{"id":235,"date":"2015-12-15T22:43:10","date_gmt":"2015-12-15T22:43:10","guid":{"rendered":"http:\/\/www.earth-site.co.uk\/Education\/?page_id=235"},"modified":"2025-09-13T13:27:55","modified_gmt":"2025-09-13T12:27:55","slug":"lithium","status":"publish","type":"post","link":"https:\/\/www.earth-site.co.uk\/Education\/lithium\/","title":{"rendered":"Lithium – alkali metal"},"content":{"rendered":"
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Lithium is a soft silver-white metal with a range of applications including medication,batteries and fireworks. <\/em><\/span><\/p>\n

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Basic Information<\/a><\/span><\/p>\n

Discovery of Lithium <\/a><\/span><\/p>\n

Sources of Lithium <\/a><\/span><\/p>\n

Uses of Lithium <\/a><\/span><\/p>\n

Lithium Tablets <\/a><\/span><\/p>\n

Lithium Batteries <\/a><\/p>\n

Lithium In Fireworks <\/a> <\/p>\n

Lithium’s Cell Structure<\/a><\/span><\/p>\n

Absorption Lines of Lithium <\/a><\/span><\/p>\n

Emission Lines of Lithium <\/a><\/span><\/p>\n

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\"Lithium\"                                       <\/span>\"Lithium\"<\/span> <\/span><\/p>\n

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Lithium<\/span> (from the Greek Lithos meaning Stone)<\/span><\/p>\n

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\"Lithium\" <\/span><\/p>\n

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<\/a><\/h2>\n

Classification: Alkali metal<\/span><\/p>\n

Atomic Mass: [6.941 (2)] g\/mol<\/span><\/p>\n

Density: 0.534g\/cm3<\/span><\/p>\n

Colour: metallic silver or greyish white <\/span><\/p>\n

Boiling Point: 1615K (1342°C)<\/span><\/p>\n

Melting Point: 453.69K (180.54°C)<\/p>\n


\nCritical Temperature:3223K (2950°C)<\/p>\n

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<\/a>Discovery of Lithium<\/span><\/h2>\n
\n

Lithium (3<\/sub>Li) was first discovered in the mineral petalite (LiAlSi4O10) by Johann Arfvedson in Sweden 1817. <\/span><\/p>\n<\/blockquote>\n

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<\/a>Sources<\/span><\/h2>\n
\n

It is harvested from compounds found in most igneous rocks<\/a>, clay, brine sources and through electrolysis of compounds like lithium chloride.<\/span><\/p>\n

 <\/p>\n

3<\/sub>Li is a highly reactive and flammable metal like all the alkali metals and is only found in nature as part of a compound. A pure sample is a metallic silver metal however this very quickly changes into a dull whitish grey or black colour as it reacts with moisture or oxygen in the air. 3<\/sub>Li is the only alkali metal that reacts with nitrogen. To prevent reactions with other elements it is usually stored in mineral oil which acts as a barrier or protective seal.<\/span><\/p>\n<\/blockquote>\n

<\/a>Uses<\/span><\/h2>\n
\n

<\/a><\/span>In medicine 3<\/sub>Li is used to regulate the sodium levels in the muscles and nerves reducing the effects of mania in those that suffer from manic depression or manic episodes.<\/span><\/p>\n

 <\/p>\n

\"Lithium <\/span><\/p>\n

3<\/sub>Li helps reduce some of the symptoms associated with the illness such as hyperactivity, insomnia, aggression and other behavioural problems that may stem from the illness. 3<\/sub>Li is normally administered in time release tablets to prevent overdosing and as a last resort or in extreme cases due to the severe side effects connected with this drug. The side effects include nausea, vomiting, drowsiness, muscle weakness, tremor, reduced coordination, blurred vision or ringing in your ears.<\/span><\/p>\n

 <\/p>\n<\/blockquote>\n

\n

\"Lithium <\/span><\/p>\n

 <\/p>\n

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<\/a>3<\/sub>Li is used in some batteries as the anode and magnese oxide as the cathode, the chemical reaction produces a small charge which is dispersed from the battery. 3<\/sub>Li batteries usually have a longer life than regular alkaline batteries making them ideal for pacemakers and other medical devices. These batteries are more expensive however due to the 3<\/sub>Li required. <\/span><\/p>\n

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\n

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\"Fireworks <\/span><\/p>\n

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<\/a>When placed in a flame 3<\/sub>Li produces a red flame and as it is flammable it is ideal for flares or fireworks. It is also used in various compuonds in rocket fuel and as torpedo propellant. <\/span><\/p>\n

3<\/sub>Li is also used in the form of lithium-peroxide or lithium-hydroxide to purify the air in submarines and spacecraft as it is efficient in absorbing carbon dioxide from the atmosphere. <\/span><\/p>\n

 <\/p>\n

 <\/p>\n

 <\/p>\n<\/blockquote>\n

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<\/a><\/span>Shell Structure<\/span><\/h2>\n
\n

\"Helium <\/span><\/p>\n

 <\/p>\n

 <\/p>\n

 <\/p>\n

Protons = 3 <\/span><\/p>\n

 <\/p>\n

Neutrons =4<\/span><\/p>\n

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Electrons=3<\/span><\/p>\n

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3<\/p>\n<\/td>\n

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5<\/p>\n<\/td>\n

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6<\/p>\n<\/td>\n

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<\/a>Absorption Lines<\/span><\/h2>\n

\"Helium<\/span> <\/span><\/p>\n

 <\/span><\/p>\n

<\/a>Emission Lines<\/span><\/h2>\n

\"Helium<\/h2>\n<\/blockquote>\n

 <\/p>\n

 <\/p>\n<\/div>\n","protected":false},"excerpt":{"rendered":"

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