Chem light unit

Part of a wave

Part of a wave

a. crest

b. trough

c. amplitude

d. wavelength

If the wavelength is short does it have high or low energy

high

If the wavelength is long does it have high or low energy

low

what color has the shortest wavelegth and highest energy

violet

what color has the longest wavelength and lowest energy

red

1 meter is how many nano meters

10^9 nanometers

1 nanometer is how many meters

10^-9 meters

frequency

number of wave cycles

what has the highest frequency

gamma rays

what has the lowest frequency

radio waves

what has the shortest wavelength

gamma rays

what has the longest wavelength

radio waves

Explain how atoms of different elements can emit different colors/wavelengths. Your explanation should include the terms: energy levels, electrons, energy

because of the unique arrangement of their electrons in energy levels. When an atom absorbs energy, its electrons move to higher energy levels and when the move  to lower energy levels, they release the absorbed energy in the form of light. Each element has specific energy level spacings, so when electrons transition between these levels, the emitted light corresponds to specific colors or wavelengths for each element. 

What spectrum is this

Continuous spectrum: contains all wavelengths of light in a certain range (white light —> diffraction grating —> spectrum)

What spectrum is this

Emission spectrum: showing the light in the wavelengths in a line with the color they emitted (hot gas —> diffraction grating —> spectrum)

What spectrum is this

Absorption spectrum: oppisite of emission soectrum, the color that would be emitted would be a balck line and the “background” would be the rainbow (white light —> diffraction grating —> spectrum)

how can we identify an element based on an emission spectrum

bright lines will show up corresponding to the difference between energy levels of the elements

What are the 2 parts of salt

an atomic compound made of a positive ion and a negative ion.

What is the purpose of the flame or what does the flame provide to the salt?

to determine the identity of an unknown metal and the flame provided energy to the electrons

Why do different salts give off different colored light?

As the salt burns, the extra energy is lost — as light. The color of that light depends on the amount of energy being released.

staircase analogy

The stairs represent the energy levels, it requires specfic amounts of energy for the electron to gain and loose energy to chnage energy levels, all energy levels require differnet amount of energy.

Electromagnetic radiation

A form of energy that is produced by eletric & magnetic feild working together

Amplitude

a measurement of the amount of energy transferred by a wave, lower amplitude makes light less bright ( symbol - A)

Frequency

number of wave cycles (full wave) used in hertz, high frequecny = short wavelength symbol = v (nu)

Quanta

specific individual seprate amounts of energy

Quantized

electrons can pass certain energy values

photoelectric effect

When light shines on a metal, electrons can be ejected from the surface of the metal

The photoelectric effect tells us the energy is quantized, it is discrete and absorbed into packets or photons of energy. SO important because it supports why electrons gain and lose energy in certain amounts of packets. 

photon

quantum of electromagnetic radiation

prism

when light passes through the color spectrum shows

wavelength

lambda λ

how is light produced

For light to be produced electrons must absorb a quanta of energy and move to a higher energy level than the electrons need to release the quanta of energy to produce light 

Does brightness afccts the energy

does not affect the energy same wavelength and energy

to take in

absorb

to give off

emit

where is visible light located on the electromagnetic spectrum

bewteen infrared and ultra violet