explain with example mass number. where we use mass numbers and how to identify them?
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The mass number (symbol A) is the total number of protons and neutrons in an atom’s nucleus. To find the mass number, you count the number of protons (A) and then subtract the number of neutrons (A). For example: A carbon atom has 6 protons and 6 neutrons. Its mass number is 12.
A carbon atom has 6 protons and 6 neutrons, so its mass number is 12.
The atomic number (symbol Z) is the number of protons in an atom’s nucleus. To find the atomic number, you count the number of protons (Z) and then add 1. For example: A carbon atom has 6 protons and 6 neutrons, so its atomic number is 7.
The atomic weight (symbol W) of an element is the sum of the mass of its naturally occurring isotopes. The atomic weights of natural isotopes are weighted by their relative abundances in the Earth’s crust, with the isotope of lowest abundance being given a weighting of one and others being proportional to their natural abundance. The exception is for hydrogen, which is not present as a free element in nature.