1 / 100

Alchemy Unit

Alchemy Unit. Investigation III: A Particulate World. Lesson 1: Pudding and Clouds. Lesson 2: Building Atoms. Lesson 3: Subatomic Heavyweights. Lesson 4: Life on the Edge. Lesson 5: Shell Game. Lesson 6: Go Figure. Lesson 7: Technicolor Atoms. Alchemy Unit – Investigation III. Lesson 1:

uma-terrell
Download Presentation

Alchemy Unit

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Alchemy Unit Investigation III: A Particulate World Lesson 1: Pudding and Clouds Lesson 2: Building Atoms Lesson 3: Subatomic Heavyweights Lesson 4: Life on the Edge Lesson 5: Shell Game Lesson 6: Go Figure Lesson 7: Technicolor Atoms

  2. Alchemy Unit – Investigation III Lesson 1: Pudding and Clouds

  3. ChemCatalyst • In the 5th century BCE a Greek philosopher named Leucippus and his student, Democritis, stated, “All matter is made up of particles that can be divided called atoms.” • What do you think atoms are? Unit 1 • Investigation III

  4. The Big Question • How have chemists thought about the atom through history? Unit 1 • Investigation III

  5. You will be able to: • Describe some models of an atom and explain how they differ. Unit 1 • Investigation III

  6. Notes • Atoms are extremely small particles, which cannot be seen, even with microscopes. • All matter is made up of atoms. • Scientists have created models to describe atoms. Models are similar to theories, but often include a picture or physical representation. (cont.) Unit 1 • Investigation III

  7. (cont.) • When a model is supported by scientific evidence it is often accepted by the scientific community. • Scientific evidence is a collection of observations that many people have made. Everyone agrees on the same collection of observations. • As new evidence is gathered, models are refined and changed. Unit 1 • Investigation III

  8. Activity • Purpose: This lesson will introduce you to various models for the atom that have appeared over the past two hundred years. The descriptions of five models of the atom are on a separate handout. (cont.) Unit 1 • Investigation III

  9. (cont.) • Five Models of the Atom Unit 1 • Investigation III

  10. Making Sense • Examine the date of the atomic evidence and then put the five models in the correct order of their introduction to the world of science. Unit 1 • Investigation III

  11. Notes • An atom is mostly empty space. • The rest consists of a nucleus, which is located in the very center of the atom, and electrons, which are located around the nucleus. • The nucleus is very small (it would be nothing more than a tiny speck in our drawings, if we were to draw it to scale). (cont.) Unit 1 • Investigation III

  12. Notes (cont.) • The nucleus is also very dense and consists of two types of particles—neutrons and protons. • A neutron is a neutral particle with no charge on it. • A proton is a positively charged particle. • Tightly bound together, neutrons and protons make a positively charged nucleus. (cont.) Unit 1 • Investigation III

  13. Notes (cont.) Unit 1 • Investigation III

  14. Check-In • Here is a Bohr model of a carbon atom. • List two things this model tells you about atoms. • List something this model does not tell you about atoms. Unit 1 • Investigation III

  15. Wrap-Up • All matter is made up of extremely small particles called atoms. These particles are too small to be seen even with a microscope. • Science is theoretical and dynamic. Models and theories are continually being revised, refined, or replaced with new models and theories. Unit 1 • Investigation III

  16. Alchemy Unit – Investigation III Lesson 2: Building Atoms

  17. Helium, He Berylium, Be ChemCatalyst • A Bohr model of a helium atom and a beryllium atom are given below. (cont.) Unit 1 • Investigation III

  18. (cont.) • List three similarities and three differences. • How do you think a gold atom is different from a copper atom? Unit 1 • Investigation III

  19. The Big Question • What does the periodic table tells us about the structures of different atoms? Unit 1 • Investigation III

  20. You will be able to: • Use the periodic table to identify the properties of an elements atom. Unit 1 • Investigation III

  21. Notes • Atomic number is the number of protons in the nucleus of an atom. • Mass number is the mass of an individual atom. Unit 1 • Investigation III

  22. Beryllium Atom Fluorine Atom Carbon Atom Activity • Purpose: This lesson will formally introduce you to atomic structure. (cont.) Unit 1 • Investigation III

