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Atoms: The Building Blocks of Matter

Atoms: The Building Blocks of Matter. Unit 2 Resource for Periodic Table Basics PTL! (Periodic Table Live) www.chemeddl.org/resources/ptl ). Introduction to the Atom Modern Atomic Theory Subatomic Particles Isotopes Ions. Essential Standards and objectives:

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Atoms: The Building Blocks of Matter

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  1. Atoms: The Building Blocks of Matter Unit 2 Resource for Periodic Table Basics PTL! (Periodic Table Live) www.chemeddl.org/resources/ptl)

  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. Agenda 2/10: Purpose: To determine the structure of an atom • Warm-up • Review: • Isotopes & how they are represented • Number & purpose of the subatomic particles • Calculating Average Atomic Mass • Moles –

  4. Warm-up (1) • Complete “What’s inside of atoms?”

  5. Warm-up (2) Analyze the compounds CCl₄ Al₂S₃ Count the number of atoms of each element Determine the type of compound Write its correct name. • Count the number of atoms of each element • Determine the type of compound • Write its correct name.

  6. 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?

  7. Review: What is Z? What is A? Determine the number of protons, neutrons, and electrons. In Nature, 12 C 6 6 C Carbon 12.011 Occurs 98.89% frequency 13 C 6 Occurs 1.11 % frequency

  8. Review: Average Atomic Mass • Weighted Average Mass of isotopes • Based on the percentage of each isotope present. Mass Abundance • C-12 12.0 x 98.89 = • C-13 13.0 x 1.11=

  9. Practice - Worksheet • Atomic Number & Isotopes • Correct symbol: A & Z • Complete the table • Complete the questions.

  10. Atomic Number & Isotope

  11. Practice: - worksheet • 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

  12. Find Average Atomic Mass

  13. Isotopes: Atomic Number & Mass Number

  14. Electrons in an Atom: • Review: • What determines the number? • Charge? • Mass? • Location?

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

  16. Atom: Scanning Tunneling MicroscopeDetect the negative charge of electrons

  17. Bohr - Discovery Education Video

  18. Quantum Model • Electron Cloud model of the atom

  19. Representing atoms with the Bohr model

  20. Representing atoms with the Bohr Model

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

  22. Bohr Model & the Periodic Table Making Conclusions Compare and Contrast • Why are elements placed in a group (column)? • Why are elements placed in a period (row?)

  23. Moles Counting Unit in Chemistry

  24. Agenda: • Size of Atoms • Moles: a counting unit in chemistry • What is a mole? • Why do we use moles? • Mole calculations • Factor Label Method

  25. Atoms are very, very small particles • Too small to see • To small to use an optical microscope • Use a scanning tunneling microscope that is able to detect the electron clouds (due to the negative charge of the electrons)

  26. Size of Atoms: DiameterSome estimates • Atoms including the electron cloud • 1 x 10⁻¹⁰ meters • Nucleus • 1 x 10⁻¹²m • Proton • 1 x 10⁻¹³ m (note: mass: 1x 672 x 10⁻²⁴g) • Electron • 1 x 10⁻¹⁶m

  27. Atoms are so small: 1 x 10⁻¹⁰ metersQuarks to Quasars, Powers of Ten

  28. Review: Scientific Notation:aka: exponents, power of ten, etc. • Positive exponents: • 1 x 10⁶ atoms • Negative exponents: • 1 x 10⁻⁶ atoms • Multiplying with exponents: • (1.5 x 10³ atoms) x ( 4.2 x 10⁶ atoms) • (3.4 x 10³ atoms) x (2.0 x 10⁻⁶ atoms) • Dividing with exponents: • (1.5 x 10³ atoms) / ( 4.2 x 10⁶ atoms) • (3.4 x 10³ atoms) / (2.0 x 10⁻⁶ atoms) More information: Appendix near the back of the textbook

  29. Moles Counting Unit in Chemistry

  30. Counting – alternative names for numbers Gross of pencils

  31. and

  32. When we buy these items, how do we determine the amount?

  33. Moles • Video: 4+ minutes • http://ed.ted.com/lessons/daniel-dulek-how-big-is-a-mole-not-the-animal-the-other-one • Review: • http://ed.ted.com/lessons/daniel-dulek-how-big-is-a-mole-not-the-animal-the-other-one#review • DigDeeper • http://ed.ted.com/lessons/daniel-dulek-how-big-is-a-mole-not-the-animal-the-other-one#digdeeper

  34. The Mole and Avogadro’s Number • What is a mole in chemistry? • How much is a mole? • - • - • - • When are moles used?

  35. Moles • How are they measured? (Standards) • The amount of substance that contains as many particles as there are in exactly 12 grams of C-12. • The amount of substance that contains Avogadro’s number of particles. • Molar mass – using the Periodic Table

  36. Moles • Why are moles used?

  37. Moles • http://www.youtube.com/watch?v=Qg0Lajwew3A A mole is a unit - song • http://www.youtube.com/watch?v=U1frmqkNqW0

  38. Salt particle- NaClModel of NaCl as an ionic compound Each salt particle in this photomicrograph would require the model to be multiplied by 10⁶ or more New Term Formula Unit: NaCl Represents the repeating units that make up an ionic compound Such as NaCl, CaCl, Al₂O₃

  39. Amounts:How can we determine the amount of salt particles in this picture?

  40. Mole Conversions(Factor Label Method) • Moles ↔ Grams 3.5 moles of He = ? Grams 40 grams of He = ? Moles Molar mass: 1 mole of He = ? Grams

  41. Review scientific notation Mole Conversions • Moles ↔ Particles (atoms, molecules, compounds, etc.) 3.5 moles of He = ? Atoms 12.04 x 10²³ atoms of He = ? Moles 1 mole = atoms

  42. Mole Conversions • Moles ↔ Volume of Gas (at STP) 3.5 moles of He = ? Liters 100 Liters of He = ? Moles 1 mole of a gas = Liters

  43. Mole Flow Chart Mole

  44. Practice problems: Moles and Mass • What is the mass of 0.5 moles of S? • How many grams is equivalent to 0.137 moles of Fe? • 4.63 mol P = ? grams P

  45. Practice problems • How many moles are in 84.3 grams of Si? • 50 grams of Ne = ? moles of Ne

  46. Mole and Atom Conversions • How many atoms of Al are in 2.5 moles? • How many atoms of Ag are in 0.26 moles? • How many atoms of He are in 0.0023 moles?

  47. Mole and Atom Conversion • How many moles of P contains 1.0 x 10²³ atoms? • How many moles of Au are in 2.8 x 10²º atoms?

  48. Moles, Moles, Moles Lab Sample in a jar Mass Moles Atoms 1 mole = ? grams 1 mole = ? atoms

  49. Molar Mass of Compounds Review types of compounds & names • NaClCH₄ • H₂O CO₂ • MgCl₂ MgO

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