If your asking "how does the mass show there are isotopes", then the answer is this: Isotopes are found by using a mass spectrometer, and the abundance (percent amount) of each isotope is determined. Using this percent of abundance, the AVERAGE mass is reported on the Periodic Table. For example, if carbon 12 had mass of 12 and carbon 13 had mass of 13, but the percent abundance of 12 was 99% and the abundance of 13 was 1%, then the atomac mass would be
12*.99+13*.01=12.01
You can tell it has isotopes by seeing that the mass is a decimal and not a whole number. It is harder to tell with carbon, because it's only off by .01, but looking at chlorine it is more clear. Most isotope weights are very close to being whole numbers, like Cl35 mass is 34.98 and Cl37 is 36.97. But looking at Cl atomic weight, it is 35.45; the .45 tells you it is a average because the value lies between the whole numbers as a decimal. Cl is 35.45, which is an average of 35 and 37 that's 76% and 24% abundance respectively.
No. A carbon atom has both an atomic number and an atomic mass. All carbon atoms have an atomic number of 6. The most common carbon atom has an atomic mass of 12. See the Related Questions for more information about carbon, isotopes and atomic number and atomic mass.Go to Answers.com and punch in "carbon isotopes" and it will show you various isotopes and the atomic mass (u) associated with each (shown as isotopic mass).
They show that the periodic table isn't arranged on the basis of increasing atomic mass because iodine has a mass lesser than tellurium. Iodine has a mass of 126.90 and tellurium has a mass of 127.60.
In the modern periodic table, an atom of the isotope carbon-12 has a mass of exactly 12.0000 dalton.Until around 1970 the basis was oxygen (natural mixture of isotopes) = 16.000 dalton, but by then the inconvenience of the fact that the "natural" mixture of isotopes was somewhat variable had made this concept rather difficult to work with, and the benefits of working with a defined isotope had been recognized. Carbon-12 had a mass very close to 12 on the old scale, so its adoption as the basis meant that the older tables of atomic mass could be used without modification.
When you do the drawing; Carbon 12 has 6 neutrons whereas Carbon 14 has 8 neutrons. Other tan that they're identical.
no you do not need to know the atomic number, as that only equates to the number of protons in an atom. Most periodic charts will show you the atomic mass of an element
No. A carbon atom has both an atomic number and an atomic mass. All carbon atoms have an atomic number of 6. The most common carbon atom has an atomic mass of 12. See the Related Questions for more information about carbon, isotopes and atomic number and atomic mass.Go to Answers.com and punch in "carbon isotopes" and it will show you various isotopes and the atomic mass (u) associated with each (shown as isotopic mass).
Isotopes have same number of electrons, same atomic no. but different mass no. They are from the same element like isotopes of carbon. They are not having same number of neutrons. They show same electronic configuration.
Isotopes have same number of electrons, same atomic no. but different mass no. They are from the same element like isotopes of carbon. They are not having same number of neutrons. They show same electronic configuration.
They show that the periodic table isn't arranged on the basis of increasing atomic mass because iodine has a mass lesser than tellurium. Iodine has a mass of 126.90 and tellurium has a mass of 127.60.
In the modern periodic table, an atom of the isotope carbon-12 has a mass of exactly 12.0000 dalton.Until around 1970 the basis was oxygen (natural mixture of isotopes) = 16.000 dalton, but by then the inconvenience of the fact that the "natural" mixture of isotopes was somewhat variable had made this concept rather difficult to work with, and the benefits of working with a defined isotope had been recognized. Carbon-12 had a mass very close to 12 on the old scale, so its adoption as the basis meant that the older tables of atomic mass could be used without modification.
When you do the drawing; Carbon 12 has 6 neutrons whereas Carbon 14 has 8 neutrons. Other tan that they're identical.
no you do not need to know the atomic number, as that only equates to the number of protons in an atom. Most periodic charts will show you the atomic mass of an element
The Atomic Mass is the total mass of all the sub atomic particles (i.e. the mass of the whole atom): Electrons, Neutrons and Protons. Therefore, it identifies isotopes (as they have different number of sub atomic particales - even for the same element) and thus total mass differs. There can be a fair amount of difference between the Atomic Mass of the most common isotope of an element and its Atomic Weight - which is averaged (weighted average). This makes a difference for single atom calculations, but makes little real difference in bulk calculations.
* Carbon = 79.9g, hydrogen = 20.1g (work out the mass of each element) * 79.9/12 = 6.66, 20.1/1 = 20.1 (divide mass by atomic mass number) * Ratio = 6.66 : 20.1 = 1:3 (simplify to find lowest ratio) * Therefore the simplest ratio and the empirical formula is CH3.
Different atoms of the same element possessing different atomic masses but having same atomic number are known as Isotopes. Since the isotopic atoms have the same atomic number, they must contain an equal number of protons. As their atomic masses are different, there must be a difference in the number of neutrons they possess. They will show similar chemical properties but their physical properties will be different due to different masses.
if you are referring to the isotope number and the hyphen isn't making the six negative rather than just connecting it to the word lithium, then the atomic mass would be 6, if you are meaning to show the negative 6 as the ion, let me first start off by saying that a negative 6 ion would not affect the atomic mass on an atom because the atomic mass is not influenced by electrons, which is what forms ions, this is because an electron is very small, and about 1/1,800 the weight of an atom, it is approximate, but that is the general area
Uranium has many isotopes and each isotope has a different number of neutrons (N). N = atomic weight of the isotope - atomic number of uranium (A=92) The number of neutrons of the isotope 92U238 is 238-92=146 and the number of neutrons of the isotope 92U235 is 235-92=143.