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Wave
- The way in which light travels through space. Made up of successive crests and troughs. Three primary characteristics.
- 1. amplitude
- 2. wavelenth
- 3. Frequency
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Wavelength
Represented by lambda(λ), it is the distance in nanometers or meters between two successive crests or troughs
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Frequency
Represented by nu(ν), it is the number of successive crests or troughs that pass a given point in a given unit time. the measure Hertz(hz) that represents one cycle per second.
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Electromagnetic radiation
Energy released as waves on the electromagnetic spectrum with both magnetic and electic fields and properties
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Electromagnetic spectrum
The entire continuous spectrum of electromagnetic radiation from gamma rays to long radio waves.
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Atomic spectrum
The characteristic spectrum of electomagnetic energy given off by each element with specific wavelenths.
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Photon
a stream of particles that we consider light to be generated as whose energy is given in joules
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Quantum numbers
Groups of numbers that represent states of sublevels of atoms.
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First Quantum Number
- represented by n;
- These are the principle energy levels.
- n can only be integral values starting with 1.
- n = 1, 2, 3, 4, ...
- n = 1 is considered the principal energy level and n = 2 the second primary energy level.
- As n increases so does evergy of the elecron
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Second Quantum Number
- Represented by l.
- l can take any integral value and starting with 1 and ending with (n-1).
- l = 0, 1, 2, ... , (n-1)
- in general in the nth energy level there are n different sublevels.
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l, sublevel
- the ublevels are represented by letters associated with values.
- 0 = s
- 1 = p
- 2 = d
- 3 = f
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Third Quantum Number
represented by ml this shows the direction in space of the electron cloud surrounding the nucleus.
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ml orbital
- This number is the value of any integral number between l and -l, including 0.
- for example for l = 1, ml could = -1,0,1
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Fourth Quantum Number
This is associated with electron spin and represented by ms.
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ms
Has nothing to do with the other quantum numbers and can only be two values. -1/2 or 1/2
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Pauli Exclusion Principle
Ir requires that no two electrons in an atom can have the same set of four quantum numbers.
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