Barium is a chemical element with
symbol Ba and atomic number 56. It is the fifth
element in Group 2, a soft silvery metallic alkaline earth metal.
Because of its high chemical reactivity, barium is
never found in nature as a free element. Its hydroxide, known in pre-modern
history as baryta, does not occur as
a mineral, but can be prepared by heating barium carbonate.
The most common naturally occurring minerals of barium
are barite (barium sulfate, BaSO4)
and witherite (barium carbonate, BaCO3), both insoluble in water.
The barium name originates from the alchemical derivative "baryta",
from Greek βαρύς (barys),
meaning "heavy." Baric is the adjective form of barium. Barium
was identified as a new element in 1774, but not reduced to a metal until 1808
with the advent of electrolysis.
Radium is a chemical element with
symbol Ra and atomic number 88. It is the sixth
element in group 2 of the periodic table, also known as the alkaline earth metals.
Pure radium is silvery-white, but it readily combines with nitrogen (rather
than oxygen) on exposure to air, forming a black surface layer of radium
nitride (Ra3N2). All isotopes of radium are highly radioactive, with the most stable isotope being radium-226, which has a half-life of 1600 years and decays into radon gas (specifically the isotope radon-222). When radium decays, ionizing radiation is a
product, which can excite fluorescent chemicals and cause radioluminescence.
How does barium and radium differ when reacting?
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Barium: reactions of elements
Reaction of barium with air
Barium is a silvery white metal. The surface of barium metal is covered with a thin layer of oxide that helps protect the metal from attack by air, but to a lesser extent than the corresponding layer in magnesium. Once ignited, barium metal burns in air to give a mixture of white barium oxide, BaO, and barium nitride, Ba3N2. Barium oxide is more normally made by heating barium carbonate. The superoxide BaO2 apparently is also formed in this reaction. Barium, three places below magnesium in the periodic table is more reactive with air than magnesium.
2Ba(s) + O2(g) → 2BaO(s)
Ba(s) + O2(g) → BaO2(s)
3Ba(s) + N2(g) → Ba3N2(s)
Reaction of barium with water
Barium reacts readily with water to form barium hydroxide, Ba(OH)2 and hydrogen gas (H2). The reaction is quicker than that of strontium (immediately above barium in the periodic table) but probably slower than that of radium (immediately below barium in the periodic table).
Ba(s) + 2H2O(g) → Ba(OH)2(aq) + H2(g)
Reaction of barium with the halogens
I expect barium is very reactive towards the halogens, but I've not yet found explicit references to that effect. So, it is epxected that chlorine, Cl2 bromine, Br2, or iodine, I2, would burn to form the dihalides barium(II) chloride, BaCl2, barium(II) bromide, BaBr2, and barium(II) iodide, BaI2 respectively. The reactions with bromine and with iodine wolud probably require heat.
Ba(s) + Cl2(g) → BaCl2(s)
Ba(s) + Br2(g) → BaBr2(s)
Ba(s) + I2(g) → BaI2(s)
Radium, like barium, is a highly reactive metal and always exhibits its group oxidation state of +2.[3] It forms the colorless Ra2+ cation in aqueous solution, which is highly basic and does not form complexes readily.[3] Most radium compounds are therefore simple ionic compounds,[3] though participation from the 6s and 6p electrons (in addition to the valence 7s electrons) is expected due to relativistic effects and would enhance the covalent character of radium compounds such as RaF2 and RaAt2.[8] For this reason, the standard electrode potential for the half-reaction Ra2+ (aq) + 2e− → Ra (s) is −2.916 V, even slightly lower than the value −2.92 V for barium, whereas the values had previously smoothly increased down the group (Ca: −2.84 V; Sr: −2.89 V; Ba: −2.92 V).[9] The values for barium and radium are almost exactly the same as those of the heavier alkali metals potassium, rubidium, and caesium.[9]
HapusSolid radium compounds are white as radium ions provide no specific coloring, but they gradually turn yellow and then dark over time due to self-radiolysis from radium's alpha decay.[3] Insoluble radium compounds coprecipitate with all barium, most strontium, and most lead compounds.[10]
Radium oxide (RaO) has not been characterized well past its existence, despite oxides being common compounds for the other alkaline earth metals. Radium hydroxide (Ra(OH)2) is the most readily soluble among the alkaline earth hydroxides and is a stronger base than its barium congener, barium hydroxide.[11] It is also more soluble than actinium hydroxide and thorium hydroxide: these three adjacent hydroxides may be separated by precipitating them with ammonia.[11]
Can you mention the physical properties of barium and radium?
BalasHapusPure radium is a volatile silvery-white metal, although its lighter congeners calcium, strontium, and barium have a slight yellow tint.[2] Its color rapidly vanishes in air, yielding a black layer of radium nitride (Ra3N2).[3] Its melting point is either 700 °C (1,292 °F) or 960 °C (1,760 °F)[a] and its boiling point is 1,737 °C (3,159 °F). Both of these values are slightly lower than those of barium, confirming periodic trends down the group 2 elements.[4] Like barium and the alkali metals, radium crystallizes in the body-centered cubic structure at standard temperature and pressure: the radium–radium bond distance is 514.8 picometers.[5] Radium has a density of 5.5 g/cm3, higher than that of barium, again confirming periodic trends; the radium-barium density ratio is comparable to the radium-barium atomic mass ratio,[6] due to the two elements' similar crystal structures.
