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Unit 4 - Electron Arrangement (2017/2018)
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- 2. 4.1 Electromagnetic Radiation I willbe able to… • Define electromagnetic radiation, wavelength, frequency, electromagnetic spectrum, and photon. • Solve wave speed problems. • Identify the seven types of electromagnetic radiation. • Explain the duality of light.
- 3. 4.1 Electromagnetic Radiation •ElectromagneticRadiation – energy that exhibits wavelike qualities and travels through space at the speed of light.
- 4. 4.1 Electromagnetic Radiation •Wavelength– the distance between two consecutive peaks/crests or troughs in a wave. • Unit = m •Frequency – the number of waves (cycles) per second that pass a given point in space. • Unit = 1/s = hertz = Hz
- 5. 4.1 Electromagnetic Radiation •Thespeed of electromagnetic waves is the speed of light. • Speed of light = c = 300,000,000 m/s.
- 6. 4.1 Electromagnetic Radiation MeasurementSymbol Unit speed 𝑣 m/s frequency 𝑓 1/s = Hertz = Hz wavelength m
- 7. 4.1 Electromagnetic Radiation EXAMPLES •Awave along a guitar string has a frequency of 100.0 Hz and a wavelength of 0.05 meters. Calculate the speed of the wave.
- 8. 4.1 Electromagnetic Radiation EXAMPLES •Thespeed of sound in air is about 340 m/s. What is the wavelength of sound waves produced by a guitar string vibrating at 550 Hz?
- 9. 4.1 Electromagnetic Radiation EXAMPLES •Thespeed of light is 2.998 x 108 m/s. What is the frequency of microwaves with a wavelength of 0.0100 meters?
- 10. 4.1 Electromagnetic Radiation •ElectromagneticSpectrum – all of the frequencies or wavelengths of electromagnetic radiation.
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- 12. 4.1 Electromagnetic Radiation •Electromagnetic Spectrum • Radio Waves • Microwaves • Infrared Rays • Visible Light • Ultraviolet Rays • X-Rays • Gamma Rays
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- 14. 4.1 Electromagnetic Radiation • Light(EM radiation) acts as both a wave and a particle. • Duality of Light • Wave • Travels through space and carries energy like a wave. • Particle • When it interacts with matter it behaves like a stream of tiny particles of energy.
- 15. 4.1 Electromagnetic Radiation •Photons– a particle/packet of electromagnetic radiation. • High frequency waves = high energy photons • Low frequency waves = low energy photons
- 16. 4.1 Assignments •4.1 ElectromagneticRadiation WS •Wave Calculations WS •Wave WS A •EM Spectrum and Visible Light WS •EM Spectrum Project 4.1 Electromagnetic Radiation
- 17. 4.2 Atoms andEnergy I will be able to… • Define excited state, ground state, quantized energy levels, emission line spectrum, and spectroscope. • Describe how photons are emitted from excited atoms.
- 18. 4.2 Atoms andEnergy •When atoms receive energy, they become excited and move to an excited state. •Excited State – a state in which an atom has more energy than it does in its ground state.
- 19. 4.2 Atoms andEnergy •When excited atoms lose energy, they release energy and go to a lower energy state. • The energy is released as a photon. •Ground State – the lowest energy state.
- 20. 4.2 Atoms andEnergy
- 21. 4.2 Atoms andEnergy
- 22. 4.2 Atoms andEnergy
- 23. 4.2 Atoms andEnergy • Energy Gained (Excited) = Energy Release (Photon)
- 24. 4.2 Atoms andEnergy
- 25. 4.2 Atoms andEnergy •Every time a hydrogen atom gets excited and releases a photon the same things happens. • One of the following photons, with a wavelength in the visible spectrum, is released.
- 26. 4.2 Atoms andEnergy •Quantized Energy Levels – energy levels where only certain values are allowed.
- 27. 4.2 Atoms andEnergy •Line Emission Spectrum – spectrum of colors emitted when an excited atom releases energy/photons.
- 28. 4.2 Atoms andEnergy
- 29. 4.2 Atoms andEnergy •Spectroscope – A device that splits light into a spectrum. • Can be used to determine what distant stars are made of.
- 30. 4.2 Atoms andEnergy 4.2 Assignments •4.2 Atoms and Energy WS •Bunsen Burner WS •Flame Test LAB •Spectrum Tube LAB •Star Emission Spectrum WS
- 31. 4.3 Atomic Orbitals Iwill be able to… • Define principle energy levels and sublevels. • Identify where the s-block, p- block, d-block, and f-block are located on the periodic table. • Explain the Pauli exclusion principle.
- 32. 4.3 Atomic Orbitals •PrincipleEnergy Levels – distinct energy levels where electrons can be found. • Principle Energy Level = Quantum Number •Sublevels – a subdivision of the principle energy levels.
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- 35. 4.3 Atomic Orbitals •Orbitalsare regions of the atom where electrons are most likely found. •Sublevels Sublevel Number of Orbitals Maximum Number of Electrons s 1 2 p 3 6 d 5 10 f 7 14
- 36. 4.3 Atomic Orbitals •MoreEnergy = Larger Orbitals
- 37. 4.3 Atomic Orbitals •PauliExclusion Principle • Each orbital can hold a maximum of two electrons. • If an atom has an odd number of electrons one orbital may contain only one electron. • Each electron must also have opposite spins. • One spins up • One spins down
- 38. 4.3 Atomic Orbitals 4.3Assignments •4.3 Atomic Orbitals WS
- 39. 4.4 Electron Arrangements I willbe able to… • Define electron configuration, valence electrons, and core electrons. • Determine the electron configuration, orbital diagram, and noble gas notations for given elements. • Explain Hund’s rule and the Aufbau principle. • Differentiate between valence electrons and core electrons.
- 40. 4.4 Electron Arrangements •ElectronConfiguration – the arrangement of electrons in an atom.
- 41. 4.4 Electron Arrangements •1 = • 2 = • 3 = • 5 = EXAMPLES Electron Configuration Notation • 8 = • 13 = • 16 = • 18 =
- 42. 4.4 Electron Arrangements •1 = • 2 = • 3 = • 5 = EXAMPLES Orbital Diagram/Box Diagram Notation • 8 = • 13 = • 16 = • 18 =
- 43. 4.4 Electron Arrangements •Hund’sRule • each orbital in a sublevel is filled with one electron before a second electron can be added to an orbital. • Electrons do not want to “share rooms” (orbital) if they do not have to.
- 44. 4.4 Electron Arrangements •AufbauPrinciple • Lowest energy levels get filled first. • Rooms on the lowest “floors” (orbitals) get filled first.
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- 46. 4.4 Electron Arrangements •1 = • 2 = • 3 = • 5 = EXAMPLES Noble Gas Notation • 8 = • 13 = • 16 = • 18 =
- 47. 4.4 Electron Arrangements •ValenceElectrons – electrons in the outermost shell/orbital of an atom. • Important for bonding atoms (spoiler). • Electrons in unfilled energy levels. • Noble gases have no valence electrons, their out shell is completely filled.
- 48. 4.4 Electron Arrangements •CoreElectrons – an inner electron in an atom; not located in the outer shell/orbital. • Electrons in filled energy levels.
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- 50. 4.4 Electron Arrangements 4.4Assignments • 4.4 Electron Arrangements WS • Electron Configurations and Orbital Notations WS • Electron Configuration, Orbital and Noble Gas Notations WS • Periodic Table and Electron Configurations WS
- 51. Unit 4: ElectronArrangement Unit 4 Test Review ASSIGNMENT •Unit 4 Test Review WS