Matter and Atomic Structure

1. Matter and Atomic Structure Chap. 3 • What are elements? • How atoms combine • States of matter

2. What makes a gold atom different from a silver atom?

3. Objectives What are elements? – 3.1 • Describe the particles within atoms and the structure of atoms • Relate the energy levels of atoms to the chemical properties of elements • Define the concept of isotopes

4. Element

5. Element Substance that cannot be broken down into simpler substance by physical or chemical means.

6. Element • Element names Carbon 6 C 12.011

7. Element • Element names • Element symbols Carbon 6 C 12.011

8. Element • Element names • Element symbols • Elements are made of atoms

9. Atoms

10. Atom Smallest particle of an element.

11. Atoms • Composed of 3 particles

12. Atoms • Composed of 3 particles • Protons

13. Atoms • Composed of 3 particles • Protons • Neutrons

14. Atoms • Composed of 3 particles • Protons • Neutrons nucleus

15. Atoms • Composed of 3 particles • Protons • Neutrons • Electrons

16. Atoms • Composed of 3 particles • Atomic number

17. Atomic number Number of protons. proton neutron

18. Atomic number Number of protons. proton neutron 5

19. Atoms • Composed of 3 particles • Atomic number • Mass number

20. Mass number Sum of the number of protons and neutrons proton neutron

21. Mass number Sum of the number of protons and neutrons proton neutron 11

22. Atoms • Electrons in Energy Levels

23. Electron Energy Levels Energy levelElectron Capacity First 2 Second 8 Third 18 Fourth 32

24. Model of Oxygen

25. Self Check – Ex. 1 Draw a model of the lithium-7 atom. Include protons, neutrons, and electrons.

26. Self Check – Ex. 2 Draw a model of the chlorine-35 atom. Include protons, neutrons, and electrons.

27. Atoms • Electrons in Energy Levels • Core electrons

28. Atoms • Electrons in Energy Levels • Core electrons • Valence electrons

29. Valence electron Outermost electron found in a shell.

30. Isotopes

31. Isotopes Atoms with the same number of protons, but different numbers of neutrons.

32. Isotopes • Isotopes have different masses

33. Isotopes • Isotopes have different masses • Nature contains a variety of isotopes

34. Isotopes • Isotopes have different masses • Nature contains a variety of isotopes • Isotopes used to find atomic mass of element

35. Atomic mass The average of the masses of each isotope present for a give element.

36. Isotopes • Radioactivity

37. Radioactivity The spontaneous decay of an atom’s nucleus into a new nucleus.

38. Abundance • In Universe

39. Abundance in Universe

40. Abundance • In Universe • In Earth’s crust

41. Abundance in Earth’s Crust

42. The End

43. How atoms combine – 3.2 Objectives • Describe the chemical bonds that unit atoms to form compounds • Relate the nature of chemical bonds that hold compounds together to the physical structures of compounds • Distinguish between different types of mixtures and solutions

44. Compounds

45. Compound More than one element chemically combined.

46. Compounds • Covalent compounds share electrons

47. Compounds • Covalent compounds share electrons • Sharing electrons helps atoms get full electron set

48. Compounds • Covalent compounds share electrons • Sharing electrons helps atoms get full electron set • Sharing may not be equal: this makes polar molecules

49. Compounds • Ionic compounds transfer electrons

50. Compounds • Ionic compounds transfer electrons • When an atom gains an electron it becomes _______