Electrons in atoms.

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Presentation transcript:

Electrons in atoms

Models of atomic structure: Dalton: Tiny, hard spheres JJ Thompson: Plum Pudding model Rutherford Bohr: Planetary model ALL WRONG The quantum mechanical model and electron configuration can tell us nearly exactly where to find any electron in the atom

Quantum Mechanical Model Quantum: energy required to move an electron to the next energy level Einstein knew that electrons were jumping energy levels because when he electrified them, light was given off. This indicated that the electrons were giving off energy, or jumping back to the ground state The amount of energy required to jump energy levels is quantized, or measurable This amount of energy and the jumps can be observed with a spectroscope Elemental finger print = emission spectrum!!!

What does the quantum mechanical model look like? QUANTUM NUMBERS Principle quantum number (n) = Energy levels (1-7) Second Quantum number (l) = Sublevels (s, p, d, f) s = sphere p= dumbbell d= clover f= flower

Magnetic quantum number (ml) Orbitals (2 electrons in each one) (orientations) s has 1, can hold max 2 electrons p has 3, can hold max 6 electrons d has 5, can hold max 10 electrons f has 7, can hold max 14 electrons Think ‘seats on a bus’

Spin quantum number (m s): ½, -1/2 Electrons repel one another, sooooo To get 2 ‘in the same seat on the bus’ they must have opposite spin. This creates a slightly attractive force No 2 electrons can have the same 4 quantum numbers. This is a ‘map’ to the specific electron

Why clouds? Electrons are small and move very, very quickly. Think of a photograph and a videotape: If you take a photograph can you know the exact location of an electron? YES! Can you know the electron’s speed? NO! If you take a video, can you know the exact location of the electron? NO! Can you know the speed? YES! Heisenberg Uncertainty Principal: it is impossible to know the exact location and speed of an electron at any given time We use ‘probability clouds’ to describe location. These are where the electron is most likely to be located.

Homework Pg 366, 1-4 Pg 386, 20-24