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Atomic Number and Mass Number
Transcript of Atomic Number and Mass Number
More protons than electrons: positive (+ve) charge. Unless it is important to distinguish between isotopes, it is common to use only the element symbol and the Charge. Isotopes Two atoms of the same element can have different numbers of neutrons These atoms would therefore have a different mass number. Atoms of the same element that have different mass numbers are called Isotopes. Carbon has 3 naturally occurring isotopes Carbon-12 : C 12 6 The nuclide symbol is This form of carbon has 6 protons and 6 neutrons. The 12 represents the mass number. Carbon-13 : C 13 6 The nuclide symbol is 6 protons and 7 neutrons. Much rarer than carbon-12 Carbon-12 and carbon-13 are the two stable isotopes of carbon. Carbon-14 C 14 6 The nuclide symbol is 6 protons and 8 neutrons. The only naturally occurring radio-isotope of carbon. (Radioactive) Used in carbon dating. N = A - Z Atomic Mass Units (amu or u) Defined using the mass of the carbon-12 atom. 1 carbon-12 atom has a mass of 12 amu 1 proton has a mass of approximately 1.007 amu 1 neutron has a mass of approximately 1.009 amu 1 amu is exactly 1/12 the mass of a carbon atom. Every element has a unique symbol. Many element symbols begin with the first letter of the element. MANY DON'T... Some symbols have two letters (second is lowercase). O 16 8 2- 8 -2 = - x No. of electrons = 10 electrons no. of protons charge = 8 x = + 2 - no. of electrons