what does atomic mass represent?
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The atomic mass of a chemical element is the mass of an atom at rest, most often expressed in unified atomic mass units. The atomic mass is often synonymous with relative atomic mass, average atomic mass and atomic weight; however, it is subtly different in that it can either be the abundance-weighted average of isotope masses of an element or the mass of a single isotope.\n\nThe relative atomic mass (also known as atomic weight and average atomic mass) is the average of the atomic masses of all the chemical element's isotopes as found in a particular environment, weighted by isotopic abundance. Periodic tables usually list these with reference to the local environment of Earth's crust and atmosphere. An uncertainty in parenthesis is often included. For artificial elements the nucleon count of the most stable isotope is listed in brackets as the atomic mass
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the R.A.M. is the average mass of an atom of an element, taking account of its natural isotopes & their percentage abundance.\neg: the R.A.M. of CaCl2  :\n     the exam paper will give you the the R.A.M. s of Calcium-40 & Chlorine - 35.5,so the answer is,\n         = (1*40)+(2 * 35.5)\n         = 40+71\n         = 111\n     hope this helped.Cheerz!
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To calculate atomic mass of an element, it is just a weighted average of the naturally occuring isotopes.  For example:\n\nIf element A has two isotopes, A-23 and A-24, the masses are 23.5 and 24.5 respectively, and the percentage abundance is 93.0% for A-23 and 7.00% for A-24, you would:\n\nMultiply mass of A-23 (23.5g) to the decimal of the percentage (ie.  93.0%/100 = .930).  You would then do the same thing with A-24, and now you will have two numbers.  The final step, you sum the two numbers you obtained by the previous calculations.\n\nI know this is a general example with a made up element and made up numbers, but it is all that comes to mind when I read your question.  I hope this helps.
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The mass of the planet Earth is 5.97 * 1024 kilograms (from Ask.com)\n\nMass From Wikipedia, the free encyclopedia\nJump to: navigation, search\nFor other uses, see Mass (disambiguation).\nMass is a property of a physical object that quantifies the amount of matter and energy it contains. Unlike weight, the mass of something stays the same regardless of location. In relativity, the quantity invariant mass, which is closest in content to the classical idea of mass, also does not vary between single observers in different reference frames. Mass is a central concept of classical mechanics and related subjects, and also several forms of mass appear in relativistic kinematics (see mass in special relativity).
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Atomic Mass: 58.9332 Amu
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If you have a family, why do you describe it with more than one number? The weight of the family, and the number of family members?\n\nThe number of moles is just the number of particles. The mass is the amount of material.
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Atomic Number: 47 \nAtomic Mass: 107.8682 amu \nMelting Point: 961.93 °C (1235.08 K, 1763.474 °F) \nBoiling Point: 2212.0 °C (2485.15 K, 4013.6 °F) \nNumber of Protons/Electrons: 47 \nNumber of Neutrons: 61 \nCrystal Structure: Cubic \n\nNumber of Energy Levels: 5 \n\nFirst Energy Level: 2 \nSecond Energy Level: 8 \nThird Energy Level: 18 \nFourth Energy Level: 18 \nFifth Energy Level: 1
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Take a look at any good Periodic Table of the Elements.  Here's a good one:\n\nhttp://www.webelements.com/\n\nThe number given under atomic weight. is given in standard atomic mass units (defined by taking the mass of a carbon-12 atom, and dividing it by 12).  For all practical purposes, we can assume that it is the mass of a proton/neutron (which again, for all practical purposes, we can assume have the same mass; we neglect the mass of electrons because the mass of an electron is about 1/3000 that of a proton or neutron).  \n\nFor example, the atomic mass of hydrogen is 1.  This is because hydrogen consists of 1 proton orbited by 1 electron.  However, on the perodic table, you will notice that the number is actually 1.00794.  This is bcause this number is the average of all isotopes.  An isotope is an element that has a different number of neutrons.  For example, a hydrogen atom with one proton and neutron in the nucleus, and an electron orbiting it is still hydrogen, but is known as deuterium (It is still defined as hydrogen by the number of protons in the nucleus), but has an atomic mass of 2. The other isotope of hydrogen (Tritium) has 2 neutrons in the nucleus and an electron orbiting it (an atomic mass of 3). Because these isotopes are so rare, the average mass of all existing hydrogen is close to 1, but is slightly higher.\n\nYou can find mass in Kg by dividing the atomic mass by avogadro's number (6.02 X 10^23).  There are 6.02X10^23 atomic mass units in 1Kg.
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I believe you already asked that a few days ago. But here is a refresher of the best answer yoy chose.:\nChemistry is Chemistry (derived from alchemy) is the science of matter and study of inner molecules and atoms. You study metal properties, its characteristics and behaviour. You study about Organic and InOrganic Materials. You will also learn about mixing chemicals - Reactants and Products. Don't worry now, it will soon become interesting.\n\nThe atomic mass of a chemical element is the mass of an atom at rest and Atomic number (Z) is the number of protons found in the nucleus of an atom.
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Mass has energy equivalent values but to blindly say that enegy has mass is not necessarily correct.  When an atom is in tact, it has a certain mass but if you break it down into its constituent parts, you will see that the sum of the parts is less than the whole.  This is accounted for in what is called the mass defect.  This mass defect is the binding energy required to hold the atom together against the reulsive forces of like charges located in the nucleus (protons).  As an atom gets bigger, the mass defect will also increase (up to a point)
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Use the periodic table to find the atomic mass of the element and subtract from this the atomic number.  \n\nThe atomic mass is equal to sum of proton and neutrons, and the atomic number is the number of protons an atom has.  Electrons have such a small mass that they don't really have any noticable effect on the atomic mass.\n\nEx: Oxygen (atomic mass - 16, atomic number - 8)\n\n16 - 8 = 8, therefore the number of protons is equal to 8
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it describes the # of protons & electrons in that element.
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one way is that the atomic number is the same as the number of protons and the other way is to subtract the neutron by the mass
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there are many elements in the world.\nthe mass of the laptop is 5000 pounds.\nthe table there is a matter.\ni don't know what atom is
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Atoms have mass which can sometimes have volume and there are about 6.022x10^23 particles in a mole of an element. A mole of an element is the atomic mass in grams. Now, you can use all this and do some further research on the Internet and in books to write a nonfiction book on atoms and how the periodic table of the elements is set up.
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The mass is a property of an object, a fundamental measure of the amount of matter in the object. The usual symbol for mass is m and its SI unit is the kilogram.\n\nThe weight of an object is the force of gravity on the object and may be defined as the mass times the acceleration of gravity, w = mg. Since the weight is a force, its SI unit is the newton.
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7 because atomcic number(# of protons)=mass number-# of nuetrons.