Topic 1-Dynamic Earth

1. Topic 1-Dynamic Earth Outcomes: By the end of this chapter you should be able to: Describe evidence that the Australian continental landmass began developing 4.1 billion years ago (byo). Explain how radioisotopes can be used to date rocks Outline geological evidence that provides information about patterns of continental movement Explain how convection currents in the asthenosphere can cause the movements of plates Explain the interaction of paltes during subduction, collision and break-up Outline the movements of Australia through geological history

2. Topic Overview There are 3 parts to this topic • Radiometric Dating • Plate Tectonics-The Birth of a Theory • Plate Interactions

3. Part 1-Lesson 1 Radiometric dating

4. Introduction There is evidence to suggest that the Australian continental landmass began developing 4.1 billion years ago. In this first part of Dynamic Earth, you will be looking at the sort of evidence that leads scientists to this conclusion. The discovery of radioactivity around 1900 was a huge step forward in this understanding.

5. Atomic Structure To understand why some elements are radioactive, you must understand the structure of an atom. Structure of an Atom: • Nucleus • Protons • Neutrons • Electrons

6. Nucleus The Nucleus is the central part, or core of an atom and contains protons and neutrons. Protons: positively charges Neutrons: No charge, neutral As a result, the nucleus has an overall positive charge. Protons and neutrons have approximately the same mass.

7. Electrons Electrons are quite different in a number of ways. They: • Orbit the nucleus • Carry a negative charge • Are much lighter than protons and neutrons (less dense) In a neutral atom, the number of electrons orbiting the nucleus equals the number of protons.

8. Atomic Number Elements are characterised by the number of protons present in the nucleus. We call this the atomic number. It is this atomic number that is used to arrange the elements on the periodic table.

9. Atomic Mass We already know the majority of the mass of an atom is in the nucleus. The atomic mass of an atom is obtained by adding the number of protons and neutrons together. This is a diagram representing Helium. This atom has 2 protons, 2 neutrons and 2 electrons. What is the atomic mass of helium?

10. Atomic Mass-continued The number of protons in the nucleus of an atom never varies. However the atomic mass of an atom can vary. Remember: atomic mass = protons + neutrons. Question: If the number of protons cannot vary, what do you think causes the variation in mass?

11. Isotopes Isotopes are varying types of atoms for the one element. The variation is in the number of neutrons and therefore the mass of the atom. Isotopes of an element have the same number of protons and are therefore placed in the same position in the Periodic Table.

12. Isotopes-continued Lets look at an Example: Lead (Pb) All lead atoms contain 82 protons in their nucleus and therefore have an atomic number of 82. However, using a mass spectrometer , it has been found that lead has four different variations, each having a different mass. This variation in mass is caused by a variation in the number of neutrons in their nucleus.

13. Isotopes-continued The four lead isotopes are: • Lead 204 • Lead 206 • Lead 207 • Lead 208 The number refers to the atomic mass of each atom Complete the table

14. Summary • Protons (in nucleus): positive charge: Atomic number • Neutrons (in nucleus): no charge • Electrons (orbits around nucleus): Negative charge • Protons+Neutrons=nucleus=atomic mass • Isotopes=Same element with different number of neutrons

15. Homework • Read pages 116-117 Prelim Spotlight Text • Start Electronic Vocab list of bold terms in Reading Eg: Dynamic Earth Vocab List • Proton: Lie in the central nucleus of an atom and have a positive charge. • Etc…

16. Part 1-Lesson 2 Radioactivity

17. Review • Protons (in nucleus): positive charge: Atomic number • Neutrons (in nucleus): no charge • Electrons (orbits around nucleus): Negative charge • Protons+Neutrons=nucleus=atomic mass • Isotopes=Same element with different number of neutrons

18. Introduction As stated in the previous lesson, the number of protons in the nucleus of a stable atom never varies. However, all atoms are not stable, particularly the larger heavier atoms such as uranium and thorium located at the bottom of the Periodic Table.

19. Radioactivity Unstable atoms can emit protons and neutrons from their nuclei and break down to form different elements. An unstable atom is said to be radioactive.

20. What makes an atom Radioactive? To understand what an unstable or radioactive atom is we must look again at the structure of the nucleus. Remember the nucleus has an overall positive charge because it is made up of protons (+) and neutrons (= no charge)

21. What makes an atom Radioactive? It would be expected that the protons in a nucleus would be repelling against each other because they have the same charge.

