From 0 to 3 isotopes per element are stable.
Isotopes of the same element have different number of neutrons.
The element with atomic number eight is oxygen, and anyatom of oxygen is an isotope. Let's see how that works.The word isotope speaks to the number of neutrons in a given atom of a given element. When we speak of oxygen, we might consider any of its isotopes, but all atoms of this element have eight protons in their nucleus. They're all oxygen, and all have atomic number eight. Oxygen has three stable isotopes, and they are O-16, O-17 and O-18. All atoms of these isotopes have eight protons in them, but they have eight, nine and ten neutrons in their nuclei, respectively.
Two different neutral isotopes of the same element have the same number of protons in their nucleus, which determines the element's identity. The isotopes differ in the number of neutrons they have, which leads to variations in atomic mass but not in chemical properties.
What is the average mass of an element's naturally occurring atom or isotopes?The average mass of an element's naturally occurring isotopes is the sum of the (isotope's atomic mass * % Natural abundance)Below are the 3 naturally occurring isotopes of Oxygen and their % Natural abundance.O-16 15.99491463 99.757%O-17 16.9991312 0.038%)O-18 17.9991603 0.205%Now multiply and find the average atomic weight of OxygenO-16 (15.99491463 * .99757) = 15.95605O-17 (16.9991312 * 0.00038) = 0.00646 O-18 17.9991603 * 0.00205) = 0.036898Sum =15.95605 + 0.00646 + 0.036898 = 15.9994My periodic table has the atomic mass of Oxygen as 15.999. Yee Haw!
An isotope is one of two or more atoms with the same atomic number but different atomic weights because of having more or less neutrons. An isomer is a molecule of a compound that exists in more than one form, each form having different arrangements of atoms but the same molecular weight.
The 103rd element on the periodic table is Lawrencium (Lr). It is a synthetic element and is named after Ernest O. Lawrence, a physicist who invented the cyclotron. Lawrencium is a radioactive element with no stable isotopes.
Isotopes of the same element have different number of neutrons.
If you mean oxygen: like most elements, it has both stable isotopes, and unstable (i.e., radioactive) isotopes. 16O, 17O and 18O are stable; the unstable (radioactive) isotopes include 15O and 14O.
These are the natural isotopes of C, O and H.
The element with atomic number eight is oxygen, and anyatom of oxygen is an isotope. Let's see how that works.The word isotope speaks to the number of neutrons in a given atom of a given element. When we speak of oxygen, we might consider any of its isotopes, but all atoms of this element have eight protons in their nucleus. They're all oxygen, and all have atomic number eight. Oxygen has three stable isotopes, and they are O-16, O-17 and O-18. All atoms of these isotopes have eight protons in them, but they have eight, nine and ten neutrons in their nuclei, respectively.
Two different neutral isotopes of the same element have the same number of protons in their nucleus, which determines the element's identity. The isotopes differ in the number of neutrons they have, which leads to variations in atomic mass but not in chemical properties.
Natural oxygen isotopes are: O-16, O-17, O-18.
What is the average mass of an element's naturally occurring atom or isotopes?The average mass of an element's naturally occurring isotopes is the sum of the (isotope's atomic mass * % Natural abundance)Below are the 3 naturally occurring isotopes of Oxygen and their % Natural abundance.O-16 15.99491463 99.757%O-17 16.9991312 0.038%)O-18 17.9991603 0.205%Now multiply and find the average atomic weight of OxygenO-16 (15.99491463 * .99757) = 15.95605O-17 (16.9991312 * 0.00038) = 0.00646 O-18 17.9991603 * 0.00205) = 0.036898Sum =15.95605 + 0.00646 + 0.036898 = 15.9994My periodic table has the atomic mass of Oxygen as 15.999. Yee Haw!
What is the average mass of an element's naturally occurring atom or isotopes?The average mass of an element's naturally occurring isotopes is the sum of the (isotope's atomic mass * % Natural abundance)Below are the 3 naturally occurring isotopes of Oxygen and their % Natural abundance.O-16 15.99491463 99.757%O-17 16.9991312 0.038%)O-18 17.9991603 0.205%Now multiply and find the average atomic weight of OxygenO-16 (15.99491463 * .99757) = 15.95605O-17 (16.9991312 * 0.00038) = 0.00646 O-18 17.9991603 * 0.00205) = 0.036898Sum =15.95605 + 0.00646 + 0.036898 = 15.9994My Periodic Table has the Atomic Mass of Oxygen as 15.999. Yee Haw!
Dalton's theory said that "atoms of the same element are the same as each other in terms of mass, color, and size." We know that this cannot be true because isotopes of the same element, oxygen for example O-16 and O-17, have different mass numbers (atomic mass). Dalton's theory said that "atoms of the same element are the same as each other in terms of mass, color, and size." We know that this cannot be true because isotopes of the same element, oxygen for example O-16 and O-17, have different mass numbers (atomic mass).
An isotope is one of two or more atoms with the same atomic number but different atomic weights because of having more or less neutrons. An isomer is a molecule of a compound that exists in more than one form, each form having different arrangements of atoms but the same molecular weight.
That's 12 gram / mole. The isotope carbon-12 has exactly this mass per mole (by definition). The natural mixture of carbon isotopes is near this number, too. However, there are also other isotopes that have a mass of 12 gram/mole. As you can see in http://en.wikipedia.org/wiki/Table_of_nuclides_(complete), this includes isotopes of Li, Be, B, C, N, O.