CHEM 1300 Lecture Notes - Lecture 4: Uncertainty Principle, Quantum Number, Bohr Model

• School: University of Manitoba
• Department: Chemistry
• Course: CHEM 1300
• Professor: Elena Smirnova

Document Summary

Brogile noticed that e= pc , p= momentum , c = speed of light , e = energy. Each electron has the same mass ((cid:1865)(cid:3039)(cid:3042)(cid:3041)= 9. (cid:1005)(cid:1004)9 (cid:1005)(cid:1004) (cid:1007)(cid:1005)(cid:1863)) and charge (cid:4666)(cid:1869) = (cid:1005). (cid:1010)(cid:1004)(cid:1006) (cid:1005)(cid:1004) (cid:1005)9(cid:4667) = (cid:1865) = ? m = 9. (cid:1005)(cid:1004)9 (cid:1005)(cid:1004) (cid:1007)(cid:1005)(cid:1863) V = 1. 00 (cid:1005)(cid:1004)(cid:1009)(cid:1865)/ h = 6. 63 (cid:1005)(cid:1004) (cid:1007)(cid:1008)j s or 6. 63 (cid:1005)(cid:1004) (cid:1007)(cid:1008)kg(cid:1865)(cid:1006)/ = (cid:1868) p = mv(velocity) (cid:4666)9. (cid:1005)(cid:1004)9 (cid:1005)(cid:1004) (cid:1007)(cid:1005)(cid:1863)(cid:4667)(cid:4666)(cid:1005). (cid:1004)(cid:1004) (cid:1005)(cid:1004)(cid:1009)(cid:1865)/ (cid:4667) A particle occupies a particular location, but a wave has no exact position. Because of their wave like properties, electrons are always spread out in space. As a result, the position of an electron cannot be precisely defined. therefore, electrons are delocalized, rather than pinpointed. The heisenberg uncertainty principle - the more accurately we know position, the more we are about motion and vice versa. O i(cid:374)stead, (cid:449)e ide(cid:374)tif(cid:455) (cid:862) p(cid:396)o(cid:271)a(cid:271)le lo(cid:272)atio(cid:374)(cid:863) of the ele(cid:272)t(cid:396)o(cid:374)s i(cid:374) a(cid:374) ato(cid:373), (cid:374)ot a(cid:374) e(cid:454)a(cid:272)t one. momentum.