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Atoms: The Building Blocks of Matter

Atoms: The Building Blocks of Matter. Unit 2. Introduction to the Atom Modern Atomic Theory Subatomic Particles Isotopes Ions. Essential Standards and objectives: 1.1.1 Analyze the structure of atoms, isotopes, and ions. 1.1.2 Analyze an atom in terms of the location of electrons.

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Atoms: The Building Blocks of Matter

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  1. Atoms: The Building Blocks of Matter Unit 2

  2. Introduction to the Atom • Modern Atomic Theory • Subatomic Particles • Isotopes • Ions • Essential Standards and objectives: • 1.1.1 Analyze the structure of atoms, isotopes, and ions. • 1.1.2 Analyze an atom in terms of the location of electrons. • 1.1.3Explain the emission of electromagnetic radiation in spectral form in terms • of the Bohr model. • 1.1.4 Explain the process of radioactive decay using nuclear equations and half-life. • 2.2.5 Analyze quantitatively the composition of a substance. (Introduction to moles)

  3. The Atom: Smallest particle of an element that retains the chemical properties of the element. Essential Questions: What is an atom? What is its structure? What determines properties of an element?

  4. Atoms act in orderly, predictable ways.

  5. PHET Build an Atom • Use this in the search window • Share a computer with a partner • Individual work (write your answers on a separate paper) • http://phet.colorado.edu/en/simulation/build-an-atom

  6. Explain: How does this graphic demonstrate the characteristics of an atom? Make sure that you include each graphic (portions) in your explanation

  7. Reading: Cornell notes Essential questions: What are the characteristics of an atom? In your notes: address both individual atoms and atoms of an element

  8. Modern Atomic Theory • All matter: • Atoms of a given element: • Atoms cannot be created nor destroyed in: • In chemical reactions, atoms are

  9. Atomic Theory (cont.) • To form compounds: Law of Definite Proportions Law of Multiple Proportions

  10. Summary Table: Atomic Structure- Subatomic Particles SubatomicLocationChargeMassImportance ParticleAMU

  11. Designation of Atomic Structure • Atomic number (Z): • On the Periodic Table: • Mass number (A): • On the Periodic Table:

  12. Representing atoms • Information from symbols and the Periodic Table

  13. What does this symbol tell us? Protons: Neutrons: Electrons:

  14. 20 Ca 40.08 Designations for the Atomic Structure Atomic number (Z): • On the Symbol • On the Periodic Table Mass number (A): • On the Symbol • On the Periodic Table

  15. Review: What is Z? What is A? Determine the number of protons, neutrons, and electrons. 31 Ga Gallium 69.72 32 Ge Germanium 72.61

  16. Periodic Table: an Important Tool in Chemistry but no set rules for what is included and where 16 S 32.06 S 16 32.06 How can we tell which is the atomic number and the mass number?

  17. AMU = relative measurement and used for comparison Atomic Mass Unit AMU The “amu” is defined as one twelfth of the mass of an atom of carbon-12  (with 6 protons and 6 neutrons) and has a value of 1.660538921×10−27kg.

  18. Organization of the Periodic Table • Columns – Groups • All the elements have similar chemical and physical properties • All will chemically react in a similar way • Names of groups • Rows – Periods • Elements have same number of energy levels

  19. Isotopes

  20. Isotopes

  21. Isotopes: • Atoms of an element with different masses • Naturally occurring • Some are stable and some are radioactive (unstable) • Isotopes of an element have the same number of ___________ and a different number of ______________.

  22. Identifying Isotopes • Isotope Notation 1. 2. On the Periodic Table, the number with the Decimal point is:

  23. Atoms of the Same Element

  24. Atoms of the Same Element

  25. Atoms of the Same Element

  26. Atomic Mass • Weighted Average Mass of isotopes • Based on the percentage of each isotope present.

  27. Grades are often computed using a weighted average. • Suppose that homework counts 10%, quizzes 20%, Labs 10% and tests 60%. • If: homework grade is 92 quiz grade is 68 lab grade is 88 test grade is 81 What’s the overall grade?

  28. Practice • Atomic Structure • Identify the number of proton, neutron, & electrons of an atom of a specific element • Rounding the atomic mass on the Periodic Table gives the mass of the most common isotope • Atomic Number & Isotopes • Correct symbol: A & Z • Complete the table • Complete the questions.

  29. Practice: • Find the Average Atomic Mass • Nucleus of each atom is represented • Graphic below #4 - explains #5-7 • Isotopes: Atomic Number & Mass Number • Determine based on the chart – not the PT • 2 Isotope notations • Element – A (X-A) A ZX

  30. Find Average Atomic Mass

  31. Atomic Number & Isotope

  32. Isotopes: Atomic Number & Mass Number

  33. What is the atomic mass of Nitrogen given: • N-14 is 99.64% of all nitrogen • N-15 is 0.36% of all nitrogen

  34. What is the atomic mass of Indium if: • In-113 is 4.24% • In-115 is 95.72%

  35. Calculate % Abundances from Masses • Requires the use of 2 equations and 2 unknowns. • Isotope 1(X) + Isotope 2(Y) = Atomic Mass • X + Y = 1 • Substitute and solve for X or Y!

  36. What are the percent abundances of Vanadium if • V-50 + V-51 = 50.94 amu

  37. What are the percent abundances for Gallium if: • Ga-69 + Ga-71 = 69.72

  38. Atom: Scanning Tunneling Microscope

  39. Study of atomic particles

  40. Scanning Tunneling Microscrope

  41. Development of the Atomic Theory • Essential Question: Why do elements have different properties?

  42. Here are several models of the atom as they were developed in history: ............ ...... ................ Development of the Modern Atomic Model

  43. Ancient Question

  44. Atomic investigation

  45. Bohr

  46. Quantum Model • Electron Cloud model of the atom

  47. Representing atoms with the Bohr model

  48. Representing atoms with the Bohr Model

  49. Bohr Model – Simplified but Useful Model P1 P2 P3

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