CHEM103 Lecture Notes - Lecture 12: Shining Light, Joule, Electromagnetic Spectrum

• School: University of Delaware
• Department: Chemistry and Biochemistry
• Course: CHEM103
• Professor: Graves Ph D, Kimberly Susan

Document Summary

Electronic structure of atoms: electrons are the ultimate determinant of the properties & reactivity of atoms, understanding how electrons behave and what influences them is critical to understanding chemistry. Electronic structure of atom models: late 1800s early 1900s saw an increased understanding of atomic structure, jj thompson plum pudding model (1904, gold foil experiment, bohr model (1913) The electromagnetic spectrum: continuous range of radiant energy (also called electromagnetic radiation) Wave properties of light: wavelength ( ): the distance from crest to crest or trough to trough, frequency ( ): the number of crests of a wave passing a stationary point of. 6-10m: 1 x 10^9 nm = 1m. Using wavelength and frequency relationship: your (cid:374)eigh(cid:271)or ow(cid:374)s a ha(cid:373) radio a(cid:374)d (cid:271)road(cid:272)asts his daily (cid:862)(cid:374)ews(cid:863) progra(cid:373) i(cid:374) Morse code at a frequency of 2. 8 x 10^7 hz. What wavelength of radiation (in m) carries his insights: = c.