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Chapter 22
Main-Group Elements I: Metals

 
 
 
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p 873-3
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Flame tests illustrate the emission of light by metals
Notes
Flame tests for metals. When a metal is placed in a flame it absorbs energy causing its electrons to be promoted to higher energy levels. The characteristic colors observed result from the energy released as the electrons fall to lower energy levels. The frequency of the emitted light depends on the differences in energy between the energy levels of the specific metal. Li produces a red flame, Na produces a yellow flame, and K produces a blue flame.
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p 1126-3
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Surfactant molecules form micelles in water and associate with oil droplets to remove them from clothing.
Notes
Surfactant molecules. A surfactant molecule has a hydrophobic (nonpolar) tail and a hydrophilic (polar) head. In water surfactants form micelles (clusters of surfactant molecules) in which the hydrophobic tails interact with each other in the middle and the hydrophobic heads interact with water on the surface. If an oil droplet is present the hydrophobic tail of the surfactant is embedded in the oil and the polar group is in contact with water.
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p 890-3
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The reaction between Al and Br2 to form AlBr3 is demonstrated.
Notes
Formation of Aluminum Bromide. When Al is placed on the surface of Br2 an exothermic reaction occurs. The Al is oxidized to Al3+ by the Br2, which is reduced to Br- ions. The ionic product, AlBr3, can be observed on the watch glass after the reaction.
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movie
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The reactions of metallic sodium and potassium with water are demonstrated.
Notes
When a small piece of Na is added to a solution containing an indicator, evidence of the reaction can be observed by the change in the color of the solution as NaOH is formed, by the melting of the Na and by the movement of the Na caused by formation of hydrogen gas. K is more reactive than Na as demonstrated by its reaction with water. This reaction produces enough heat to ignite the H2 produced.
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movie
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The exothermic reaction between Fe2O3 and aluminum is demonstrated.
Notes
In the thermite reaction, Al reduces Fe2O3 to Fe in an extremely exothermic reaction in which Al is oxidized to Al2O3. The reaction produces enough heat to melt the iron. Because of the extreme heat produced in the thermite reaction, it is used industrially to weld iron.
22.0.2UN
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Cutting metallic sodium. Note that the sodium, an active metal, is covered with a thick oxide coating.
22.1
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22-1
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hydration of a Li+ ion
Notes
hydration of a Li+ ion
22.1.1UN
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xray photo of artificial pacemaker
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xray photo of artificial pacemaker
22.2
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22-2
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Preparation of sodium compounds.
22.2.1UN
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p 877-1a
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sea salt stacks
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sea salt stacks
22.3
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22-3
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Diagonal relationships.
22.4
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22-4
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Notes
The Solvay process for the manufacture of NaHCO3.
22.4.1UN
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oxide ion, peroxide ion, superoxide ionsodium sulfate process
Notes
sodium sulfate process
22.4.2UN
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palmitic acid, sodium palmitate (a soap)
Notes
palmitic acid, sodium palmitate (a soap)
22.5.1UN
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photo of beryl- a bright green crystal
Notes
photo of beryl- a bright green crystal
22.5
Title
22-5
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structure o fa detergent molecule and it's cleaning action
Notes
structure o fa detergent molecule and it's cleaning action
22.6
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22-6
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covalent bonds in BeCl2
Notes
covalent bonds in BeCl2
22.7
Title
22-7
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the Dow process for the production of Mg
Notes
the Dow process for the production of Mg
22.8
Title
22-8
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electrolysis of molten MgCl2
Notes
electrolysis of molten MgCl2
22.8.1UN
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p 885-1
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The decomposition (calcination) of limestone is carried out in a long rotary kiln, whether for the production of quicklime, CaO, or the manufacture of Portland cement.
22.9
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22-9
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Stalactites and stalagmites in Carlsbad Caverns, New Mexico.
22.9.2UN
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limescale in a domestic metal pipe
Notes
limescale in a domestic metal pipe
22.9.3UN
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A sodium soap is added to soft (distilled) water (left) and hard water (right).
22.10C
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22-10
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ion exchange process
Notes
ion exchange process
22.11C
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22-11
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three photos of beakers to show purifying bauxite
Notes
three photos of beakers to show purifying bauxite
22.12
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22-12
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electrolysis cel for aluminum production
Notes
electrolysis cel for aluminum production
22.13.1UN
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p 893-1a
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AlCl3 is the Lewis acid and diethyl ether is the Lewis base
Notes
AlCl3 is the Lewis acid and diethyl ether is the Lewis base
22.13
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22-13
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bonding in Al2Cl6
Notes
bonding in Al2Cl6
22.13.2UN
Title
p 894-1
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photo of anodized aluminum cups
Notes
photo of anodized aluminum cups
22.13.3UN
Title
p 895-1
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potassium alum crystals
Notes
potassium alum crystals
22.14
Title
22-14
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graph comparing lead in gasoline and in blood
Notes
graph comparing lead in gasoline and in blood
22.14.1UN
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Solar cells employing gallium arsenide (gold and red) placed on a silicon-based solar cell.
22.14.2UN
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review question 25
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review question 25
22.14.3UN
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Lake Mono in California
Notes
Lake Mono in California
p 888-1a
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p 888-1a
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molecular zoom art
p 888-1b
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p 888-1b
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molecular zoom art
p 981-1a
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p 981-1a
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Purifying bauxite.
p 981-1b
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p 981-1b
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Purifying bauxite.
p 981-1c
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p 981-1c
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Purifying bauxite.
p 873-1
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p 873-1
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photo of spodumene from Afghanistan
p 886-1
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p 886-1
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plaster of paris/ white city buildings at Chicago World's Fair, 1893
p 888-1c
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p 888-1c
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photo of ion exchange column with liquid being poured through it
Table 22.1
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Table 22.1
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Group 1 elements: abundances
Table 22.2
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Table 22.2
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Notes
Some properties of the Group 1 metals
Table 22.3
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Table 22.3
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Notes
Group 2 elements: abandances
Table 22.4
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Table 22.4
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Notes
Some properties of the Group 2 metals
Table 22.5
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Table 22.5
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Notes
Some properties of the group 13 metals
Table 22.6
Title
Table 22.6
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Notes
some properties of tin and lead