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For example, the three isotopes of carbon have atomic masses of 12, 13, and 14 and are named Carbon-12, Carbon-13, and Carbon-14, respectively. Each of these isotopes has the same atomic number (6 ...
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.
Example 1: What is the isotopic notation for the isotope carbon-14? From the periodic table, we see that the atomic number (number of protons) for the element carbon is #6#. The name carbon-14 tells us that this isotope's mass number is #14#. The chemical symbol for carbon is #"C"#. Now write the isotopic notation for carbon-14. #""_6^14"C"#
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.
The difference is the number of neutrons. Carbon 12, 13 and 14 are carbon isotopes, meaning that they have additional neutrons: Carbon 12 has exactly 6 protons and 6 neutrons ( hence the 12 ) Carbon 13 has 6 protons and 7 neutrons Carbon 14 has 6 protons and 8 neutrons Because molecular mass is calculated by adding the number of protons and neutrons, you could also say that the difference ...
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 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 ...
See Below Carbon has 3 isotopes. Carbon-12, Carbon-13, and Carbon-14 All of them have an atomic number of 6, which means all of them have 6 protons (if they had different numbers of protons, they'd be different elements). Since they all have 6 protons, in their elemental forms, they all have 6 electrons, too. Carbon-12: Atomic number: 6 Mass number: 12 protons: 6 electrons: 6 neutrons: 6 ...
METHOD 1. To find the average atomic mass, you take a certain number of atoms, find the total mass of each isotope, and then divide the total mass of all the atoms by the total number of atoms. Assume that you have, say, 10 000 atoms of carbon. Then you have 9893 atoms of 12C and 107 atoms of 13C. Mass ofl12C = 9893atoms × 12 u 1atom = 118 716 ...
Answer link. Because each isotope of the element HAS THE SAME NUMBER OF ELECTRONS. To a first approximation, the chemistry of an element depends on the exchange and sharing of electrons between atoms to make and break strong chemical bonds. While isotopes has different numbers of neutrons, massive, neutrally charged, nuclear particles, they ...