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Both stable isotopes of carbon occur in nature, carbon-12 being the overwhelming majority and carbon-13 being almost all the rest. Carbon-14 accounts for just one part per trillion of naturally occurring carbon, but we can detect its radiation.
The correct answer is option A. Carbon-12 is more abundant than carbon-13 because the average atomic mass is closer to the mass of carbon-12.The atomic mass of an element is the weighted average mass of all the isotopes of that element. The average atomic mass of carbon is 12.011 amu. This value is closer to the mass of carbon-12 than carbon-13.
Explanation: Carbon exists in several isotopes. The most common of these is carbon 12, 13, 14. All of these isotopes have the same atomic number but different mass numbers. Carbon has the atomic number of 6 which means that all isotopes have the same proton number. However, the number of neutrons is different, thus giving different mass numbers.
Atoms come in many different types: Carbon, Oxygen, Nitrogen, Sulfur, and so forth, and these different types are called elements. The number of protons in the nucleus of an atom determines what kind of element it is. Isotopes are versions of the same element, they have the same number of protons, but a different number of neutrons.
The answer is the radioactive isotope reacts in the same way as stable isotopes in the chemical reactions in the body. C-14 and C-12 are carbon isotopes used to measure the approximate age of organic remains. C-12 is stable, and it does not break down into other elements over time. C-14 is not stable. It breaks down into N-14.
Yes, carbon (atomic number 6) is a stable element with both stable and unstable isotopes. The most common stable isotope of carbon is carbon-12, which makes up about 98.9% of naturally occurring ...
Here are some key details about the stable carbon isotopes: Carbon-12 (¹²C): This is the most common carbon isotope, making up approximately 98.89% of all carbon found on Earth. It has 6 protons and 6 neutrons in its nucleus. Carbon-13 (¹³C): This isotope is less common, comprising about 1.11% of carbon on Earth.
The relative atomic mass of carbon is 12.011. The relative atomic mass of carbon can be calculated using the given abundances of its isotopes, C-12 and C-13, and following these steps: Convert the percentages of the isotopes to decimal form. C-12 abundance: 98.9% = 0.989 C-13 abundance: 1.1% = 0.011
The most abundant carbon isotope is carbon-12. The relative atomic mass of carbon is 12.011, which is extremely close to 12.0. This means that the masses C-13, and C-14 are practically negligible when contributing to the relative atomic mass of carbon. In fact, the C-12 isotope makes up 98.9% of carbon atoms, C-13 makes up 1.1% of carbon atoms, and C-14 makes up just a trace of carbon atoms as ...
Carbon-12 (C-12) is more abundant than carbon-13 (C-13). This is because carbon-12 has a lower atomic mass and is therefore more stable and abundant. The average atomic mass of carbon (12.011 amu) reflects the weighted average of the two most common isotopes, carbon-12 and carbon-13, taking into account their relative abundances in nature.