Presentation on theme: "Conservation of energy -Energy cannot be created or destroyed-"— Presentation transcript:
1Conservation of energy -Energy cannot be created or destroyed- The difference between each energy level is called a QuantumWhen energy is added to an electron, the electron will become “excited” moving to a higher energy levelWhen the electron comes back down to its ground state energy is released----in the form of light.
2Electron Configuration -Each electron is a given set of 4 quantum numbersPrinciple Quantum Number or Energy Level- represent by the letter “n”n= 1 <2 <3 < 4- generally, the larger the value of “n” , the further away the electron is from the nucleus.n=1 can hold a max of 2 e-n=2 can hold a max of 8 e-n=3 can hold a max of 18 e-n= 4 can hold a max ofn = 5 can hold a max of
32nd is L 4 main orbitals—(each orbital can hold 2 electrons) Provides a code for the shapes of orbital- represented by the letter “l”4 main orbitals—(each orbital can hold 2 electrons)s-orbital –can hold 2 electrons-lowest in energy level-spherical in shapep-orbital-(can hold six electrons)-3 different p-orbitals (Px, Py, Pz)- shaped like a dumbbell
43. Magnetic quantum number (ml) - spatial orientation of the orbital that the electron occupies.Is it in Px, Py, Pz etc.4. Spin quantum number (ms)-indicates the way the electron is spinning- ±1/2
5Writing Electron configurations Copy the following on your periodic tableOr you can use the Aufbau diagram(below)
7Rules of electron configurations Pauli Exclusion Principle – No 2 e- can have the same set of four quantum numbers.The Aufbau Principle- Electrons fill in lowest energy levels first1s2 2s2 2p6 3s2 3p6Hund’s Rule (Bus Back seat Rule)- electron will fill up empty orbitals before pairing up.
8At Higher levels there will be an overlap of energy levels- Writing electron configurationsEx: F= 1s2 2s2 2p Ar= 1s2 2s2 2p6 3s2 3p6K= 1s2 2s 22p6 3s2 3p6 4s1or [ Ar] 4s1Try these:Cl:Na:Orbital Diagrams ---same conceptOxygen 8e- 1s2 2s2 2p4