From 0 to 3 isotopes per element are stable.
We don't know, we haven't discovered them all. If you include unstable ones, there are several hundred.
It has 3 stable things hahahahaahahaha
one, iodine-127
three - 16, 17, 18.
Isotopes of the same element have different number of neutrons.
Neutral isotopes are atoms of the same element which have the same number of protons and electrons, but different numbers 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.
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.
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.
Neutral isotopes are atoms of the same element which have the same number of protons and electrons, but different numbers 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.
These are the natural isotopes of C, O and H.
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!
3 stable isotopes, magnesium-24 mgnesium-25 and magnesium-26
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.
Oxygen (O) has 8 protons and 8 electrons.