Electrons are important because they determine how elements will bond and react with other elements.   

Bohr versus the REAL THING Electrons are important because they determine how elements will bond and react with other elements.    Bohr versus the REAL THING

Quantum Mechanical Model of the Atom (today’s model) Electrons DO occupy energy levels but their path is not definite; it is unknown!

Quantum Mechanical Model of the Atom (today’s model) Electrons DO occupy energy levels but their path is not definite; it is unknown! Heisenberg Uncertainty Principle - It is impossible to know the exact location and speed of an electron

Electron Configuration Tells us the probable location of an element’s electrons.

Electron Configuration Tells us the probable location of an element’s electrons. If YOU were an electron…. Atom = school

Electron Configuration Tells us the probable location of an element’s electrons. If YOU were an electron…. Atom = school Energy Levels = hallways

Electron Configuration Tells us the probable location of an element’s electrons. If YOU were an electron…. Atom = school Energy Levels = hallways Sub levels = classrooms Does every classroom have the same size and shape?

Electron Configuration Tells us the probable location of an element’s electrons. If YOU were an electron…. Atom = school Energy Levels = hallways Sub levels = classrooms Orbitals = desks

Electron Configuration Tells us the probable location of an element’s electrons. If YOU were an electron…. Atom = school Energy Levels = hallways Sub levels = classrooms Orbitals = desks Electrons = students

give the general distance from the nucleus Energy Levels – give the general distance from the nucleus   E N E R G Y

Energy Levels – give the general distance from the nucleus   Sublevels – the areas within the energy levels where the electrons are found.

give the general distance from the nucleus Energy Levels – give the general distance from the nucleus   Sublevels – the areas within the energy levels where the electrons are found. s “sphere”

1 2 3 4 5 6 7 1s 1s 2s 3s 4s 5s 6s 7s

give the general distance from the nucleus Energy Levels – give the general distance from the nucleus   Sublevels – the areas within the energy levels where the electrons are found. s p “sphere” “propeller”

1 2 3 4 5 6 7 1s 1s 2s 2 p 3s 3 p 4s 4 p 5s 5 p 6s 6 p 7 p 7s

give the general distance from the nucleus Energy Levels – give the general distance from the nucleus   Sublevels – the areas within the energy levels where the electrons are found. s p d “sphere” “propeller” “double propeller”

1 2 3 4 5 6 7 1s 1s 2s 2 p 3s 3 p 4s 3 d 4 p 5s 4 d 5 p 6s 5 d 6 p 6 d 7 p 7s

give the general distance from the nucleus Energy Levels – give the general distance from the nucleus   Sublevels – the areas within the energy levels where the electrons are found. s p d f “sphere” “propeller” “double propeller” “flower” (too complex)

1 2 3 4 5 6 7 1s 1s 2s 2 p 3s 3 p 4s 3 d 4 p 5s 4 d 5 p 6s 5 d 6 p 7s 6 d 7 p 4f 5f

Electron Configuration 1s2 Energy Level – Principal Quantum # (possibilities are 1-7)

Electron Configuration 1s2 Energy Level – Principal Quantum # (possibilities are 1-7) Sublevel (s, p, d, or f)

Electron Configuration 1s2 # of electrons s: 1 or 2 p: 1-6 d: 1-10 f: 1-14 Energy Level – Principal Quantum # (possibilities are 1-7) Sublevel (s, p, d, or f)

Electron Configuration 1s2 # of electrons s: 1 or 2 p: 1-6 d: 1-10 f: 1-14 Energy Level – Principal Quantum # (possibilities are 1-7) Sublevel (s, p, d, or f) If you add up all of the electrons, it should equal the atomic # of the element

Aufbau Principle Electrons fill sublevels of the lowest energy first.

1 2 3 4 5 6 7 1s 1s 2s 2 p 3s 3 p 4s 3 d 4 p 5s 4 d 5 p 6s 5 d 6 p 7s 6 d 7 p 4f 5f

Name the element and circle the sublevel with the highest energy: _____ 1s2 2s2 2p6 3s2 3p6 4s2 3d6 _____ 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d6 _____ 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p3 Fe Os Bi

Write the electron configuration: Br Pb Er 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f11

Noble Gas Configuration – shortcut to electron configs based on the last noble gas. Noble gases are found in Group 18. Example: [Ar] 4s2 3d8 Where [Ar] represents Argon – the last noble gas filled

Name the element: S _____ [Ne] 3s2 3p4 _____ [Xe] 6s2 4f14 5d6 Os _____ [Kr] 5s2 4d10 5p3 Os Sb

Write the noble gas configuration: Se Mo Ar [Ar] 4s2 3d10 4p4 [Kr] 5s2 4d4 [Ne] 3s2 3p6

Orbital Notation – visually shows the location of the electrons. Only 2 electrons fit in each orbital. Example: __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ [Xe] 6s2 4f14 5d10 6p5 You must draw each orbital, even if it is empty. Hund’s Rule – One electron enters each orbital until all orbitals have one electron with parallel spins Pauli Exclusion Principle – No 2 electrons can have the same location and same spin ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ Energy Levels Sublevels # of Orbitals Maximum # of electrons s p d f 1 - 7 1 2 2 - 7 3 6 3 - 6 5 10 4 - 5 7 14

Draw the orbital notations for the following elements: Fe – O –

Lewis Dot Structures – shows the valence electrons. Valence Electrons – outershell electrons You can count valence electrons by looking at the group #. (if it’s a double digit, subtract 10) Remember Hund’s Rule when drawing Lewis Dots BUT draw all “s” electrons together on the right. Examples: C Br Ba N