Why is lithium the most reactive metal

In a reactivity series, the most reactive element is placed at the top and the least reactive element at the bottom. More reactive metals have a greater tendency to lose electrons and form positive ions.

A reactivity series of metals could include any elements. For example:. A good way to remember the order of a reactivity series of metals is to use the first letter of each one to make up a silly sentence. Observations of the way that these elements react with water, acids and steam enable us to put them into this series.

These have been found on each of the 6 inhabited continents, but they are mined primarily in Western Australia, China, and Chile. Mineral sources of lithium are becoming less essential, as methods have now been developed to make use of the lithium salts found in saltwater. The mineral forms of lithium are heated to a high enough temperature K - K in order to crumble them and thus allow for subsequent reactions to more easily take place. After this process, one of three methods can be applied.

The lithium chloride obtained from any of the three methods undergoes an oxidation-reduction reaction in an electrolytic cell, to separate the chloride ions from the lithium ions. The chloride ions are oxidized, and the lithium ions are reduced. Saltwater naturally contains lithium chloride, which must be extracted in the form of lithium carbonate, then it is re-treated, separated into its ions, and reduced in the same electrolytic process as in extraction from lithium ores.

Only three saltwater lakes in the world are currently used for lithium extraction, in Nevada, Chile, and Argentina. Saltwater is channeled into shallow ponds and over a period of a year or more, water evaporates out to leave behind various salts.

Lime is used to remove the magnesium salt, so that the remaining solution contains a fairly concentrated amount of lithium chloride. The solution is then treated with sodium carbonate in order for usable lithium carbonate to precipitate out. Introduction Lithium was first identified as a component of of the mineral petalite and was discovered in by Johan August Arfwedson, but not isolated until some time later by W.

Properties Lithium is the lightest of all metals and is named from the Greek work for stone lithos. Table 1. Properties of lithium. Atomic Number 3 Atomic Mass 6.

Periodic Trends of Lithium Being on the upper left side of the Periodic Table, lithium has a fairly low electronegativity and electron affinity as compared to the rest of the elements. In the body, sodium ions regulate osmotic pressure and blood pressure, and sodium and potassium ions together play a major role in the transmission of nerve impulses. One of the most important compounds of sodium is sodium chloride, NaCl, also known as table salt. Commercially prepared sodium chloride is either mined in the form of halite, from deposits formed by ancient, dried-out sea beds, or by the evaporation of water from sea water.

Sodium chloride is subjected to electrolysis in an apparatus called a Downs cell, which produces sodium metal and chlorine gas; the construction of the cell is designed to keep the sodium and chlorine separate from each other as they are produced. Sodium carbonate, Na 2 CO 3 , also known as soda or soda ash, has been used for centuries in washing clothes it helps to remove highly charged metal cations, such as calcium and magnesium, from hard water and in the manufacture of glass, paper, and detergents.

Sodium hydroxide, NaOH, also known as caustic soda or lye, is a strong base; it is used in drain cleaners, and in the manufacture of detergents sodium hydroxide breaks down triglycerides — fats and oils such as lard, shortening, olive oil, vegetable oils, etc.

Sodium bicarbonate, NaHCO 3 , also known as sodium hydrogen carbonate, is the main ingredient in baking soda, and is used as a leavening agent in the making of bread and other baked goods. Potassium is a soft, silvery metal that reacts extremely vigorously with water, and tarnishes rapidly in air. Its name is derived from the English word "potash," for potassium carbonate, a compound found in high concentrations in wood ashes.

The symbol "K" is derived from the Latin name for the element, kalium. Potassium is the eighth most abundant element in the Earth's crust 2. Potassium is essential for plant growth, and is heavily used in fertilizers.

In the body, potassium plays a vital role in the contraction of muscle tissue; the movement of sodium and potassium ions in nerve cells plays a major role in the transmission of nerve impulses. When heated, potassium salts glow with a purple color, and are used in fireworks. Like sodium, metallic potassium is usually stored under mineral oil or some other hydrocarbon; it can also react with oxygen in dry air to produce potassium superoxide, KO 2 see below.

Potassium undergoes a a reaction with water similar to that of sodium; the products of the reaction are potassium hydroxide and hydrogen gas. This reaction releases a great deal of heat energy, often igniting the hydrogen gas that is produced. Potassium, which accounts for 0. It undergoes electron capture to produce argon; a comparison of the ratio of potassium to argon in rocks can be used to determine the age of the rock potassium-argon dating. Trace amounts of potassium are found in all sources of potassium; in a typical human, about , atoms of potassium decay every second.

The energy released by the decay of potassium is partially responsible for the interior heat of the Earth, along with the decays of thorium and uranium. There are a number of widely-used compounds of potassium. Potassium chloride, KCl, is used in salt substitutes mixed with sodium chloride to improve its flavor , and in fertilizers; massive amounts of potassium chloride are used in lethal injections to cause rapid death by cardiac arrest.

Potassium carbonate, K 2 CO 3 , also known as potash, is used in the manufacture of glass. Potassium hydroxide, KOH, also known as caustic potash, is used in making soaps and detergents.

Potassium nitrate, KNO 3 , also known as saltpeter, is a powerful oxidizer, and is one of the ingredients of gunpowder. Potassium chlorate, KClO 3 , is a very powerful oxidizer, and is used in match heads and fireworks. Potassium superoxide, KO 2 , reacts with carbon dioxide to produce potassium carbonate and oxygen gas; it is used in rebreathers and respiration equipment to generate oxygen, and is also used in mines, submarines, and spacecraft.

Rubidium is a soft, white metal; it is similar to sodium and potassium in its reaction with water, but the reaction is even more violently exothermic. Its name is derived from the Latin word for deep red ruby , rubidius. It is found in the Earth's crust at a concentration of 90 ppm, making it the 22nd most abundant element.

It is not found in any unique minerals, but is present in trace amounts in lepidolite, pollucite, carnallite, zinnwaldite, and leucite. Metallic rubidium spontaneously combusts in air.

In flame tests, rubidium salts produce a reddish-violet color, and are sometimes used in fireworks. Rubidium is used in the manufacture of vacuum tubes and cathode ray tubes CRTs , and is used in some atomic clocks.

Cesium undergoes the same reaction in water as lithium, sodium, and potassium, but even more violently; because cesium is a very large atom, the outermost electron is lost very easily, and the process is extremely exothermic. The name is derived from the Latin word caesius , which means "sky blue," because salts of cesium produce a blue color when heated. Cesium is found in the Earth's crust at a concentration of 3 ppm, making it the 46th most abundant element.

The main ore of cesium is pollucite [CsAlSi 2 O 6 ]; the refining of pure cesium is made even more difficult by the presence of trace amounts of rubidium in the ore, which is chemically very similar to cesium and thus difficult to separate. These electrons are easier to remove, so the atoms readily form chemical bonds.

In other words, as you increase the size of atoms of metals in a group, their reactivity also increases. Actively scan device characteristics for identification. Use precise geolocation data. Select personalised content. Create a personalised content profile.

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