1. Thursday, 30 Oct 14 You’ll need the handouts on the table, a periodic table, and calculator. Begin answering the review questions on the slides handout. Everyone will be called on, so be prepared!

2. Atomic Structure - Review Isotopes of an element have the same number of protons as each other, but different ___. Ions of an element have the same number of protons as each other, but different ___. Protons have ___ charges. Electrons have ___ charges.

3. Atomic Structure - Review The atomic mass of an isotope of Manganese is 61. Write both expressions of this isotope. The atomic mass of an isotope of Gold is 200. Write both expressions of this isotope. The atomic mass of an isotope of Bismuth is 215. Write both expressions of this isotope.

4. Atomic Structure - Review The atomic mass of Krypton is 84. How many neutrons does it have? The atomic mass of Potassium is 39. How many neutrons does it have? The atomic mass of Zinc is 65. How many neutrons does it have?

5. Atomic Structure - Review An atom of Tin has 22 protons and 26 neutrons. What is its mass? An atom of aluminum has 13 protons and 14 neutrons. What is its mass? An atom of Seaborgium has 106 protons and 157 neutrons. What is its mass?

6. Atomic Structure - Review Mn +3 Li + S 2- Al 5- Ca 2+ Br - F - B 3+

7. Atomic Structure - Review An atom of Palladium that *was* stable gains two electrons. What is its charge? An atom of Yttrium that was stable loses 3 electrons. What is its charge? An atom of Silver that was stable loses one electron, but then gains two. What is its charge?

8. Atomic Structure - Review Who is responsible for what we call the “Plum Pudding” Model? Describe the Plum Pudding model. Who was responsible for the Gold Foil experiment? Describe the Gold Foil experiment.

9. Atomic Structure - Review Atomic mass = ? + ? Atomic Number = # of ?

10. Electron Configuration Every element on the periodic table consists of an atom which is composed of protons, neutrons, and electrons. We are mostly concerned with electrons.

11. Electron Configuration Electrons exhibit a negative charge and are found around the nucleus of the atom. Electron orbitals are the position of the electrons around the nucleus and is determined as the volume of space in which the electron can be found within 95% probability.

12. Bohr Models The first energy level can only contain 2 electrons. It corresponds to the first period of the Periodic Table. The second and third energy levels can only contain 8 electrons. These correspond to the second and third periods of the Periodic Table.

13. Bohr Models You must fill the first energy level before you can fill the second level, and you must fill the second level before you can fill the third, and so on.

14. Bohr Models Draw Bohr Models for Lithium, Boron, Neon, Sodium, and Chlorine.

15. Valence Electrons Valence electrons are found in the outermost electron orbitals and are the electrons that are used in chemical reactions.

16. Valence Electrons The number of valence electrons in the outermost orbital determines what kinds of chemical bonds it can form.

17. Lewis Dot Structures for Elements The chemical symbol for the atom is surrounded by a number of dots corresponding to the number of valence electrons. Draw Lewis Dot Structures for Carbon, Helium, Oxygen, Magnesium, Phosphorus, and Argon.

18. 31 Oct 14 Grab a periodic table and a calculator and study for your quiz!

19. When you are done: Turn in your quiz to the bin up front Pick up the handouts on the table Sit quietly until everyone is finished (yes, you may read, work on stuff for another class, listen to music, or put your head down)

20. Electron Configuration – Heisenberg Uncertainty Principle Heisenberg showed it was impossible to take any measurements of an object without disturbing it. Example: Finding a helium balloon in a dark room

21. Electron Configuration – Heisenberg Uncertainty Principle Heisenberg Uncertainty Principle: It is fundamentally impossible to know both the velocity and the position of a particle at the same time.

22. Electron Configuration – Heisenberg Uncertainty Principle This principle also means that it is impossible to assign fixed paths for electrons, as described in the Bohr Model. The only thing we can know for sure is the probability of an electron being in a particular region around a nucleus.

23. Electron Configuration – Schrödinger Wave Equation Schrödinger derived an equation that treated the hydrogen atom’s electron as a wave. This equation allows us to make predictions on where the electron is likely to be. These allow us to predict orbitals.

24. Electron Configuration Orbital – a three-dimensional region around the nucleus An atomic orbital is like a fuzzy cloud in which the density at a given point is proportional to the probability of finding the electron at that point. Orbitals do not have defined boundaries.

25. Electron Configuration The modern electron configuration of each element is unique to its position on the periodic table. There are 4 electron orbitals: s, p, d, and f.

26. Electron Configuration Energy levels are determined by the period. Amount of electrons is determined by the atomic number of the element. Orbitals on different energy levels are similar to each other, but they occupy different areas in space. They also have different shapes.

27. Electron Configuration – Shapes of Orbitals s orbitals are spherical

28. Electron Configuration – Shapes of Orbitals p levels are dumbbell shaped and are oriented along the three perpendicular x, y, and z axes.

29. Electron Configuration Each orbital can be represented by specific blocks on the periodic table. The s-block is the region of the Alkali metals including Helium (groups 1 & 2) the d-block is the Transition metals (groups 3 to 12) the p-block are the main group elements from group 13 to 18 f-block are the Lanthanides and Actinides series.

31. Electron Configuration Each of the 4 orbitals can only contain certain numbers of electrons. s can only contain 2 electrons. p can only contain 6 electrons. d can only contain 10 electrons. f can only contain 14 electrons.

32. Electron Configuration electrons in an atom would fill the principal energy levels in order of increasing energy (the electrons are getting farther from the nucleus). The order of levels filled would look like this: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, and 7p

33. Electron Configuration Write the electron configuration for Lithium. 1s 2 2s 1 How many electrons are in its outer energy level? 1 What is the maximum number of electrons it can have in its outer energy level? 2

34. Electron Configuration Example: Beryllium Example: Sulfur Example: Hassium

35. Electron Configuration Shorthand Notation Example: Calcium Example: Barium Example: Lead

36. Electron Configuration