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Chemestry 1
| Proton | Carrier of positive charge, has 1,836 times as much mass as an electron, forms together with the neutrons the atomic nucleus. | |
| Electron | Carrier of negative charge, compensates positive charge of the atomic nucleus, fills a space that is 100,000 times larger than that of the atomic nucleus. | |
| Neutron | Electrically neutral, roughly the same weight as a proton has, is contained in all atomic nuclei except hydrogen, 1 to 1.5 times as often as protons. | |
| Ion | By too many negative or too few, or no electrons, positively charged particles, can consist of one or more atoms. | |
| Elementary charge | Smallest charge of free particles. Each occurring charge is an integer multiple of the elementary charge. | |
| Atomic number | Number of positive elementary charges, corresponds to the number of protons in the atomic nucleus. | |
| Mass number | Sum of the protons and neutrons of the atomic nucleus corresponds to atomic mass, which is negligible to that of the other particles and electrons. | |
| Isotop | Atoms, the number of which is the same and the mass number different by the number of neutrons. | |
| Atomic mass | Not absolute, only relatively determinable, approximately integral to the hydrogen atom, more precisely: a twelfth of a certain carbon isotope. | |
The term 'mole' is an abbreviation of 'moles' (lat.) and meens an amount or quantity. It was first used by Amedeo Avogadro (1776-1856). He probably wanted better to imagine the size of the smallest particles known so
far. And not only approximately, but precisely. Thus the so-called Avogadro's number (Avogadro constant) occurred.
This is the number, of course, referred to the element with the smallest atomic mass, the hydrogen. They are, incidentally, in two versions.
1. Its mass
1,66 * 10-27 kg/parts
1,66 * 10-
24 g/parts. | |
If 1 gram is divided by this number, the more known number of particles is generated in one gram.
| 2. Its number | 602.200.000.000.000.000.000.000
= 6,022 * 1023
(602 three thousand trillions) |
And as all atomic masses (see above), with slight deviations, are an integral multiple of those of hydrogen, we can now determine the number of particles in all atoms. Finally, an isotope of carbon with 6
neutrons has been agreed as an SI unit.
And since all atomic masses (see above), with slight deviations, are an integral multiple of those of hydrogen, we can now determine the number of particles in all atoms. Finally, an isotope of carbon with 6
neutrons has been agreed as an SI unit. One must now take a twelfth and is again with very slight deviation in the Avogadro constant. 02/17
In the first video is claimed, with 602 Trilliarden Marshmallows one could fill the globe completely.
And what volume has 1 gram of hydrogen?
M = 2,01588 g/mol
m = 1g
n = m/M = 1 g/2,01588 g/mol = 0,496 mol
The molar volume Vm is always the same for all gases. It is 22.73 liters/mol at 0°C and 1013 hPa.
V = n * Vm = 0,496 mol * 22,73 liters/mol = 11,274 liters
(Slightly more than the content of a normal bucket.)
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