CHE 101 Lecture Notes - Lecture 6: Matter Wave, Uncertainty Principle, Bohr Model

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greenreindeer649

17 Oct 2016

School

University at Buffalo

Department

Chemistry

Course

CHE 101

Professor

Atwood Jim

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Chapter 6

Electronic Structure of Atoms

A. Atoms

B. Wave Mechanics

C. Orbitals

D. Electron Spin

E. Orbital Filling

F. Electronic Configurations

A. Atoms and Atomic Theory

Postulates:

1. Lucretius – sour atoms have barbs; bland atoms are smooth

2. Dalton’s Atomic Theory- Atoms of different elements are different and not changed into

each other by chemical reactions- Alchemy refuted

3. Electrons are discovered-

a. Mass = 9.11 x 10 ^-28 g

b. Charge= 1.6 x 10 ^ -19coul

4. Rutherford Gold Foil- all weight (mass) is in the nucleus

5. Spectroscopy- Line spectra are different for each element- light

a. Wavelength: Lambda

b. Frequency: Nu

c. Frequency x Wavelength = C (Speed of light: 3.0 x 10^8 m/s)

6. Bohr Atom- A planetary model- quantum condition

a. Nucleus in the middle and orbitals around it

b. Labeled with quantum numbers

7. De Broglie- wave nature of an electron

a. 2pi r = n lambda

b. lambda = h/mv

i. h= Planck’s constant

ii. m= mass

iii. v= velocity

iv. (page 223)

8. Heisenberg Uncertainty Principle

a. (Deltax)(Delta p) is Greater than or equal to h/4pi

B. Wave Mechanics- Electrons as waves P. 226

Using classical physics equations for waves one can solve for the energy of an electron-

Schrodinger

- ( h^2 ) d^2 x Wave function (psi) + V x Wave function = E (Energy) x Psi

8 pi^2m dx^2

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Document Summary

Electronic structure of atoms: atoms, wave mechanics, orbitals, electron spin, orbital filling, electronic configurations, atoms and atomic theory. Using classical physics equations for waves one can solve for the energy of an electron- ) d^2 x wave function (psi) + v x wave function = e (energy) x psi. The bohr theory gave energy, e n, and radius r n. Quantum mechanics gives wave functions psi n, l, Since an electron can"t be precisely located, one must be satisfied with probability which is proportional to (psi)^2. The wave functions are called orbitals and have corresponding energies. Each orbital is described by three quantum numbers, psi n, l, mf, n is the principle quantum number and may take integer values greater than or equal to one (n. Larger values of n mean that the lectron spends more time away from the nucleus. L is the azimuthal quantum number that defines the shape of the orbital.

Related Questions

provided to determine AH rxn for the following reaction: urf (klimol) CH4(g) + 3 Cl2(g) â CHCI3() + 3 HCI(g) airrxn-? A)-151 kJ B)33SkJ C) +662kJ D) +117kJ E)-217 kJ A) 4.1 atm B) 5.0 atm c) 6.4 atm D)1.1 atm E) 2.3 atm kg) of the copper sample if the specific heat capacity of copper is 0 CH4(g) 75 CHCI3() -134 HCI(g) -92 8) What pressure will 14.0 g of CO exert in a 3.5 L container at 75 C? 9) A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 50.0Â°C, determine the mass (in .385 J/g C A) 226 kg B) 0.235 kg C)6.64 kg D) 119kg E)5.10 kg 10) Which of the following processes is exothermic? A) the ionization of a melting snow atom B) the breaking of a boiling of water bond C) the boiling of water D) the condensation of water E) All of the above processes are exothermic 11) Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. B)4.27 x 10-19J C) 2.34 x 10-19J D)6.45 x 10-19J E) 2.83 x 10-19J A)3.54 Ã 10-19J 12) Identify the color of a flame test for potassium D) yellow A) violet B) red C) white E) blue 13) Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true. 14) Calculate the wavelength of an electron (m-9.11 x 10-28 g) moving at 3.66 Ã 106 m/s. A)1.99 x 10-10m B)5.03 x 10-10 m C) 1.81Ã10-10 m D)5.52 Ã 10-9 m E) 2.76 Ã 10-9 m 15) Which of the following quantum numbers describes the shape of an orbital? A) principal quantum number B) magnetic quantum number C) spin quantum number D) SchrÃ¶dinger quantum number E) angular momentum quantum number 16) Determine the energy change associated with the transition from n = 2 to n-5 in the hydrogen atom. A)-218Ã10-19J B)+654 Ã 10-19 J C) +4.58 x 10-19 J D)-1.53 x 10-19 J E) +3.76 Ã 10-19J 17) If two electrons in the same atom have the same value of I, they are A) in the same sublevel, but not necessarily in the same level. me level, but different sublevel. C) in the same orbital. D) in different levels and in different shaped orbitals. E) none of the above.

CHE 101 Lecture Notes - Lecture 6: Matter Wave, Uncertainty Principle, Bohr Model

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