Periodic Table Of Elements Download Free [UPDATED]
Cristal Hoggle
Many scientists worked on the problem of organizing the elements, but Dmitri Mendeleev published his first version of the periodic table in 1869, and is most often credited as its inventor. Since then, the periodic table has evolved to reflect over 150 years of scientific development and understanding in chemistry and physics. Today, with 118 known elements, it is widely regarded as one of the most significant achievements in science.
The latest release of the Periodic Table (dated 4 May 2022) includes the most recent abridged standard atomic weight values released by the IUPAC Commission on Isotopic Abundances and Atomic Weights (CIAAW), compiled as part of the 2021 Table of Standard Atomic Weights 2021. For elements that lack isotopes with a characteristic isotopic abundance in natural terrestrial samples, the mass number of the nuclide with the longest confirmed half-life is listed between square brackets. See PAC (AOP 4 May 2022; -2019-0603) for full details or visit Commission II.1 @ciaaw.org
By virtue of its work in relation with the chemical elements, IUPAC can dispense a periodic table that is up-to-date. IUPAC involvement covers various aspects of the table and data that it unveils, and several reports and recommendations, some quite recent, attest of that input.
The table is yours to use. Details about the latest release are provided above. Details below provide multiple references to IUPAC journal in Pure and Applied Chemistry (PAC) and magazine Chemistry International (CI).
Claims for the discoveries of new elements appear time to time in the scientific literature. IUPAC, along with IUPAP, is involved in assessing these claims. In result, IUPAC technical reports are released that review each pertaining references and recognize the laboratory(ies) whose claims fulfill the agreed criteria.
When the discovery of a new element has been validated and the priority for its discovery has been assigned, the naming process can begin. The Laboratory to which the discovery has been assigned is invited to propose a name and symbol. IUPAC will then review the proposal, and if agreed, after an additional 5-month public review, will formalize the name. The most recent example of such recommendations were published in 2012 and for the names and symbols of the elements 114 and 116; See PAC 2012, Vol. 84, No. 7, pp. 1669-1672; -REC-11-12-03
The question of precisely which elements should be placed in group 3 has been debated from time to time. An IUPAC project has been recently initiated to resolve the question. Will group 3 consist of Sc, Y, Lu, and Lr or, will it consist of Sc, Y, La and Ac?
You may also use the color-coded periodic table chart with names, symbols, and atomic weights to find specific information you need for your work. Easy-to-use filters allow you to sort by metals, nonmetals, physical states, group, period, and more.
These elements are very reactive, and usually occur in nature already combined with other elements. They have a silver-like luster, high ductility, and are excellent conductors of electricity and heat. Alkali metals have low melting points, ranging from 28.5 to 179C.
Alkaline Earth metals form Group 2 of the periodic table. Except for radium, all of the elements in this group are used in commercial applications. Magnesium and calcium are two of the six most common elements on Earth, and are essential to some geological and biological processes.
These elements have a shiny gray-white appearance. They are good conductors of electricity and have higher melting and boiling points than the alkali metals. Melting points range from 650 to 1,287C and boiling points range from 1,090 to 2,471C.
Similar to the metals, transition metals are malleable and ductile, conduct heat and electricity, and form positive ions. However, these elements are more electronegative and more likely to form covalent compounds. Transition metals can form useful alloys with other transition or metallic elements.
Lanthanides oxidize rapidly in moist air, dissolve quickly in acids, and react slowly with oxygen at room temperature. These elements are used in superconductors and hybrid car components, primarily as magnets and batteries. They are also used in the production of specialty glass.
The 15 metallic elements with atomic numbers 89 to 104, actinium through lawrencium, are referred to as the actinides. All of these elements are radioactive, relatively unstable, and release energy in the form of radioactive decay. However, they can form stable complexes with ligands, such as chloride, sulfate, carbonate, and acetate.
The most commonly recognized metalloids include boron, silicon, germanium, arsenic, antimony, and tellurium. Their properties are a mixture of or fall between those of metals and nonmetals, and the number of elements included in this category can vary.
Halogens are the non-metallic elements found in group 17 of the periodic table: and include fluorine, chlorine, bromine, iodine, and astatine. They are the only group whose elements at room temperature include solid, liquid, and gas forms of matter. When halogens react with metals, they produce a range of useful salts, including calcium fluoride, sodium chloride, silver bromide, and potassium iodide.
