The English name for lithium is Lithium, the chemical symbol Li, which is in the s region of the periodic table, alkali metal; atomic number 3; relative atomic mass 6.941. Lithium metal is solid at 298K and its color is silver or gray. In the air, lithium quickly loses its luster.
Lithium is a **periodic element containing a valence electron and its density is about 1/2 of that of water. The atomic radius (empirical value) of the lithium element is 145 pm, the atomic radius (calculated value) is 167 pm, the covalent radius (empirical value) is 134 pm, the van der Waals radius is 182 pm, and the ionic radius is 68 pm. The chemical properties of lithium are shown in Table 1-1. Since lithium has only one valence electron, its binding energy is weak in tightly packed cells. Lithium metal is very soft and has a low melting point, so lithium-sodium alloy can be used as a nuclear reactor refrigerant.
Lithium has a higher melting point and hardness than other alkali metals, and its conductivity is weak. The chemical properties of lithium are inconsistent with the changes in the chemical properties of other alkali metals. The standard electrode potential E (Li+/Li) of lithium is very low in the same group of elements, which is related to the large heat of hydration of Li+(g). When lithium is burned in air, it can directly react with nitrogen to form a nitride, which is due to its small ionic radius and thus a large contribution to the lattice. Lithium is very low in the lithosphere and is mainly found in some silicic acid mines. The density of lithium is only 0.53 g/cm3, and lithium has the melting point and boiling point of ** in the alkali metal and the longest liquid range, and has an exceptionally high specific heat capacity. These characteristics make it an excellent refrigerant in heat exchange. However, lithium is more corrosive than other liquid metals, and it is often used as a deaerator for reduction, desulfurization, copper, and copper alloys.
Due to the low ionization enthalpy of the lithium outer electron, the lithium ion of the 18650 lithium battery is spherical and low polarity, so the lithium element is +1. Compared to divalent magnesium ions, monovalent lithium ions have a particularly small ionic radius and therefore have a particularly high charge-to-radius ratio. The properties of lithium compounds are unusual compared to the elements of other ** main groups, similar to the properties of magnesium compounds. These anomalous properties are particularly stable due to their high lattice energy for lithium salts with low charge anions, and are relatively unstable for salts of highly charged, high valence 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 in red heat; Li 2 CO 3 is unstable. It is easily decomposed into Li2O and CO2. The solubility of the lithium salt is similar to that of the magnesium salt. LiF is slightly soluble (0.17/100g•water at 18°C) and can be precipitated from ammonium fluoride solution; Li3PO4 is hardly soluble in water; LiCl, LiBr, LiI, especially LiClO4 are soluble in ethanol, acetone and acetic acid Among the esters, LiCl is soluble in pyrimidine. The high solubility of LiClO4 is attributed to the strong solubility of lithium ions. High concentrations of LiBr dissolve cellulose. Unlike other alkali metal sulfates, Li2SO4 does not form isomorphous compounds.
The high electrode potential of lithium metal shows its application prospects on the battery. For example, the positive electrode is a lithium plate, and the negative electrode is a lithium ion secondary battery composed of a composite transition metal oxide material.
Among the ** main group elements, the activity of reacting with other substances (except nitrogen) increases from lithium to lanthanum. The activity of lithium is usually **, such as lithium and water react at 25 ° C, while sodium reacts violently, potassium and water burn, 铷 and 铯 have explosive reaction; reaction with liquid bromine, lithium and sodium It is alleviated, while other alkali metals react violently. Lithium cannot replace weakly acidic hydrogen in C6H5C≡CH, while other alkali metals can be substituted.
A fundamental chemical difference between lithium and congeners is the reaction with oxygen. When the alkali metal is burned in air or oxygen, lithium forms Li2O and Li2O2 is present, while other alkali metal oxides (M2O) react further to form peroxide M2O2 and (K, Rb and Cs) superoxide. MO2. Lithium does not form peroxide when burned in excess oxygen, but produces a normal oxide.
Lithium can be directly combined with nitrogen to form a nitride, and lithium and nitrogen react to form a ruby-colored crystal Li3N (magnesium and nitrogen to form Mg3N2); the reaction is slow at 25 ° C, and the reaction is rapid at 400 ° C. With this reaction, both lithium and magnesium can be used to remove nitrogen gas in a mixed gas. When co-heated with carbon, lithium and sodium react to form Li2C2 and Na2C2. The heavy alkali metal can also react with carbon, but produces a non-metering gap compound, which is a slow reaction of the alkali metal lithium with water.
Lithium hydroxide is a medium-strong alkali, and its solubility is not large. It can be decomposed into lithium oxide when heated. Certain salts of lithium, such as fluorides, carbonates, and phosphates, are poorly soluble in water. Their carbonates decompose to the corresponding oxides and carbon dioxide under heating. Lithium chloride is soluble in organic solvents and exhibits covalent properties.
