The alkali metals, including lithium, sodium, potassium, rubidium, caesium, and francium, are known for their high reactivity and distinctive properties. These Group 1 elements share characteristics like softness, low density, and low melting points, and are essential in various industries. Lithium batteries, sodium in glassmaking, and potassium in agriculture are just a few examples of their diverse applications. Their reactivity trends, flame test identification, and thermal stability of their compounds are also discussed.
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Alkali metals are a group of elements located in Group 1 of the periodic table
Single Valence Electron
Alkali metals are characterized by their possession of a single electron in their outermost electron shell, which contributes to their high reactivity
Decreasing Ionization Energy
As one moves down the group, the ionization energy of alkali metals decreases, making them more reactive
Alkali metals are soft, have low densities, and exhibit lower melting and boiling points compared to other metals
The size and charge density of alkali metal cations play a key role in determining the thermal stability of their compounds
The thermal stability of alkali metal compounds generally increases as one moves down the group
Flame tests involve exciting electrons in alkali metals to higher energy levels, resulting in the emission of specific colors of light
Different alkali metals produce distinct colors during flame tests, such as crimson, bright yellow-orange, lilac, reddish-violet, and blue-violet
Lithium is used in rechargeable batteries for portable electronics and electric vehicles due to its high electrochemical potential
Sodium has various applications in the production of soap, glass, and street lighting
Potassium is essential in the agricultural sector as a fertilizer ingredient and is also used in the manufacture of soaps and detergents
Rubidium and caesium have niche uses, such as in the production of specialty glasses and highly accurate atomic clocks, respectively
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Alkali metals' position in periodic table
Located in Group 1, s-block due to single valence electron.
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Characteristic reaction of alkali metals with water
React vigorously, forming hydroxides and releasing H2 gas.
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Trend in reactivity of alkali metals down the group
Reactivity increases down Group 1 due to easier loss of valence electron.
