1. Ch. 11 Notes---Electrons in Atoms Atomic Models (See Fig. 13.2)‏ (1) Model: a ball of (+) charge containing a number of e - no ________________ often described as the “________ _______________” atom. (2) Model: a ____________ of (+) charge surrounded by a number of e - no _____________ and no e - orbitals Thomson nucleus plum pudding

3. Ch. 13 Notes---Electrons in Atoms Atomic Models (See Fig. 13.2)‏ (1) Model: a ball of (+) charge containing a number of e - no ________________ often described as the “________ _______________” atom. (2) Model: a ____________ of (+) charge surrounded by a number of e - no _____________ and no e - orbitals Thomson nucleus plum pudding Rutherford nucleus neutrons

5. (3) Model: a nucleus of (+) charge that also contains ______________ nucleus is encircled by e - ’s located in definite orbits (or paths). e - ’s have ___________ energies in these orbits e - ’s do not lose energy as they orbit the nucleus (4) Mechanical Model: no definite ____________ to the e - path (“fuzzy” cloud)‏ orbits of e - ’s based on the _________________ of finding the e - in the particular orbital shape. Atomic Models Bohr neutrons fixed

8. Let us have a moment of silence

9. (3) Model: a nucleus of (+) charge that also contains ______________ nucleus is encircled by e - ’s located in definite orbits (or paths). e - ’s have ___________ energies in these orbits e - ’s do not lose energy as they orbit the nucleus (4) Mechanical Model: no definite ____________ to the e - path (“fuzzy” cloud)‏ orbits of e - ’s based on the _________________ of finding the e - in the particular orbital shape. Atomic Models Bohr neutrons fixed Quantum shape probability

11. Schroedinger's Cat

13. Quantum Mechanical Model

14. Diagram: (Fig. 13.3)‏ The energy levels in an atom are sort of like _________ of a ladder. The more energy an electron has, the __________ away from the nucleus it usually will be. The energy levels are not evenly spaced. They get ___________ together as you travel farther away. To move from one “rung” to another requires a “____________” of energy. Energy Levels rungs farther closer quantum

15. continuous energy levelsquantized energy levels

16. Quantum Numbers Describe the ______________ of the e - ’s around the nucleus. Quantum #’s are sort of like a home _____________ for the electron. This information about the location of the e - ’s in an atom can be used to: (1) determine chemical & physical _____________ for the elements. (2) show how the _______________ __________ is organized. (3) show _____ and _____ elements combine to form compounds. location address properties Periodic Table howwhy

17. The Four Quantum Numbers Principal Q. #: Describes the _____________ that the electron is from the nucleus. The bigger the number, the ___________ away the electron is. Example: (1=closest, 2, 3, 4...farther away) These distances are sometimes called _______________ ______________ ____________. 1 2 3nucleus distance farther principal energy levels

18. Orbital Q. #: Describes the __________ of the electron’s path around the nucleus with a letter: (s, p, d, & f) These are sometimes called “_____________”. s=_____________ cloud; p=_____________ or a 3-D figure 8; shape sublevels sphericalellipsoid

19. d & f orbital shapes are complex ________- _______________ ellipsoids, and some d’s and f’s are an ellipsoid with a doughnut or two around the middle. All of these orbital shapes are based on the probability of finding the electron in the cloud. (See p. 365)‏ d - orbitals f - orbitals criss crossing

20. Magnetic Q. #: tells how many _________________ in 3-D there are about the nucleus for each orbital shape. s=___ orientation p= ___ orientations... (x, y, and z) d= ___ orientations f= ___ orientations Spin Q. #: describes how the electron in an orientation is spinning around the nucleus. This spin can be thought of as “____” or “________”. (Some like to imagine it spinning “clockwise” and “counterclockwise”.) The spin is represented as an ___________ in the direction of the spin. orientations 1 3 5 7 up down arrow

21. For our class this means that in each orientation there can be up to two electrons. s=___ electronsp= ___ electrons d= ___ electrons f= ___ electrons Remember, the four quantum numbers tell us the location, or “address” of each electron in an atom. This information is vital in understanding the layout of the Periodic Table and the reasoning behind why and how atoms form bonds. 2 6 10 14

22. Electron Configurations (Energy Level Diagrams)‏ 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p… ↑↓ ↑ ↓ ↓ ↓ ↑ ↑ ↑ ↑ ↑↑↓↓

