Chapter 7. DeBroglie Waves Heisenberg s Uncertainty Quantum Numbers Electron Configuration
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1 Chapter 7 DeBroglie Waves Heisenberg s Uncertainty Quantum Numbers Electron Configuration
2 Are Electrons Particles or Waves? De Broglie ( ) If electromagnetic radiation behaves as a particle, could a particle in motion, such as an electron, behave as a wave? De Broglie s equation: hc hc h λ = = = = 2 E mc mc h mu λ = de Broglie wavelength, m = mass of electron (in kg), u = velocity (in m/s), and h = Planck s constant 2
3 What is the speed of an electron that is travelling at a speed of 2.2 x 10 3 km/sec? The mass of an electron is x kg. hc hc h λ = = = = 2 E mc mc A. 3.3 x 10-7 m B x 10 9 m C x 10 6 m D. 3.3 x m E. none of these h mu h = x Jsec J = kgm 2 /sec 2 Convert mass to kg Convert speed (u) to m/sec
4 Electrons as Waves Electrons behave like circular waves oscillating around nucleus. No defined stationary ends Stable circular waves of circumference = nλ 4
5 The Uncertainty Principle Wave theory vs. particle theory: Each yields a different answer for location of electron around nucleus. Impossible to predict both location and velocity accurately Heisenberg Uncertainty Principle: We cannot determine both the position and the momentum of an electron in an atom at the same time. Δx mδv h 4π 5
6 Electron Wave Equations Erwin Schrödinger (1925) Developed mathematical equations to describe behavior of electron waves, which became the basis of quantum mechanics Wave functions (ᴪ) ᴪ describes the motion of electron waves as they vary with location and time. ᴪ 2 defines an orbital or region of high probability for locating an electron. 6
7 Wave Equations and Quantum Numbers Mathematical solutions to wave equations (Ψ 2 ) are identified by unique combination of three integers. Quantum numbers: Principle quantum number (n) indicates shell and relative size of orbital(s). n = 1, 2, 3 Angular momentum quantum number (l) defines shape of orbital and subshell. l = 0 (n 1) Magnetic quantum number (m l ) defines orientation of orbital around nucleus. m l = l +l Magnetic spin, (m s ) describes electron spin: m s = +½ or ½. 7
8 Quantum Numbers 8
9 Spin Magnetic Quantum Number Spinning of electron creates magnetic field oriented either up or down. Fourth quantum number (m s ) describes electron spin: m s = +½ or ½. Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers. 9
10 Comparison of s Orbitals One s orbital in each shell The number of nodes increases as the n value increases. 10
11 The Three 2p Orbitals Three p orbitals in each shell with n 2 The nodes are at the nucleus. 11
12 The Five 3d Orbitals Five d orbitals in each shell with n 3 The nodes are at the nucleus. 12
13 Rules to Fill by: Aufbau principle: Fill the lowest energy orbitals first Hund s Rule: Fill all of the same energy orbitals before pairing electrons Pauli exclusion principle: No two electrons in an atom can have the same set of quantum numbers, so electrons in the same orbital must have opposite spins. 13
14 Orbital Diagrams Orbital diagram depiction of the arrangement of electrons in an atom or ion using boxes to represent orbitals Up/down arrows indicate e with +/ spin. 14
15 Orbital Diagrams for Hydrogen and Helium 15
16 Orbital Diagrams for Multi-electron Atoms 16
17 Draw the electron configuration for: Boron 1s 2 2s 2 2p 1 How many valence electrons in each? Boron = 3 valence electrons Silicon Oxygen 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2 2s 2 2p 4 Silicon = 4 valence electrons Oxygen = 6 valence electrons Sulfur 1s 2 2s 2 2p 6 3s 2 3p 4 Sulfur = 5 valence electrons
18 How many valence electrons are in sulfur A. 4 B. 2 C.3 1s 2 2s 2 2p 6 3s 2 3p 4 D.6 E. 1
19 Orbital Energies in Multi-electron Atoms Orbitals are filled from lowest energy to highest energy (Auf bau principle): Within a given shell, subshells fill in order of s, p, d, f. Due to small energy differences there is some overlap of subshells at higher values of n. 4s is filled before 3d. 6s is filled before 4f. 19
20 20 Periodic Table: s, p, d and f Blocks
21 Periodic Table: Filling of Orbitals 21
22 Write the electron configuration for Bromine Bromine: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 How many valence electrons does Bromine have? A. 5 B. 7 C. 2 D. 28 E. none of these
23 Anomalies in Configurations Chromium and copper do not follow pattern: Cr = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5 Cu = 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1 3d 10 Anomalies arise from stability associated with half-filled and completely filled d-subshells. 23
24 What is the Aufbau principle? A. No two electrons in an atom can have the same quantum numbers B. Fill all orbitals that have the same energy with one electron before pairing electrons. C. Fill the lowest energy orbitals first D. Be sure to take off the electrons before filling the orbitals E. None of these
25 What do electrons in the same orbit have opposite spins? A. The Aufbau principle B. The Pauli exclusion principle C. Hund s Rule D.The forbidden quantum spin state principle E. None of these
26 Why are there three unpaired electrons in Nitrogen? A.Pauli Exclusion Principle B.Hund s Rule C.Aufbau principle D.Schroedinger s equation E.None of these
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