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Chapter 4 Electrons In Atoms Properties of Light ___________________: a form of energy that exhibits wavelike behavior as it travels through space. (ex. Visible light, x-rays, UV, IR, radio) ____________________: all forms of electromagnetic radiation together make up the spectrum. 4-2 Properties of Light Characteristics of Waves There are 4 main characteristics of waves: 1) ___________: The height of the wave measured from it’s origin to it’s peak. When you increase the intensity, or brightness of light, you are increasing it’s amplitude. 4-4 Characteristics of Waves 3 4 Characteristics of Waves 2)________________: the distance between corresponding points on adjacent waves. Wavelength is designated by the Greek symbol __________. Wavelength = ___ 4-6 Characteristics of Waves 5 4 Characteristics of Waves 3) ___________: the number of waves that pass a given point in a specific time. Measured in cycles per second (cycle/second, or s-1) The SI unit for this is Hertz. 1.0 Hz = 1.0 s-1 Frequency is designated by the Greek symbol ___. Frequency = ____ 4-8 Characteristics of Waves Characteristics of Waves 4) _________: the speed of light is constant. It is rounded to _________ m/s. The speed of light is represented by the letter ____. ___ = λυ 4-10 The Photoelectric Effect Refers to the emission of _________ from a metal when light shines on the metal. __________: the minimum amount of energy that can be lost or gained by an atom ____________, a German physicist studied quanta of light and found: 4-11 The Photoelectric Effect E = _____ Where h is Plank’s Constant and has a value -34 of 6.6262 x 10 Js (energy) 4-12 The Photoelectric Effect Einstein expanded upon this to propose that light has a ______________, acting as a _______ under some circumstances and a ____________ under others. __________: a particle of electromagnetic radiation having zero mass and carrying a quantum of energy. 4-13 Line Emission Spectrum ______________: the lowest energy state of an atom _____________: a state in which an atom has a higher potential energy than it has in it’s ground state. 4-14 Line Emission Spectrum _____________________: a graph that indicates the degree to which a substance emits radiant energy with respect to ______________. ______________________: the emission of a continuous range of frequencies of electromagnetic radiation. 4-15 H Emission Spectrum _____________: a Danish physicist who proposed a hydrogen-atom model that linked the atom’s electron to photon emission. (electrons circle the nucleus in “_______”) 4-16 H Emission Spectrum Emission Line Spectrum: a graph that indicates the degree to which a substance emits radiant energy with respect to wavelenth. Continuous Spectrum: the emission of a continuous range of frequencies of electromagnetic radiation. 4-17 H Emission Spectrum Emission Line Spectrum: a graph that indicates the degree to which a substance emits radiant energy with respect to wavelenth. Continuous Spectrum: the emission of a continuous range of frequencies of electromagnetic radiation. 4-18 The Quantum Model ____________________________: states that it is impossible to determine simultaneously both the ___________ and _______________ of an electron or any other particle. ___________________: describes mathematically the wave properties of electrons and other very small particles. 4-19 The Quantum Model ______________________: specify the properties of atomic orbitals and the properties of electrons in orbitals. Quantum numbers were developed based on the ____________________, developed by Austrian physicist Erwin Shrödenger. 4-20 The Quantum Model __________________________: indicates the main energy level occupied by the electron. Values are positive integers only (1, 2, 3, 4 with 1 being the lowest energy level closest to the nucleus) _______________________: indicates the shape of the orbital. Values are 0, 1…n-1) 4-21 The Quantum Model l=0=s l=1=p l=2=d l=3=f The Quantum Model Magnetic Quantum Number (m): indicates the orientation of an orbital around the nucleus. Values, including zero, are –l to +l l = 0 = s orbital has only one orientation (sphere) l = 1 = p has three orientations l = 2 = d has five orientations l = 3 = f has seven orientations 4-23 The Quantum Model The Quantum Model The Quantum Model The Quantum Model ________________________: indicates the two fundamental spin states of an electron in an orbital. Values are +1/2 or -1/2. ______________________: the arrangement of electrons in an atom. 4-27 Orbital Filling Diagrams There are ____________, named after the scientists that discovered them, that govern the filling of these orbitals with electrons… 1) The ________________: an electrons occupies the lowest energy orbital that can receive it. 4-28 Orbital Filling Diagrams 2) The ________________________: no two electrons in the atom can have the same set of four quantum numbers. 3) _______________: Electrons occupy equal energy orbitals so that a maximum numbered of unpaired electrons results, and all e- in singly occupied orbitals must have the same spin. 4-29 Orbital Filling Diagrams When using this form, each electron is designated as an _______ ________ pointing up or down to show opposite spins. Each orbital is designated with a labeled line: ____ or __ __ __ 1s 2p ____________lines show multiple orbitals (1 for s, 3 for p, 5 for d) 4-30 Orbital Filling Diagrams Orbitals fill going _____________ each period (_____) on the periodic table, from the lowest energy level up. (Aufbau). Don’t forget, when they pair, they have ____________ (Pauli), but they won’t pair until each available orbital has an unpaired electron in it first (Hund) 4-31 Orbital Filling Diagrams 4-32 Orbital Filling Diagrams _____________, with one electron, would have an orbital filling diagram of: 1s __________, with 2 electrons, would be: 1s Now your at the end of the first period, start again in the 2nd period with 2s… 4-33 Orbital Filling Diagrams Lithium: 1s 2s Be: 1s 2s B: _ _ 1s 2s 2p Orbital Filling Diagrams Which of these would be correct for oxygen (with 8 e-): O: ? 1s 2s 2p OR 1s 2s 2p ____________ is correct, the _________ example violates the Pauli Exclusion Principle. 4-35 Practice Write the orbital filling notation for the following elements: 1) Be:_________________________ 2) F:__________________________ 3) Ar:_________________________ 4) Cu:_________________________ 4-36 Electron Configurations Now your ready to write electron configurations. These are simply the orbital diagrams written out with superscripts: Lithium: 1s 2s would be written out as 1s2 2s1 Be: 1s 2s would be written out as 1s2 2s2 B: _ _ 1s 2s 2p would be written out as 1s22s22p1 4-37 Practice Write the electron configuration for the following elements: 5) Mg:________________________ 6) N:_________________________ 7) Cr:________________________ 8) Cl:________________________ 4-38 Electron Configurations ___________________: refers to an outer main energy level occupied by eight e Once a __________ is complete at the end of a period, you can write subsequent configurations as having the _______ of the ___________ with the additional ___________ electrons. Sodium Na would have a noble gas notation of: Ne3s1 4-39 Practice Write the noble gas notation for the following elements: 9) Na:_________________________ 10) Sb:_________________________ 11) Y:__________________________ 12) F:__________________________ 4-40 Ch. 4 The End 4-41