23. How Electron Configurations Relate to the Organization of the Periodic Table s p d f

24. Electron Configurations & Properties How do electron configurations relate to the chemical and physical properties of an element? All elements with the _________ outer shell e - configurations have the ________ properties. This means that elements in the same ____________ group have similar properties. Examples: (1) Li, Na, K, Rb, and Cs all have __ lone “__” e - for their last orbital... (_____, _____, _____, etc.) This makes all of them ___________ reactive. They all react with __________ to produce hydrogen gas. (2) Ne, Ar, Kr, Xe, and Rn all have the outer energy level completely __________ with electrons...(________, ________, ________, etc.) This makes all of them ______________. They do not produce __________________! same similar vertical 1s 1s 1 2s 1 3s 1 verywater filled 2s 2 2p 6 3s 2 3p 6 4s 2 4p 6 inert compounds

25. More Practice Problems (1) Which element has its last electron as a 4p 5 ? ___________ (2) Which elements are similar in properties as Bromine? __________ (3) What would the last outer shell electron configuration be for the element underneath Radon, (Rn)? (6) What is the shape of the last orbital filled in Calcium, (Ca)? _____ (7) How many electrons are in the last “p-orbital” of Sulfur, (S)? ____ Bromine F, Cl, I, At 7p 6 sphere 4

26. Electromagnetic Radiation Any wave of energy traveling at a speed of ___________ is called electromagnetic radiation. There are many types of electromagnetic radiation and each type has a different _______________ and _______________. Here are the types of electromagnetic radiation from longest to shortest wave or lowest to highest frequency. These are also in order from lowest to highest energy. (See Fig. 13.10)‏ light frequencywavelength

27. Electromagnetic Radiation

28. (1) Radio Waves -- used in __________________ (2) Microwaves-- broadcasts TV signals and used to _____ _______. (3) Infrared (IR) -- we feel this as _____; _________ & ______ can “see” this. infrared image of a cat infrared image of heating pipes under a floor heat cook food communications Snakesowls

29. Infrared Vision

30. IR Mr. T Taken at NASA Goddard Space Center in Maryland

31. Electromagnetic Radiation (4) Visible Light -- the only radiation we can detect with our eyes. It can be separated into the colors of the spectrum with a __________. ROYGBIV (5) Ultraviolet (UV) -- gives you a _____________; _________ can “see” this; some of this radiation from the sun gets blocked by the ___________ layer flower photo under normal lightflower photo under UV light prism sunburnBees ozone

32. Electromagnetic Radiation (6) X-rays -- used in medicine Ouch!

33. Electromagnetic Radiation (6) X-rays -- used in medicine Macy Slade’s shoulder injury CT scan. OH SNAP.

34. Electromagnetic Radiation (7) Gamma Rays-- some radioactive substances give it off The last type of radiation is sometimes grouped with gamma rays… (8)_______________Rays – not trueenergy radiation; almost all of this radiation from the sun is blocked by the ozone layer and our magnetic field. Consists of charged particles like protons and electrons. Interesting superhero facts: Superman has x-ray vision. The Incredible Hulk was “created” by an accidental overdose of gamma radiation. The Fantastic Four were “created” by cosmic rays. Cosmic

35. How Light is Produced When atoms get hit with energy (by _____________ them with electricity or by ____________ them up), the electrons absorb this energy and __________ to a higher energy level. Figure (a) As they immediately fall back down to the “____________ state”, they give off this energy in the form of a particle of ___________ (or other types of electromagnetic radiation) called a _____________. Figure (b)‏ zapping heating jump ground light photon

36. How Light is Produced Each photon emitted has a specific ___________ (or frequency). The color of the light that is given off depends on how _____ the electron _______ (which depends on how big of a jump it originally made.) The farther the fall, the ___________ energy the photon has. color farfell greater

37. How Light is Produced Since electrons are located only in certain __________ levels (or orbitals) around the nucleus, only certain specific _________ of light are emitted. Scientists use a _________________ to separate these colors into bands of light. These bands of color look like a ______ code of color which is characteristic of that element. No two elements produce the same ______________ of colors. This can be used to distinguish one element from another contained in a sample. (See Fig. 13.11)‏ energy color spectroscope bar spectrum

38. Emission Spectrum Hydrogen Spectrum Neon Spectrum

39. How hydrogen produces the four visible photons