Lithium is a **periodic element containing a valence electron and its density is about 1/2 of that of water. The atomic radius (empirical value) of the lithium element is 145 pm, the atomic radius (calculated value) is 167 pm, the covalent radius (empirical value) is 134 pm, the van der Waals radius is 182 pm, and the ionic radius is 68 pm. The chemical properties of lithium are shown in Table 1-1. Since lithium has only one valence electron, its binding energy is weak in tightly packed cells. Lithium metal is very soft and has a low melting point, so lithium-sodium alloy can be used as a nuclear reactor refrigerant.
Lithium has a higher melting point and hardness than other alkali metals, and its conductivity is weak. The chemical properties of lithium are inconsistent with the changes in the chemical properties of other alkali metals. The standard electrode potential E (Li+/Li) of lithium is very low in the same group of elements, which is related to the large heat of hydration of Li+(g). When lithium is burned in air, it can directly react with nitrogen to form a nitride, which is due to its small ionic radius and thus a large contribution to the lattice. Lithium is very low in the lithosphere and is mainly found in some silicic acid mines. The density of lithium is only 0.53 g/cm3, and lithium has the melting point and boiling point of ** in the alkali metal and the longest liquid range, and has an exceptionally high specific heat capacity. These characteristics make it an excellent refrigerant in heat exchange. However, lithium is more corrosive than other liquid metals, and it is often used as a deaerator for reduction, desulfurization, copper, and copper alloys.
Due to the low ionization enthalpy of the lithium outer electron, the lithium ion of the 18650 lithium battery is spherical and low polarity, so the lithium element is +1. Compared to divalent magnesium ions, monovalent lithium ions have a particularly small ionic radius and therefore have a particularly high charge-to-radius ratio. The properties of lithium compounds are unusual compared to the elements of other ** main groups, similar to the properties of magnesium compounds. These anomalous properties are particularly stable due to their high lattice energy for lithium salts with low charge anions, and are relatively unstable for salts of highly charged, high valence 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 in red heat; Li 2 CO 3 is unstable. It is easily decomposed into Li2O and CO2. The solubility of the lithium salt is similar to that of the magnesium salt. LiF is slightly soluble (0.17/100g•water at 18°C) and can be precipitated from ammonium fluoride solution; Li3PO4 is hardly soluble in water; LiCl, LiBr, LiI, especially LiClO4 are soluble in ethanol, acetone and acetic acid Among the esters, LiCl is soluble in pyrimidine. The high solubility of LiClO4 is attributed to the strong solubility of lithium ions. High concentrations of LiBr dissolve cellulose. Unlike other alkali metal sulfates, Li2SO4 does not form isomorphous compounds.
The high electrode potential of lithium metal shows its application prospects on the battery. For example, the positive electrode is a lithium plate, and the negative electrode is a lithium ion secondary battery composed of a composite transition metal oxide material.
Among the ** main group elements, the activity of reacting with other substances (except nitrogen) increases from lithium to lanthanum. The activity of lithium is usually **, such as lithium and water react at 25 ° C, while sodium reacts violently, potassium and water burn, 铷 and 铯 have explosive reaction; reaction with liquid bromine, lithium and sodium It is alleviated, while other alkali metals react violently. Lithium cannot replace weakly acidic hydrogen in C6H5C≡CH, while other alkali metals can be substituted.
A fundamental chemical difference between lithium and congeners is the reaction with oxygen. When the alkali metal is burned in air or oxygen, lithium forms Li2O and Li2O2 is present, while other alkali metal oxides (M2O) react further to form peroxide M2O2 and (K, Rb and Cs) superoxide. MO2. Lithium does not form peroxide when burned in excess oxygen, but produces a normal oxide.
Lithium can be directly combined with nitrogen to form a nitride, and lithium and nitrogen react to form a ruby-colored crystal Li3N (magnesium and nitrogen to form Mg3N2); the reaction is slow at 25 ° C, and the reaction is rapid at 400 ° C. With this reaction, both lithium and magnesium can be used to remove nitrogen gas in a mixed gas. When co-heated with carbon, lithium and sodium react to form Li2C2 and Na2C2. The heavy alkali metal can also react with carbon, but produces a non-metering gap compound, which is a slow reaction of the alkali metal lithium with water.
Lithium hydroxide is a medium-strong alkali, and its solubility is not large. It can be decomposed into lithium oxide when heated. Certain salts of lithium, such as fluorides, carbonates, and phosphates, are poorly soluble in water. Their carbonates decompose to the corresponding oxides and carbon dioxide under heating. Lithium chloride is soluble in organic solvents and exhibits covalent properties.
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