Electrons in Atoms Chapter 5: Today we will learn:

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Presentation transcript:

Electrons in Atoms Chapter 5: Today we will learn: 5.3:Physics of the Quantum Mechanical model Electromagnetic spectrum Light Atomic Spectra Quantum Mechanics Chemistry _ Notes Dr. Chirie Sumanasekera 10 /24/ 2017

1. Electro magnetic spectrum

1. Electro magnetic (E.M.) spectrum Electro magetic spectrum: The total spectrum of radiation from radio waves to gamma rays The energy and frequency of the waves are proportional ( they increase or decrease together) But the Amplitude is inversely proportional to the Frequency (or energy). This means that when the Amplitude increases the frequency and energy decreases, and vice versa.

1. Electro magnetic (E.M.) spectrum Light: Is both a particle and a wave Particles of light are called “photons” It is a form of electromagnetic radiation Sun light is made up of a spectrum of color, each with a different wave length (the rainbow colors). Red has the lowest energy, frequency and highest wave length. Violet has highest frequency, energy and the lowest wave length. When sunlight passes through a prism, the mixture of colors separate based on wave length The speed of light is 2.998 x 108 m/s

Atomic spectra When atoms absorb energy, electrons move from their usual principal energy level (ground state) to a higher principal energy level. Then, electrons lose this energy by emitting it as light energy as they approach ground state. Atomic spectrum = the range of specific E.M. radiation frequencies emitted or absorbed by an atom Each atom has a distinct Atomic spectrum that is unique to each element. Atomic spectra can be used to identify the composition of unknown mixtures of metals, chemicals and even the make up of distant planets

Hydrogen Atomic spectrum Lyman series Ultra violet radiation emitted when electrons reach, n=1 Balmer series Visible light emitted when electrons reach, n=2 Paschen series Infrared radiation emitted when electrons reach, n=3 E = h. v E = amount of quantum energy released v = frequency h= Plank’s constant (6.626 x 10-34 JS)

3. Quantum mechanics Classical mechanics describes the motion of bodies larger than electrons while quantum mechanics describes the motion of atoms and sub atomic particles as waves. Heisenberg’s uncertainty principle: it is impossible to know exactly the velocity and the position of a particle at the same time. This principle does not a[ply to large bodies.