Chapter 5

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Bohr Model of the Atom

Electrons occupy circular orbits which represent quantum energy levlels

Quantum Mechanical Model (Schrodinger)

Utilizes an electron cloud which represents where the electron would be 90% of the time

Atomic Orbital

A region of space where there is a high probability of finding an electron.

n = what?

energy levels

s, p, d and f equal what?

energy sublevels

Aufbau Principle

electrons occupy the orbitals of lowest energy levels first

Pauli Exclusion Principle

2 electrons per orbital; must have opposite spin

Hund's Rule

1 electron per orbital until all orbitals of equal energy are filled

shorter wavelength =

higher frequency = higher energy

higher frequency = higher energy =

shorter wavelength

EM spectrum from long to short

radio - micro - infrared - visible light - ultraviolet - x-rays - gamma rays

What is true about atomic spectra

No two elements have the same emission spectrum!

ground state

the electron has its lowest possible energy

excited state

an electron moves to a higher energy level by absorbing a certain quantum of energy

light transmission

occurs when the electron drops back down to a lower energy level; this light is proportional to the energy change of the electron

classical mechanics

the physics of describing the motions of bodies larger than atoms

quantum mechanics

describes the motions of subatomic particles

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