The Quantum Model of the Atom
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| the photoelectric effect and hydrogen’s emission-line spectrum revealed what | that light could behave as both a wave
and a particle
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| bending of a wave as it passes by the edge of an object or through a small opening | Diffraction
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| occurs when waves overlap | Interference
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| How are electrons detected | Electrons are detected by their interaction with photons
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| states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. | Heisenberg uncertainty principle
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| describes mathematically the wave properties of electrons and other very small particles. | Quantum theory
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| the principle that states that determining both the position and velocity of an electron or any other particle simultaneously is impossible | Heisenberg uncertainty principle
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| specify the properties of atomic orbitals and the properties of electrons in orbitals | Quantum numbers
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| first three quantum numbers result from solutions to the Schrödinger equation indicate | indicate the main energy level, the shape, and the orientation of an orbital
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| The fourth number, the spin quantum number,describes | a fundamental state of the electron that occupies the orbital
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| symbolized by n, indicates the main energy level occupied by the electron | principal quantum number,
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| Values of n in teh Principal quantum number are what type of integer | Positive integers only
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| As n increases | the electron’s energy and its average distance from the nucleus increase
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| The total number of orbitals that exist in a given shell, or main energy level is equal to | n2.
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| symbolized by l, indicates the shape of the orbital | angular momentum quantum number
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| For a specific main energy level, the number of orbital shapes possible is equal to | n
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| The values of l allowed are | zero and all positive integers less than or equal to n − 1.
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| The Orbital Letter Designations According to Values are | L = 0 and L = 1; 1 = P; 2 = d; 3 = f
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| What shape corresponds to the s orbital | spherical
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| What shape corresponds to the p orbital | dumbbell shapes
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| what shape corresponds to the d orbital | It is more complex
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| How can Atomic orbitals be similar and different | Similar shape but different orientations around the nucleus
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| What is symbolized by m which indicates the orientation of an orbital around the nucleus | magnetic quantum number
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| What values correspond to m | Whole numbers including zero, from -l to +l
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| the number of orbitals at each main energy level equals | the square of the principal quantum number, n2
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| has only two possible values—(+1/2 , −1/2)—which indicate the two fundamental spin states of an electron in an orbital | spin quantum number
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| A three dimensional region around the nucleus that indicates the probable location of an electron. | Orbital
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