CHEM 1A Lecture Notes - Lecture 15: Bohr Model, Magnetic Quantum Number

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pucehedgehog993

9 Jan 2019

School

UCSB

Department

Chemistry and Biochemistry

Course

CHEM 1A

Professor

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CHEM 1A Full Course Notes

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Document Summary

2 18 must be whole nz. ru. Z equation only works for system in 1 electron of protons. Calculate of light emitted when the in the. Hinton goes from a 4 to n 2 z 1. 2. 18 4. 09 9 if if: e is, e is t then energy is released in light frmf emitted then energy is absorbed in form of light absorbed. Most add energy to remove the electron remove. Calculate the ground state ionization energy for he. Lowest energy state for a e system this is. Ionization remove e nil to to a final. 218 x 20 2: e nil remove take the state of i. 1 convert to using e 23 run. For a standard wave i only allow integarnnnhe. To determine each energy level quantum n prmgdhumher the number of orbitals present use quantum numbers orbital sized energy. C each mc value represents a differentorbital mtz. co. L mio so theres only one level nil in orbital energy.

Related Questions

1. Theabsorption spectra of ions have been used to identify the presenceof the elements in the atmospheres of the sun and other stars. Whatis the wavelength of light (in nm) that is absorbed byHe⁺ ions, when an electron is excited from the Bohrorbit with n = 2 to the n = 7 state? The energy of an electron inthe nth level is

E_n =

BZ²

n²

where B = 2.18 x 10^-18 J and Z = charge onnucleus (number of protons).

2. Anelectron in the 4^th energy level of the H atom drops tothe 1^st energy level. In other words an excited electrondrops to the ground state. What is the energy (in J) of the emittedphoton)? The energy of an electron in the nth level is

E_n =

n²

2.18 x 10^-18 J

n²

3.The photoelectric effect for a certain alloy has a thresholdfrequency of 8.40 x 10¹⁴ Hz. For light of thisfrequency, find the energy of one mole of photons (inkJ).