Since halogens are one electron short of having full shells, they can combine with many different elements. They are highly reactive and can be lethal in concentrated amounts. Commercially, halogens are used in disinfectants, lighting, and drug components.
When Dmitri Mendeleev created the periodic table in the late 19th century, he grouped elements by atomic weight. When grouped by weight, the behavior of the elements appeared to occur in regular intervals or periods. The columns of the modern periodic table represent groups of elements and rows represent the periods. The groups are numbered one through 18. Elements in the same group can be expected to behave in a similar way because they have the same number of electrons in their outermost shell.
Oxygen is a component of hundreds of thousands of organic compounds and readily combines with most elements. Oxygen has nine isotopes. Its allotrope ozone (O3) is formed when oxygen is subjected to an electrical discharge or ultraviolet light.
Neon is very inert, but a fluorine-neon compound has been reported. It also forms an unstable hydrate. Neon has more refrigerating capacity per volume than liquid helium and more than triple that of liquid hydrogen.
Sodium is never found free in nature. It is a soft, bright, silvery metal that floats on water. It can ignite spontaneously in water, and normally will not ignite in air at temperatures below 115C. Its most common compound is sodium chloride (table salt), but it occurs in soda niter, cryolite, amphibole, zeolite, and many other minerals.
In nature, chlorine is found only in a combined state, mostly as common salt (NaCl), carnallite, and sylvite. A greenish-yellow gas, it combines with nearly all elements. Chlorine gas is a respiratory irritant and prolonged exposure can be fatal.
Argon is used in incandescent and fluorescent light bulbs and in photo and glow tubes. Argon is used as a gas shield for arc welding and cutting, acts as a blanket when producing titanium and other reactive elements, and offers a protective atmosphere for silicon and germanium crystal growth.
Principal sources of zinc are sphalerite (sulfide), smithsonite (carbonate), calamine (silicate), and franklinite (zinc, manganese, iron oxide) ores. Naturally occurring zinc includes five stable isotopes, and sixteen other unstable isotopes are known.
Amorphous selenium is red (powder form) or black (vitreous form); the crystalline monoclinic version is deep red, and the stable crystalline hexagonal form is metallic gray. Selenium naturally contains six stable isotopes, and fifteen others have been found.
Krypton is one of the noble gases and is characterized by its brilliant green and orange spectral lines. Solid krypton is a white crystalline substance with a structure common to all rare gases. Naturally occurring, krypton has six stable isotopes. Seventeen unstable isotopes have also been identified. Although it is considered to be inert, some compounds of krypton have been shown to exist.
A mixture of four stable isotopes forms natural strontium and sixteen unstable isotopes are also known to exist. Volatile strontium salts, which impart a crimson color to flame, are used in pyrotechnics and flares.
Rhodium is used primarily in alloys to harden platinum and palladium, which are then used for furnaces, thermocouple elements, bushings, aircraft spark plugs, and laboratory crucibles. It is corrosion-resistant and its low electrical resistance makes it a good electrical contact material. Rhodium is also used as a catalyst, in optical instruments, and for jewelry and decoration.
Pure silver is a lustrous and brilliant white. A little harder than gold, it is malleable and ductile, with high electrical and thermal conductivity and low contact resistance. Silver is stable in pure air and water and tarnishes with exposure to ozone, hydrogen sulfide, or air that contains sulfur.
Ordinary tin is a silver-white, malleable metal that is somewhat ductile and highly crystalline. The distortion of the crystals causes an audible cry" when a piece of tin is bent. Tin comprises nine stable isotopes, and 18 more unstable isotopes are known.
Barium is found only in combination with other elements. This alkaline earth metal is metallic, soft, and silvery white when pure, resembling calcium. The metal oxidizes easily and must be kept under petroleum or other oxygen-free liquids.
Gadolinium is silvery white with a metallic luster and is both malleable and ductile. The metal is relatively stable in dry air but tarnishes in moist air. It reacts slowly with water and dissolves in dilute acid. Natural gadolinium is comprised of seven isotopes, and 17 are actually recognized in total.
This element has a bright metallic luster and is relatively stable at room temperature. Dysprosium can be cut with a knife and machined without sparking if not overheated. Minute impurities can significantly affect its physical properties.
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