ATOMIC_STRUCTURE_CORE(MAH)_(NXPowerLite) Opp

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2.1.1 State the position of protons, neutrons and electrons in the atom 2.1.2 State the relative mass and relative charge of protons, electrons and neutrons. The accepted values are: Relative Mass Charge proton 1 +1 neutron 1 0 electron 5x10 -4 -1 2.1.3 Define the terms mass number (A), atomic number (Z) and isotopes of an element. 2.1.4 Deduce the symbol for an isotope given its mass number and atomic number. Use the notation A Z X eg 12 6 C.
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2.1.5 Calculate the number of protons, electrons and neutrons in atoms and ions from the mass number, atomic number and charge. 2.1.6 Compare the properties of the isotopes of an element Isotopes have the same chemical properties but different physical properties. Examples include 1 2 3 12 14 35 37 1 H , 1 H , 1 H ; 6 C , 7 C ; 17 Cl 17 Cl . Discuss the uses of radioisotopes Examples should include 14 C in radiocarbon dating, 60 Co in radiotherapy and 131 Iodine and 125 Iodine as medical tracers Aim 7: Students should be aware of the dangers to living things of radioisotopes but also justify their usefulness with the examples above.
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NUCLIDES AND THE PERIODIC TABLE Nuclides: A = Mass Number 7 Chemical Symbol of Element Li Z = Atomic Number 3 1. What is the atomic number of an element? 2. What is the mass number of an element? 3. Write down the nuclide notation for a sodium atom that has 11 protons and 12 neutrons. 4. Is the relative atomic mass of a nuclide related to the atomic number or the mass number? 5. Which nuclide is used as the reference mass against which all relative atomic masses are measured?
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1. Write down the mole mass of this reference nuclide – remembering that although relative atomic masses have no units, the actual mole mass does! 2. How do isotopes of the same element differ? 3. Look at a copy of the Periodic table. Are all the relative atomic masses listed whole numbers? How can the existence of isotopes be used to explain the relative atomic masses that you see? 4. The mean relative atomic mass of an element is the weighted mean of all the relative isotope masses present in the sample. 5. Naturally occurring substances contain mixtures of different isotopes which can be separated by a mass spectrometer. Each isotope’s mass to charge ratio can be identified and the amount of each isotope present in the sample quantified. Applications include using mass spectra to identify where ancient metal samples were obtained and hence make deductions about trade routes.
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Learning check: Neon has two isotopes of mass number 20 and 22. They are present in the approximate ratio 9:1 or percentage abundances of 90% and 10%. Show that naturally occurring neon has a RAM of approx. 20.2
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The Periodic Table On the blank periodic table on the next slide or provided: Label or colour in the alkali metal group, the alkaline earth metal group, the halogens and the noble gases. Mark clearly the period that contains hydrogen and helium
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This note was uploaded on 11/17/2011 for the course PHYS 121 taught by Professor Burgeson during the Fall '11 term at BYU.

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ATOMIC_STRUCTURE_CORE(MAH)_(NXPowerLite) Opp - 100s of free...

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