Element |Symbol |Atomic # |Mass # |#Protons |#Electrons |#Neutrons | |Iron |Fe |26 |26+26=52 |26 |26 |26 | |Copper |Cu |29 |29+29=58 |29 |29 |29 | |Sodium |Na |11 |11+11=22 |11 |11 |11 | |Magnesium |Mg |12 |12+12=24 |12 |12 |12 | |Chlorine |Ci |17 |17+17=34 |17 |17 |17 | |Fluorine |F |9 |9+9=18 |9 |9 |9 | |Carbon |C |6 |6+6=12 |6 |6 |6 | |Hydrogen |H |1 |1+0=1 |1 |1 |0 | |Oxygen |O |8 |8+8=16 |8 |8 |8 | |
2-Define Isotopes give two examples of isotopes
An isotope is a variant on an element that has a different atomic weight from other variants. Except for hydrogen —this has only a proton. All atoms of an element have the same atomic number. However, some of the atoms of that element differ in mass number because they have different numbers of neutrons, though they behave identically and have the same number of protons. For example, a nitrogen atom has 7 protons and its common isotope has 7 neutrons while a radioactive isotope of the same element has 9 neutrons! Another example is carbon, where we see three isotopes of the element, Carbon-12, Carbon-13, and Carbon-14 with mass numbers 12, 13 and 14. The atomic number of carbon is 6 so that every carbon atom has 6 protons. The numbers of neutrons of these isotopes are 6, 7 and 8.
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