![]() ![]() This increases the mass of nuclei with more neutrons than protons relative to the atomic mass unit scale based on 12C with equal numbers of protons and neutrons. The neutron is slightly heavier than the proton.There are two reasons for the difference between mass number and isotopic mass, known as the mass defect: For example, 63Cu (29 protons and 34 neutrons) has a mass number of 63, and an isotopic mass in its nuclear ground state is 62.91367 u. The isotopic mass usually differs for other isotopes and is usually within 0.1 u of the mass number. One unified atomic mass unit is approximately the mass of one nucleon (either a single proton or neutron) and is numerically equivalent to 1 g/mol.įor 12C, the atomic mass is exactly 12u since the atomic mass unit is defined from it. One atomic mass unit is equal to 1.66 x 10 -24 grams. The unit of measure for mass is the atomic mass unit (amu). Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance. See also: Properties of Mercury Atomic Mass of Mercury ![]() Mercury – Properties Element Mercury Atomic Number 80 Symbol Hg Element Category Transition Metal Phase at STP Liquid Atomic Mass 200.59 Density at STP 13.534 Electron Configuration 4f14 5d10 6s2 Possible Oxidation States +1,2 Electron Affinity - Electronegativity 2 1st Ionization Energy 10.4375 Year of Discovery unknown Discoverer unknown Thermal properties Melting Point -38.9 Boiling Point 357 Thermal Conductivity 8.3 Specific Heat 0.139 Heat of Fusion 2.295 Heat of Vaporization 59.229 Mercury is a heavy, silvery d-block element, mercury is the only metallic element that is liquid at standard conditions for temperature and pressure Mercury is commonly known as quicksilver and was formerly named hydrargyrum. Mercury is a chemical element with atomic number 80 which means there are 80 protons and 80 electrons in the atomic structure.
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