Physical and chemical properties of lithium in lithium batteries

Due to the low enthalpy of ionisation of the outer electrons of lithium, the lithium ions of 18650 Lithium Batteries are spherical and have a low polarity, hence the element lithium is +1. Monovalent lithium ions have a particularly small ionic radius and therefore a particularly high charge to radius ratio compared to divalent magnesium ions. Compared to elements with other major groups, lithium compounds have unusual properties, similar to those of magnesium compounds. These unusual properties are particularly stable due to the high lattice energy of lithium salts with low-charge anions, whereas they are relatively unstable for salts with highly charged, high-valence electron anions. For example, lithium hydride has higher thermal stability than other alkali metals, LiH is stable at 900°C, LiOH is more difficult to dissolve than other hydroxides, and lithium hydroxide decomposes under red heat; li2co3 is unstable. It decomposes readily to Li2O and CO2. the solubility of lithium salts is similar to that of magnesium salts. liF is slightly soluble (0.17/100 g-water at 18°C) and can be precipitated from ammonium fluoride solutions; Li3PO4 is insoluble in water; LiCl, LiBr, LiI and especially LiClO4 are soluble in ethanol, acetone and acetic acid. Among the esters, LiCl is soluble in pyrimidine. the high solubility of LiClO4 is due to the strong solubility of the lithium ion. High concentrations of lithium bromide can dissolve cellulose. Unlike other alkali metal sulphates, Li2SO4 does not form isomeric compounds.

The high electrode potential of lithium metal shows its promise for use in LiFePO4 Battery. For example, lithium batteries Maintenance Free Battery secondary Lithium Iron Phosphate Battery consisting of a lithium electrode plate for the positive electrode and a composite transition metal oxide material for the negative electrode.

In the **main group elements, the reaction activity with other substances (except nitrogen) increases from lithium to lanthanum. The activity of lithium is usually **, for example, lithium reacts with water at 25°C, while sodium reacts violently, potassium burns with water, rubidium and caesium have explosive reactions; reacts slowly with liquid bromine, lithium and sodium, while reacting violently with other alkali metals. In C6H5C≡CH lithium cannot replace weakly acidic hydrogen, while other alkali metals can be replaced.

A fundamental chemical difference between lithium and its congeners is the reaction with oxygen. When alkali metals are burned in air or oxygen, lithium forms Li2O and Li2O2, while other alkali metal oxides (M2O) react further to form peroxides M2O2 and (K, Rb and Cs) superoxides.MO2. Lithium does not form hydrogen peroxide when burned in excess of oxygen, but produces normal oxides.

Lithium can be combined directly with nitrogen to form nitrides, and lithium and nitrogen react to form ruby-coloured crystals Li3N (magnesium and nitrogen form Mg3N2); the reaction is slow at 25°C and rapid at 400°C, and by this reaction both lithium and magnesium can be used to remove nitrogen from the gas mixture. When co-heated with carbon, lithium and sodium react to form Li2C2 and Na2C2. heavy alkali metals can also react with carbon but produce non-metric gap compounds, which are slow reactions of lithium alkali metal with water.

Lithium hydroxide is a medium to strong base with little solubility. It decomposes to lithium oxide when heated. Certain lithium salts, such as fluorides, carbonates and phosphates, are insoluble in water. Their carbonates decompose to the corresponding oxides and carbon dioxide when heated. Lithium chloride is soluble in organic solvents and is covalent in nature.