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How it is different a.m.u of carbon isotopes?
The atomic mass unit (amu) of a carbon isotope refers to the average mass of carbon atoms within that isotope relative to the mass of a carbon-12 atom. Carbon has several isotopes, including carbon-12, carbon-13, and carbon-14. The difference in amu values for carbon isotopes is due to the presence of different numbers of neutrons in the nucleus, which affects the overall mass of the isotope.
What is the atom with same atomic number but different mass number?
We can find atomic mass and mass number in chemical elements. Atomic mass is about weight of the atom. Mass number is about total of neutrons and protons.
Two atoms with the same atomic number but different atomic weight?
Two atoms with the same atomic number but different atomic weight are known as isotopes. Isotopes have the same number of protons and electrons, but a different number of neutrons, resulting in different atomic weights. For example, carbon-12 and carbon-14 are isotopes of carbon with the same atomic number (6) but different atomic weights due to a difference in neutron count.
What has a different mass number than the normal atom?
We can find atomic mass and mass number in chemical elements. Atomic mass is about weight of the atom. Mass number is about total of neutrons and protons.
In what way are two isotopes of the same element different?
An isotope is simply a certain element with a different atomic mass, for example carbon 12 is the same element as carbon 13 because it has the same number of protons, but it has an atomic mass of 12 because it has a different number neutrons. On the periodic table, the atomic mass labeled is normally the average atomic mass, or the mass of the most stable isotope. So to answer your question two different isotopes of the same element have a different number of neutrons, but the same number of protons and electrons.
What is the same in isotopes?
isotopes always have the same? mass # & atomic #, or atomic # and atomic weight, or atomic # but different mass #'s
What are three isotopes and isobars of carbon?
isotopes of carbon are atomic no. 6 mass 12 , atomic no.6 mass 13 , atomic no. 6 mass 14
Atoms of an element with different atomic names but the same atomic number?
Atoms of an element with different atomic names but the same atomic number refer to isotopes. Isotopes are variants of a particular chemical element that have the same number of protons (and thus the same atomic number) but different numbers of neutrons, leading to different atomic masses. For example, carbon-12 and carbon-14 are both isotopes of carbon, with atomic number 6 but differing in mass due to their neutron counts. These isotopes can exhibit different physical properties and stability.
Which isotopes of uncharged elements have different numbers?
Isotopes of uncharged elements have the same number of protons (which determines the element), but different numbers of neutrons. For example, carbon-12 and carbon-14 are isotopes of carbon with different numbers of neutrons but the same number of protons.
What does the symbol of isotopes of the same element look like?
Isotopes have different masses, so the superscript preceding the symbol will be different. An example could be carbon with atomic mass 12 and carbon with atomic mass 14. 12C and 14C with the 12 and 14 being superscripts, identifies the different isotopes.
Carbon 12 and carbon 14 are examples of?
Carbon 12 and carbon 14 are isotopes of carbon. Isotopes of an element have the same number of protons but different numbers of neutrons, resulting in variations in their atomic mass.
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).
