It is impossible to measure simultaneously the position and momentum of a small particle (subatomic particle) with absolute accuracy or certainty The
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1 Mr.V
2 It is impossible to measure simultaneously the position and momentum of a small particle (subatomic particle) with absolute accuracy or certainty The concept of the orbital was based on the probability factor and this principle
3 It is a three dimensional space around the nucleus where there is a very high probability of locating an electron Example of orbital's s-orbital p-orbital d- orbital f-orbital
4 ORBIT ORBITAL It is a well defined circular path around the nucleus in which the electron revolves It is circular in shape It represents the movement of an electron around the nucleus in one plane. It states with certainty the momentum and position of an electron. Violates the Heisenberg s uncertainty principle The maximum number of electrons in an orbit is n. It is a region in three dimensional space around the nucleus where there is a very high probability of locating the electron s, p and d orbitals are spherical, dumbbell and double dumbbell in shape respectively It represents the movement of an electron around the nucleus in a three dimensional space. It is a consequence of Heisenberg s uncertainty principle..i.e. The position and momentum cannot be known with certainty The maximum noof electrons in an orbital is
5 Orbital s that have the same energy for the sub-shell s are called degenerate orbital s The three p orbitals are degenerate The five d orbitals are degenerate when not under the influence of a magnetic field or electric field
6 It is called the orbital wave function When you square the value you get the electron density = This is because the motion of the electron is considered to be in the form of waves. Look under diffraction patterns of electrons
7 Equation x y z 8 m( E n h V ) 0
8 The equation needed for calculating the energy of an electron is given by me 4 z E n h
9 E = -.17 x J/Atom or -1.31x10 6 J/Mole.
10 These are a set of 4 integers necessary to specify the energy, position, shape, size and orientation of orbital s to which electrons belong.
11 It specifies the location and energy of an electron, It is a measure of the effective volume or size of the electron cloud The letter n is used to indicate it n can have values 1,,3,4...
12 It determines the shape of the orbital. It takes integral values from 0 (n-1) where n is the principal quantum number. When l = 0, 1,, the shapes of the orbital s are s Spherically symmetrical, p dumbbell, and d double dumbbell.
13 l value Orbital s p d f g Shape Spherically Symmetrical Dumbell Double Dumbell
14 Flash File Hybrv18.swf
15 It gives the orientation of the orbital s in space. (how many sub shells) It takes integral values ranging from -l l s orbital has got one orientation, p orbital has got 3 orientations, d orbital has got 5 orientations f orbital has got 7 orientations.
16 It indicates the direction in which the electron spins on its own axis or the magnetic property that is associated with it. This value is quantised the two values that are permitted They are + ½ and - ½
17 Aufbau Order or principle According to the principle the electrons are filled in the various sub-shells in the order of their increasing energies.
18 (n + l) Rule: The subshell with lower n+l value will posses lower energy and will be filled first. This information can be used instead of Aufbau order. Or you can verify the order of the orbitals written.
19 1s < s < p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 4f...
20 Electron pairing will not take place in degenerate orbitals (same energy subshell) until each orbital is first singly filled with electrons having parallel spins. Or Electron pairing will take place only after each sub shell has one electron each.
21 Half Filled d orbital configurations are preferred as there is extra stability because of the symmetrical distribution of the electrons in the orbitals. The Exchange energy is High for Cr, Mo & W. and Cu, Ag and Au Exchange energy can be calculated using the following equation Where n is the number of electrons having parallel spins. In the equation given below n stands for the number of unpaired electrons in the d orbital. ExchangeEnergy n! n( n )!
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