Mass Of Elements



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  • The mass-abundance of the nine most abundant elements in the Earth's crust is approximately: oxygen 46%, silicon 28%, aluminum 8.3%, iron 5.6%, calcium 4.2%, sodium 2.5%, magnesium 2.4%, potassium 2.0%, and titanium 0.61%. Other elements occur at less than 0.15%. For a complete list, see abundance of elements in Earth's crust.
  • This is a list of the 118 chemical elements which have been identified as of 2021. A chemical element, often simply called an element, is a species of atoms which all have the same number of protons in their atomic nuclei (i.e., the same atomic number, or Z).
From Simple English Wikipedia, the free encyclopedia

Hydrogen is estimated to make up more than 90% of all the atoms three quarters of the mass of the universe! This element is found in the stars, and plays an important part in powering the universe through both the proton-proton reaction and carbon-nitrogen cycle.

An atomic mass (symbol: ma) is the mass of a single atom of a chemical element. Linux for mac powerpc. It includes the masses of the 3 subatomic particles that make up an atom: protons, neutrons and electrons.

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Atomic mass can be expressed in grams. However, because each atom has a very small mass, this is not very helpful. Instead, atomic mass is expressed in unified atomic mass units (unit symbol: u). 1 atomic mass unit is defined as 1/12 of the mass of a single carbon-12 atom.[1]:18 1 u has a value of 1.660 539 066 60(50) × 10−27kg.[2]

A carbon-12 atom has a mass of 12 u. Because electrons are so light, we can say that the mass of a carbon-12 atom is made of 6 protons and 6 neutrons. Because the masses of protons and neutrons are almost exactly the same, we can say that both protons and neutrons have a mass of roughly 1 u.[1]:18 Hence, we can get a rough value of an atom's mass in atomic mass units by working out the sum of the number of protons and the number of neutrons in the nucleus, which is called the mass number. The atomic mass of an atom is usually within 0.1 u of the mass number.

The number of protons an atom has determines what element it is. However, most elements in nature consist of atoms with different numbers of neutrons.[3] An atom of an element with a certain number of neutrons is called an isotope.[1]:44 For example, the element chlorine has two common isotopes: chlorine-35 and chlorine-37. Both isotopes of chlorine have 17 protons, but chlorine-37 has 20 neutrons, 2 more neutrons than chlorine-35, which has 18.[4] Each isotope has its own atomic mass, called its isotopic mass. In the case of chlorine, chlorine-35 has a mass of around 35 u, and chlorine-37 around 37 u.

As mentioned above, note that the atomic mass of an atom is not the same as its mass number. The mass number (symbol: A) of an atom is the sum of the number of protons and the number of neutrons in the nucleus.[1]:20 Mass numbers are always whole numbers with no units. Also, relative isotopic mass is not the same as isotopic mass, and relative atomic mass (also called atomic weight) is not the same as atomic mass.

A relative isotopic mass is the mass of an isotope relative to 1/12 of the mass of a carbon-12 atom. In other words, a relative isotopic mass tells you the number of times an isotope of an element is heavier than one-twelfth of an atom of carbon-12. The word relative in relative isotopic mass refers to this scaling relative to carbon-12. Relative isotopic mass is similar to isotopic mass and has exactly the same numerical value as isotopic mass, whenever isotopic mass is expressed in atomic mass units. However, unlike isotopic mass, relative isotopic mass values have no units.

Like relative isotopic mass, a relative atomic mass (symbol: Ar) is a ratio with no units. A relative atomic mass is the ratio of the average mass per atom of an element from a given sample to 1/12 the mass of a carbon-12 atom.[5] We find the relative atomic mass of a sample of an element by working out the abundance-weighted mean of the relative isotopic masses.[3] For example, to continue the chlorine example from above, if there is 75% of chlorine-35 and 25% of chlorine-37 in a sample of chlorine,[4]

Ar=(35×75)+(37×25)100=(2625)+(925)100=3550100=35.5{displaystyle A_{r}={frac {(35times 75)+(37times 25)}{100}}={frac {(2625)+(925)}{100}}={frac {3550}{100}}=35.5}

Related pages[change | change source]

References[change | change source]

  1. ↑ 1.01.11.21.3Moore, John T. (2010). Chemistry Essentials For Dummies. Wiley. ISBN978-0-470-61836-3.
  2. ↑'atomic mass unit'. National Institute of Standards and Technology. Retrieved 2020-01-12.CS1 maint: discouraged parameter (link)
  3. ↑ 3.03.1Otter, Chris; Stephenson, Kay, eds. (2008). Salters Advanced Chemistry: Chemical Ideas (Third ed.). Heinemann. p. 17. ISBN978-0-435631-49-9.
  4. ↑ 4.04.1Salters Advanced Chemistry: Revise Chemistry For Salters AS (Second ed.). Heinemann. 2008. p. 3. ISBN978-0-435631-54-3.
  5. ↑Daintith, John, ed. (2008). A Dictionary of Chemistry (Sixth ed.). Oxford University Press. p. 457. ISBN978-0-19-920463-2.
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  • Atomic mass -Citizendium
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Molecular Weight Calculator

This online calculator you can use for computing the average molecular weight (MW) of molecules by entering the chemical formulas (for example C3H4OH(COOH)3 ). Or you can choose by one of the next two option-lists, which contains a series of common organic compounds (including their chemical formula) and all the elements. The molecular mass calculator will recognize the entered formula's, which are included in the list of organic compounds.
The calculator handles at most two different bracket levels. Make sure you enter the molecule of crystallization at last (e.g. C2HCl3O.H2O ).

!!!Lenntech BV cannot be held responsible for errors in the calculation,
the program itself or the explanation. For question or remarks please contact us.
This Calculator has been tested on Internet Explorer version 6 only,
Firefox might not show all fields correctly.


Molecular mass or molar mass are used in stoichiometry calculations in chemistry.
In related terms, another unit of mass often used is Dalton (Da) or unified atomic mass unit (u) when describing atomic masses and molecular masses. It is defined to be 1/12 of the mass of one atom of carbon-12 and in older works is also abbreviated as 'amu'.

Also, important in this field is Avogadro's number (NA) or Avogadro's constant (6.0221 x 1023).
The term 'mole' is defined in that one mole of a substance with a molecular (or atomic) mass of one (1), will have a mass of 1 gram. Or 1 mole of a substance will contain Avogadro's number of that substance. Using the above calculator you could find that e.g. a pollution of 1 gram of benzene in a certain amount of water converts to NA/78.11≈ 7.7098 × 1021 molecules polluting that water!

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