HapusBarium is a soft, silvery-white metal, with a slight golden shade when ultrapure.[5]:2 The silvery-white color of barium metal rapidly vanishes upon oxidation in air yielding a dark gray oxide layer. Barium has a medium specific weight and good electrical conductivity. Ultrapure barium is very difficult to prepare, and therefore many properties of barium have not been accurately measured yet.[5]:2
At room temperature and pressure, barium has a body-centered cubic structure, with a barium–barium distance of 503 picometers, expanding with heating at a rate of approximately 1.8×10−5/°C.[5]:2 It is a very soft metal with a Mohs hardness of 1.25.[5]:2 Its melting temperature of 1,000 K (730 °C; 1,340 °F)[6]:4–43 is intermediate between those of the lighter strontium (1,050 K or 780 °C or 1,430 °F)[6]:4–86 and heavier radium (973 K or 700 °C or 1,292 °F);[6]:4–78 however, its boiling point of 2,170 K (1,900 °C; 3,450 °F) exceeds that of strontium (1,655 K or 1,382 °C or 2,519 °F).[6]:4–86 The density (3.62 g·cm−3)[6]:4–43 is again intermediate between those of strontium (2.36 g·cm−3)[6]:4–86 and radium (~5 g·cm−3).
Can you mention the physical properties of barium and radium?
BalasHapuscan u tell me again about the electron configuration radium and barium?
BalasHapusbarium: 1s22s22p63s23p64s23d104p65s24d105p66s2
Hapusradium: 1s22s22p63s23p64s23d104p65s24d105p66s24f...
What is the fundamental difference of the element
BalasHapusImage explanation The image represents the former use of radium in luminous paint used for clock and watch dials. Appearance A soft, shiny and silvery radioactive metal. Uses Radium now has few uses, because it is so highly radioactive.Radium-223 is sometimes used to treat prostate cancer that has spread to the bones. Because bones contain calcium and radium is in the same group as calcium, it can be used to target cancerous bone cells. It gives off alpha particles that can kill the cancerous cells. Radium used to be used in luminous paints, for example in clock and watch dials. Although the alpha rays could not pass through the glass or metal of the watch casing, it is now considered to be too hazardous to be used in this way. Biological role Radium has no known biological role. It is toxic due to its radioactivity. Natural abundance Radium is present in all uranium ores, and could be extracted as a by-product of uranium refining. Uranium ores from DR Congo and Canada are richest in radium. Today radium is extracted from spent fuel rods from nuclear reactors. Annual production of this element is fewer than 100 grams per year.
HapusRadium
HapusImage explanation The image is based on x-ray radiographs of the human stomach and intestines in patients who have been given a ‘barium meal’. Appearance Barium is a soft, silvery metal that rapidly tarnishes in air and reacts with water. Uses Barium is not an extensively used element. Most is used in drilling fluids for oil and gas wells. It is also used in paint and in glassmaking.All barium compounds are toxic; however, barium sulfate is insoluble and so can be safely swallowed. A suspension of barium sulfate is sometimes given to patients suffering from digestive disorders. This is a ‘barium meal’ or ‘barium enema’. Barium is a heavy element and scatters X-rays, so as it passes through the body the stomach and intestines can be distinguished on an X-ray. Barium carbonate has been used in the past as a rat poison. Barium nitrate gives fireworks a green colour. Biological role Barium has no known biological role, although barium sulfate has been found in one particular type of algae. Barium is toxic, as are its water- or acid-soluble compounds. Natural abundance Barium occurs only in combination with other elements. The major ores are barite (barium sulfate) and witherite (barium carbonate). Barium metal can be prepared by electrolysis of molten barium chloride, or by heating barium oxide with aluminium powder.
Hi iin, please explain the most prominent thing to distinguish between barium and radium!
BalasHapusRadium is a radioactive element in Group 2 (IIA) and Row 7 of the periodic table. The periodic table is a chart that shows how chemical elements are related to each other. Radium was discovered in 1898 by Marie Curie (1867-1934) and her husband, Pierre Curie (1867-1934). It was found in an ore of uranium called pitchblende. The alkaline earth metals also include beryllium, magnesium, calcium, strontium, and barium.
HapusRadium is luminescent, meaning it gives off radiation that can be seen in the dark. Because of its radiation, however, it has relatively few uses
Iin , what characteristic from barium ?
BalasHapusBarium is a soft, silvery-white metal, with a slight golden shade when ultrapure.[5]:2 The silvery-white color of barium metal rapidly vanishes upon oxidation in air yielding a dark gray oxide layer. Barium has a medium specific weight and good electrical conductivity. Ultrapure barium is very difficult to prepare, and therefore many properties of barium have not been accurately measured yet.[5]:2
HapusAt room temperature and pressure, barium has a body-centered cubic structure, with a barium–barium distance of 503 picometers, expanding with heating at a rate of approximately 1.8×10−5/°C.[5]:2 It is a very soft metal with a Mohs hardness of 1.25.[5]:2 Its melting temperature of 1,000 K (730 °C; 1,340 °F)[6]:4–43 is intermediate between those of the lighter strontium (1,050 K or 780 °C or 1,430 °F)[6]:4–86 and heavier radium (973 K or 700 °C or 1,292 °F);[6]:4–78 however, its boiling point of 2,170 K (1,900 °C; 3,450 °F) exceeds that of strontium (1,655 K or 1,382 °C or 2,519 °F).[6]:4–86 The density (3.62 g·cm−3)[6]:4–43 is again intermediate between those of strontium (2.36 g·cm−3)[6]:4–86 and radium (~5 g·cm−3)