{"id":2378,"date":"2020-11-28T11:51:55","date_gmt":"2020-11-28T06:21:55","guid":{"rendered":"https:\/\/cbselibrary.com\/?p=2378"},"modified":"2020-11-28T17:38:02","modified_gmt":"2020-11-28T12:08:02","slug":"atomic-mass","status":"publish","type":"post","link":"https:\/\/cbselibrary.com\/atomic-mass\/","title":{"rendered":"What is the atomic mass of an element?"},"content":{"rendered":"
Atomic mass<\/strong><\/p>\n \\(Atomic\\quad mass=\\frac { Mass\\quad of\\quad 1\\quad atom\\quad of\\quad the\\quad element }{ \\frac { 1 }{ 12 } of\\quad the\\quad Mass\\quad of\\quad an\\quad atom\\quad of\\quad carbon\\quad -\\quad 12\\quad \u00a0} \\) People also ask<\/b><\/p>\n Atomic Mass of Some Elements<\/b><\/strong>Gram atomic mass<\/b><\/strong><\/p>\n Gram atomic mass of an element is defined as that much quantity of the element whose mass expressed in grams is numerically equal to its atomic mass. To find gram atomic mass we keep the numerical value the some as the atomic mass, but simply change the units from u to g. for example, atomic mass of aluminium is 27 u. Its gram atomic mass is 27 g.<\/p>\n Gram atomic mass of Isotopes :<\/b><\/strong> What is the atomic mass of an element? Atomic mass Atoms are extremely small; the heaviest atoms have masses of about 10\u201322\u00a0g. Even an ultramicrobalance cannot measure the mass of a single atom. However, relative masses of atoms of different elements can be determined. At first, the mass of the lightest atom, hydrogen. The SI … Read more<\/a><\/p>\n","protected":false},"author":8,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"spay_email":""},"categories":[84],"tags":[1032,1033,1034],"yoast_head":"\n\n
\n<\/li>\nWhat is meant by AMU?<\/strong><\/h2>\n
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\nTherefore, 1 u = \\(\\frac { 1 }{ 12 } \\)\u00a0\u00d7 1.99265 \u00d7 10\u201326<\/sup>\u00a0kg
\n1 u = 1.66 \u00d7 10\u201327<\/sup> kg<\/li>\n
\n<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n
What is the formula for calculating atomic mass?<\/strong><\/h2>\n
\nExample: \u00a0 \u00a0<\/b><\/strong>The atomic mass of magnesium is 24 u which indicates that one atom of magnesium is 24 times heavier than \\(\\frac { 1 }{ 12 } \\)\u00a0of a carbon 12 atom.<\/p>\n\n
\nGram atomic mass of Isotopes =\u00a0\\(\\frac { { M }_{ 1 }{ X }_{ 1 }+{ M }_{ 2 }{ X }_{ 2 } }{ { X }_{ 1 }+{ X }_{ 2 } } \\)
\nM1<\/sub> & M2<\/sub> are relative masses of isotopes and X1<\/sub> & X2<\/sub> are relative % content
\nExample:\u00a0<\/b><\/strong>Chlorine contains two types of atoms having relative masses 35 and 37 and their relative abundance is 3 : 1. In such cases the atomic mass of the element is the average of relative masses of different isotopes of the element.
\nAtomic mass of chlorine =\u00a0\\(\\frac { 35\\times 3+37\\times 1 }{ 4 } \\) = 35.5<\/p>\n\n\n
\n S.no<\/strong><\/td>\n Element<\/strong><\/td>\n Symbol<\/strong><\/td>\n Atomic mass<\/strong><\/td>\n<\/tr>\n \n 1<\/td>\n Hydrogen<\/td>\n H<\/td>\n 1 u<\/td>\n<\/tr>\n \n 2<\/td>\n Carbon<\/td>\n C<\/td>\n 12 u<\/td>\n<\/tr>\n \n 3<\/td>\n Nitrogen<\/td>\n N<\/td>\n 14 u<\/td>\n<\/tr>\n \n 4<\/td>\n Oxygen<\/td>\n O<\/td>\n 16 u<\/td>\n<\/tr>\n \n 5<\/td>\n Sodium<\/td>\n Na<\/td>\n 23 u<\/td>\n<\/tr>\n \n 6<\/td>\n Magnesium<\/td>\n Mg<\/td>\n 24 u<\/td>\n<\/tr>\n \n 7<\/td>\n Aluminium<\/td>\n Al<\/td>\n 27 u<\/td>\n<\/tr>\n \n 8<\/td>\n Phosphorus<\/td>\n P<\/td>\n 31 u<\/td>\n<\/tr>\n \n 9<\/td>\n Sulphur<\/td>\n S<\/td>\n 32 u<\/td>\n<\/tr>\n \n 10<\/td>\n Chlorine<\/td>\n Cl<\/td>\n 35.5 u<\/td>\n<\/tr>\n \n 11<\/td>\n Potassium<\/td>\n K<\/td>\n 39 u<\/td>\n<\/tr>\n \n 12<\/td>\n Calcium<\/td>\n Ca<\/td>\n 40 u<\/td>\n<\/tr>\n \n 13<\/td>\n Iron<\/td>\n Fe<\/td>\n 56 u<\/td>\n<\/tr>\n \n 14<\/td>\n Copper<\/td>\n Cu<\/td>\n 63.5 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n Atomic Mass Problems with Solutions<\/strong><\/h2>\n
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\nSolution:<\/strong>
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\nSolution:<\/strong>
\n<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"