Quantum Mechanical Model Electron Placement

Presentation Transcript

Quantum Mechanical Model Electron Placement

Electron nuts and bolts Carries the negative charge of the iota Has mass of 0.0006 amu (6/10000 mass of a proton) Located in district around core Has a turn that makes an attractive field Either turns clockwise ("up") Or counterclockwise ("down") Atoms are electrically impartial, subsequently, the quantity of electrons = number of protons.

B. Electron Placement 1. Not Bohr Orbits Electrons once in a while, if at any point, circle in flawlessly characterized circles.

B. Electron Placement 2. Orbitals = Regions of Probability Where electrons are probably going to be discovered Determined by electron thickness Area of high thickness = numerous electrons are there = Orbital! Territory of low thickness = couple of electrons are there = Not Orbital!

2. Orbitals = Regions of Probability Orbital Shapes: s - circular shape, focused on core p - moronic chime molded, with three conceivable introductions on x-, y-or z-tomahawks. Idiotic ringer "neck" focuses on core d - clover formed, with four conceivable introductions in xy, yz, zx, and x 2 – y 2 planes; additionally one stupid chime with-ring shape, on z-pivot. Five aggregate orbital introductions. f – exceptionally complex shapes, with seven orbital introductions. (pictures don't do this shape equity.)

B. Electron Placement 3. Vitality Levels As Bohr estimated, we trust electrons have certain levels of vitality (level = n = 1, 2, 3, and so on.) For each level of vitality, there are sublevels of vitality:

3. Vitality Levels Each level n has n sublevels Each sublevel ( s, p, d, f ) relates to orbital shapes and introductions: Sublevel s contains one s orbital Sublevel p contains three p orbitals Sublevel d contains five d orbitals Sublevel f contains seven f orbitals

B. Electron Placement 4. Fitting electrons into place: Electron Configuration Aufbau Principle: Electrons will occupy the most reduced conceivable vitality level and sublevel. Pauli Exclusion Principle: Each orbital holds a most extreme of two electrons: one of each turn. Hund's Rule: Electrons will spread themselves out in a sublevel so that a greatest number of unpaired electrons result If a sublevel were a transport, electrons wouldn't share seats unless they needed to.

3 d 4 s E N E R G Y 3 p 3 s 2 p 2 s 1 s Electron Configuration Fluorine: 9 protons, 9 electrons 1 s 2 s 2 p 5