Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
TP - Ws Quantum Theory - developed by German physicist Max Planck: atoms emit energy in small discrete bundles called ~ E = hv (quantum of energy in j~ 6.63x1~34 j-s x wave frequency) (planck’s constant) Wave - vibrating disturbance by which energy is transmitted Wavelength - k (lambda) distance between two successive peaks or crests of waves, units = nm, m, era, etc. Fre ueo~u_~ - v (nu) number of waves that pass a given point per second (cycles per second:/s) SI unit is hertz (Hz) 1Hz -- lcyele/s Amplitude - vertical distance from the midline of a wave to the crest S~ed of a wave = wavelength x freauenc~: ~ = Lv All electromagnetic radiation waves travel at the sarae speed in a vacuum.: Speed of light- "c" = 3.00 x 108 m/s Substituting "c" for rt in the above equation: c = kv P__hotoelectric effect -when electrons are ejected fromthe surface of certain metals exposed to light of a certain frequency, light is a stream of particles called photons TP-Ws _Quantum Numbers ("L" will be used to replace °T’ to better differentiate the letter from the number1) There are 4 quantum numbers that can describe the distribution of electrons: 1 - ~antum number (n) describes the average distance the electron is from the nucleus of the atom (energy levels or shells) **’~n values = 1, 2, 2 - Azimuthal (Angular Momentum) quantum number: (L) describes the shape of the orbitals (s=spherical, p=dmnbell, d=clover leaf, f=too complex) **~’L = 0 to (n-l) values = 0, 1, 2, 3, ..... (s) (p) (d) (f) Example: n = 1 L = 1-1 = 0 (s) ls subshell n = 2 L = 2-1 = l& 0 (s,p) 2s, 2p subshells (also designates the number of subshells) 3 - Ma.=~Ngneiic quantum number: (NIL) describes the orientation of the orbiltal in space (# of orbitals in a subshell: s=l, p=3, d=5, f=-7 ) ***ML = 2L + 1 -L, (-L + 1) ..... 0 .... (+L -1), +L Example: n = 2, L = 1 2p subshell ML= 2(1) + 1 = 3 values or orbitals 4 - Electron S in uantum number: (Ms) value = +1/2 or -1/2 +1/2 = elockwise~-~ -1/2 = counterclockwise ~-~ ELECTRON iN AN S ORBITAL: ELECTRON iN Py, Pz, AND P× ORBITALS: Z Py Use Type |25, |27 or 133 Film SCIENCE - I~H (~COPYRIGHT 1965 BY REINHOLD PUBLISHING CORPORATION ELECTRONS IN dz~, dyz, dxz, dxy, AND dx2 y20RBITALS Z Y X Z Z ~X lyz Z d×z Z X dxy Use Type ’125, 127 or 133 Film SCIENCE (~ COPYRIGHT 1965 BY REINHOLD PUBLISHING CORPORATION Principal Azimuthal Quantufn Quantum Number, n Number, 1 (Shell) (Subshell) Subshell Designation Number, m (Orbital) Number of Orbitals in Subshell lS 0 1 0 0 1 -1,0,+1 1 3 0 2 3 4 0 35 0 1 1 3p -1,0,+ 1 3 2 3d 0 5 1 1 4~ 4p =2,=1,0, +1,+2 0 ml, O, +1 2 4d 3 5 3 4~ -3,-2,-1, O, +1,+2, +3 7 main energy level 1 2 3 number of sublevels(n) number of orbita~s (n~) 1 1 s 1 2 4 sp 13 3 9 spd 135 4 16 spdf 1357 2610 261014 18 32 kind and no. of orbitais per subJevel maximum no. of electrons per sublevel maximum no. of eleo{rons per main leve~ 2~~) 3 Rules to Follow When Wfitin~ Eo Confi~ratio~ 1o Aulban Princi~ electrons’enter/fillup orbitals of lowest energy first orbitals in the same sublevel are equal in energy e×. p (orbital)- O×OyOz are all equal in energy sometimes energy levels ~ each other 2. Pauli Ex~elusion Princi.p.~le there is a maximum of 2eo in any one orbital these 2e- (paired) must be of opposite spins one positive/clockwise and the other negative/counterclockwise 3. Hund’s Rule. when ~ling orbitals of equal energy (spdf) one eo enters each orbital first (unpaired), until all of the orbi~als eontain one ewith spins parallel then the 2nd. eo will enter eaeh orbital to form paired spins o ex.p= ~