Electron Configuration Mrs. Paparella

Sublevel Structure: A more detailed picture of where e- are located. 1s1 is the electron configuration for Hydrogen 1 is the principle energy level : principle quantum number n=1 s is called the sublevel 1 is the # of electrons

Helium : the 1st Noble Gas The 1st energy level is filled with 2 electrons in the s sublevel. There is one orbital(represented by the box) which has 2 electrons in it.

Nitrogen: A Diatomic Element 1s2 2s2 2p3 Notice that there is one e- in each of the p orbitals , not 2 in one and 1 in the 2nd. This is a rule that must be followed when diagramming electron configurations.

Types of sublevels Sublevel # of orbitals Max # of e- s 1 2 p 3 6 d 5 10 f 7 14

Shapes of Orbitals S is a spherical shape P has x , y and z axes with a dumbbell or flower petal shape. There are a total of 3 orbitals, each holds 2 e-. See Board for drawing d has doughnut shapes. See text book, chp 13

Ground State vs Excited State All the configurations found in the inside back cover of your text book are in the ground state. Note that a shorthand is used to indicate the e- for the previous row. [Ne] is the notation for 1s22s22p6 It is then used for the next row starting with sodium.

Excited State Configuration When an atom absorbs energy from an outside source like electricity or a flame, the electrons can absorb that energy and jump to a higher energy level. This is called the excited state.

Excited State Configuration When the e- returns to the ground state, it releases that energy which is visible to us as a certain color. Each element has a characteristic bright line spectrum which shows the different wavelengths of light when viewed through a spectroscope or funky glasses.

Neon Lights Neon has the ground state configuration of 1s22s22p6 When placed in the high voltage, the electron configuration is excited. For example: 1s22s22p53s1 Notice that the number of e- still adds up to 10. One of the p e- jumped to the higher 3s sublevel.

Flame Test The metal salts that you put in the flame exhibited the excited state. Each metal has a characteristic spectrum that can be seen when the excited e- returns to the ground state.