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6.11 g/cm 3: WEL (near r.t.) 6110 kg/m 3: LNG (at 19 °C) 6.11 g/cm 3: CRC (near r.t.) 6.0 g/cm 3: 24 Cr chromium; use: 7.15 g/cm 3: WEL (near r.t.) 7140 kg/m 3: LNG (at r.t.) 7.15 g/cm 3: CRC (near r.t.) 7.15 g/cm 3: 25 Mn manganese; use: 7.21 g/cm 3: WEL (near r.t.) 7470 kg/m 3: LNG (at 20 °C) 7.21 g/cm 3: CRC (near r.t.) 7.3 g/cm 3: 26 Fe ...
The molar mass of atoms of an element is given by the relative atomic mass of the element multiplied by the molar mass constant, M u ≈ 1.000 000 × 10 −3 kg/mol ≈ 1 g/mol. For normal samples from Earth with typical isotope composition, the atomic weight can be approximated by the standard atomic weight [ 2 ] or the conventional atomic weight.
For lab and small scale preparations a mixture of chromite ore, sodium hydroxide and sodium nitrate reacting at lower temperatures may be used (even 350 C in the corresponding potassium chromate system). [2] Subsequent to its formation, the chromate salt is converted to sodium dichromate, the precursor to most chromium compounds and materials. [3]
This small radius and high weight cause it to be expected to have an extremely high density of around 46 g·cm −3, over twice that of osmium, currently the most dense element known, at 22.61 g·cm −3; element 164 should be the second most dense element in the first 172 elements in the periodic table, with only its neighbor unhextrium ...
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The abundance of the chemical elements is a measure of the occurrences of the chemical elements relative to all other elements in a given environment. Abundance is measured in one of three ways: by mass fraction (in commercial contexts often called weight fraction), by mole fraction (fraction of atoms by numerical count, or sometimes fraction of molecules in gases), or by volume fraction.
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Historically, the mole was defined as the amount of substance in 12 grams of the carbon-12 isotope.As a consequence, the mass of one mole of a chemical compound, in grams, is numerically equal (for all practical purposes) to the mass of one molecule or formula unit of the compound, in daltons, and the molar mass of an isotope in grams per mole is approximately equal to the mass number ...
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