Electron Configurations

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Presentation transcript:

Electron Configurations Day 1 - Notes Electron Configurations Introduction to Quantum Mechanical Model

After today you will be able to… Explain the organization of electrons within an atom Describe what an energy level, sublevel, and atomic orbital is Draw the shapes of each sublevel Predict how many electrons can be held in each energy level

The Quantum Mechanical Model of electrons within an atom says we cannot pinpoint where an electron is, but we can get the probability of where the electron is. Electron configurations show how electrons are distributed within an atom.

YOU COULDN’T HANDLE THE TRUTH!  Remember when. . . ? You envisioned an atom having a single center and “rings” around that center? However… that wasn’t the whole truth. YOU COULDN’T HANDLE THE TRUTH! 

Principal Energy Levels n=1,2,3,4, etc. Describes the average distance of an electron from the nucleus Energy increases as you move further from the nucleus n=2 n=1 Nucleus e-s highest in energy e-s lowest in energy

Within each energy level, electrons occupy sublevels.

Sublevels Correspond to the different areas an electron can be located in an atom. Represented by a letter Example: s, p, d, f, g, h, i, etc.

Sublevel Types s sublevel: “spherical” p sublevel: “dumbbell” d sublevel: “clover” f sublevel: “double clover”

Types of Sublevels in Energy Levels 1 1s 2 2s 2p 3 3s 3p 3d 4 4s 4p 4d 4f 5 5s 5p 5d 5f (5g)

Atomic Orbitals Each sublevel is oriented differently in 3-D space, and each orientation is called an atomic orbital Atomic orbitals can hold only two electrons

# of Atomic Orbitals in Sublevels Type of Sublevel # of Atomic Orbitals # of Electrons in sublevel s 1 2 p 3 6 d 5 10 f 7 14 [g 9 18]

(See sublevel shape diagram handout.) Orbitals for a particular sublevel are similar in shape, but different in orientation and size. (See sublevel shape diagram handout.)

# of Electrons in Each Energy Level # of Electrons in an Energy Level 1 s 2 s p 2 + 6 = 8 3 s p d 2 + 6 + 10 = 18 4 s p d f 2 + 6 + 10 + 14= 32

In general… s < p < d < f in energy within an energy level Electrons prefer to occupy the orbitals that require the least amount of energy

Questions? Complete WS 1

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