5.1 –light and quantized energy –part 3 -...
TRANSCRIPT
5.1 – Light and Quantized Energy – Part 3
• OBJECTIVES: Students will be able to (SWBAT)
1. Calculate the energy of a wave
2. Explain how an emission spectrum helps to identify an
elementelement
• 5 lecture/10 reading questions
• 5-sentence summary
The colors have a specific
wavelength/frequency
VIOLET HAS SHORTEST
WAVELENGTH �
HIGHEST FREQUENCY �
MOST ENERGY
RED HAS LONGEST
WAVELENGTH �
LOWEST FREQUENCY �
LEAST ENERGY
Planck’s Energy of a Photon Equation
• Ephoton = h×ν
– Energy of a photon = Planck’s constant × frequency
• Planck’s constant = 6.626×10-34 J·sPlanck’s constant = 6.626×10 J·s
• Energy is measured in Joules (J) or kilojoules (kJ)
Energy from the Wavelength
• Energy can also be calculated from the
wavelength of a photon/wave
photon
h×cE =
λ
• Energy and wavelength have an inverse
relationship
photonE =λ
Converting from kJ � J
• Attach “×103 J” to any value that is in kJ
• Practice:
– 3.1 kJ � J 3.1 ×103 J– 3.1 kJ � J
– 0.086 kJ � J
– 2.0×10-5 kJ �J
3.1
0.086
2.0×10-5
×103 J
×103 J
×103 J
=2.0×10-2 J
Higher frequency = Higher energy
Gamma rays
are the
highest
Radio waves
are the
lowest
energy rays highest
energy rays
Emission Spectra
• White light, with all the frequencies of all the
colors, is continuous (no dark areas)
• Emission Spectra is when some of the colors
are emitted or released but others are not (so
you see dark areas)
Atomic Emission Spectra
• Each element has a very specific emission
spectra (different bands of colors)
• An element’s emission spectra can be used to
identify the element
• Guess which element is giving the spectrum
below?below?
HYDROGEN
Key Vocabulary Revisited
1. Atomic emission spectra
2. Frequency
3. Photon
HIGHER MEANS MORE ENERGY
PARTICLE WITH NO MASS WITH A SPECIFIC
AMOUNT OF ENERGY
4. Electromagnetic radiation
5. Wavelength
6. Electromagnetic spectrum
AMOUNT OF ENERGY
ALL FORMS OF ENERGY, INCLUDING LIGHT
LONGER MEANS SLOWER
SHOWS ALL THE FORMS OF RADIATION
INCLUDING THE COLORS OF VISIBLE LIGHT