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Atomic Structure

Atomic Structure. Define the atom Structure of the Nuclear Atom Distinguish between atoms. In groups of 7 you will research the following scientists’ ideas and contributions to the atomic model.

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Atomic Structure

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  1. AtomicStructure Define the atom Structure of the Nuclear Atom Distinguish between atoms

  2. In groups of 7 you will research the following scientists’ ideas and contributions to the atomic model. • 1. John Dalton, 2. Democritus, 3. J.J Thomson, 4. Ernest Rutherford, 5. Robert Millikan, 6. Eugen Goldstein, 7. James Chadwick • You will present your findings to the class Early Models of the Atom

  3. ? Charge ? Location ? Symbol protons What are the 3 kinds of subatomic particles? neutrons electrons

  4. 23 V 50.941 Atomic number symbol • The Number of protons (atomic number) • Atoms are electrically neutral; therefore the number of protons (+) must equal the number of electrons (-) Average Atomic mass Try these! What makes one element differ from another? 6

  5. Find the difference between the mass number and atomic number Atomic number ? # of protons 14 Si 28.086 # of electrons Average atomic mass ? Round this for mass number How do you find the # of neutrons? Mass number = Atomic number = Number of neutrons=

  6. 1.Write the symbol, place the atomic number as the subscript and the mass number as the superscript to the left of the symbol. 14 Si 28.086 Si 28 14 • Also can be written with the name of the symbol • and the mass number Shorthand notation Silicon-28

  7. A. • How many neutrons are in each atom? 16 8 O 32 16 S 108 47 Ag practice p+ = e- = n0= p+ = e- = no = p+ = e- = no =

  8. Tellurium Remember!!Atomic # = protons = electronsMass # = Protons + NeutronsNeutrons = Mass # - ProtonsProtons = Mass # - Neutrons

  9. Atoms that have the same number of protons, but different numbers of neutrons, therefore having different mass numbers • Isotopes are chemically alike due to the # of protons and electrons • There are 3 known isotopes of hydrogen. • Each isotope has one proton • Most common = hydrogen-1 or H • 2nd isotope has one neutron (mass # of 2) = _____________or hydrogen-2 or H • 3rd isotope has 2 neutrons (mass # of 3) = • ___________or hydrogen-3 or H 1 1 2 1 Isotopes 3 1

  10. Three isotopes of oxygen are oxygen-16, oxygen-17, oxygen-18. Write the symbol for each, including the atomic number and mass number. • Three isotopes of chromium are chromium-50, chromium-52, and chromium-53. How many neutrons are in each isotope, given that chromium has an atomic number of 24? 16 8 O 17 8 O 18 8 O Practice Chromium-50 = ____ neutrons Chromium-52 = ____neutrons Chromium-53 = ____ neutrons

  11. Research common isotopes (radioistopes) • Create a display over commonly used isotopes. • Include the isotope and its use • Also may include pictures, etc. Extra Credit

  12. Atomic Mass • Atomic mass unit- (amu)- • Atomic mass= Calculating the atomic mass Multiply the mass of each isotope by the natural abundance, expressed as a decimal, and then add the products

  13. Element X has 2 natural isotopes. The isotope with a mass of 10.012 amu (10X) has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu (11X) has a relative abundance of 80.09%. Calculate the atomic mass of this element knowns unknowns Practice Calculate For 10X: 10.012 amu x 0.01991= 1.993 amu For 11X: 11.009 amu x 0.8009 = 8.817 amu For element X: atomic mass =10.810 amu * Atomic mass of element X ? *isotope 10X mass = 10.012 amu rel. abun= 19.91% or 0.1991 *Isotope 11X: mass = 11.009 amu rel. abun.= 80.09% or 0.8009

  14. Practice 1. The element of copper has naturally occurring isotopes with mass number of 63and 65. The relative abundance and atomic masses are 69.2% for mass = 62.93 amu, and 30.8% for mass = 64.93 amu. Calculate the average atomic mass of copper 2. Calculate the atomic mass of bromine. The 2 isotopes of bromine have atomic masses and relative abundance of 78.92 amu (50.69%) and 80.92 amu (49.31%)

  15. periods Groups 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 1 2 3 4 5 6 7

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