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Quantum Numbers, Spectra Calculations • Objective – Today I will be able to: • Illustrate the location of an electron by drawing an orbital diagram • Identify the location of valance electrons in an atom • Identify the properties of the 4 types of quantum numbers • Determine the quantum numbers for various electrons in an atom • Calculate frequency, wavelength and energy using the appropriate equations • Evaluation/ Assessment – Informal assessment – student responses when reviewing electron configuration problems, orbital diagrams, valence electrons, quantum numbers and spectra calculations on practice sheets – Formal Assessment – collecting and analyzing students responses to quantum number and spectra calculations on the practice sheets Lesson Sequence • Warm – Up • Evaluate: Students will draw orbital diagrams on the board and explain their answers (informal assessment) • Explain: Review Valance Electrons Notes • Evaluate: Students will share responses to the worksheet • Explore: Students will use a textbook to research the four types of quantum numbers • Explain: Quantum Numbers • Elaborate: Writing quantum numbers practice • Evaluate: Review quantum numbers practice • Explain: Electromagnetic spectra calculations • Elaborate: Electromagnetic spectra calculations • Exit Ticket Warm - Up • What are valance electrons? • How do you determine the number of valance electrons in an atom? • How many valance electrons are there in the following elements: – Mg –O – Ge – Cr Objective • Today I will be able to: – Illustrate the location of an electron by drawing an orbital diagram – Identify the location of valance electrons in an atom – Identify the properties of the 4 types of quantum numbers – Determine the quantum numbers for various electrons in an atom – Calculate frequency, wavelength and energy using the appropriate equations Homework • Spectra Calculations • STEM Fair Data Table and Graphs Due Monday, November 26 • Electrons Exam – A – Day – Thursday, November 15 – B – Day – Friday, November 16 Agenda • • • • • • Warm – Up Review Orbital Diagrams Review Valance Electrons Quantum Numbers Spectrum Calculations Exit Ticket Review the Electron Configuration and Orbital Diagram Practice Worksheet Valence Electron Notes Valence Electrons • Electrons in the outermost energy level • Determines the number of electrons an atom gains, loses, or shares • These are the electrons that are involved in bonding Valence Electrons (skip) • Write the electron configuration for oxygen • 1s2 2s2 2p4 • Oxygen has six valence electrons (2s2 and 2p4) Valence Electrons (skip) • Write the electron configuration for potassium • 1s2 2s2 2p6 3s2 3p6 4s1 • Potassium has 1 valence electron (4s1) Valence Electrons • • • • Exceptions are the d and f sublevels! Use the number of electrons in the last s sublevel (and the p sublevel, if available) Write the electron configuration for Bromine 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 Bromine has seven valence electron (4s2 and 4p5) Foreshadowing: Octet Rule • Most atoms want 8 electrons in their outermost level OR full s and/or p sublevels • Atoms will form bonds to achieve the desired amount of electrons • Atoms are most stable when they have a full outer shell Complete Valence Electrons Worksheet Review Valence Electrons Worksheet as a class Quantum Numbers Activity Quantum Numbers • Quantum numbers tell us properties of the atomic orbitals, and electrons, in an atom. • Like giving each electron its own addres • An orbital is a 3-D region of an atom where there is a high probability of finding electrons (NOT an actual ring & NOT like the planetary orbitals) Principal Quantum Number Angular Momentum Quantum Number Magnetic Quantum Number Spin Quantum Number Textbook • You will need a textbook to look up information about the quantum numbers. Know for each Quantum # • • • • • Definition Symbol The allowed values An example A visual representation of the quantum number Review Quantum Numbers as a Class Discussion of the 4 types of quantum numbers and there properties Quantum Number Review Notes Quantum Numbers • Used to describe various properties of the orbitals • Each electron is assigned a set of four quantum numbers which, in order, are n, l, ml , and ms • Like giving each electron its own address Principle quantum number • Definition: indicates the main energy level occupied by the electron • Symbol: n • Values: (written as integers) 1,2,3,4,5,6,7 Angular Momentum Quantum Numbers • Definition: indicates the shape of the orbital • Symbol: l • Values: –0=s –1=p –2=d –3=f • For a specific energy level, the number of orbital shapes available is equal to n -1 Magnetic Quantum Numbers • Definition: represents the orientation of an orbital around the nucleus • Symbol: ml • Values: for a p-orbital -1, 0 , 1 Spin Quantum Numbers • Definition: represents the spin states of electrons in an orbital • Symbol: ms • Values: +1/2, - ½ Can an e- be described by the following set of quantum numbers? n=2, l=1, ml= -1 All quantum numbers are allowed values Can an e- be described by the following set of quantum numbers? n=1, l=1, ml= +1 Not possible. The value of l must be less than the value of n. Can an e- be described by the following set of quantum numbers? n=7, l=3, ml= +3 All the quantum numbers are allowed values. Can an e- be described by the following set of quantum numbers? n=3, l=1, ml=-3 Not possible. The value of ml must be in the range -l to +l Replace the ? Mark with an appropriate quantum number. n=3, l=1, ml=? n=4, l=?, ml=-2 n=?, l=3, ml=? Can an e- be described by the following set of quantum numbers? n=2, l=1, ml=-2 n=3, l=2, ml=+2 n=4, l=3, ml=+3 n=5, l=2, ml=+3 Writing Quantum Numbers • You can identify the quantum numbers for any electron in an element • Start by writing out the the electron configuration and orbital diagram for the element • Locate the electron in the orbital diagram that you are solving the quantum number for • Determine the 4 quantum numbers Hydrogen’s electron • • • • • • Write electron configuration Draw orbital diagram n= 1 l= 0 ml= 0 ms= +1/2 Helium’s second electron • • • • • • Write electron configuration Draw orbital diagram n= 1 l= 0 ml= 0 ms= -1/2 Lithium’s third electron • • • • • • Write electron configuration Draw orbital diagram n= 2 l= 0 ml= 0 ms= +1/2 Flourine’s 6th electron • • • • • • Write electron configuration Draw orbital diagram n= 2 l= 1 ml= 0 ms= +1/2 Review Notes: Spectra Calculations Electromagnetic Spectrum Electromagnetic Spectrum Electromagnetic Spectrum • Wavelength (λ - lambda) – distance between crests in a wave - Measured in meters or nanometers • Frequency (v - nu) – number of complete waves passing a point in a given amount of time - Measured in Hertz (Hz) • (λ)(v) = c (velocity of light = 3.0 x 108 m/s) • Amplitude - distance from wave origin to peak or crest Electromagnetic Spectrum Visible light has a wavelength of about 10-6 m The frequency of visible light is about 3 x 1014 Hz The range of visible light is between 200 nm and 900 nm Most sunlight available at ground level is between 400 nm and 700 nm, because our atmosphere strongly absorbs both longer and shorter wavelengths - The human eye is most sensitive in this range Electromagnetic Spectrum • The light of the sun is called White Light, and contains all the colors of the visible spectrum • Violet (400 nm) Red (700 nm) • Objects appear to us to be the color that is being reflected (chlorophyll) Max Planck • Scientists wondered why different ranges of wavelengths are emitted at different temperatures • Ex: A space heater getting warmer • Max Planck – Energy emitted or absorbed by an object is restricted to “pieces” of particular size - He called these pieces quantum, which means fixed amounts Max Planck • Max Planck (continued) - E = hυ (equation developed by Einstein) - h = Planck’s constant (6.6262 x 10-34 J-s) - E = energy - υ = frequency of radiation • Notice h is very small. Each quantum of energy is very small • Used by astronomers to determine the temperatures of distant planets and stars by measuring the wavelengths of the EM radiation they emit Example • What is the energy associated with a wave that has a frequency of 4.74 x 1014 Hz? • E = hυ • E = (6.6262 x 10-34 J-s) x (4.74 x 1014 Hz) • E = 3.14 x 10-19 J Wavelength, Frequency and Energy Calculations Complete the worksheet. Be sure to show all work Review Energy, Frequency and Wavelength Calculations Students will record samples on the board Exit Ticket • What are the quantum numbers for the last electron in Neon?