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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.
What else can I help you with?
Carbon atom with atomic no of 6 and atomic mass of 12 considered isotopes of one another?
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).
How tellurium and iodine show the periodic table is not arranged on basic of increasing atomic 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.
Do you need atomic number to find atomic mass?
No, you do not need the atomic number to find the atomic mass of an element. The atomic mass is the weighted average of the masses of the isotopes of an element, whereas the atomic number is the number of protons in the nucleus.
Is a element whose common isotopic form is the basis of the atomic mass unit?
It's not just an element, it's a particular isotope of a particular element. The currently accepted standard is carbon-12, which by definition has a mass of precisely 12 atomic mass units when at rest, isolated, and in its nuclear and electronic ground states. Before 1961, the scale was based on oxygen instead, but since this standard came into being before isotopes were known, it was a bit confusing: Before 1929, or before 1961 if you were a chemist, an atomic mass unit was 1/16 of the isotopically weighted average mass of an oxygen atom. However, if you were a physicist, between 1929 and 1961 an atomic mass unit was 1/16 the mass of an oxygen-16 atom. The two definitions differed by about 0.03% - not a lot, but enough to show up in high precision work, which is the reason for the 1961 redefinition. (Originally, the mass of hydrogen was used as the standard. I can't find any information on precisely when the switch to oxygen took place, but it would almost certainly have been after 1875.)
What does the atomic mass of an element show you?
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 atom with atomic no of 6 and atomic mass of 12 considered isotopes of one another?
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).
How are isotops the same and how are they different?
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.
How tellurium and iodine show the periodic table is not arranged on basic of increasing atomic 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.
How do isotopes of a given element differ How are they similar?
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.
Do you need atomic number to find atomic mass?
No, you do not need the atomic number to find the atomic mass of an element. The atomic mass is the weighted average of the masses of the isotopes of an element, whereas the atomic number is the number of protons in the nucleus.
Is a element whose common isotopic form is the basis of the atomic mass unit?
It's not just an element, it's a particular isotope of a particular element. The currently accepted standard is carbon-12, which by definition has a mass of precisely 12 atomic mass units when at rest, isolated, and in its nuclear and electronic ground states. Before 1961, the scale was based on oxygen instead, but since this standard came into being before isotopes were known, it was a bit confusing: Before 1929, or before 1961 if you were a chemist, an atomic mass unit was 1/16 of the isotopically weighted average mass of an oxygen atom. However, if you were a physicist, between 1929 and 1961 an atomic mass unit was 1/16 the mass of an oxygen-16 atom. The two definitions differed by about 0.03% - not a lot, but enough to show up in high precision work, which is the reason for the 1961 redefinition. (Originally, the mass of hydrogen was used as the standard. I can't find any information on precisely when the switch to oxygen took place, but it would almost certainly have been after 1875.)
What does the atomic mass of an element show you?
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.
How can you identify isotopes of an element through its mass spectrum?
Isotopes of an element can be identified through their mass spectrum by observing peaks at different mass-to-charge ratios corresponding to the different isotopes. Each isotope will have a unique peak pattern due to their differing atomic masses. By comparing the peaks in the mass spectrum to known isotopic masses, isotopes can be identified.
What is isotope and show us List of atoms having isotopes.?
Isotopes are atoms of the same element with the same number of protons but different number of neutrons. Some examples of atoms with isotopes are hydrogen (protium, deuterium, tritium), carbon (carbon-12, carbon-13, carbon-14), and uranium (uranium-235, uranium-238).
Draw a label a picture of a carbon-12 atom and a carbon-14 atom What if your diagram should show electrons and their shells the nucleus protons and neutrons List the atomic number and atomic mass of e?
In a carbon-12 atom, there are 6 protons and 6 neutrons in the nucleus, with 6 electrons in two electron shells around the nucleus. In a carbon-14 atom, there are 6 protons and 8 neutrons in the nucleus, with 6 electrons in two electron shells. The atomic number for both is 6, while the atomic mass for carbon-12 is 12, and for carbon-14 it is 14.
What is the empirical formula of a hydrocarbon with 85.7 mass carbon?
* 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.
Why isn't mass number listed with each element on the periodic table?
the periodic table isn't aranged by mass because itd be much more complicated to make sense out of it and itd be inconsistent, uranium is the heaviest element but its the 12th element acording to its atomic number, also all of the gases and liquids would be all over the periodic table
