hall © 2002 General Chemistry: Chapter 23 Slide 10 of 51
Production and Uses of Halogens
• Iodine– Also obtained from inland brines and certain sea plants.
– NaIO3 is found in large deposits in Chile.
• Usually reduced with bisulfite.
• Many useful compounds can be formed from halogens.
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Table 23.2 Some Important Inorganic Compounds of Fluorine
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Hydrogen Halides
SiO2(s) + HF(aq) → 2 H2O(l) + SiF4(g)
CaF2(s) + H2SO4(aq) → CaSO4(s) + 2 HF(g)
H2(g) + X2(g) → 2 HX(g)
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Table 23.4 Oxoacids of the Halogens
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Oxoanions of Chlorine
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Table 23.5 Some Interhalogen Compounds
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Structures of Interhalogen Compounds
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Polyhalide Ions
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23-3 Group 16: The Oxygen Family
• S and O are clearly nonmetallic in behavior• Similar compounds:
– H2S and H2O CS2 and CO2 SCl2 and Cl2O
• Important differences– Due to properties and characteristics of O.
• Small size, high electronegativity and inability to employ an expanded valence shell.
– Hydrogen bonding in water but not in H2S.
– OS (O) -2, -1 and 0, but OS(S) -2 to +6 inclusive.–
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Allotropy and Polymorphism
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Occurrence of S and O
• Oxygen is most abundant element in earths crust (45.5%) and seawater (90%), in the atmosphere it is second only to N2 (23.25% by mass).
• Sulfur is 16th most abundant element in the crust (0.0384%).– Main use is conversion to sulfuric acid.
– Also used in vulcanization and for dusting grapevines.
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The Frasch Process
Sulfur is also obtained from oil and gas deposits and is recovered in the refining process.
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Sources and Uses of S and its Oxides
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Oxides, Oxoacids and Oxoanions of S
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Sulfur Oxoacids
SO3(g) + H2SO4(l) → H2S2O7(l)
H2S2O7(l) + H2O(l) → 2 H2SO4(l)
• Dilute H2SO4
– A diprotic acid.
• Concentrated H2SO4
– High affinity for water.
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Sulfates and Sulfites
• Gypsum and Plaster of Paris.• Sulfites solubilize lignin.
• Thiosulfate S2O32-.
– The two sulfurs are not equivalent.
– Photographic processes.
– Analytical reagent (determination of I-)
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Environmental Issues
• Smog consists mainly of particulate (ash and smoke), SO2 and H2SO4 mist.
– Main contributor is the emission of SO2.
– Acid rain.
– Levels of SO2 and H2SO4 above 0.10 ppm are considered potentially harmful.
• Especially to respiratory tract.
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23-4 Group 15: The Nitrogen Family
• Rich chemistry that can only be touched on here.– Nitrogen can exist in many oxidation states.
• N and P are nonmetallic.• As and Sb are metalloid.• Bi is metallic.
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Oxidation States of N
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Table 23.7 Selected Properties of Group 15 Elements
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Allotropy of P
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Production and Use
• P is 11th most abundant element in the earths crust (0.11%).– Originally purified from putrefied urine.
– Now obtained by heating apatites (phosphate rock of various compositions) in a furnace, for example:
2 Ca3(PO4)2(s) + 10 C(s) + 6 SiO2(s) →
6 CaSiO3(s) + 10 CO(g) + P4(s)
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Production and Use
• As obtained by heating metal sulfides.– FeAsS gives FeS and As(g).
• Sb is also obtained from sulfide ores.• As and Sb used to manufacture alloys.
– Added to lead for electrodes in storage batteries.
– Semiconductor doping.
• Bi is a biproduct of other metal refining.
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Nitrides
3 Mg(s) + N2(g) → Mg3N2(s) A very strong base.
Mg3N2(s) + H2O(l) → 3 Mg(OH)2(s)+ NH3(g)
With other non-metals nitrides form covalent bonds.
(CN)2 P3N5 As4N4 S2N2 S4N4
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Hydrides of Nitrogen
N2H4(l) + O2(g) → N2(g) + 2 H2O(l) ΔH° = -622.2 kJ/mol
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Hydrazoic Acid and Azides
• A weak acid.• Salts (azides) decompose explosively.
– Pb salts used in detonators.
– Na salts used in air-bag systems.
– Salts are also useful in organic synthesis for the introduction of nitrogen functionality.
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Oxides of Nitrogen
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Phosphorus Compounds
P4(s) + 3 OH-(aq) + 3 H2O(l) → 3 H2PO2-(aq) + PH3(g)
PCl3(l) + 6 H2O(l) → 3 H3PO3(aq) + 3 H3O+(l) + 3 Cl-(aq)
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Oxides and Oxoacids of P
+ 6 H2O(l) → 4 H3PO3(l)
+ 6 H2O(l) → 4 H3PO4(l)
phosporus acid
phosporic acid
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Polyphosphoric Acids
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Eutrophication
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23-5 Group 14 Nonmetals: Carbon and Silicon
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Carbon
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Carbon
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Inorganic Compounds of Carbon
• CaC2
– Reaction with H2O produces acetylene.
– miner’s lamps.
• CS2
– Flammable, volatile, poisonous.
– Important solvent.
• CCl4
– Known carcinogen.
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Production and Use of Si
• Reduce quartz or sand with C in a furnace.
• Oxides of Si, only one is stable, SiO2.
silica silicate mica
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Ceramics and Glasses
• Hydrated silicate polymers are important in the ceramic industry.– Sol-gel process produces exceptionally lightweight
ceramic materials.
– Electrical, magnetic and optical applications.
– Mechanical and structural properties are also important.
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Silanes and Silicones
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23-6 The Group 13 Nonmetal: Boron
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Other Boron Compounds
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Focus On Glassmaking
• Soda-lime glass.– The oldest form of glass.
– Na2CO3 + CaCO3 + SiO2
– Fused at 1300C.
• Small amounts of impurities impart beautiful colors.– Fe2O3 green
– CoO blue
• Adding B2O3 gives strength.– Borosilicate glass – Pyrex®
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Chapter 23 Questions
Develop problem solving skills and base your strategy not on solutions to specific problems but on understanding.
Choose a variety of problems from the text as examples.
Practice good techniques and get coaching from people who have been here before.