CHE 106 Lecture Notes - Lecture 14: Joule, Energy Level, Photon

• School: Syracuse University
• Department: Chemistry
• Course: CHE 106
• Professor: J.French

Document Summary

635 kj/mol + 2(-92. 3 kj/mol) (-795. 8 kj/mol) + (-241. 8 kj/mol) H = n products h - m reactants h. (cid:857)(cid:866)(cid:857)-(cid:872)(cid:874)5(cid:863)(cid:873) (cid:924)j(cid:864)(cid:926)o(cid:925)(cid:858)(cid:858) + (cid:857)(cid:866)(cid:857)-241. 8 k/mol)) - (cid:857)(cid:866)(cid:857)-635 (cid:924)j(cid:864)(cid:926)o(cid:925)(cid:858)(cid:858) + (cid:857)(cid:867)(cid:857)-92. 3 kj/mol)) 1 calorie does not equal 1 cal (1 calorie x 1000 = 1 cal) In 1885, j. j. balmer showed that the wavelengths, , in the visible spectrum of hydrogen could be reproduced by the following formula. The known wavelengths of the four visible lines for hydrogen correspond to values of n = Energy level postulate: each electron has a specific energy level available to it. Transitions between energy levels: an electron is able to move between different energy levels. Move between levels with a gain/loss of energy. Ground state: lowest energy state available (every other energy level is considered excited) Bohr derived the following formula for the energy levels of the electron in the hydrogen atom.