1. Intro to Chemistry 9.29.15

2. Chemistry: The study of

3. Chemistry: The study of matter Matter:

4. Chemistry: The study of matter Matter: Anything with mass that takes up space

5. The Atom Atom: Smallest differentiable unit of matter – Composed of

6. The Atom Atom: Smallest differentiable unit of matter – Composed of protons, neutrons, and electrons

7. Subatomic Particles Neutron: – Found in the

8. Subatomic Particles Neutron: – Found in the nucleus – Charge of

9. Subatomic Particles Neutron: – Found in the nucleus – Charge of 0 – Mass of

10. Subatomic Particles Neutron: abbr? – Found in the nucleus – Charge of 0 – Mass of 1 amu (atomic mass unit)

11. Subatomic Particles Neutron: n 0 – Found in the nucleus – Charge of 0 – Mass of 1 amu (atomic mass unit)

12. Subatomic Particles Proton: – Found in

13. Subatomic Particles Proton: – Found in the nucleus – Charge of

14. Subatomic Particles Proton: – Found in the nucleus – Charge of +1 – Mass of

15. Subatomic Particles Proton: – Found in the nucleus – Charge of +1 – Mass of 1 amu

16. Subatomic Particles Proton: p + – Found in the nucleus – Charge of +1 – Mass of 1 amu

17. Subatomic Particles Electron: – Found

18. Subatomic Particles Electron: – Found orbiting the nucleus at a great distance – Charge of

19. Subatomic Particles Electron: – Found orbiting the nucleus at a great distance – Charge of -1 – Mass of

20. Subatomic Particles Electron: – Found orbiting the nucleus at a great distance – Charge of -1 – Mass of 0 amu (not actually zero, but mass is so small that it is ignored)

21. Subatomic Particles Electron: e - – Found orbiting the nucleus at a great distance – Charge of -1 – Mass of 0 amu (not actually zero, but mass is so small that it is ignored)

22. Electron Orbitals Electrons orbit the nucleus in discrete orbits or “shells” – First orbital holds

23. Electron Orbitals Electrons orbit the nucleus in discreet orbits or “shells” – First orbital holds 2 e - – 2 nd =

24. Electron Orbitals Electrons orbit the nucleus in discreet orbits or “shells” – First orbital holds 2 e - – 2 nd = 8 e - – 3 rd = 8 e - – 4 th = 10 e -

25. Electron Orbitals Electrons orbit the nucleus in discreet orbits or “shells” – First orbital holds 2 e - – 2 nd = 8 e - – 3 rd = 8 e - – 4 th = 10 e - Important: The valence electrons (outer shell) are the only important ones for forming bonds with other atoms

26. Al 13 S 283283 Aluminum 26.982

27. Al 13 S 283283 Aluminum 26.982

28. Al 13 S 283283 Aluminum 26.982 Element Symbol

29. Al 13 S 283283 Aluminum 26.982 Element Symbol Element Name

30. Al 13 S 283283 Aluminum 26.982 Element Symbol Element Name # of p + (Atomic Number)

31. Al 13 S 283283 Aluminum 26.982 Element Symbol Element Name # of p + (Atomic Number) Average atomic mass (# of p + + n 0 )

32. Al 13 S 283283 Aluminum 26.982 Element Symbol Element Name # of p + (Atomic Number) Average atomic mass (# of p + + n 0 ) # of e - in each shell

33. Al 13 S 283283 Aluminum 26.982 Element Symbol Element Name # of p + (Atomic Number) Average atomic mass (# of p + + n 0 ) # of e - in each shell Physical state at STP (0 o @ sea level)

34. Models of the Atom Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)

35. Models of the Atom Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell) Mg

36. Models of the Atom Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell) B O

37. Bohr Diagram Shows complete e - configuration (sometimes shows details of nucleus) Ex: Mg

38. Bohr Diagram Shows complete e - configuration (sometimes shows details of nucleus) Try: F and Ca

39. Isotopes Isotope: An atom with a different # of n 0 than normal, which therefore also has a different

40. Isotopes Isotope: An atom with a different # of n 0 than normal, which therefore also has a different atomic mass

41. Isotopes Ex: C-12 vs. C-14 – p + = p + =

42. Isotopes Ex: C-12 vs. C-14 – p + = 6 p + = 6 – n 0 = n 0 =

43. Isotopes Ex: C-12 vs. C-14 – p + = 6 p + = 6 – n 0 = 6n 0 = 8 – e - = e - =

44. Isotopes Ex: C-12 vs. C-14 – p + = 6 p + = 6 – n 0 = 6n 0 = 8 – e - = 6e - = 6 – Isotopes only differ in their mass, not in their charge or their bonding behavior