1. Modern Atomic Model and EMR

2. Understand how line spectra are created.
Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy.
Understand how line spectra are created.
Additional KEY Terms
Spectroscopy Emission Quantum
Line spectrum

3. Composed of radiated waves of both electrical and magnetic energy.
Maxwell (1860) - all energy radiated from objects (including visible light) is electromagnetic radiation.
Composed of radiated waves of both electrical and magnetic energy.

4. Amplitude: height of the wave from origin to crest.
Wavelength (λ - “lambda”): distance from point to the same point on the next wave.
Frequency (ν – “nu” or ƒ): number of wavelengths, or cycles, that pass a point per unit time.
Frequency measured in cycles per second (s-1), or the SI unit hertz (Hz)
Amplitude: height of the wave from origin to crest.
Wavelength and frequency do not affect amplitude
Wavelength and frequency are inversely related

5. Types of Electromagnetic radiation
f and λ determine what you see or hear, amplitude determines how loud or bright

6. c = λƒ c = λν All EMR radiates at 3.00 x 108 m/s in a vacuum.
This universal value (c) is a product of the wavelength and frequency of the radiated energy.
“speed of light”
c = λƒ
c = λν

7. Sunlight (white light) shone through a prism separates into a continuous spectrum of colours.
Each colour represents light of a different frequency – increasing frequency - ROY G BIV

8. Planck (1900)
Elements give off a unique colour of light when burned - used to detect the presence of a metal
This is known as a
Colour
Element
green
copper
yellow
sodium
red
strontium
yellow-green
barium
orange-red
calcium
purple
potassium
purple-red
lithium
If the light emitted is focused through a prism, a spectrum with distinct lines is produced.

9. Disclaimer – This is not as simple as my drawing.

10. Energy emitted by a heated element can be separated – producing emission spectrum.
(line spectrum)

11. The colored lines of the atoms (or Spectral Lines) are a kind of "signature" for the atoms.

12. Spectroscopy and spectrophotometry are techniques used to determine a substance’s emission spectrum

13. Planck's law: postulated that energy can only be gained or lost in discrete amounts – quanta.
Quantum is the minimum amount of energy gained or lost by an atom.
Energy contained in a quantum was directly related to the frequency of radiation emitted.
E = hf

14. E = hf E – energy of a quantum (Joules)
h – Plank’s constant (6.626 x J s)
f – frequency of absorbed or emitted EMR

15. Understand how line spectra are created.
CAN YOU / HAVE YOU?
Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy.
Understand how line spectra are created.
Additional KEY Terms
Spectroscopy Emission Quantum
Line spectrum