22. What makes an atom Radioactive? Why these protons are held together in the nucleus is still not fully understood but it is thought that an enormous amount of energy is used to hold these protons together and that the neutrons have something to do with it.

23. What makes an atom Radioactive? If the nucleus breaks apart, some of this energy is released in the form of radiation. This is what happens in an unstable atom.

24. Radiation and Decay The nuclei of unstable atoms can emit (give off) or radiate protons and neutrons in two forms: • Alpha • Beta

25. Radiation and Decay • An Alpha particle consists of two protons and two neutrons. A stream of these particles is know as: Radiation Question: What would the mass of an particle be?

26. Radiation and Decay • An particle has an atomic number of 2 (2 protons) and an atomic mass of 4 (2 protons+2 neutrons) KEY CONCEPT: Every time an unstable or radioactive atom emits an particle, its atomic mass decreases by 4 and its atomic number decreases by 2.

27. Radiation and Decay

28. Radiation and Decay Not only can large and heavy atomic nuclei result in an unstable atom, nuclei that have to many neutrons for the number of protons can also be unstable. If a nuclei has to many neutrons, these excess neutrons change into protons and as a result electrons are then emitted. These emitted particles are called particles.

29. Radiation and Decay Atoms that emit radiation increase the number of protons in their nucleus at the expense of neutrons. How will this effect the atom’s: Atomic Mass: (Stay the same) nothing is lost, only changed. Atomic Number: (goes up by 1) neutrons are changed into protons

30. Radiation and Decay

31. Homework • Read Pages 117-119 Prelim Spotlight Text • Update vocab list • Complete DOT Point 1.1 pg85

32. Part 1-Lesson 3 Half-lives and Dating rocks

33. Radiation and Decay In the previous chart, uranium-238 decays to the more stable lead-206. Below is a list of other examples of atoms decaying to become more stable : • Uranium-235 to lead-207 • Thorium-232 to lead 208 • Rubidium-87 to strontium-87 • Potassium-40 to argon-40 • Carbon-14 to nitrogen-14 In these examples, the unstable atoms on the left are called the parent material and the more stable atoms on the right are called the daughter product or remnant isotope.

34. Determining ages from half-lives The time taken for each of the parent atoms to decay to their daughter products varies from millions of years to minutes. KEY CONCEPT: The time taken for half of the parent material to decay into its daughter product is know as the Half Life of that parent material.

35. Determining ages from half-lives The half-life for each radioactive element remains the constant. For example it takes 5370 years for half a sample of carbon-14 to decay to nitrogen-14

36. Determining ages from half-lives It will take another 5370 years for half the remaining carbon-14 to decay into nitrogen-14. This is known as the second half-life. This means it has taken 10740 years for ¾ of the original carbon-14 to decay. (two half-lives)

37. Determining ages from half-lives • This diagram shows the relationship between half-life and amount of radioactive parent material

38. Dating Rocks KEY CONCEPT: Using the half-lives from radioactive elements to calculate age is known as radiometric dating. Dating rocks using radioactive elements can indicate a particular time of formation.

39. Dating Rocks When minerals in igneous rocks are first formed after cooling, the amount of each radioactive mineral present at this time is 100% Immediately after formation these unstable radioactive minerals begin to break down

40. Dating Rocks Think about this: If you were given two samples of rock, one sample containing 95% of the original radioactive parent element and the other sample had 30% of the same original radioactive parent element, which of these rocks do you think would be oldest? Why?

41. Dating the oldest rocks in Australia Radiometric dating methods have enabled scientists to determine the time of mineral formation of some of the oldest rocks on Earth. The oldest minerals ever dated in Australia are zircon crystals found in quartzite rock at Mt. Narryer in the Murchison region of Western Australia.

42. Dating the oldest rocks in Australia

43. Methods Used to Date Precambrian Rocks The correct types of radiometric isotopes have to be used to date Precambrian rocks. Precambrian time starts about 4.7 billion years ago when the Earths crust began to form to the start of the Cambrian about 542 million years ago.

44. Methods Used to Date Precambrian Rocks Because the Precambrian dates back to far, uranium/lead isotopes are used to date rocks within this period of time. Naturally occurring uranium contains two radioactive isotopes both with very long half-lives. Uranium usually occurs as trace elements in minerals such as zircon.

45. Homework • Complete DOT Point 1.2, 1.3 and 1.4 • Complete activity 4.2 pg 120 Prelim Spotlight Text • Update vocab list