Quantum Mechanical Model of the Atom. Honors Chemistry Chapter 13
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1 Quantum Mechanical Model of the Atom Honors Chemistry Chapter 13
2 Let s Review Dalton s Atomic Theory Thomson s Model Plum Pudding Rutherford s Model Bohr s Model Planetary Quantum Mechanical Model cloud of probability
3 Study of Light Light consists of electromagnetic waves. Electromagnetic radiation includes the following spectrum.
4
5 Waves Parts of a wave: Amplitude, crest, trough Wavelength distance from crest to crest or trough to trough Frequency how many waves pass a point during a given unit of time
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7 Wave Equations Frequency is inversely related to the wavelength by the speed of light. c = where = wavelength, = frequency, and c = speed of light = 3 x 10 8 m/s
8 Dual Nature of Light Light also has properties of particles. These particles have mass and velocity. A particle of light is called a photon.
9 Energy How much energy is emitted by a photon of light can be calculated by where E = h E = energy of the photon, h = Planck s constant = x J s = frequency
10 h mv Wave and Particle To relate the properties of waves and particles, use DeBroglie s equation: = h/mv Where = wavelength, h = Planck s constant, m = mass and v = velocity.
11 Typical Units = waves per second (s-1) = meters, (m) (note: 1 m = 1 x 10 9 nm), E = Joules (J), h, Planck s constant = Joules x Seconds, (J s) m = kilograms v = meters per second, m/s
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13 Quantum Mechanical Model or Wave model Small, dense, positively charged nucleus surrounded by electron clouds of probability. Does not define an exact path an electron takes around the nucleus. Electron cloud the volume in which the electron is found 90% of the time
14 Energy Level the region around a nucleus where an electron is likely to be moving. Planck s Hypothesis - energy is given off in little packets, or quanta, instead of continuously.
15 A Quantum of energy A packet of energy or the amount of energy required to move an electron from its present energy level to the next higher one.
16 Splitting Light
17 Spectrums The lines on the emission or absorption spectrums of an element are produced when the electrons in that atom change energy levels.
18 Spectrums
19 Sources of Spectrums
20 Quantum Numbers Used to describe an electron s behavior or likely location There are four with variables: n, l, m, & s
21 Principal Quantum Number (n) Corresponds to the energy levels 1 through n. However, we will only deal with 1-7. Average distance from the nucleus increases with increasing principal quantum number, therefore n designates the size of the electron cloud Maximum # of electrons in each energy level is calculated by 2n 2 where n = the energy level (1-7).
22 Energy Sublevels (l) 2nd quantum number The number of sublevels equals the value of the principal quantum number (n) for that level. Sublevels are named in the following order - s, p, d, f. The l number designates the shape of the electron cloud.
23 S sublevel spherical shape
24 P sublevel - dumbbell shaped
25 D sublevel clover-leaf shaped
26 F sublevel irregularly shaped
27 Orbitals (m) 3rd quantum number (m) The space occupied by a pair of electrons in a certain sublevel. Sublevel s - 1 orbital p - 3 orbitals d - 5 orbitals f - 7 orbitals Each orbital can hold two electrons. m represents the orientation in space of the orbitals (x axis, y axis, z axis)
28 Spin (s) 4th quantum number Distinguishes between the electrons in the same orbital. describes the electrons spin as either clockwise or counterclockwise
29 Shape of the electron cloud Size (diameter) is related to n, the principle quantum number. The larger n, the larger the electron cloud. Shape is given by the sublevel, (l). The direction in space is given by the orbital,(m).
30 Electron Configurations Must follow these rules: Aufbau Principle electrons enter orbitals of lowest energy first. Pauli Exclusion Principle only 2 electrons can occupy an orbital and they must have opposite spins. Hund s Rule When electrons occupy orbitals of equal energy (degenerate orbitals), one electron enters each orbital until all the orbitals contain one with parallel spins, then they will pair up.
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