  23. (cont.) Unit 1 • Investigation III

  24. Making Sense • If you know the atomic number of an element, what other information can you figure out about the atoms of that element? • If you know the atomic number of an element, can you figure out how many neutrons an atom of that element has? Can you come up with a close guess? Explain. Unit 1 • Investigation III

  25. Notes • Mass number is the number of protons plus the number of neutrons. • Atomic mass is the “weight” or mass of a single atom. • Atomic weight is the decimal number on the periodic table. Unit 1 • Investigation III

  26. Check-In • Use your periodic table to identify the following elements: • a) Atomic number 18 • b) Has three electrons • c) Atomic mass of 16.0 Unit 1 • Investigation III

  27. Wrap-Up • Each successive element has one more proton than the element preceding it. • The atomic number is equal to the number of protons. (cont.) Unit 1 • Investigation III

  28. (cont.) • The number of electrons is equal to the number of protons (as long as the atom is neutral). • The mass number is equal to the number of protons plus the number of neutrons (most of the mass is found in the nucleus). Unit 1 • Investigation III

  29. Alchemy Unit – Investigation III Lesson 3: Subatomic Heavyweights

  30. ChemCatalyst • A chemist investigating a sample of lithium found that some atoms have a lower mass than other atoms. The chemist determined that the structures of the two types of atoms would be similar to the two drawings below. (cont.) Unit 1 • Investigation III

  31. (cont.) • What is different about the two atoms? • What is the atomic number of each atom? • What is the mass number of each atom? • Do you think they are both lithium atoms? Why or why not? Unit 1 • Investigation III

  32. The Big Question • How do isotopes of an atom account for the atomic weight of an element? Unit 1 • Investigation III

  33. You will be able to: • Predict the isotopes of an element. Unit 1 • Investigation III

  34. Notes • Atoms of the same element that have different numbers of neutrons are called isotopes. • Atomic mass units (amu) are “invented” measurement units of the atomic mass. Unit 1 • Investigation III

  35. Activity • Purpose: In this lesson you will investigate isotopes and how they affect atomic weight. (cont.) Unit 1 • Investigation III

  36. (cont.) (cont.) Unit 1 • Investigation III

  37. (cont.) Unit 1 • Investigation III

  38. Making Sense • Explain why the atomic weights listed in the periodic table are not usually whole numbers. Unit 1 • Investigation III

  39. Notes • While the element iron is defined as being made up of neutral atoms with 26 protons and 26 electrons, not every iron atom has the same number of neutrons. • Atoms that have the same number of protons but different numbers of neutrons are called isotopes. (cont.) Unit 1 • Investigation III

  40. Notes(cont.) • What we call the atomic weight on the periodic table is actually the average atomic mass of that element’s naturally occurring isotopes. • Isotopes have similar chemical properties in that they combine with other elements to form similar compounds. (cont.) Unit 1 • Investigation III

  41. (cont.) • Atomic Weight is the weighted average of the atomic masses of different isotopes taking into account their abundance. (cont.) Unit 1 • Investigation III

  42. (cont.) Unit 1 • Investigation III

  43. Check-In • Predict the isotopes of carbon, C. Which isotope is more abundant? How do you know? Unit 1 • Investigation III

  44. Wrap-Up • Elements may have anywhere from 2 to 10 naturally occurring isotopes. • The atomic weight of an element listed on the periodic table is actually the average mass of the naturally occurring isotopes of that element. • Isotopes have the same number of protons and electrons, but different numbers of neutrons. (cont.) Unit 1 • Investigation III

  45. (cont.) • Isotopes of a single element exhibit similar properties in that they form similar compounds. • Isotopes are referred to by their mass numbers. Unit 1 • Investigation III

  46. Alchemy Unit – Investigation III Lesson 4: Life on the Edge

  47. ChemCatalyst • The three atoms below have similar reactivity and chemical behavior. • Where are these elements located on the periodic table? • What do you think might be responsible for their similar properties? (cont.) Unit 1 • Investigation III

  48. (cont.) Unit 1 • Investigation III

  49. The Big Question • What accounts for the similar chemistry of elements in the same group? Unit 1 • Investigation III

  50. You will be able to: • Give the number of valence electrons for an element. Unit 1 • Investigation III

More Related